Chem Exam 3
The oxidizing agent in a redox reaction is itself
reduced
gain of electrons
reduced
In Cl2(g) + 2NaBr(aq) -> Br2(aq) + 2NaCl(aq) Br
reduced; oxidizing agent
In S(s) + O2(g) -> SO2(g) sulfur
reducing agent
The substance that causes the reduction is
reducing agent
in equilibrium expression, square brackets
refer to molar concentrations
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 0.92%(m/v) NaCl solution
remain unaffected
in a solution, solutes
remain uniformly distributed & will not settle out w time
When 60.0 mL of a 1.00 M solution is diluted by adding 30.0 mL of water, the amount of solute present
remains the same
conjugate base is the species that
remains when proton is removed from Bronsted-lowry acid
displacement reaction aka
replacement reaction
in HA(aq) + H2O(l) <=> H3O+(aq) + A-(aq) A (in HA)
represents any acid
Breaking the bonds of the reactants
requires energy; bond formation releases energy
Predict the solubility of each of the following solutes in the solvent indicated. Na2SO4 (an ionic solid) in water
soluble
Predict the solubility of each of the following solutes in the solvent indicated. ethyl alcohol (a polar liquid) in chloroform (a polar liquid)
soluble
Predict whether the following compound is soluble or insoluble in water: CuBr2
soluble
Predict whether the following compound is soluble or insoluble in water: NH4Br
soluble
C6H6(g) + 3H2(g) -> C6H12(g) + heat Indicate if the following will shift the equilibrium to the right or left. Also indicate if the changes will change the value of Keq. Increasing the concentration of H2
right; no
C6H6(g) + 3H2(g) -> C6H12(g) + heat Indicate if the following will shift the equilibrium to the right or left. Also indicate if the changes will change the value of Keq. Increasing the pressure
right; no
Identify the solute in: salt (NaCl) in water
salt
KCl is an example of
salt
NH4Br is an example of
salt
Na2SO4 is an example of
salt
NaCl is an example of
salt
Indicate whether the osmotic pressure of a 0.1 M NaCl solution will be less than, the same as, or greater than that of each of the following solutions. 0.1 M NaBr
same
ALPHA PARTICLE
same as helium nucleus w no electrons
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 0.28 M glucose
same size
Will red blood cells swell, remain the same size, or shrink when placed in 0.14 M in both glucose and sucrose
same size
Will red blood cells swell, remain the same size, or shrink when placed in 0.28 M glucose
same size
Will red blood cells swell, remain the same size, or shrink when placed in 0.92%(m/v) NaCl solution
same size
Predict whether the following compound is soluble or insoluble in water: Pb(NO3)2
soluble
Classify each of the following solutions as saturated, unsaturated, or supersaturated based on the following observations. excess undissolved solute is present at the bottom of the solution container.
saturated
Classify each of the following solutions as saturated, unsaturated, or supersaturated based on the following observations. heating the solution causes excess undissolved solute present to dissolve.
saturated
Using Table 8-2, classify each of the following types of ionic compounds using the solubility categories soluble, soluble with exceptions, insoluble, or insoluble with exceptions. nitrates
soluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. Cu(NO3)2
soluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. CuCl2
soluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. CuSO4
soluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. ammonium phosphate
soluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. calcium nitrate
soluble
A compound has a solubility in water of 35 g/L at 0°C. If 25 g of this compound is added to 0.5 L of water at 0°C, is the resulting solution saturated or unsaturated?
saturated solution
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. sodium phosphate
soluble
Zn(NO3)2 is a
soluble ionic compound
Using Table 8-2, classify each of the following types of ionic compounds using the solubility categories soluble, soluble with exceptions, insoluble, or insoluble with exceptions. chlorides
soluble with exceptions
In the common case of solid-in-liquid solutions in which
solute is ionic compound, "like dissolves like" is not adequate.
Dialysis is the movement of
solutes across semipermeable membrane
When a substance produces charged particles when dissolved in water
solution conducts electricity & substance is classified as electrolyte
A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0°C. Based on the data in Table 8-1, should this solution be characterized as saturated or unsaturated
unsaturated
Classify each of the following solutions as saturated, unsaturated, or supersaturated based on the following observations. The amount of solute dissolved is less than the maximum amount that could dissolve under the conditions at which the solution exists.
unsaturated
supersaturated solution
unstable solution that temporarily contains more dissolved solute than that present in saturated solution
Almost all radionuclides
used in nuclear medicine are synthetic radionuclides.
the more acidic you are, pKa
value goes down
If the temperature changes,
value of Keq also changes
For CO(g) + 2H2(g) <- ——> CH3OH(g) At this new equilibrium state,
value of [H2] will be lower bc more has reacted w added CO & value of [CH3OH] will be higher
Adding a nonvolatile solute to a pure solvent produces which of the following effects? a. vapor-pressure lowering b. freezing-point elevation c. boiling-point depression d. no correct response
vapor-pressure lowering
Solution has
variable composition
Predict whether the following solutes are very soluble or slightly soluble in water. CH3OH (a polar liquid)
very soluble
%(v/v)
volume of solute/volume of solution x 100
Ionizing radiation is radiation
w sufficient energy to remove electron from atom or molecule.
Identify the solute in: a solution containing 50.0 mL of methanol and 30.0 mL of water
water
Identify the solvent in: CO2(g) in water
water
Identify the solvent in: a solution containing 10.0 g of LiBr and 100.0 g of water
water
Identify the solvent in: a solution containing 3.0 g of AgNO3 and 15 mL of water
water
Identify the solvent in: a solution of 3.0 x 10^1% ethanol and 7.0 x 10^1% water
water
Identify the solvent in: salt (NaCl) in water
water
For each solute, identify the better solvent: water or carbon tetrachloride CH2O
water (H2O)
For each solute, identify the better solvent: water or carbon tetrachloride CaCl2
water (H2O)
With Osmosis,
water always moves in direction to dilute things
when red blood cells are placed in physiological saline solution, a 0.92%(m/v) sodium chloride solution,
water flow is balanced [neither hemolysis nor crenation occurs]
When salt water is taken into the stomach,
water flows out of stomach wall membranes & into stomach; [tissues become dehydrated]
Osmosis is the process in which
water flows through semipermeable membrane (ex: cell membrane) from lower concentration of ions to higher concentration of ions
Why is O2 soluble in water?
water has a dipole; oxygen has only london forces [so oxygen is just a little soluble in water]
Why does the use of a salt solution in Kimchi act as a preservative against bacterial decay?
water passes into salt solution, dehydrating bacterial cells and making them harmless
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other CH3COOH
weak acid
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other HCN
weak acid
a small percentage of its protons are transferred to water
weak acid
Combo for good buffer is
weak acid & equal amount of its conjugate base
Buffer solutions contain either
weak acid & salt of that weak acid or weak base & salt of that weak base.
HF is a
weak acid but will kill you bc yanks calcium out of you
Buffers are composed of a __________ and its ____________.
weak acid, conjugate base
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other (CH3)3N
weak base
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other NH3
weak base
Classify these compounds as strong electrolytes, weak electrolytes or nonelectrolytes H2CO3
weak electrolyte
HF(aq) <=> H^+(aq) + F^-(aq)
weak electrolyte
You get conjugate acid/base
when dissolve acid/base in water
A special group of physical properties that change
when solute is added are colligative properties.
The value of the equilibrium constant tells us
whether have mostly reactants or mostly products or nearly equal amount of each.
Value of Ka tells you
whether or not comes apart when put in water
you have to be told
whether reaction releases gamma ray [can't predict]
The concentrations of pure liquids and pure solids,
which are constants, are never included in equilibrium expression.
in 238U92 -> 4He2 + 234Th90
written same as 12C6 [atomic number on bottom]
Does the following ion form a compound with Pb2+ that is soluble in water? C2H3O2^-
yes
Does the following ion form a compound with Pb2+ that is soluble in water? NO3^-
yes
Identify whether or not the following set contains an acid-base conjugate pair HNO2 and NO2^-
yes
Identify whether or not the following set contains an acid-base conjugate pair HS^- and H2S
yes
Identify whether or not the following set contains an acid-base conjugate pair NH3 and NH4^+
yes
Indicate whether or not each of the following chemical reactions represents a combustion reaction. ( 4Fe + 3O2 -> 2Fe2O3
yes
Indicate whether or not each of the following chemical reactions represents a combustion reaction. ( 4NH3 +3O2 -> 2N2 +6H2O
yes
Indicate whether or not each of the following chemical reactions represents a combustion reaction. ( C2H6O + 3O2 -> 2CO2 + 3H2O
yes
Indicate whether or not product formation increases if the size of the reaction container is increased for each of the equilibrium systems in 2KClO3(s) + heat <=> 2KCl(s) + 3O2(g)
yes
Indicate whether or not product formation increases w increasing temperature in each of the following equilibrium systems 2KClO3(s) + heat <=> 2KCl(s) + 3O2(g)
yes
Indicate whether or not product formation increases w increasing temperature in each of the following equilibrium systems N2(g) + 2O2(g) + heat <=> 2NO2(g)
yes
Indicate whether or not product formation increases w increasing temperature in each of the following equilibrium systems heat + 2N2(g) + 6H2O(g) <=> 4NH3(g) + 3O2(g)
yes
Indicate whether or not the two members of each of the following pairs of compounds have like solubility (both soluble or both insoluble). CaCO3 and Ca3(PO4)2
yes
Indicate whether or not the two members of each of the following pairs of compounds have like solubility (both soluble or both insoluble). KNO3 and K2SO4
yes
Indicate whether or not the two members of each of the following pairs of compounds have like solubility (both soluble or both insoluble). NH4Cl and NH4Br
yes
Indicate whether or not the two members of each of the following pairs of compounds have like solubility (both soluble or both insoluble). Ni(OH)2 and Ni3(PO4)2
yes
Will the following combination make a buffer solution? H2CO3 and NaHCO3
yes
Will the following combination make a buffer solution? HC2H3O2 and KC2H3O2
yes
Will the following increase the rate of reaction? increasing the concentration of a reactant
yes
if you remove H,
you remove its positive charge
if you get more oxygen,
you're oxidized
If you lose oxygens,
you're reduced
in Cl2(g) + 2NaBr(aq) -> Br2(aq) + 2NaCl(aq) what is the charge of Br2 (on the product side)
zero bc bromine is in elementary state [not an ion]
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? 500 g (0.500 kg)
-3.7 degrees celsius
What is the freezing point of the solution 3.00 moles of glucose (a molecular compound)
-5.58 degrees celsius
What is the freezing point of the solution 3.00 moles of lactose (a molecular compound)
-5.58 degrees celsius
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? 250 g (0.25 kg)
-7.4 degrees celsius
What is the oxidation number of S in each of the following molecules? S8
0
pH ranges between
0 to 14 in aqueous solutions at 24°C.
The concentration of bilirubin in a blood sample is found to be 0.55 mg/dL. express this concentration in the following units: g/100 mL
0.00055 g/100 mL
The concentration of bilirubin in a blood sample is found to be 0.55 mg/dL. express this concentration in the following units: mass-volume percent
0.00055% (m/v)
What is the molarity of the solution prepared by diluting 25.0 mL of 0.220 M NaCl to each of the following final volumes? 2.00 L
0.00275 M
The concentration of bilirubin in a blood sample is found to be 0.55 mg/dL. express this concentration in the following units: g/L
0.0055 g/L
For each of the following NaOh solutions, the volume of the solution and its molarity are given. Calculate the number of moles of NaOh present in each solution. 125 mL solution, 0.125 M
0.0156 moles
In a sulfuric acid (h2SO4)-sodium hydroxide (NaOh) acid-base titration, 17.3 mL of 0.126 M NaOh is needed to neutralize 25.0 mL of h2SO4 of unknown concentration. Find the molarity of the h2SO4 solution, given that the neutralization reaction that occurs is H2SO4(aq) +2NaOH(aq) -> Na2SO4(aq) + 2H2O(l)
0.0436 mol/L
How many moles of NaCl are present in 225 mL of a 0.355 M NaCl solution?
0.0799 moles
If 200.0 mL of a 0.40 M NaCl solution is diluted with water to form 800.0 mL of solution, the molarity of the new solution is
0.10 M
What has a higher solute concentration between 0.10 M glucose and 0.07 M glucose solution?
0.10 M glucose
The hCl in a 0.10 M hCl solution is 100% dissociated. What are the molar concentrations of hCl, h3O+, and Cl− in the solution?
0.10 M in both H3O^+ and Cl^- ions and zero in HCl
The number of grams of NaCl present in 10.0 g of a 1.00 %(m/m) NaCl solution is
0.100 g
Which of the following solutions is isotonic with respect to red blood cells? a. 0.20 M lactose b. 0.28 M lactose c. 0.35 M lactose d. no correct response
0.28 M lactose
What is the molarity of 0.500 L of NaOH solution if it contains 6.00 g of NaOH?
0.300 M
Normal saline solution that is used to dissolve drugs for intravenous use is 0.92%(m/v) NaCl in water. how many grams of NaCl are required to prepare 35.0 mL of normal saline solution?
0.32 g NaCl
Determine the molarities of the following solutions. 20.0 g of NaOH are dissolved in enough water to give 1.50 L of solution.
0.333 mole NaOH/L solution
A solution contains 0.23 mole of sulfate ion (SO4^2−). how many equivalents of SO4^2− ion are present in the solution?
0.46 Eq SO4^2-
The concentration of bilirubin in a blood sample is found to be 0.55 mg/dL. express this concentration in the following units: mg/100 mL
0.55 mg/100 mL
Calculate the mass, in grams, of K2SO4 needed to prepare 32.00 g of 2.000%(m/m) K2SO4 solution.
0.6400 g
How many moles of KCl are present in 355 mL of a 2.50 M KCl solution?
0.888 moles
For each of the following hCl solutions, the moles or grams of solute present and the total solution volume are given. Calculate the molarity of each solution. 30.0 g HCl, 875 mL solution
0.940 M
For each of the following hCl solutions, the moles or grams of solute present and the total solution volume are given. Calculate the molarity of each solution. 1.40 moles HCl, 1.45 L solution
0.966 M
For each of the following hCl solutions, the moles or grams of solute present and the total solution volume are given. Calculate the molarity of each solution. 0.850 mole hCl, 0.867 L solution
0.980 M
The results of dissolving these solutes in water are: NaCl
1 mole of NaCl produces 2 moles of particles [ions] bc soluble ionic solutes dissociate into ions
The results of dissolving these solutes in water are: glucose [molecular solute]
1 mole of glucose produces 1 mole of particles [molecules] bc molecular solutes remain in molecular form in solution
For ions with a charge of 2 (plus or minus) the mole-equivalent relationship is
1 mole of ion = 2 equivalents of ion
Monoprotic acids supply
1 proton [H+ ion] during acid- base reaction
For a complete neutralization reaction between 0.10 M Ca(OH)2 and 0.10 M HNO3, the base and the acid will react in which of the following molar ratios?
1 to 2
Major types of chemical reactions:
1) Combination 2) Decomposition 3) Displacement 4) Exchange 5) Combustion
Sources of Background Radiation
1) Cosmic radiation 2) Rocks/soil & minerals in body 3) Food & drink 4) Radon seepage in buildings [55%]
Ways to recognize redox reactions?
1) Gain or loss of oxygen 2) Gain or loss of electrons
Identify the conjugate acid-base pairs associated with the following acid-base reaction. HC2H3O2 + H2O -> H3O+ + C2H3O2−
1) HC2H3O2 and C2H3O2^- 2) H2O and H3O^+
HCN + NH2^- <=> CN^- + NH3 Name the conjugate pairs
1) HCN and CN^- 2) NH2^- and NH3
What are the commonly encountered strong acids?
1) HCl 2) HBr 3) HI 4) HNO3 5) HClO3 6) HClO4 7) H2SO4
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) what are the 2 conjugate acid-base pairs related by the loss/gain of H^+
1) HF and F^- 2) H3O^+ and H2O
Theraputic criteria are
1) Hi energy 2) Short duration 3) Internal or external
Diagnostic examples
1) Identification [infection/tumor] 2) Function [heart/thyroid]
Tell me the factors that increase chemical reaction rate
1) Increase in State of Subdivision 2) Increase in Reactant Concentration 3) Increase in temp 4) addition of catalyst
What are the group IA strong hydroxide bases?
1) LiOH 2) NaOH 3) KOH 4) RbOH 5) CsOH
What are the commonly encountered strong hydroxide bases?
1) LiOH 2) NaOH 3) KOH 4) RbOH 5) CsOH 6) Ca(OH)2 7) Sr(OH)2 8) Ba(OH)2
What are the 3 different ways to represent percent concentration?
1) Percent by mass 2) Percent by volume 3) Mass-volume percent
2 methods of expressing concentration:
1) Percent concentration 2) Molarity
Tell me the 4 factors that affect reaction rate
1) Physical nature of reactants 2) Reactant concentrations 3) Reaction temp 4) Presence of catalysts
Name some salts
1) Sodium chloride [table salt] 2) Sodium bicarbonate [baking soda]
Name some colligative properties
1) Vapor-pressure lowering 2) Boiling-point elevation 3) Freezing-point depression 4) Osmotic pressure
How can you tell if a redox reaction is occurring?
1) When ions are involved, determine if there is change in charges 2) For reactions w metals & nonmetals, predict gain or loss of electrons
Types of radioactive emissions
1) alpha (α) particle 2) beta (β) particle 3) gamma (γ) ray
What are the three central concepts associated with collision theory?
1) collision orientation 2) activation energy 3) molecular collisions
examples of ionizing radiation
1) cosmic rays 2) X rays 3) UV light
Detection of radiation
1) film badges 2) geiger counters
What controls how fast a reaction goes?
1) physical reaction [s, l, g] 2) high concentration reacts faster 3) high temp reacts faster
Examples of non-ionizing radiation
1) radiowaves 2) microwaves 3) infrared light 4) visible light
List the four major sources of low-level exposure to background radiation for an average American.
1) radon seepage 2) cosmic radiation 3) rocks & minerals 4) food & drink
Components of a solution
1) solvent 2) solute
What are the factors affecting the rate of solution formation?
1) state of subdivision of solute 2) degree of agitation during solution preparation 3) temp of solution components
how do nuclear equations differ from chemical equations?
1) symbols in nuclear equations stand for nuclei rather than atoms. 2) Mass numbers & atomic numbers [nuclear charge] are always specifically included in nuclear equations 3) elemental symbols on both sides of equation frequently are not same in nuclear equations.
Consider the solution of NaOH made by dissolving 100.0 g of solute in 250.0 mL of solution. Calculate the molarity.
10.00 M
Give me a conversion factor for the percent concentration 25%(m/v) sucrose solution
100mL solution/25g sucrose
What is the boiling point of a solution that contains 1.00 kg of water and each of the following quantities of solute? 3.00 moles of glucose (a molecular compound)
101.53 degrees celsius
What is the boiling point of a solution that contains 1.00 kg of water and each of the following quantities of solute? 3.00 moles of lactose (a molecular compound)
101.53 degrees celsius
how many grams of glucose must be added to 275 g of water in order to prepare each of the following percent- by-mass concentrations of aqueous glucose solution? 31.0%
124 g
how many grams of glucose must be added to 275 g of water in order to prepare each of the following percent- by-mass concentrations of aqueous glucose solution? 5.00%
14.5 g
For each of the following solutions, how many milliliters of water should be added to yield a solution that has a concentration of 0.100 M? 50.0 mL of 3.00 M NaCl
1450 mL
"there are 15g of NaCl in 100g of solution"
15 is measured; 100 is not [so 2 sig figs]
how many meq of hCO3− are present in a solution that also contains 75 meq of Na+, 83 meq K+, 10 meq Ca2+, and 153 meq Cl−?
15 mEq
Calculate the mass-volume percent of MgCl2 in each of the following solutions. 85 g of MgCl2 in enough water to give 580 mL of solution
15% (m/v)
A solution is prepared by adding 15.0 g C6H12O6 to 75.0 g H2O. What is the mass percentage of C6H12O6 in this solution?
16.7%
Calculate the number of grams of NaOH needed to prepare each of the following amounts of solution. 2.00 L of 2.00 M NaOH
160. g
115 g of CaCl2 are needed to make 276.4 g of a solution that is 41.5% calcium chloride in water. How many grams of water are needed to make this solution?
161 g H2O
State the composition of an alpha particle in terms of protons and neutrons.
2 protons & 2 neutrons
What is the ratio of the osmotic pressures of 0.30 M NaCl and 0.10 M CaCl2?
2 to 1
Which member of each of the following pairs of compounds has the higher boiling point? 1.0 M KBr or 2.0 M KBr
2.0 M KBr
Calculate the mass-volume percent of MgCl2 in each of the following solutions. 5.0 g of MgCl2 in enough water to give 250 mL of solution
2.0% (m/v)
Calculate the number of grams of NaOH needed to prepare each of the following amounts of solution. 0.100 L of 0.50 M NaOH
2.00 g
After all of the water is evaporated from 10.0 mL of a CsCl solution, 3.75 g of solid CsCl remains. Calculate the original concentration of the CsCl solution in the following units. molarity
2.23 M
Calculate the ph for each of the following solutions. [H3O+] = 5.70 × 10^−3
2.244
25.0 g of C2H4O2 are added to enough water to produce 175.0 mL of solution. What is the molarity of this solution?
2.38 M
For each of the following aqueous NaCl solutions, the mass of solute and the mass of solvent present are given. Calculate the mass percent of NaCl present in each solution. 520.0 mg NaCl, 2.00 g H2O
20.6% (m/m)
If 100.0 mL of 8.0 M NaCl solution is diluted with water to form a 4.0 M solution, what is the volume, in mL, of the new solution?
200.0 mL
Approximately how many laboratory-produced radionuclides are known?
2000
For the reversible reaction: A(g) <=> B(g) which K values would indicate that there is more B than A at equilibrium? A) K = 5 x 10^-5 B) K = 0.4 C) K = 2000 D) K = 1 x 10^9
2000 & 1 x 10^9
Which of the following is the daughter nuclide for the alpha decay of 212Po84
208Pb82
A typical dose of iron(II) sulfate (FeSO4) used in the treatment of iron-deficiency anemia is 0.35 g. how many milliliters of a 0.10 M iron(II) sulfate solution would be needed to supply this dose?
23 mL solution
How many grams of sucrose are needed to make 775 mL of a 30.0% (w/v) sucrose solution?
233 g sucrose
Isopropyl alcohol is mixed with water to produce a 33.0% (v/v) alcohol solution. How many milliliters of each component are present in 705 mL of this solution?
233 mL alcohol & 472 mL water
Beta Particle Decay (β):
234Th90 -> 234Pa91 + 0e-1
Alpha particle decay (α)
238U92 -> 4He2 + 234Th90
Gamma Ray Emission (γ):
238U92 -> 4He2 + 234Th90 + 2 0Y0
For the reaction H2(g) + I2(g) -> 2HI(g) The equilibrium concentrations at 25°C are [H2] = 0.0510 mol/L, [I2] = 0.174 mol/L and [HI] = 0.507 mol/L. Use the equilibrium expression to determine the value of Keq at 25°C.
29.0
Consider the following equilibrium system. N2(g) + O2(g) <=> 2NO(g) Write the chemical equation for the reverse reaction.
2NO(g) -> N2(g) + O2(g)
Determine the final concentration of each of the following solutions after 20.0 mL of water has been added. 30.0 mL of 5.0 M AgNO3 solution
3.0 M
Determine the final concentration of each of the following solutions after 20.0 mL of water has been added. 30.0 mL of 5.0 M NaCl solution
3.0 M
What is the final concentration when 0.50 L of 6.0 M HCl stock solution is diluted to a final volume of 1.0 L?
3.0 M
The ph of a solution with [h3O+] = 2.2 × 10^−4 is between
3.0 and 4.0
If you have a 0.150 M solution of Na2SO4 what is the concentration of Na^+ ions?
3.00 x 10^-1 moles Na^+
A solution is prepared by dissolving 10.0 grams of glucose in enough water to give 325 mL of solution. What is the mass-volume percent concentration of glucose in the solution?
3.08% (m/v)
How many milliliters of 11.0 M HCl(aq) are needed to prepare 345.0 mL of 1.00 M HCl(aq)?
3.14 x 10^1 mL
Calculate the pKa for HF given that the Ka for this acid is 6.8 × 10^-4
3.2
If pH = 4.50 then [H3O+] =
3.2 x 10^-5
How many moles of NaOH are present in 27.5 mL of 0.120 M NaOH?
3.30 x 10^-3 mol
For each of the following aqueous NaCl solutions, the mass of solute and the mass of solvent present are given. Calculate the mass percent of NaCl present in each solution. 20.0 g NaCl, 565.0 g H2O
3.42% (m/m)
What is the pH of a solution with a [H+] of 3.2 x 10 - 4 M.
3.49
how many grams of glucose must be added to 275 g of water in order to prepare each of the following percent- by-mass concentrations of aqueous glucose solution? 1.30%
3.62 g
If 1.50 gram of a 2.00-gram sample of a radioactive substance undergoes decay in 60 minutes, then the half-life of the sample is
30 minutes
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. Table salt in water with P = 1 atm and T = 60°C Table salt in water with P = 1 atm and T = 50°C
60 degrees celsius
how many grams of glucose must be added to 275 g of water in order to prepare each of the following percent- by-mass concentrations of aqueous glucose solution? 20.0%
68.8 g
Give me a conversion factor for the percent concentration 6%(v/v) methanol solution
6mL methanol/100mL solution
How many strong acids are there?
7 [three Halo & 4 others]
how many liters of a 0.100 M solution can be prepared from 60.0 g of each of the following solutes? NaNO3
7.06 L
Calculate the mass percent of solute in the following solutions. 6.50 g of NaCl dissolved in 85.0 g of H2O
7.10% (m/m)
Calculate the ph for each of the following solutions. [H3O+] = 7.23 × 10^−8
7.141
Calculate the number of grams of NaOH needed to prepare each of the following amounts of solution. 552 mL of 0.333 M NaOH
7.35 g
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. Table sugar in water with P = 2 atm and T = 40°C Table sugar in water with P = 1 atm and T = 70°C
70 degrees celsius
The ph for a solution with [Oh−] = 1.0 × 10^−6 is
8.00
What is the molarity of a solution when 25.0 mL of 0.500 M NaCl is diluted to 150.0 mL?
8.33 x 10^-2 M
What is the pH of an aqueous solution with a hydrogen ion concentration of [H^+] = 4.1 x 10^-9 M
8.39
What is the percent-by-mass, %(m/m), concentration of sucrose (table sugar) in a solution made by dissolving 7.6 g of sucrose in 83.4 g of water?
8.4%
Calculate the pH of a solution that is 0.129 M HCl
8.894 x 10^-1
Calculate the value of the equilibrium constant for the equilibrium system 2NO(g) -> N2(g) + O2(g) at 1000°C, given that the equilibrium concentrations are 0.0026 M for NO, 0.024 M for N2, and 0.024 M for O2.
85
For each of the following solutions, how many milliliters of water should be added to yield a solution that has a concentration of 0.100 M? 1.45 L of 6.00 M NaCl
85,600 mL
A solution is 0.0030 M in PO4^3− ion. What is this ion concentration in mEq/L?
9.0 mEq PO4^3-/L
Calculate the mass percent of solute in the following solutions. 12.5 g of KNO3 dissolved in 125 g of H2O
9.06% (m/m)
how many liters of a 0.100 M solution can be prepared from 60.0 g of each of the following solutes? HNO3
9.52 L
A 125-mL sample of a mouthwash contains 12 mL of ethyl alcohol. What is the percent-by-volume concentration of ethyl alcohol in the mouthwash?
9.6% (v/v)
The beta decay of 234Th90 produces a nuclide of which of the following elements?
91
What is the highest-atomic-numbered naturally occurring element?
92
Which of the following combinations of substances would produce a buffer? a. a strong acid and a salt of the strong acid b. a weak acid and a salt of the weak acid c. a salt of a strong acid and a salt of a weak acid d. no correct response
a weak acid and a salt of the weak acid
Strong acids yield
a weak conjugate base
What is the oxidation number of chlorine in each of the following chlorine-containing compounds? a) NaClO b) NaClO3 c) HClO4 d) PCl3
a) +1 b) +5 c) +7 d) -1
A solution contains 48 meq of Ca ion. Based on this information, a. how many eq of Ca2+ ion are present? b. how many moles of Ca2+ ion are present?
a) 0.048 Eq b) 0.024 mole
Determine the molarity of a NaOh solution when each of the following amounts of acid neutralizes 25.0 mL of the NaOh solution. a. 5.00 mL of 0.250 M hNO3 b. 20.00 mL of 0.500 M h2SO4 c. 23.76 mL of 1.00 M hCl d. 10.00 mL of 0.100 M h3pO4
a) 0.0500 M b) 0.800 M c) 0.950 M d) 0.120 M
The half-life of an isotope is 2.5 hours. How much, in grams, of a 1.00 g sample of this isotope will remain after A) a period of 4 lives? B) a period of 10 hours?
a) 0.0625 b) 0.0625
Indicate the number of equivalents in each of the following molar quantities of ions. a. 1 mole Na+ b. 1 mole NO3− c. 1 mole Mg2+ d. 1 mole hCO3−
a) 1 Eq b) 1 Eq c) 2 Eq d) 1 Eq
indicate how many acidic hydrogen atoms and how many nonacidic hydrogen atoms are present in a) hClO3 (chloric acid) b. hC3h5O4 (glyceric acid) c. h3C6h5O7 (citric acid) d. h3pO4 (phosphoric acid)
a) 1 acidic; 0 nonacidic b) 1 acidic; 5 nonacidic c) 3 acidic; 5 nonacidic d) 3 acidic; 0 nonacidic
Without writing an equation, specify the molecular ratio in which each of the following acid-base pairs will react. a. hNO3 and NaOh b. h2SO4 and NaOh c. h2SO4 and Ba(Oh)2 d. hNO3 and Ba(Oh)2
a) 1 to 1 b) 1 to 2 c) 1 to 1 d) 2 to 1
What is the [h3O+] value in solutions with each of the following ph values? a) 5.00 b) 7.00 c) 3.45 d) 7.15
a) 1.0 x 10^-5 M b) 1.0 x 10^-7 M c) 3.5 x 10^-4 M d) 7.1 x 10^-8 M
Determine the half-life of a radionuclide if after 5.4 days the fraction of undecayed nuclides present is a. 1/16 b. 1/64 c. 1/256 d. 1/1024
a) 1.4 days b) 0.90 day c) 0.68 day d) 0.54 day
What is [Oh−] in aqueous solutions with the following [h3O+] concentrations? a. 5.5×10^−2 b. 9.4×10^−5 c. 2.3×10^−7 d. 6.6 × 10^−12
a) 1.8 x 10^-13 M b) 1.1 x 10^-10 M c) 4.3 x 10^-8 M d) 1.5 x 10^-3 M
Write balanced nuclear equations for the beta decay of each of the following nuclides. a) 10Be4 b) carbon-14 c) 21F9 d) sodium-25
a) 10Be4 -> 0B-1 + 10B5 b) 14C6 -> 0B-1 + 14N7 c) 21F9 -> 0B-1 + 21Ne10 d) 25Na11 -> 0B-1 + 25Mg12
Write nuclear equations for each of the following radioactive decay processes. a. Beta emission produces mercury-199 as a product. b. palladium-109 undergoes beta emission. c. Alpha emission produces terbium-148 as a product. d. Fermium-249 undergoes alpha emission.
a) 199Au79 -> 0B-1 + 199Hg80 b) 109Pd46 -> 109Ag47 + 0B-1 c) 152Ho67 -> 148Tb65 + 4a2 d) 249Fm100 -> 245Cm98 + 4a2
how many ions, per formula unit, are produced when each of the following soluble salts (strong electrolytes) dissolves in water? a) NaCl b) Mg(NO3)2 c) K2S d) NH4CN
a) 2 b) 3 c) 3 d) 2
Indicate the number of equivalents in each of the following molar quantities of ions. a. 2 moles K+ b. 3 moles h2pO4− c. 2 moles hpO42− d. 7 moles Ca2+
a) 2 Eq b) 3 Eq c) 4 Eq d) 14 Eq
What is the molar hydronium ion concentration in aqueous solutions with the following hydroxide ion concentrations? a. 3.5 × 10^−3 M b.4.7×10^−6M c. 1.1 × 10^−8 M d. 8.7 × 10^−10 M
a) 2.9 x 10^-12 M b) 2.1 x 10^-9 M c) 9.1 x 10^-7 M d) 1.1 x 10^-5 M
Write a balanced nuclear equation for each of the reactions a. polonium-210 decays to lead-206 b. thorium-225 decays to protactinium-225 c. parent = pt-190; daughter = Os-186 d. parent = O-19; daughter = F-19
a) 210Po84 -> 4a2 + 206Pb82 b) 225Th90 -> 225Pa91 + 0B-1 c) 190Pt78 -> 186Os76 + 4a2 d) 19O8 -> 19F9 + 0B-1
Calculate the pKa value for each of the following acids. a. Nitrous acid (hNO2), Ka = 4.5 × 10−4 b. Carbonic acid (h2CO3), Ka = 4.3 × 10−7 c. Dihydrogen phosphate ion (h2pO4−), Ka = 6.2 × 10−8 d. Sulfurous acid (h2SO3), Ka = 1.5 × 10−2
a) 3.35 b) 6.37 c) 7.21 d) 1.82
How many protons and neutrons are present in each of the following nuclides? a) 10Be4 b) 23Na11 c) silver-108 d) S-34
a) 4,6 b) 11, 12 c) 47, 61 d) 16, 18
Supply a complete symbol, with superscript and subscript, for each of the following types of radiation. a. Alpha particle b. Beta particle c. Gamma ray
a) 4a2 b) 0B-1 c) 0Y0
Supply the missing nuclear symbol in each of the following equations for bombardment reactions. a. 24Mg12 + ? -> 27Si14 + 1n0 b. 27Al13 + 2H1 -> ? + 4a2 c. 9Be4 + ? -> 12C6 + 1N0 d. 6Li3 + ? -> 4He2 + 3He2
a) 4a2 b) 25Mg12 c) 4a2 d) 1p1
Calculate the ph of solutions with the following hydronium ion concentrations. a. 1.00 × 10^−5 M b. 1.00 × 10^−8 M c. 4.75×10^−6M d. 8.88×10^−8M
a) 5.000 b) 8.000 c) 5.323 d) 7.052
Using Table 11-2 as your information source, determine how many of the transuranium elements have a half-life a. greater than 1 year b. less than 1 day
a) 7 b) 17
What is the molar hydronium ion concentration in solutions with each of the following ph values? a. 3.13 b. 3.25 c. 3.50 d. 3.75
a) 7.4 x 10^-4 M b) 5.6 x 10^-4 M c) 3.2 x 10^-4 M d) 1.8 x 10^-4 M
Write a balanced nuclear equation for the decay of each of the following radioactive nuclides. The mode of decay is indicated in parentheses. a. 70Ga31 (beta emission) b. 144Nd60 (alpha emission) c. 248Fm100 (alpha emission) d. 113Ag47 (beta emission)
a) 70Ga31 -> 0B-1 + 70Ge32 b) 144Nd60 -> 4a2 + 140Ce58 c) 248Fm100 -> 4a2 + 244Cf98 d) 113Ag47 -> 0B-1 + 113Cd48
A buffer solution has a ph value of 8.2. Which value in the set of ph values 7.1 8.1 8.2 8.3 9.3 is the most likely value for the buffer solution ph after a. a small amount of strong acid has been added? b. a small amount of strong base has been added?
a) 8.1 b) 8.3
For the generalized chemical reaction A(g) + B(g) -> C(g) + D(g) determine whether the concentration of A in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of B is increased b. concentration of C is decreased c. concentration of D is increased d. concentration of D is decreased
a) decrease b) decrease c) increase d) decrease
Indicate whether each of the solutions are acidic, basic, or neutral. (these are the H3O^+) a. 5.5×10^−2 b. 9.4×10^−5 c. 2.3×10^−7 d. 6.6 × 10^−12
a) acidic b) acidic c) acidic d) basic
Indicate whether each of the following samples is acidic, basic, or neutral. a. milk, ph 6.4 b. seawater, ph 8.5 c. drinking water, ph 7.2 d. strawberry, ph 3.4
a) acidic b) basic c) basic d) acidic
Classify each of the following decay reactions as alpha decay or beta decay. a. polonium-210 decays to lead-206 b. thorium-225 decays to protactinium-225 c. parent = pt-190; daughter = Os-186 d. parent = O-19; daughter = F-19
a) alpha b) beta c) alpha d) beta
Indicate whether each of the solutions are acidic, basic, or neutral. (these are the OH) a. 3.5 × 10^−3 M b.4.7×10^−6M c. 1.1 × 10^−8 M d. 8.7 × 10^−10 M
a) basic b) basic c) acidic d) acidic
Which of the naturally occurring radiation types (alpha, beta, and gamma) have the ability to "pass through" a. a thick sheet of paper b. 1 cm thick Al foil c. 5 cm thick concrete d. outer layers of human skin
a) beta, gamma b) gamma c) gamma d) gamma
Indicate whether solutions of each of the following substances contain ions, molecules, or both. a. acetic acid, a weak acid b. sucrose, a nonelectrolyte c. sodium sulfate, a soluble salt d. hydrofluoric acid, a weak electrolyte
a) both b) molecules c) ions d) both
Consider the following four solutions: (1) apple juice, ph 3.8, (2) pickle juice, ph 3.5, (3) carbonated beverage, ph 3.0, and (4) drinking water, ph 7.2. a. Which solution has the highest [h3O+]? b. Which solution has the highest [Oh−]? c. List the solutions in order of increasing acidity. d. List the solutions in order of decreasing basicity.
a) carbonated beverage b) drinking water c) drinking water, apple juice, pickle juice, carbonated beverage d) drinking water, apple juice, pickle juice, carbonated beverage
What is the effect of alpha decay on the a. atomic number of the parent nuclide b. mass number of the parent nuclide
a) decrease by 2 b)decrease by 4
Which of the following reactions are endothermic, and which are exothermic? a) C2H4 +3O2 -> 2CO2 + 2H2O + heat b) N2 +2O2 +heat -> 2NO2 c) 2H2O+ heat -> 2H2 +O2 d) 2KClO3 -> 2KCl + 3O2 + heat
a) exothermic b) endothermic c) endothermic d) exothermic
In a certain chemical reaction, the average energy of the products is lower than the average energy of the reactants. a. Is the chemical reaction exothermic or endothermic? b. Is energy released or absorbed in the chemical reaction?
a) exothermic b) released
For each of the following pairs of solutions, indicate whether the first listed solution has a higher or lower ph than the second listed solution. a. 1.0 M NaOh and 1.0 M hCl b. 1.0 M hNO3 and 0.10 M hNO3 c. 0.10 M hClO4 and 0.10 M hCN d. [h3O+] = 3.3 × 10−3 and [h3O+] = 9.3 × 10−3
a) higher b) lower c) lower d) higher
Indicate whether each of the following pairings of concepts is a correct or an incorrect pairing. a) reducing agent and gain of electrons b) substance oxidized and loss of electrons c) oxidizing agent and increase in oxidation number d) oxidizing agent and substance oxidized
a) incorrect b) correct c) incorrect d) incorrect
For each of the changes listed will the rate of the following chemical reaction increase, decrease, or remain the same? Cu(s) + H2SO4(aq) -> CuSO4(aq)+ H2(g) a) the concentration of H2SO4 is increased b) the copper is ground into a powder c) the mixture is stirred rapidly d) the temperature of the solution is increased
a) increase b) increase c) increase d) increase
For the reaction C6H6 (g) + 3H2 (g) -> C6H12 (g) + heat determine in what direction the equilibrium will be shifted by each of the following changes. a. Increasing the concentration of C6H12 b. Decreasing the concentration of C6H6 c. Increasing the temperature d. Decreasing the pressure by increasing the volume of the container
a) left b) left c) left d) left
Compare the two acids below 1. Acetic acid dissolved in water CH3COOH (aq) + H2O (l) ⇔ H3O+ (aq) + CH3COO - (aq) 2. Carbonic acid dissolved in water H2CO3 (aq) + H2O (l) ⇔ H3O+ (aq) + HCO3- (aq) Based on the value of Ka in the table, which is the stronger acid acetic acid or carbonic acid?
acetic acid
Indicate if the following is a Brønsted-Lowry acid, base or neither. H2CO3
acid
Indicate if the following is a Brønsted-Lowry acid, base or neither. HNO3
acid
In each conjugate pair,
acid is one w more hydrogen atoms
polyprotic =
acid that has more than one hydrogen
define polyprotic acid
acid that supplies 2 or more protons [H+ ions] during acid-base reaction
In an Arrhenius acid-base theory context, the compounds hCl, hNO3, and NaOh, when dissolved in water, are, respectively, which of the following?
acid, acid, base
The [H3O+] concentration of a solution is 2.5 x 10^-4 Is this solution acidic or basic?
acidic
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral [H^+] = 3.8 x 10^-3
acidic
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral [OH^-] = 2.3 x 10^-8
acidic
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral pH = 5.87
acidic
if H3O^+ is 1.0 x 10^-2 M and OH^- is 1.0 x 10^-12, type of solution is
acidic
if H3O^+ is 2.5 x 10^-5 M and OH^- is 4.0 x 10^-10, type of solution is
acidic
pH < 7
acidic
[H3O+] > [OH-]
acidic solution
The minimum combined kinetic energy reactant molecules must possess in order for their collision to result in a chemical reaction is called the
activation energy
Which of the following factors will influence the rate of a chemical reaction? A) changing the surface area B) changing the temperature C) changing the concentration of the reactants D) adding a catalyst
all of the above
There are 7 strong acids
all other acids are weak
the strong bases are hydroxides of groups IA and IIA [metal hydroxides]
all other bases are weak
Acids, bases, and soluble salts
all produce ions in solution [all produce solutions that conduct electricity]
Which of the following types of radioactive emissions has a subatomic particle compo-sition of two protons and two neutrons?
alpha particle
Which of the following correctly orders the three types of naturally occurring radiation in terms of increasing penetrating power into matter?
alpha, beta, gamma
Major damage occurs when
alpha-emitting radionuclides are ingested [contaminated food]
results that agree with "like dissolved like" are nearly
always obtained in cases of gas-in-liquid & liquid-in-liquid solutions & for solid-in-liquid solutions in which solute is not ionic compound
concentration of a solution
amount of solute in specified amount of solution
Define concentration
amount of solute present in specified amount of solution
Concentration=
amount of something/some unit of volume
Water is something
amphiprotic [bc can behave as acid or base]
What weak acid would be best to use when preparing a buffer solution with a pH of 8.00?
an acid with Ka = 1.0 x 10^-8
in a chemical reaction, The chemical reactivity of
an element depends on element's state of combination [free element, compound, etc]
Weak acids have?
an equilibrium [like HF]
Keq is used to denote
an equilibrium constant
Kw = [H3O+] [OH-] This value is
an equilibrium constant
IONIZATION: The process whereby, in
aqueous solution, positive & negative ions are produced from molecular compound.
Not all hydrogens
are acidic
in a nuclear equation, mass numbers and atomic numbers (nuclear charge)
are always specifically included in nuclear equations
All common soluble salts
are completely dissociated into ions in solution
Two components [in buffers]
are in equilibrium
in a nuclear reaction, Reaction rates
are independent of temp, pressure, catalysts & reactant concentrations.
CO2 and H2O
are low energy [stable]
All solutions
are mixtures [but only homogeneous mixtures are solutions]
in a chemical system in an equilibrium state product molecules
are reacting w each other
in a chemical system in an equilibrium state reactant molecules
are reacting with each other
The particles that are allowed to pass through semipermeable membrane (usually just solvent molecules like water)
are relatively small.
If both substances (in a solution)
are same state, substance present in greatest amount is generally considered solvent
All nitrates
are soluble
Most chlorides & bromides
are soluble [except w silver, lead(II) and mercury(I)]
in equations with strong electrolytes
arrow only to right
pH decreases
as [H^+] increases
What is the relationship between gas pressure and solubility?
as pressure of gas above liquid increases, solubility of gas increases
Using collision theory, indicate why each of the following factors influences the rate of a reaction. Temperature of reactants
as temp increases, so does number of collisions per second
explain how each of the following radionuclides is used in diagnostic medicine. Thallium-201
assessment of blood flow in heart muscle
When a percent concentration is given without specifying which of the three types of percent concentration it is,
assumed to mean percent by mass.
in a hyperbaric chamber,
atmospheric pressure is increased & controlled
# of protons tells you
atomic number & what it is
Hydrogen stays
attached to water
Opposite charges
attract
Which of the following chemical reactions is a nonredox reaction? a. Ca + S -> CaS b. SO3 + h2O -> h2SO4 c. 2NO+O2 -> 2NO2 d. no correct response
b
Which of the following is not a balanced nuclear equation? a. 121Sn50 -> 0B-1 + 121Sb51 b) 238U92 - 4a2 + 232Th90 c) 10Be4 -> 10B5 + 0B-1 d) no correct response
b
HNO3 (aq) + H2O (l) → H3O+ (aq) + NO3- (aq) here water is
base
Indicate if the following is a Brønsted-Lowry acid, base or neither. Cl^-
base
Using the Arrhenius theory, classify the following as either an acid or a base: Al(OH)3
base
Using the Arrhenius theory, classify the following as either an acid or a base: CsOH
base
Determining the concentration of an acid using an acid-base titration involves completely reacting a measured volume of the acid with a measured volume of
base of known concentration
The selectivity of a semipermeable membrane is
based on size differences of molecules.
A solution with pH = 8.5 is defined as
basic
The [H3O+] concentration of a solution is 2.5 x 10^-9 Is this solution acidic or basic?
basic
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral [H^+] = 1.5 x 10^-10
basic
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral [OH^-] = 6.1 x 10^-4
basic
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral pH = 9.59
basic
if H3O^+ is 1.0 x 10^-8 M and OH^- is 1.0 x 10^-6, type of solution is
basic
if H3O^+ is 5.0 x 10^-11 M and OH^- is 1.0 x 10^-4, type of solution is
basic
pH > 7
basic
If H3O^+ is 2.5 x 10^-9 and OH^- is 4.0 x 10^-6 is this solution acidic or basic?
basic bc OH is higher
[H3O+] < [OH-]
basic solution
Why does H2CO3 and CO3^2- not contain an acid-base conjugate pair?
bc differs by 2 hydrogens
in NH3 + H2O -> NH4 + OH^- why is NH4^+ the conjugate acid?
bc getting one proton [so get its positive charge]
Why is CH3OH soluble in water?
bc has a hydrogen bond
Why does a reaction happen faster with a high concentration?
bc more stuff = more chance of collision
Most acid base reactions reach equilibrium
bc most acids are too "weak" to completely ionize & donate all their protons
If you add hydrogen to H2(g) + I2(g) <=> HI(g) value of Keq will not change. Why?
bc only thing that can change Keq value is temp
for osmosis, why is the rate of flow into the concentrated solution is greater than the rate of flow in the other direction
bc presence of solute molecules diminishes ability of water molecules to cross membrane.
in C6H6(g) + 3H2(g) -> C6H12(g) + heat why would increasing the pressure shift equilibrium to the right?
bc right has fewer moles of gas
buffers work
bc there's an equilibrium
in a nuclear reaction, Elements may
be changed into other elements during nuclear reactions.
Le Chatelier's Principle says If more products have
been produced as result of disruption, equilibrium has shifted to right
H at the
beginning of formula are acidic hydrogens
Which of the following types of radioactive emissions has a charge and mass identical to that of an electron?
beta particle
Internal exposure to
beta radiation is as serious as internal alpha exposure
Water has a
big dipole
acetic acids have
bigger value for Ka than carbonic acid [means more product]
At 24°C, the molar concentrations of H3O+ and OH− ions in pure water are
both 1.00 × 10^−7 M
An amphiprotic substance is a substance that can function as
both a Brønsted-Lowry acid and a Brønsted-Lowry base
in HC2H3O2 and H3C6H5O7
both acidic & nonacidic hydrogen atoms are present
13C6 and 14C6
both are unstable [both spontaneously change into another element]
polyprotic acid includes
both diprotic and triprotic acids
Film badges, worn by technicians working with radiation, can detect
both extent and type of radiation exposure
Film badges
both low & high energy
When an ionic solute dissolves in water, the water molecules hydrate
both positive ions & negative ions
Solution formation occurs more rapidly at higher temperatures because molecules of
both solute & solvent move more rapidly
The term nuclide is a term used to describe
both stable and unstable atoms
Reactions go
both ways
alpha particle is like
bowling ball
In which of the following pairs of acids are both members of the pair strong acids? a. H2CO3 and H2SO4 b. HCl and HF c. HCl and HNO3 d. no correct response
c
In which of the following pairs of substances are both members of the pair salts? a. NaCl and NaOH b. HBr and NaBr c. KNO3 and KCN d. no correct response
c
Which of the following changes will decrease the reaction rate for the chemical reaction S(s) + O2(g) -> SO2(g) a. increase the state of subdivision of the solid-state S b. increase the amount of O2 present in the reaction mixture c. decrease the amount of S present in the reaction mixture d. no correct response
c
Which of the following changes will shift the position of the equilibrium to the left for the chemical reaction N2(g) + 3H2(g) -> 2NH3(g) a. decrease the concentration of Nh3 b. increase the concentration of h2 c. decrease the concentration of N2 d. no correct response
c
Which of the following does not describe an acidic solution at 24°C? a. the ph is less than 7.0 b. the [h3O+] is greater than the [Oh−] c. the [h3O+] is 1.0 ×10^−8 d. no correct response
c
Which of the following hypothetical solutions of ions is out-of-balance relative to ion charge? a. 1.0 meq Na+, 2.0 meq Ca2+, and 3.0 meq Cl− b. 2.0 meq Mg2+, 1.0 meq Cl−, and 1.0 meq NO3− c. 2.0 meq Na+, 2.0 meq K+, and 2.0 meq pO43− d. no correct response
c
Which of the following ions cannot be present in a salt? a. Na+ b. SO4^2− c. OH− d. no correct response
c
Which of the following is a conjugate acid-base pair? a. H2CO3/CO3^2− b. H3PO4/PO4^3− c. HCN/CN^− d. no correct response
c
Which of the following is an inappropriate designation for a salt? a. insoluble salt b. completely dissociated salt c. weak salt d. no correct response
c
Which of the following is not a characteristic of a chemical system in an equilibrium state? a. product molecules are reacting with each other b. reactant molecules are reacting with each other c. product molecules are reacting with reactant molecules d. no correct response
c
Which of the following is not a general property of radionuclides used is diagnostic medical procedures? a. must be detectable by instrumentation placed outside the body b. must have a known mechanism for elimination from the body c. must have a long half-life d. no correct response
c
Which of the following molar amounts of an ion is not equal to one equivalent of ion? a. 1.0 mole Cl^− b. 0.50 mole SO4^2− ion c. 0.50 mole Nh4+ ion d. no correct response
c
Which of the following produces a alpha particle? a) 68Ga31 + 0e-1 -> 68Zn30 b) 62Cu29 -> 0e+1 + 62Ni28 c) 212Fr87 -> 4He2 + 208At85 d) 129Sb51 -> 0e-1 + 129Te52
c
Which of the following will produce a compound with sulfate that is not soluble. lithium calcium ammonium sodium
calcium
More than one solute
can be present in same solution.
If you have two cups and one looks like it has more
can be same amount but diff concentration [diff amount of water]
in a solution, solute generally
can be separated from solvent by physical means such as evaporation
Solutes and solvents
can be solids, liquids or gases
It's an acid if
can donate a hydrogen
Define amphiprotic substance
can either lose or accept proton [can function as either bronsted-lowry acid or bronsted-lowry base]
Unsaturated solution is like
can jam more stuff into it
in ionizing radiation,
can remove electrons so it's bad
in dilution problems,
can use any unit as long as they match
Classify each of the following reactions as (1) a redox reaction (2) a nonredox reaction or (3) "can't classify" because of insufficient information A displacement reaction in which both of the reactants are compounds
can't classify
Na^+ and Pb^+
can't make a compound bc both positive
What is happening in Fe2O3(s) + 3CO(g) -> 2Fe(s) + 3CO2(g)
carbon got oxidized [reducing agent]; iron got reduced [oxidizing agent]
ethanol is a polar solvent and carbon tetrachloride is a nonpolar solvent. In which of these two solvents are each of the following solutes more likely to be soluble? Cooking oil, nonpolar
carbon tetrachloride
For each solute, identify the better solvent: water or carbon tetrachloride C6H14
carbon tetrachloride (CCl4)
The hydrogen atoms
carry partial positive charge
Determining the concentration of an acid using an acid-base titration involves what
carrying out an acid-base neutralization reaction
Using collision theory, indicate why each of the following factors influences the rate of a reaction. presence of a catalyst
catalyst lowers activation energy
gamma ray can?
cause burn on skin
Increasing the temperature at which a chemical reaction occurs will cause which of the following effects?
cause more reactant collisions to take place within a given time
A hypotonic solution can be used to
cause water to flow from blood into surrounding tissue [decrease bp]
Adding a solute to a pure solvent
causes solvent's physical properties to change
in physiological saline solution,
cells neither swell nor shrink [an isotonic solution]
Concentrated sodium chloride solution is hypertonic with respect to red blood cell fluid,
cells undergo crenation when placed in it
Distilled water is hypotonic with respect to red blood cell fluid,
cells will hemolyze when placed in it
Suppose that a sample of red blood cells are placed into a solution of brine (salt water). What is the expected effect on the cells?
cells will shrivel as water flows out of cells into brine solution
Properties of a solution
change as ratio of solute to solvent is changed
What can change the value of an equilibrium constant?
change in reaction temp
N2(g) + 3H2(g) <- ——> 2NH3(g) what happens here ultimately?
changes offset each other so value of equilibrium constant K remains constant
With concentration changes!
changes offset each other so value of equilibrium constant K remains constant
Tell me what a neutralization reaction is
chemical reaction between acid & hydroxide base in which salt & water are products
exchange reaction [double displacement]
chemical reaction in which 2 substances exchange parts w another & form 2 diff substances
Displacement reaction
chemical reaction in which atom or molecule displaces atom or group of atoms from compound
Combination reaction
chemical reaction in which single product is produced from 2 or more reactants
Decomposition reaction
chemical reaction in which single reactant is converted into 2 or more simpler substances [elements or compounds]
Nonoxidation-Reduction (Nonredox) Reaction
chemical reaction; no transfer of electrons from 1 reactant to another reactant
Oxidation-Reduction (Redox) Reaction
chemical reaction; transfer of electrons from 1 reactant to another reactant
Elements maintain their identity in
chemical reactions but not in nuclear reactions.
Ch1-10 has been
chemistry of electrons
The more you...
chop things up, more soluble
electrons
circle around nucleus
The effect of 1 mole of CaCl2 on
colligative properties will be 3x that of 1 mole of glucose on colligative properties
Classify each of the following chemical reactions as a combination, decomposition, dis- placement, exchange, or combustion reaction. 3Mg + N2 -> Mg3N2
combination
Classify each of the following chemical reactions as a combination, decomposition, displacement, exchange, or combustion reaction. HCl(g) + NH3(g) → NH4Cl(s)
combination
Classify each of the following reactions as a combination, decomposition, displacement, exchange, or combustion reaction. 2P + 3H2 -> 2PH3
combination
Classify each of these reactions: CaO + CO2 -> CaCO3
combination [synthesis]
Classify the following reaction: CaO + CO2 -> CaCO3
combination [synthesis]
2H2 + O2 -> 2H2O
combination reaction
X + Y -> XY
combination reaction
Indicate to which of the following types of reactions each of the statements listed applies: combination, decomposi- tion, displacement, exchange, and combustion. More than one answer is possible for a given statement. A compound may be a product.
combination, decomposition, displacement, exchange, & combustion.
Indicate to which of the following types of reactions each of the statements listed applies: combination, decomposi- tion, displacement, exchange, and combustion. More than one answer is possible for a given statement. A compound may be a reactant.
combination, decomposition, displacement, exchange, & combustion.
Indicate to which of the following types of reactions each of the statements listed applies: combination, decomposition, displacement, exchange, and combustion. More than one answer is possible for a given statement. An element may be a reactant.
combination, displacement, combustion
Buffers are a
combo of 2 things you add to water so pH doesn't change
Classify each of the following chemical reactions as a combination, decomposition, displacement, exchange, or combustion reaction. 4NH3 + 5O2 → 4NO + 6H2O
combustion
What type of reaction is shown below? 2C2H6 + 7O2 → 4CO2 + 6H2O
combustion
C3H8 + 5O2 → 3CO2 + 4H2O
combustion reaction
pH = -log[H3O^+]
compact way to represent solution acidity
if reaction goes to right,
concentration is higher
Substances burn more rapidly in pure oxygen than in air. explain why.
concentration of O2 has increased from 21% 100%
CSVS = CDVD
concentration of stock solution x volume of stock solution = concentration of diluted solution x volume of diluted solution
For solid solutions,
concentrations are expressed as percent by mass concentration %(m/m)
For liquid solutions,
concentrations are expressed as percent by volume concentration %(v/v)
tell me about strong electrolytes
conduct strong electric current in water [salts, strong acids & bases]
tell me about weak electrolytes
conduct weak electrical current [weak acids & bases]
Every bronsted-lowry base has
conjugate acid
Every bronsted-lowry acid has
conjugate base
In determining which pair of molecules will mix together to form a homogeneous solution,
consider intermolecular forces
Weak bases tend to
contain nitrogen
Any compound that
contains a group 1 cation is soluble
The half-life of cobalt-60 is 5.2 years. This means that after 5.2 years a cobalt-60 sample
contains half as many cobalt-60 atoms as it did originally
What does the term reversible reaction mean?
conversion of reactants to products and conversion of products to reactants occur simultaneously
Identify the solvent in: bronze (an alloy of 95% copper and 5% tin)
copper
C6H12O6 is!
covalent
Acids are!
covalent [but sometimes H comes off & attaches itself to water]
HF is what?
covalent [so should not come apart in water]
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 0.28 M NaCl
crenate
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 0.28 M in both glucose and sucrose
crenate
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 5.0%(m/v) NaCl solution
crenate
In which of the following pairs of bases are both bases weak bases? a. NaOH and KOH b. Ca(OH)2 and Ba(OH)2 c. LiOH and Sr(OH)2 d. no correct response
d
Which of the following produces a beta particle? a) 68Ga31 + 0e-1 -> 68Zn30 b) 62Cu29 -> 0e+1 + 62Ni28 c) 212Fr87 -> 4He2 + 208At85 d) 129Sb51 -> 0e-1 + 129Te52
d
Drano is
dangerous to you
The greater the
decay rate for radionuclide, shorter its half-life.
Classify each of the following chemical reactions as a combination, decomposition, dis- placement, exchange, or combustion reaction. 2KNO3 -> 2KNO2 + O2
decomposition
If the ph of a solution increases from 4.0 to 6.0 the hydronium ion concentration [h3O+]
decreases by a factor of 100
We use polarity to
describe covalent compounds
Hemolysis
destruction of RBC
Film Badges are used to
detect person's exposure to radiation
explain how each of the following radionuclides is used in diagnostic medicine. Barium-131
detection of bone tumors
explain how each of the following radionuclides is used in diagnostic medicine. potassium-42
determination of intercellular spaces in fluids
two factors rather than one
determine number of particles present.
Number of sig figs in [H3O+] or [OH-] value
determines number of digits past l decimal in pH value
Contrast the behavior of different isotopes of an element in nuclear and chemical reactions.
diff isotopes of element have same chemical properties but diff nuclear properties
Conjugate base pairs...
differ by a hydrogen
The members of a conjugate acid-base pair
differ from each other through loss or gain of proton
You never start
dimensional analysis problems w conversion factors
2 protons per molecule transferred in an acid-base reaction
diprotic acid
H2CO3 would be an example of
diprotic acid
H2SO4 would be an example of
diprotic acid
why does vapor pressure decrease when solute is added
direct consequence of some of solute molecules or ions occupying positions on surface of liquid [presence decreases probability of solvent molecules escaping]
Stirring solution components
disperses solute particles more rapidly, increasing possibilities for solute- solvent interactions [rate of solution formation is increased]
Classify each of the following chemical reactions as a combination, decomposition, dis- placement, exchange, or combustion reaction. Zn + 2AgNO3 -> Zn(NO3)2 + 2Ag
displacement
Classify each of the following chemical reactions as a combination, decomposition, displacement, exchange, or combustion reaction. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
displacement
Classify each of the following reactions as a combination, decomposition, displacement, exchange, or combustion reaction. 3CuSO4 + 2Al -> Al2(SO4)3 + 3Cu
displacement
Classify each of these reactions: ZnSO4 + Mg -> Zn + MgSO4
displacement & redox
Classify the following reaction: ZnSO4 + Mg -> Zn + MgSO4
displacement [single replacement]
X + YZ -> Y + XZ
displacement reaction
Zn + 2HCl -> ZnCl2 + H2
displacement reaction
Arrhenius theory says a base
dissociates in water to produce hydroxide ions
nonpolar + nonpolar
dissolve
Nonpolar solvents
dissolve nonpolar solutes
Polar solvents
dissolve polar & ionic solutes
Although possible, a reaction at equilibrium
does not necessarily have equal concentrations of products & reactants
Stable nucleus
does not readily undergo change
example: HA(aq) + H2O(l) <=> H3O+(aq) + A-(aq) you
don't put pure water in equilibrium expressions bc concentration can't change
A bronsted lowry acid is a substance that can
donate a proton [H^+ ion] to some other substance
A Brønsted-Lowry acid is a substance that can
donate a proton to some other substance
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) in this acid-base reaction, an acid HF
donates H^+ to form its conjugate base [F^-]
in HCl + H2O -> Cl^- + H3O^+ HCl
donates proton
Acid does what
donates proton when put in water
exchange reaction aka
double displacement
Classify each of these reactions: NaNO2 + HCl -> NaCl + HNO2
double displacement [exchange/metathesis]
Classify the following substance & description as an electrolyte or nonelectrolyte a soluble ionic compound
electrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte potassium iodide, KI
electrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte sodium chloride, NaCl
electrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte sodium hydroxide, NaOH
electrolyte
swell
enlarge in size
What are the catalysts in the human body?
enzymes
Use the given Keq value and the terminology in Table 9-2 to describe the relative amounts of reactants and products present in each of the following equilibrium situations. 2HCl(g) <=> H2(g) + Cl2(g) Keq at 25 degrees celsius = 3.2 x 10^-34
essentially all reactants
if Value of Keq is very small (10^−30) what is Relative Amount of Products and Reactants & Description of Equilibrium Position
essentially all reactants & far to the left
Identify the solute in: a solution of 3.0 x 10^1% ethanol and 7.0 x 10^1% water
ethanol
ethanol is a polar solvent and carbon tetrachloride is a nonpolar solvent. In which of these two solvents are each of the following solutes more likely to be soluble? LiNO3, ionic
ethanol
Identify the solute and the solvent in solutions composed of the following: 60.0 mL of methyl alcohol and 20.0 mL of ethyl alcohol
ethyl alcohol solute; methyl alcohol solvent
If you dissolve HCl in water, precedes 100% to right
every molecule of HCl comes completely apart bc HCl is very strong
When we dissolve 1 mole of CaCl2 in 1 liter of water we have 1 mole of chemical and 3 moles of charge (1 mole of Na+ and 2 mole of Cl -).
example of why we care about electrolytes
All reactions
except explosions go forward and then back
Classify each of the following chemical reactions as a combination, decomposition, dis- placement, exchange, or combustion reaction. Ni(NO3)2 + 2NaOh -> Ni(Oh)2 + 2NaNO3
exchange
Classify each of the following reactions as a combination, decomposition, displacement, exchange, or combustion reaction. 2AgNO3 + K2SO4 -> Ag2SO4 + 2KNO3
exchange
Classify the following reaction: NaNO2 + HCl -> NaCl + HNO2
exchange [double replacement]
AX + BY -> AY + BX
exchange reaction [double displacement]
Na2SO4(aq) + Pb(NO3)2(aq) → 2NaNO3(aq) + PbSO4(s)
exchange reaction [double displacement]
heat energy production is a characteristic of
exothermic chemical reactions
CH4 + O2 -> CO2 + H2O + heat is example of
exothermic reaction [bc energy is product]
Indicate whether each of the following statements about the general properties of solutions is true or false. The solutes present in a solution will "settle out" with time if the solution is left undisturbed.
false
Is the following statement concerning a saturated solution true or false? undissolved solute must be present
false
true or false: Solutions readily separate into solute and solvent if left undisturbed for 24 hours.
false
true or false: at equilibrium, the concentrations of reactants and products are equal
false
true or false: to determine whether a collision between 2 reactant molecules will result in a reaction, the energies of the colliding particles must be equal to each other
false
true or false: to determine whether a collision between 2 reactant molecules will result in a reaction, the particles must be charged
false
true or false? the activation energy is the energy difference between the energy of the products and the energy of the reactants
false
true or false? when the activation energy is low, the reaction rate is slow
false
Why do technicians who work around radiation usually wear film badges?
films record extent of exposure to radiation
If a solute and solvent can
find any way to interact w each other, then it can be dissolved
Pure substance =
fixed composition
Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through Based on each of the following identities for solutions A and B, indicate whether the liquid level in compart- ment A, with time, will increase, decrease, or not change. A = 5.0%(m/v) glucose solution and B = 4.0%(m/v) glucose solution
increase
Indicate whether each of the following actions will increase or decrease the rate of dissolving of a sugar cube in water. Breaking the sugar cube up into smaller "chunks"
increase
Will the changes listed increase or decrease the rate of the following chemical reaction? 2CO + O2 -> 2CO2 Adding a catalyst to the reaction mixture
increase
Will the changes listed increase or decrease the rate of the following chemical reaction? 2CO + O2 -> 2CO2 Adding some O2 to the reaction mixture
increase
How does reactant concentration influence chemical reaction rate?
increase in concentration of reactant causes increase in rate of reaction.
Indicate the effect of the following on the rate of this reaction: 3H2 (g) + N2 (g) -> 2NH3 (g) Add a catalyst
increase rate
What is the effect of temperature on solids?
increase temp = most solids become more soluble in water
For reactants in the solid state, reaction rate
increases as subdivision of solid increases.
High temperature
increases energy of collision
Subdivision
increases solid-state surface areas.
If we add hydrogen to H2(g) + I2(g) <=> HI(g)
initially H2 go up, I2 down, HI up [value of Keq will not change]
A compound has a solubility in water of 250 mg/L at 25°C. Should this compound be characterized as a soluble or insoluble compound at 25°C?
insoluble
Predict the solubility of each of the following solutes in the solvent indicated. AgCl (an ionic solid) in water
insoluble
Predict the solubility of each of the following solutes in the solvent indicated. Methane (a nonpolar gas) in water
insoluble
Predict whether the following compound is soluble or insoluble in water: BaSO4
insoluble
Predict whether the following compound is soluble or insoluble in water: FeCO3
insoluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. Cu(OH)2
insoluble
Using Table 8-2, indicate whether each of the following ionic compounds is soluble or insoluble in water. silver chloride
insoluble
Using Table 8-2, classify each of the following types of ionic compounds using the solubility categories soluble, soluble with exceptions, insoluble, or insoluble with exceptions. carbonates
insoluble with exceptions
Using Table 8-2, classify each of the following types of ionic compounds using the solubility categories soluble, soluble with exceptions, insoluble, or insoluble with exceptions. phosphates
insoluble with exceptions
Why do oil and water not mix?
intermolecular forces between water molecules are so strong that after oil-water mixture is shaken, water layer re-forms, squeezing out oil molecules
"100% dissociation for electrolytes" means
ion pairing can be ignored
Kw
ion product constant for water
NaCl is!
ionic
The rule "like dissolves like" is not adequate when predicting solubility in water when the solute is a(n)
ionic solid
Hydrogen atoms can
ionize to form H^+/H3O^+
Strong electrolytes do what?
ionize/dissociate 100% in water, producing positive & negative ions
A Geiger counter operates on the principle that radiation
ionizes atoms and molecules
Weak electrolytes do what?
ionizes/dissociates only slightly in water
in Fe2O3(s) + 3CO(g) -> 2Fe(s) + 3CO2(g)
iron gained 3 electrons
Why is Fe(s) + Cu^2+ -> Fe^2+ Cu(s) a redox reaction?
iron gave up 2 electrons; gave them to copper
Fe2O3
iron(III) oxide
vitamin C
is an acid
The only thing that changes the value of Keq
is change in temp
Typically, a buffer system
is composed of weak acid & its conjugate base.
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 0.28 M glucose
isotonic
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 0.14 M in both glucose and sucrose
isotonic
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 0.92%(m/v) NaCl solution
isotonic
osmolarity relative to body fluids is equal
isotonic
osmotic effect on cells is: equal water flow into and out of cells
isotonic
osmotic pressure relative to body fluids is equal
isotonic
An atom or ion is reduced if
it gains electrons
if a formula ends in COOH,
it is an acid
Why does seawater evaporate more slowly than fresh water at the same temperature?
it's more concentrated solution so has lower vapor pressure
Water-water hydrogen bonds
keep water from mixing w nonpolar molecules
for equilibrium constant, 29
kind of in middle [50-50 reaction]
As the temperature of a solution increases,
kinetic energy of molecules increases
Synthetic radionuclides are now
known for each of naturally occurring elements.
Strong acids have a ______ value of Ka and the equlibrium for the reaction with water lies far to the _______.
large, right
C6H6(g) + 3H2(g) -> C6H12(g) + heat Indicate if the following will shift the equilibrium to the right or left. Also indicate if the changes will change the value of Keq. increasing the concentration of C6H12
left; no
For the reaction H2 + I2 <---> 2HI if the value of Keq is 0.001 then the equilibrium lies to the _______ and the reaction contains mostly ____________.
left; reactants
C6H6(g) + 3H2(g) -> C6H12(g) + heat Indicate if the following will shift the equilibrium to the right or left. Also indicate if the changes will change the value of Keq. Increasing temperature
left; yes
For exothermic chemical reactions the average energy of the products is
less than that of the reactants
The polarity of water
lets it dissolve compounds
"radiation" =
light
"Activation energy" is like
lighting a flame
What is the main solubility rule?
like dissolves like
The word "like" in the solubility rule "like dissolves like" refers to
like polarity
explain how each of the following radionuclides is used in diagnostic medicine. a. Gallium-67
locate sites of infection
Indicate whether each of the following substances loses or gains electrons in a redox reaction. The reducing agent
loses
Indicate whether each of the following substances loses or gains electrons in a redox reaction. The substance undergoing oxidation
loses
the reducing agent does what?
loses electrons
in terms of electron transfer: oxidation
loss of electrons
What are characteristics of the process of oxidation?
loss of one or more electrons & oxidation number increase
hydrocarbons have
lots of energy
Excitation
low energy radiation excites electron from electron from occupied orbital into empty, higher-energy orbital.
If almost everything comes apart
low pH; strong acid
Alpha Particle Effects have
low penetrating power & cannot penetrate body's outer layers of skin
A nonvolatile solute is one that has
low vapor pressure & therefore low tendency to vaporize
Catalysts are substances that
lower activation energy for chemical reaction
High concentration of hydrogen ions means
lower pH
Identify the solvent in: a solution containing 50.0 mL of methanol and 30.0 mL of water
methanol
What definition best describes the term activation energy?
minimum kinetic energy that particles must possess for chemical reaction to occur
Two substances that
mix w each other are said to be miscible
Osmolarity is the
molarity × i [i is number of particles produced from dissociation of 1 formula unit of solute]
The three core concepts upon which collision theory is based are:
molecular collisions, collision orientation, activation energy
Methanol is a
molecular compound & does not produce ions when dissolved in water
Nonelectrolytes do not conduct an electric current
molecular compounds [not acids]
Chemical reactions occur when what happens?
molecules or atoms collide, bonds between atoms are broken & new bonds are formed
Moles of solute before dilution =
moles of solute after dilution
Molarity
moles of solute in solution divided by liters of solution
Molarity (M) =
moles of solute/liters of solution
The defining equation for the molarity concentration unit is
moles solute/L solution
HCl would be an example of
monoprotic acid
HNO3 would be an example of
monoprotic acid
one proton per molecule transferred in an acid-base reaction
monoprotic acid
pyruvic acid, which is produced in metabolic reactions, is C3H4O3 Would you predict that this acid is a mono-, di-, tri-, or tetraprotic acid? Give your reasoning.
monoprotic bc only 1 H atom is involved in polar bond
more H ions
more acidic
Higher the pH,
more basic
More stuff = [as far as chemical reaction rate]
more chance of collision
High temperature increases energy of collision
more collisions & more chances of successful collision
as the temperature and kinetic energy increases,
more gas can escape from solution
stronger acid =
more product
Use the given Keq value and the terminology in Table 9-2 to describe the relative amounts of reactants and products present in each of the following equilibrium situations. H2(g) + Br2(g) <=> 2HBr(g) Keq at 25 degrees celsius = 2.0 x 10^9
more products than reactants
if Value of Keq is large (10^10) what is Relative Amount of Products and Reactants & Description of Equilibrium Position
more products than reactants & to the right
if Value of Keq is small (10^−10) what is Relative Amount of Products and Reactants & Description of Equilibrium Position
more reactants than products & to the left
Dilution is the process in which
more solvent is added to solution to lower its concentration
If energy goes down
more stable
alpha particles are the
most damaging if get inside bc big
Decreasing pressure
moves reaction to left
a decomposition reaction must have
multiple products but only one reactant
Solute and solution volumes
must always be expressed in same units when percent by volume units are used
In a redox reaction the substance oxidized
must be a reactant
Osmotic pressure is the pressure that
must be applied to prevent net flow of solvent through semipermeable membrane from lower to higher solute concentration
The largest source of radiation exposure from all sources, for the average American, is
natural sources
#1 source of exposure to radioactive is
natural world [radon gas]
radon gas is!
naturally occuring
on the periodic table, the ...
naturally occuring are dark filled in ones
What is background radiation?
naturally occuring ionizing radiation
Tell me about this: HF + H2O <=> H3O^+ + F^-
need more F but not more H so add NaF
the "p" in pH
negative log
the "p" in pKa
negative log
beta particle is like
negatively charged particle
Indicate if the following is a Brønsted-Lowry acid, base or neither. Mg^+
neither
how will the gas-phase equilibrium CH4(g) + 2H2S(g) + heat -> CS2(g) + 4H2(g) be affected by each of the following? The addition of CS2(g)
shift to left
how will the gas-phase equilibrium CH4(g) + 2H2S(g) + heat -> CS2(g) + 4H2(g) be affected by each of the following? An increase in the temperature
shift to right
how will the gas-phase equilibrium CH4(g) + 2H2S(g) + heat -> CS2(g) + 4H2(g) be affected by each of the following? An increase in the volume of the container (a decrease in pressure)
shift to right
how will the gas-phase equilibrium CH4(g) + 2H2S(g) + heat -> CS2(g) + 4H2(g) be affected by each of the following? The removal of H2(g)
shift to right
Increasing the pressure does what
shifts equilibrium in direction that decreases number of molecules in gas phase & thus decreases pressure.
CoCl4^2- + 6H2O -> Co(H2O)6^2+ + 4Cl^- + heat what happens if you cool the mixture (remove heat)?
shifts equilibrium to right
Decreasing the volume [Le Chatelier & pressure]
shifts equilibrium toward side w fewer moles of gas.
in equations, strong electrolytes
show formation of 100% ions in aqueous(aq) solutions
What happens in hypertonic solution?
shrink
Will red blood cells swell, remain the same size, or shrink when placed in 0.28 M NaCl
shrink
Will red blood cells swell, remain the same size, or shrink when placed in 0.28 M in both glucose and sucrose
shrink
Will red blood cells swell, remain the same size, or shrink when placed in 5.0%(m/v) NaCl solution
shrink
Crenation
shrinking of RBC
When red blood cells are placed in a concentrated sodium chloride solution,
shrivel [crenation]
Use the given Keq value and the terminology in Table 9-2 to describe the relative amounts of reactants and products present in each of the following equilibrium situations. COCl2(g) <=> CO(g) + Cl2(g) Keq at 395 degrees celsius = 0.046
significant amounts of both reactants & products
Use the given Keq value and the terminology in Table 9-2 to describe the relative amounts of reactants and products present in each of the following equilibrium situations. SO2(g) + NO2(g) <=> NO(g) + SO3(g) Keq at 460 degrees celsius = 85.0
significant amounts of both reactants & products
if Value of Keq is near unity (between 10^3 and 10^−3) what is Relative Amount of Products and Reactants & Description of Equilibrium Position
significant amounts of both reactants and products & neither to the right nor to the left
Chlorides, bromides, and iodides are soluble in water except for those of
silver, lead & mercury
Predict whether the following solutes are very soluble or slightly soluble in water. AgCl [an ionic solid]
slightly soluble
Predict whether the following solutes are very soluble or slightly soluble in water. CBr4 [a nonpolar liquid]
slightly soluble
Predict whether the following solutes are very soluble or slightly soluble in water. O2 [a nonpolar gas]
slightly soluble
During a bombardment reaction the particles colliding with target nuclei are
small and traveling very fast
Energy changes in chemical reactions are
small compared to those in nuclear reactions.
Why are the radionuclides used for diagnostic procedures usually gamma emitters?
so radiation can be detected externally
Identify the solute and the solvent in solutions composed of the following: 5.00 g of sodium chloride (table salt) and 50.0 g of water
sodium chloride solute; water solvent
Henry's law states that
solubility of gas in liquid is directly proportional to partial pressure of gas over liquid
Indicate whether each of the following solutes will be soluble in the indicated solvent (in parentheses) CH3OH mixed with water (H2O)
soluble
Indicate whether each of the following solutes will be soluble in the indicated solvent (in parentheses) N2 mixed with methane (CH4)
soluble
Indicate whether each of the following solutes will be soluble in the indicated solvent (in parentheses) NH3 mixed with water (H2O)
soluble
Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through Based on each of the following identities for solutions A and B, indicate whether the liquid level in compart- ment A, with time, will increase, decrease, or not change. A = 2.0 M KCl solution and B = 2.0 M KNO3 solution
not change
catalysts do
not change anything about bonds in reaction
Strong acids will!
not create buffers because there is no equilibrium
Equilibrium is like
not static, but is highly dynamic situation.
Nonacidic hydrogen atoms are
not written at front of chemical formula
So nuclear chemistry =
now protons & neutrons are getting involved
theraputic criteria
now we want to destroy [not protect]
bombardment reaction
nuclear reaction brought about by bombarding stable nuclei w small particles traveling at very high speeds.
Transmutation reaction
nuclear reaction in which nuclide of 1 element is changed into nuclide of another element.
Radioactive nuclide/radionuclide
nuclide w unstable nucleus from which radiation is spontaneously emitted.
Transuranium elements
occur right after uranium on periodic table [elements 93 to 118]
Ionization
occurs when radiation carries enough energy to remove an electron from atom or molecule.
in a chemical reaction, Different isotopes
of an element have identical chemical properties
in a nuclear reaction, Different isotopes
of element have diff nuclear properties
in a nuclear equation, the elemental symbols
on both sides of equation frequently are not same
the effect of 1 mole of NaCl
on colligative properties will be twice that of 1 mole of glucose
in a nuclear reaction, the number
on left & right have to add up
For chemical equilibrium
on molecular level, there is frantic activity
[osmosis] Because there is a greater concentration of solute molecules
on one side of membrane than on other, flow rates differ.
if two cups have same amount but diff concentration [diff amount of water]
one is concentrated & one is dilute
What would be considered large for equilibrium constant?
one million
A conjugate acid has...
one more H in formula & increase in charge by one unit
alpha decay =
one of products is 4He2
Pressure influences an equilibrium
only if 1 or more of substances involved is a gas
pH and sig figs
only place sig figs show up in pH is after the decimal
A change in temperature is
only thing that leads to new equilibrium constant K
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other NaCl
other
OILRIG
oxidation is loss; reduction is gain
Redox reactions involve a change in
oxidation state for one or more elements
Loss of electrons
oxidized
Mg -> MgO
oxidized so is reducing agent
The substance that causes the oxidation is
oxidizing agent
in S(s) + O2(g) -> SO2(g) oxygen
oxidizing agent
Match each of the following statements about the dis- solving of the ionic solid NaCl in water with the term hydrated ion, hydrogen atom, or oxygen atom. The portion of a water molecule that is attracted to a Na+ ion
oxygen atom
Combustion reactions are always characterized by
oxygen being one of the reactants
Anytime there is
oxygen in reaction, will be combustion
For the following reaction, identify which element is reduced 2C2H6 + 7O2 -> 4CO2 + 6H2O
oxygen is reduced
pH =
pH = -log[H3O^+]
When acid or base is added to buffer,
pH change is small
if have glass with NaOH & pH 7 if you add base,
pH go up
the more H ions [more acidic]
pH value gets lower
if have glass with HCl & pH 7 if you add acid,
pH will go down
The defining equation for the calculation of a pKa value is
pKa = −log Ka
acidic hydrogen atoms do what?
participate in acid-base reactions
alpha particle
particle in which 2 protons & 2 neutrons are present that is emitted by certain radioactive nuclei
conjugate base =
partner base
The term osmosis implies
passage of solvent only.
Tell me what osmosis is
passage of solvent through semipermeable membrane separating dilute solution [or pure solvent] from more concentrated solution
Number of digits [pH]
past decimal in pH value determines number of sig figs in [H3O+] or [OH-]
Beta Particle Effects can
penetrate much deeper than alpha particles & can cause severe skin burns if source remains in contact w skin for appreciable amount of time
If you dissolve HCl in water,
precedes 100% to right
Why is the vapor pressure of a solution that contains a nonvolatile solute always less than that of pure solvent?
presence of solute molecules decreases ability of solvent molecules to escape
solvent
present in greatest amount
solute
present in lesser amount; substance being dissolved
It is the total number of particles (ions or molecules
present in solution that determines magnitude of colligative property effect.
What is the effect of pressure on liquids?
pressure has little effect on solubility of liquids in water
What is the effect of pressure on solids?
pressure has little effect on solubility of solids in water
What is the effect of pressure on gases?
pressure has major effect on solubility of gases in water
Buffer do what?
prevent major changes in solution pH when small amounts of acid or base are added to it
Chemical reaction is
process in which at least 1 new substance is produced as result of chemical change
supersaturated solution will
produce crystals rapidly, often in dramatic manner, if slightly disturbed or if "seeded" w tiny crystal of solute
bronsted-lowry acid and Bronsted-lowry base
production must occur simultaneously [can't have one without other]
What circumstances have to exist for 2 things to react & make new thing?
properties have to bump into each other/collide at right orientation & need exactly right energy
Brønsted-Lowry base
proton acceptor
Brønsted-Lowry acid
proton donor
Conjugate base is the species formed when
proton is accepted by Bronsted-Lowry base
Catalysts increase reaction rates by
providing alternative reaction pathways that have lower activation energies than original, uncatalyzed pathway
"ionize" =
pull electrons off of it
gamma ray is like
pure energy
Non - ionizing radiation
radiation w insufficient energy to remove electron from atom or molecule
in ionizing radiation, after the radiation removes electron from atom or molecule
radiation w slightly decreased energy will interact w another atom
"spontaneous emission of either energy of a particle =
radioactivity
Radioactive nuclide aka
radionuclide
The largest source of background radiation exposure, for the average American, is
radon gas
Solution formation occurs more
rapidly as temp is increased.
How will the following action affect a reaction rate? decrease the concentration of a reactant
rate decreases
How will the following action affect a reaction rate? decrease the surface area of a solid reactant
rate decreases
How will the following action affect a reaction rate? add a catalyst
rate increases
Predict the solubility of each of the following solutes in the solvent indicated. AgNO3 (an ionic solid) in water
soluble
Classify each of the following reactions using one selection from the choices redox and nonredox combined with one selection from the choices combination, decomposition, displacement, exchange, and combustion Zn + Cu(NO3)2 -> Zn(NO3)2 + Cu
redox & displacement
Fe (s) + Cu2+ (aq) -> Fe2+ (aq) + Cu (s)
redox bc change in ion charges
C6H12O6 + 6O2 -> 6CO2 + 6H2O
redox reaction
Fe(s) + Cu^2+ -> Fe^2+ Cu(s)
redox reaction
Loss of oxygen
reduced
For each of the following NaOh solutions, the volume of the solution and its molarity are given. Calculate the number of moles of NaOh present in each solution. 0.800 L solution, 0.100 M
0.0800 moles
What is the mass-volume percent glucose concentration in blood plasma if the glucose concentration is known to be 92 mg/dL?
0.092% (m/v) glucose
Name some acids
1) Acetic acid [vinegar] 2) citric acid [tartness in lemons]
Name some bases
1) Bleach 2) Drano
What are the group IIA strong hydroxide bases?
1) Ca(OH)2 2) Sr(OH)2 3) Ba(OH)2
Diagnostic: criteria
1) Low concentration 2) Short half life 3) Know mechanism for eliminations 4) Known chemical properties
Collision theory involves
1) Molecular Collisions 2) Collision Orientation 3) Activation Energy
In a molarity problem you need 2 things:
1) Moles of solute 2) Liters of solution
What are the conjugate acid-base pairs in the reaction NH3(g) + H2O(l) <=> NH4^+(aq) + OH^-(aq)
1) NH3 and NH4^+ 2) H2O and OH^-
What is the molarity of the solution prepared by concentrating, by evaporation of solvent, 2212 mL of 0.400 M K2SO4 solution to a volume of 853 mL?
1.04 M
What is the hydrogen ion concentration of a solution with pH = 10.75?
1.8 x 10^-11
How many grams of KCl are present in 250.0 grams of a 7.50 % (m/m) KCl solution?
1.88 x 10^1 g KCl
What is the osmolarity of the following solution? 2 M CaCl2
6 osmol
What is the osmolarity of the following solution? 2 M in both NaCl and glucose
6 osmol
The dL volume unit is equivalent to
100 mL
What is the pH of a solution of 0.0100 M NaOH?
12.00
how many grams of sucrose (table sugar, C12H22O11) are present in 185 mL of a 2.50 M sucrose solution?
158 g C12H22O11
Give me a conversion factor for the percent concentration 15%(m/m) NaCl solution
15g NaCl/100g solution
how many grams of NaCl are present in 50.0 mL of a 7.50%(m/v) NaCl solution?
3.75 g
Calculate the number of moles of solute in 26.75 mL of 0.1405 M K2Cr2O7(aq)
3.77 x 10^-3 mol
How many grams of solute are present in 725 mL of 0.460 M KBr?
3.97 x 10^1 g
Determine the %(m/m) of glucose when 10.0 g of ethanol is added to 40.0 g of water
20.0
For each of the following aqueous NaCl solutions, the mass of solute and the mass of solvent present are given. Calculate the mass percent of NaCl present in each solution. 10.0 g NaCl, 40.0 g H2O
20.0% (m/m)
for a solute to dissolve in a solvent
2 types of interparticle attractions must be overcome [solute-solute attractions & solvent-solvent attractions]
If [H3O^+] = 1.00 x 10^-8, then pH=
8
For the following reaction, indicate which substance is oxidized and which substance is reduced. Identify the oxidizing and reducing agents. Ca + Cl2 → CaCl2
Ca is oxidized [reducing agent] and Cl2 is reduced [oxidizing agent]
Give the conjugate base for the acid below: H3PO4
H2PO4^-
Write the chemical formula of each of the following. The conjugate base of H3PO4
H2PO4^-
Write an equation for each of the following buffering actions. The response of H2PO4^−/HPO4^2− buffer to the addition of h3O+ ions
H2PO4^2- + H3O^+ -> HPO4^- + H2O
Identify which substance is the oxidizing agent and which substance is the reducing agent in each of the redox reactions 3H2SO3 + 2HNO3 -> 2NO + H2O + 3H2SO4
H2SO3 reducing agent; HNO3 oxidizing agent
Give the formula for the conjugate acid of HSO4^-
H2SO4
Write the balanced molecular equation for the neutralization reaction between H2SO4 and KOH in aqueous solution
H2SO4 + 2KOH -> K2SO4 + 2H2O
Le Chatelier's Principle
If stress is applied to system in equilibrium, system will readjust in direction that best reduces stress imposed on system
synthetic elements
Over 2000 bombardment produced radionuclides are known.
Assign an oxidation number to each element in the following compounds or polya- tomic ions. P2O5
P = +5, O = -2
Two liquids react faster than a liquid and a gas
More contact between the reactants.
Which of the following will be soluble in Hexane (C6H12) C2H6 More than one correct answer N2 CH3OH
More than one correct answer
When acid is added to this buffer H3O^+ + C2H3O2^- ⇔ HC2H3O2 + H2O
Most of H3O^+ added is converted to HC2H3O2 and pH changes very little.
When base is added to this buffer HC2H3O2 + OH^- ⇔ C2H3O2^- + H2O
Most of OH^- added reacts w acid & is converted to H2O and pH changes very little.
Which of the following aqueous solutions would give rise to a greater osmotic pressure? 7.00 g of NaCl in 775 mL of solution or 6.00 g of NaBr in 275 mL of solution
NaBr
NaCl has...
Na^+ and Cl^-
NH3 (aq)+H2O(l)→NH4+ (aq)+OH- (aq) here water is
acid
Using the Arrhenius theory, classify the following as either an acid or a base: CH3NH3^+
acid
Acid A has a pKa value of 4.23, and acid B has a pKa value of 3.97. Which of the two acids is stronger?
acid B
in buffers,
acid absorbs the base & vice versa
What is constantly changing for a system in a state of chemical equilibrium?
actual reactant molecules present
to create a conjugate acid,
add hydrogen
This results in a decreased vapor pressure for the solution
adding solute to solvent
Which of the following chemical equations is that for an acid-base neutralization reaction? a. H2SO4 +Zn -> ZnSO4 +H2 b. HNO3 +KOH -> KNO3 + H2O c. AgNO3 + NaCl -> AgCl + NaNO3 d. no correct response
b
ionizing radiation =
bad; makes them die
Cl^- is
base bc can accept
Strong acids/bases are
better electrolytes than weak acids/bases bc strong acids come completely apart when put in water
Chemical Reactions occur
between electrons
All nuclides of all elements
beyond bismuth [Z = 83] in periodic table are radioactive
if the number on top is
big & bottom is small, equilibrium constant will be big
alpha particle size
big [so can't go very fast]
14N7 + 4α2 -> 17O8 + 1p1
bombardment reaction
Combustion reaction
chemical reaction between substance & oxygen [usually from air] that proceeds w evolution of heat & light [usually from flame]
HClO3
chloric acid
Classify each of the following reactions as a combination, decomposition, displacement, exchange, or combustion reaction. K2CO3 -> K2O + CO2
decomposition
Classify the following reaction: Ba(ClO3)2 -> BaCl2 + 3O2
decomposition
What general reaction type is characterized by there being a single reactant?
decomposition
Classify each of these reactions: Ba(ClO3)2 -> BaCl2 + 3O2
decomposition & redox
2H2O -> 2H2 + O2
decomposition reaction
BaCO3(s) -> BaO(s) + CO2(g) is what type of reaction?
decomposition reaction
XY -> X + Y
decomposition reaction
Indicate to which of the following types of reactions each of the statements listed applies: combination, decomposi- tion, displacement, exchange, and combustion. More than one answer is possible for a given statement. An element may be a product.
decomposition, displacement
Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through Based on each of the following identities for solutions A and B, indicate whether the liquid level in compart- ment A, with time, will increase, decrease, or not change. A = 1.0 M NaCl solution and B = 2.0 M NaCl solution
decrease
Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through Based on each of the following identities for solutions A and B, indicate whether the liquid level in compart- ment A, with time, will increase, decrease, or not change. A = 1.0 M glucose solution and B = 1.0 M NaCl solution
decrease
Indicate whether each of the following actions will increase or decrease the rate of dissolving of a sugar cube in water. Cooling the sugar cube-water mixture
decrease
Will the changes listed increase or decrease the rate of the following chemical reaction? 2CO + O2 -> 2CO2 Lowering the temperature of the reaction mixture
decrease
Will the changes listed increase or decrease the rate of the following chemical reaction? 2CO + O2 -> 2CO2 removing some CO from the reaction mixture
decrease
Indicate the effect of the following on the rate of this reaction: 3H2 (g) + N2 (g) -> 2NH3 (g) Decrease concentration of N2
decrease rate
When red blood cells are placed in a hypotonic solution
hemolysis occurs
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 0.92%(m/v) glucose solution
hemolyze
Why does adding solute increase boiling point?
higher temp will be needed to raise depressed vapor pressure of solution to atmospheric pressure
A solution is
homogeneous mixture of 2 or more substances
proticity
how many H an acid has
generally in a solution
dissolved solutes are present as individual particles [molecules, atoms or ions]
for mass-volume percent, "volume of solution" goes on bottom
do not add together on bottom bc diff units
Most molecular solutes
do not produce ions or charged particles when dissolved in water
For percent by mass & percent by volume,
do not put 100% in calculator [put percent in answer]
Increasing the pressure associated with an equilibrium system by adding an inert gas (a gas that is not a reactant or a product in the reaction)
does not affect position of equilibrium.
Dilution with water
does not alter numbers of moles of solute present
Nonpolar oil
does not interact w polar water
Value of Ka
does not tell you if acid is dangerous
Adding an inert gas
doesn't affect the equilibrium.
Kw value
doesn't change bc it's a constant
in a reaction, catalyst
doesn't move you to left or right
Strong acids...
don't exist in equilibrium
oil and water
don't mix
in HF + H2O <=> H3O^+ + F^- HF
donates H to water molecule
in terms of electron transfer: oxidizing agent
electrons gained
in terms of electron transfer: reducing agent
electrons lost
CO2 + H2O + heat -> C6H12O6 + O2 is example of
endothermic reaction
What is happening in an endothermic reaction?
energy is absorbed
In an exothermic reaction,
energy is product of reaction [ex: burning of fuel]
in an endothermic reaction,
energy is reactant in reaction [ex: photosynthesis in plants]
What is happening in an exothermic reaction?
energy is released
The charge-balance requirement for a solution of ions requires that
equal equivalents of positive and negative ions are present
[osmosis] The net transfer of solvent across the membrane continues From this point on, there is
equal flow of solvent in both directions across membrane & volume of liquid on each side of membrane remains constant.
If 25.0 mL of 1.0 M NaOh is needed to completely react with 25.0 mL of a monoprotic acid in an acid-base titration, the molarity of the acid is
equal to 1.0 M
in equation with weak electrolytes
equilibrium between undissociated form & ions in aqueous(aq) solutions
Keq =
equilibrium constant
acid ionization constant
equilibrium constant for reaction of weak acid w water.
Kw
equilibrium constant for water
for weak acids, the
equilibrium constant is really small
Products high
equilibrium constant really high; reactions go to right
HF + H2O <=> H3O^+ + F^- if H3O^+ on right side goes down
equilibrium goes to right; pH stays same
Tell me about the equilibrium in H2O(l) + H2O <=> H3O^+ + OH^-
equilibrium lies really far to left
HF + H2O <=> H3O^+ + F^- is
equilibrium process
The reaction between nitrogen and hydrogen to produce ammonia is described as
equilibrium reaction
If you add acid or base to water,
equilibrium will shift so product will always be 1.0 x 10^-14
H2CO3(aq) + H2O(l) <=> HCO3^-(aq) + H3O^+(aq) What will happen to the equilibrium if the amount of carbonic acid is decreased?
equilibrium will shift to left
H2CO3(aq) + H2O(l) <=> HCO3^-(aq) + H3O^+(aq) What will happen to the equilibrium if the concentration of bicarbonate ion is decreased?
equilibrium will shift to right
if Value of Keq is very large (10^30) what is Relative Amount of Products and Reactants & Description of Equilibrium Position
essentially all products & far to the right
ethanol is a polar solvent and carbon tetrachloride is a nonpolar solvent. In which of these two solvents are each of the following solutes more likely to be soluble? NaCl, ionic
ethanol
ethanol is a polar solvent and carbon tetrachloride is a nonpolar solvent. In which of these two solvents are each of the following solutes more likely to be soluble? Sugar, polar
ethanol
true or false? if the energy of the products is higher than the energy of the reactants, the reaction is exothermic
false [if product energy is higher, it's endothermic]
A very small value for an equilibrium constant characterizes a chemical reaction where the equilibrium position lies
far to the left
"smaller"
faster reaction
Two liquids react
faster than a liquid and a gas
nuclear medicine
field of medicine in which radionuclides are used for diagnostic & therapeutic purposes
How much product do you make before you start going backward?
find out by measuring concentrations
for example if this is the problem: Determine the pH of the following solution: 1.0 × 10^-4 M OH^-
first find H3O^+ then find pH
To go from pH to
hydrogen of concentration, use 10^ button on calculator
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 0.28 M NaCl
hypertonic
causes cells to hemolyze/burst
hypotonic
osmotic pressure relative to body fluids is less than
hypotonic
Polar vs nonpolar
if same, will mix
DISSOCIATION: The process whereby,
in aqueous solution, positive & negative ions are released from ionic compound.
Like dissolves like works
in general
Indicate whether each of the following actions will increase or decrease the rate of dissolving of a sugar cube in water. Crushing the sugar cube to give a granulated form of sugar
increase
Indicate whether each of the following actions will increase or decrease the rate of dissolving of a sugar cube in water. Stirring the sugar cube-water mixture
increase
Oxidation involves
increase in oxidation number.
Indicate the effect of the following on the rate of this reaction: 3H2 (g) + N2 (g) -> 2NH3 (g) Increase concentration of H2
increase rate
What is the effect of temperature on gases?
increase temp = gas solubilities in water decrease
The more you increase
increase temperature, more soluble [for solids in liquids]
In general, the solubilities of gaseous solutes in water
increase with increasing pressure
Decreased volume
increased pressure
The rate at which a chemical reaction occurs decreases as the activation energy
increases
Increased available surface area
increases likelihood of reactant collisions.
dilution has
indirect relationship
Predict whether the following compound is soluble or insoluble in water: AgI
insoluble
in osmosis, the rate of flow
into concentrated solution is greater than rate of flow in other direction
In an aqueous solution of a weak acid, HA, the concentration of A^− ion
is equal to that of H^+
in a nuclear reaction, The nuclear reactivity of an element
is independent of state of chemical combination.
Mixing an ionic substance with a nonpolar substance
is like mixing polar w nonpolar
What actually changes when acid or base is added to this buffer: HC2H3O2/C2H3O2^-
is proportion of HC2H3O2 to C2H3O2^-
Not every compound
is soluble in water bc the ionic bonds are too strong
Indicate whether the osmotic pressure of a 0.1 M NaCl solution will be less than, the same as, or greater than that of each of the following solutions. 0.1 M MgCl2
less
The mass of solute per 100 mL of solution is abbreviated as
m/v
Hydrocarbons
made of only hydrogen & carbon
Group 1 and ammonium
makes bond weak
little p
makes things backward [pH, pKa]
Mass of solution =
mass of solute + mass of solvent
%(m/v)
mass of solute(g)/volume of solution(mL) x 100
%(m/m)
mass of solute/mass of solution x 100
The percent concentration unit most often encountered in a hospital (medical) setting is
mass-volume percent
As [H3O+] goes down
means less hydrogen ions so pH goes up [more basic]
The largest source of radiation exposure from human activities, for the average American, is
medical X-rays
Semi-permeable membrane is what?
membrane that allows certain types of molecules to pass through it but prohibits passage of other types of molecules
Salt =
metal & nonmetal
The more you stir it,
more soluble
hypertonic solution will cause the
net transfer of water from tissues to blood
Nonacidic hydrogen atoms do
not participate in acid-base reactions
The presence of water is
not prerequisite for a solution
Nonelectrolytes do
not produce ions in water [do not conduct an electric current]
Acids do...
not react w other acids
Indicate whether each of the following solutes will be soluble in the indicated solvent (in parentheses) CCl4 mixed with water (H2O)
not soluble
Acid A is weaker than acid B if, at equal concentrations,
percent ionization of A is less than that of B
HClO4
perchloric acid
HCl has
permanent dipole
For which of the following types of ionic compounds are most examples insoluble in water? a. nitrates b. phosphates c. acetates d. no correct response
phosphates
Chemical equilibrium is similar to
physical equilibrium of evaporation & condensation of liquid in closed container
colligative properties
physical property of solution that depends only on number of solute particles [molecules or ions]present in given quantity of solvent & not on their chemical identities
geiger counters only
pick up gamma rays
Is H2O polar or nonpolar? Why?
polar bc angular/bent molecular geometry
NH3 gas is
polar gas [much more soluble in H2O [polar liquid] than is O2 gas [nonpolar gas]
Water is a
polar molecule
Like dissolves like works in general
polarity of water [+ & - ends] suggests all ionic compounds would be soluble
How will the following action affect a reaction rate? increase the temperature
rate increases
What condition must be met in order for a system to be in a state of chemical equilibrium?
rate of forward reaction = rate of reverse reaction
If the concentration of a reactant increases,
rate of forward reaction increases until equilibrium is reestablished
If the concentration of a product decreases,
rate of reverse reaction increases until equilibrium is reestablished
chemical reaction rate is what?
rate which reactants are consumed or products produced in given time period in chemical reaction
Enzymes control
rates of reaction
Liquid & gas
react faster than solid & gas
equilibrium constant for C(s) + h2O(g) -> CO(g) + h2(g) is [CO][H2]/[H2O]
reactant carbon (C) is solid so will not appear in equilibrium constant expression.
Molecular collisions is like
reactant molecules, ions or atoms must come in contact [collide] w one another in order for any chemical change to occur
You can think of heat as
reactant or product whose increase or decrease stresses equilibrium just as change in reactant or product concentration does
HA(aq) + H2O(l) ⇔ H3O+(aq) + A-(aq) tell me about this reaction
reactants high; products low [equilibrium lies far to left]
Le Chatelier's Principle says When disruption causes more
reactants to form, equilibrium has shifted to left
in equilibrium,
reaction hasn't stopped [just doing at same rate in both directions]
Nuclear reaction is
reaction in which changes occur in nucleus of atom
combustion:
reaction of anything w O2
When reactants are all the same physical state,
reaction rate is generally faster
When the particle size of a solid is extremely small,
reaction rates can be so fast that explosion results.
Most Acid Base
reactions reach equilibrium
"same state"
reacts faster
Unstable nucleus
readily undergoes change
Concentrations are
really small
By using oxidation numbers, determine whether the following reaction is a redox reac- tion or a nonredox reaction. 4NH3 + 3O2 -> 2N2 + 6H2O
redox
Classify each of the following reactions as (1) a redox reaction (2) a nonredox reaction or (3) "can't classify" because of insufficient information A combination reaction in which one reactant is an element
redox
Classify each of the following reactions as (1) a redox reaction (2) a nonredox reaction or (3) "can't classify" because of insufficient information A decomposition reaction in which one of the products is an element
redox
Classify each of the following reactions as (1) a redox reaction (2) a nonredox reaction or (3) "can't classify" because of insufficient information A decomposition reaction in which the products are all elements
redox
Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)
redox
Classify each of the following reactions using one selection from the choices redox and nonredox combined with one selection from the choices combination, decomposition, displacement, exchange, and combustion CH4 + O2 -> CO2 + 2H2O
redox & combustion
Different isotopes of an element have
same chemical properties but different nuclear properties
isotonic =
same concentration inside and outside
Tell me a rule for solubility
same polarity = soluble
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 0.14 M in both glucose and sucrose
same size
The processes of replacing body fluids and supplying nutrients to the body intravenously require
use of isotonic solutions
example: What is the molarity (M) of a solution prepared by diluting 0.180 L of 0.600 M HNO3 to 0.540 L? "of" = they go together on one side
so .180 and .600 go on same side
According to Le Chatelier, pressure
system will shift away from added gaseous component [If component is removed, opposite effect occurs]
in equilibrium constant expressions!
take coefficient & add as exponent
Identify the solute and the solvent in solutions composed of the following: 2.00 mL of water and 20.0 mL of ethyl alcohol
water solute; ethyl alcohol solvent
As the amount of solute & solvent changes,
way it conducts electricity will be very diff
Most solutions
we encounter fall under category of unsaturated solution
HF is very
weak [almost all reactant; very small concentration of product]
HA + H2O <——- ->H3O^+ + A^- is showing
weak acid
Identify each of the following as a strong or weak acid or base. HNO2
weak acid
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other H3PO4
weak acid
One mole of any molecular solute raises the boiling point of one kilogram of water by the same amount,
which is 0.51°C
Decreasing the surface area
will allow fewer particles to collide, decreasing the reaction rate
A crushed aspirin tablet
will dissolve in water more rapidly than a whole aspirin tablet.
Water is the
universal solvent
A radionuclide has a half-life of 6.0 hr. What fraction of the atoms in a sample of this radionuclide will remain undecayed after the following times? a. 12 hr b. 36 hr c. 3 half-lives d. 6 half-lives
a) 1/4 b) 1/64 c) 1/8 d) 1/64
Calculate the ph of solutions with the following hydroxide ion concentrations. a. 1.00 × 10^−4 M b. 1.00 × 10^−10 M c. 1.11 × 10^−3 M d. 6.05 × 10^−7 M
a) 10.000 b) 4.000 c) 11.045 d) 7.782
lodine-125 has a half-life of 60 days. How long, in days, will it take for the radiation level of an iodine-125 sample to drop to a. one-fourth its original level b. 1/16 its original level
a) 120 days b) 240 days
Ca + Cl2 -> CaCl2
Ca -> Ca^2+ and Cl2 -> 2Cl^-
H3O^+ is the conjugate acid of
H2O
Colligative molarity of Al(NO3)3 using: solution A = 0.10 M Al(NO3)3 (aq)
4(0.10 M) = 0.40 M
if the original pH problem says: "1.0 x 10^-4" and answer is 4. How should you write it?
4.00
The defining equation for percent-by-volume concentration is
(volume solute/volume solution) × 100
polarity of water
+ and - ends
Determine the oxidation number of the indicated ele- ment in each of the following ions. Al in Al^3+
+3
pKa =
-log Ka
Iodine-131 is a radionuclide that is frequently used in nuclear medicine. Among other things, it is used to detect fluid buildup in the brain. The half-life of iodine-131 is 8.0 days. How much, in grams, of a 0.16-g sample of iodine-131 will remain undecayed after a period of 32 days?
.010 g
What is the oxidation number of S in each of the following molecules? S2
0
What is the molarity of the solution prepared by diluting 25.0 mL of 0.220 M NaCl to each of the following final volumes? 457 mL
0.0120 M
What is the molarity of the solution prepared by diluting 25.0 mL of 0.220 M NaCl to each of the following final volumes? 75.0 mL
0.0733 M
What is the molarity of the solution prepared by diluting 25.0 mL of 0.220 M NaCl to each of the following final volumes? 30.0 mL
0.183 M
What is the molarity (M) of a solution prepared by diluting 0.180 L of 0.600 M HNO3 to 0.540 L?
0.200 M
Calculate the mass percent of solute in the following solutions. 0.0032 g of NaOH dissolved in 1.2 g of H2O
0.27% (m/m)
For each of the following NaOh solutions, the volume of the solution and its molarity are given. Calculate the number of moles of NaOh present in each solution. 1.35 L solution, 0.300 M
0.405 moles
how many grams of Na2CO3 are needed to prepare 25.0 mL of a 2.00%(m/v) Na2CO3 solution?
0.500 g
If you have a 0.250 M solution of CaCl2 what is the concentration of Cl^- ions?
0.500 moles Cl^-
For each of the following NaOh solutions, the volume of the solution and its molarity are given. Calculate the number of moles of NaOh present in each solution. 875 mL solution, 0.600 M
0.525 moles
For each of the following hCl solutions, the moles or grams of solute present and the total solution volume are given. Calculate the molarity of each solution. 30.0 g HCl, 1.45 L solution
0.567 M
how many equivalents of Ca2+ ion are present in a solution that contains 0.30 mole of Ca2+ ion?
0.60 Eq
The osmolarity of a 0.40 molar NaCl solution is
0.80
2 Things Can Happen to an Electron Subjected to Radiation
1 Excitation 2) Ionization
1 g/dL =
1 g/100 mL = 1%(m/v)
The density of water is approximately
1 g/mL
The results of dissolving these solutes in water are: CaCl2
1 mole of CaCl2 produces 3 moles of particles [ions] when dissociation occurs.
Two moles of ions are produced from
1 mole of NaCl
Kw = what?
1.0 × 10^-14
For each of the following aqueous NaCl solutions, the mass of solute and the mass of solvent present are given. Calculate the mass percent of NaCl present in each solution. 5.00 g NaCl, 355 g H2O
1.39% (m/m)
The pH of a solution is 5.85. What is the [H3O+] for this solution? [H3O+] = 10^-pH
1.4 x 10^-6
The ph of a solution is 6.80. What is the molar hydronium ion concentration for this solution?
1.6 x 10^-7
How many grams of Na2CO3 are present in 35.0 mL of 5.00 % (m/v) solution?
1.75 g Na2CO3
If a weak acid has a pKa value of 8.73, what is the value of Ka for the acid?
1.9 x 10^-9
After three half-lives have elapsed, the amount of a radioactive sample which has not decayed is which of the following?
1/8 the original amount
Write equilibrium constant expressions for the following reactions. Ca(s) + Cl2(g) -> CaCl2(s)
1/[Cl2]
Write equilibrium constant expressions for the following generalized reactions. 2X(g) + 3Y(g) -> 2Z(s)
1/[X]^2 [Y]^3
how many grams of sucrose must be added to 375 g of water to prepare a 2.75%(m/m) solution of sucrose?
10.6 g sucrose
how many liters of a 0.100 M solution can be prepared from 60.0 g of each of the following solutes? KOH
10.7 L
92mg glucose/1 dL solution x 10^-3 g glucose/1 mg glucose x 1 dL solution/100 mL solution
100 in 100 mL is not used in obtaining numerical answer bc definition for mass-volume percent is g solute/100 mL solution.
A 2.0%(m/v) NaCl solution contains 2.0 g of NaCl per
100.0 mL solution
What is the boiling point of a solution that contains 0.25 mole of the ionic solute NaBr per one kilogram of water?
100.26 degrees celsius
What is the boiling point of a solution that contains 1.00 kg of water and each of the following quantities of solute? 3.00 moles of NaCl (an ionic compound)
103.06 degrees celsius
What is the boiling point of a solution that contains 1.00 kg of water and each of the following quantities of solute? 3.00 moles of Na3PO4 (an ionic compound)
106.12 degrees celsius
[H3O^+] =
10^- pH
How many milliliters of ethanol are needed to prepare 125 mL of a 8.5% (v/v) solution?
11 mL ethanol
Strontium-90 is a nuclide found in radioactive fallout from nuclear weapon explosions. Its half-life is 28.0 years. How long, in years, will it take for 94% (15/16) of the strontium-90 atoms present in a sample of material to undergo decay?
112 years
How many grams of CaCl2 are needed to make 276.4 g of a solution that is 41.5% (m/m calcium chloride in water?
115 g CaCl2
Calculate pH for each H3O^+ concentration: [H3O^+] = 1 x 10^-13 M
13.0
What is the (v/v) % of a solution if 15.0 mL of ethanol is added to 95.0 mL of water?
13.6% (v/v)
If the half-life of a 2.0-gram sample of a radionuclide is 14 hours, then the half-life of a 1.0 gram sample of the same radionuclide would be
14 hours
how many liters of a 0.100 M solution can be prepared from 60.0 g of each of the following solutes? LiCl
14.2 L
How many grams is 15 mL of water?
15 g
What volume of a 2.00% (m/v) HCl solution can be prepared by diluting 25.0 mL of 14.0% (m/v) HCl solution
175 mL
What is the percent by volume of isopropyl alcohol in an aqueous solution made by diluting 22 mL of pure isopropyl alcohol with water to give a volume of 125 mL of solution?
18% (v/v)
For each of the following solutions, how many milliliters of water should be added to yield a solution that has a concentration of 0.100 M? 2.00 mL of 1.00 M NaCl
18.0 mL
How many ions per the formula unit NaNO3
2
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) in this acid-base reaction, there are
2 conjugate acid-base pairs related by loss/gain of H^+
A solution contains
2 or more components
What is the osmolarity of the following solution? 2 M glucose
2 osmol
Diprotic acids supply
2 protons [H+ ions] during acid- base reaction
Colligative molarity of NaNO3 using: solution B: 0.20 M NaNO3 (aq)
2(0.20 M) = 0.40 M
Calculate pH for each H3O^+ concentration: [H3O^+] = 0.01 M
2.0
Sufficient acidic solute is added to a quantity of water to produce a solution with [H3O+] = 4.0 × 10^−3. What is the [OH−] in this solution?
2.5 x 10^-12
Calculate the molarity of a 10.0%(m/v) NaOH solution.
2.50 M
A 0.0100 M solution of an acid, HA, is 15% ionized. Calculate the acid ionization constant for this acid.
2.6 x 10^-4
What is the concentration of a solution made by diluting 35 mL of 6.0 M HCl to a final volume of 750 mL?
2.8 x 10^-1 M
The bombardment reaction involving 23Na11 and 2H1 gives two products, one of which is 1H1. The other product is
24Na11
Triprotic acids supply
3 protons [H+ ions] during acid-base reaction
Calculate the molarity of: 0.650 mol of NaOH in 1.85 L of solution
3.51 x 10^-1 M
Calculate the molarity of: 15.7 g of NaCl in 749 mL of solution
3.59 x 10^-1 M
After all of the water is evaporated from 10.0 mL of a CsCl solution, 3.75 g of solid CsCl remains. Calculate the original concentration of the CsCl solution in the following units. mass-volume percent
37.5% (m/v)
How many milliliters of a 5.75% (v/v) ethanol solution can be prepared from 2.25 mL of ethanol?
39.1 mL solution
Finish the reaction: 3H2 + N2
3H2 + N2 <=> 2NH3
How many ions per the formula unit Al(NO3)3
4
If [H3O^+] = 1.00 x 10^-4, then pH=
4
2 M NaCl =
4 mol NaCl/2 L solution
What is the osmolarity of the following solution? 2 M NaCl
4 osmol
Determine the final concentration of each of the following solutions after 20.0 mL of water has been added. 30.0 mL of 7.5 M NaCl solution
4.5 M
Calculate the volume percent of solute in each of the following solutions. 4.00 mL of bromine in enough carbon tetrachloride to give 87.0 mL of solution
4.60% (v/v)
A 0.00300 M solution of an acid is 12% ionized. Calculate the acid ionization constant Ka.
4.9 x 10^-5
Calculate the number of grams of NaOH needed to prepare each of the following amounts of solution. 1.00 L of 1.00 M NaOH
40.0 g
A nurse wants to prepare a 1.0%(m/v) silver nitrate solution from 24 mL of a 3.0%(m/v) stock solution of silver nitrate. how much water should be added to the 24 mL of stock solution?
48 mL
Write a balanced chemical equation for a totally gaseous equilibrium system that would lead to the following equi- librium constant expression Keq = [N2]^2[H2O]^6/[NH3]^4[O2]3
4NH3(g) + 3O2(g) <=> 2N2(g) + 6H2O(g)
What is the osmolarity of the following solution? 2 M in NaCl and 1 M in glucose
5 osmol
Consider the solution of KCl made by dissolving 100.0 g of solute in 250.0 mL of solution. Calculate the molarity.
5.370 M
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. Ammonia gas in water with P = 1 atm and T = 50°C Ammonia gas in water with P = 1 atm and T = 90°C
50 degrees Celsius
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) what is the base?
H2O
Contrast alpha and beta particles in terms of how far they can travel in air before their energy is dissipated
6 cm vs 1000 cm
Calculate pH for each H3O^+ concentration: [H3O^+] = 1 x 10^-6 M
6.0
What is the (m/v) % of a solution of 5.8 g of KCl in 85 mL of solution?
6.8% (m/v)
For each of the following solutions, how many milliliters of water should be added to yield a solution that has a concentration of 0.100 M? 75.0 mL of 0.110 M NaCl
7.5 mL
After the addition of a small amount of acid, a solution that is buffered at a ph of 8.0 will have an approximate ph of
8.0
What is the osmolarity of each of the following solutions? 2.0 M in both KNO3 and NaCl
8.0 OsM
Calculate the ph for each of the following solutions. [OH−] = 1.0 × 10^−6
8.00
Determine the pH of the following solutions: 3.2 x 10^-6 M OH^-
8.51
For HF + H2O <=> H3O^+ + F^-
99.9% HF; 0.01% F^-
Soluble ionic compounds do!
dissociate into ions in solution.
Arrhenius theory says an acid
dissociates in water to produce hydrogen ions
Nonelectrolytes do what?
dissolve as molecules in water [does not dissociate]
Aqueous is like
dissolved in water
Substances burn
more rapidly in pure oxygen than in air
As the value of Ka gets bigger,
more reactant dissociates [equilibrium moves to right]
Synthetic radionuclides?
outnumber naturally occurring nuclides by a 7-to-1 ratio.
Hydroxide ions (the basic species) are produced through dissociation.
Arrhenius base
Metals tend
to lose electrons
HF(aq)+H2O(l)⇔H3O+ (aq)+F- (aq)
Acid base equilibrium
Consider the reaction shown below. CH4 + 2 H2S + heat <---> CS2 + 4 H2 What action will increase the amount of CH4?
Add H2 to the reaction
Freezing-point depression
Adding a nonvolatile solute to solvent lowers freezing point of resulting solution below that of pure solvent.
Identify the solute in: a solution containing 3.0 g of AgNO3 and 15 mL of water
AgNO3
AlCl3 has...
Al^3+ and 3Cl^-
bombardment reaction is
Always 2 reactants and 2 products.
Hydrogen ions (the acidic species) are produced through ionization.
Arrhenius acid
Consider this aqueous reaction: HNO3(aq) + Ba(OH)2(aq) -> What is the formula for the salt that forms?
Ba(NO3)2
Rank these compounds by their expected solubility in hexane, C6H14 from most to least soluble H2O, C2H6, C2H5OH
C2H6, C2H5OH, H2O
The chemical reaction that occurs when a hCN/CN− buffer system responds to the addition of a small amount of acid is
CN^− +H3O^+ -> H2O + HCN
3Ni^2+(aq) + 2Co(s) -> 2Co^3+(aq) + 3Ni(s) What is the reducing agent?
Co
3Ni^2+(aq) + 2Co(s) -> 2Co^3+(aq) + 3Ni(s) Which substance gets oxidized?
Co
Mg(s) + Cl2(g) -> Mg^2+(aq) + 2Cl^-(aq) What is the oxidizing agent?
Cl2
Mg(s) + Cl2(g) -> Mg^2+(aq) + 2Cl^-(aq) Which substance gets reduced?
Cl2
The physical properties of a solution that depend only on the concentration of solute particles in a given quantity of solute, not on the chemical identity of the particles.
Colligative properties of solutions
Acetic Acid/Sodium Acetate Buffer
Common laboratory buffer
To write Keq, it's the
Concentration of products divided by concentration of reactants
Cu(s) + 2AgNO3(aq) -> 2Ag(s) + Cu(NO3)2(aq) What is the reducing agent?
Cu
Cu(s) + 2AgNO3(aq) -> 2Ag(s) + Cu(NO3)2(aq) Which substance gets oxidized?
Cu
For the following reaction, indicate which substance is oxidized and which substance is reduced. Identify the oxidizing and reducing agents. Cu (s) + Pt2+ (aq) -> Cu 2+ (aq) + 2 Pt (s)
Cu is oxidized [reducing agent] and Pt is reduced [oxidizing agent]
Cu (s) + Pt2+ (aq) -> Cu 2+ (aq) + 2 Pt (s) What is happening to Cu and Pt here?
Cu lost 2 electrons; Pt^2+ gained 2 electrons
Fe(s) + Cu^2+(aq) -> Fe^2+(aq) + Cu(s) What is the oxidizing agent?
Cu^2+
Identify the Bronsted-Lowry base in the following reaction HF + H2O -> H3O^+ + F^-
H2O
What is the acid in H2O + NH3 → OH^- + NH4^+
H2O
the Addition of Catalysts
Do not change position of equilibrium but equilibrium is established more quickly
What is the base in HCl + H2O → Cl^- + H3O^+
H2O
Write the conjugate acid of each of the following: OH^-
H2O
If a reaction has
H2O(l), concentration can't change
Gamma ray
Form of high energy radiation without mass or charge that is emitted by certain radioactive nuclei.
Write equilibrium constant expressions for the following reactions. 2NOCl(g) -> 2NO(g) + Cl2(g)
[NO]^2[Cl2]/[NOCl]^2
Because self ionization is
an equilibrium, can write equilibrium constant [Kw = [H3O+] [OH-]
Write the equilibrium constant expression for each of the following reactions. C(s) + h2O(g) -> CO(g) + h2(g)
[CO][H2]/[H2O]
Which of the following pairs of substance could function as a buffer in aqueous solution? a. hCl and hF b. h2CO3 and NahCO3 c. Na2CO3 and NahCO3 d. no correct response
H2CO3 and NaHCO3
Fe(s) + Cu^2+(aq) -> Fe^2+(aq) + Cu(s) What is the reducing agent?
Fe
Fe(s) + Cu^2+(aq) -> Fe^2+(aq) + Cu(s) Which substance gets oxidized?
Fe
For the redox reaction FeO+CO -> Fe+CO2 identify the: oxidizing agent
FeO
Write the chemical formula of each of the following. The conjugate acid of HC2O4^−
H2C2O4
In N2(g) + 3H2(g) <- ——> 2NH3(g)
Here, increasing pressure favors product [2 moles of gas vs 4 moles of gas]
Physical nature of the reactants
Includes physical state of each reactant [s, l or g] & particle size
Which of the following is the correct equilibrium constant expression for the reaction 2D(s) -> 2E(s) + F(g)
[F]
Salt is like a what?
Ionic compound containing metal or polyatomic ion as positive ion & nonmetal or polyatomic ion [except hydroxide] as negative ion
in weak acids...
Ionization equilibrium lies far to the left
in strong acids...
Ionization equilibrium lies far to the right.
Suppose a reaction occurs that is at equilibrium, shown below A + B <---> C It is observed that the concentration of C in the mixture is much larger (100x) than the concentrations of A and B. What is true regarding the equilibrium constant [K] for this reaction?
K will have value much greater than 1
Assign an oxidation number to each element in the following compounds or polya- tomic ions. KMnO4
K= +1, Mn = +7, O =-2
Identify which substance is oxidized and which substance is reduced in each of the following redox reactions. Cl2 + 2KI -> 2KCl + I2
KI oxidized; Cl2 reduced
Identify the solute in: a solution containing 10.0 g of LiBr and 100.0 g of water
LiBr
Mg(s) + Cl2(g) -> Mg^2+(aq) + 2Cl^-(aq) What is the reducing agent?
Mg
Assign an oxidation number to each element in the following compounds or polya- tomic ions. NO3−
N = +5, O = -2
3Ni^2+(aq) + 2Co(s) -> 2Co^3+(aq) + 3Ni(s) What is the oxidizing agent?
Ni^2+
Identify the solute in: air (a solution of 78% N2, 21% O2 and various other gases)
O2
What situations describes a basic aqueous solution?
[H3O+] is less than [OH−]
Radioactivity
Radiation spontaneously emitted from unstable nucleus.
Background radiation
Radiation that comes from natural sources to which living organisms are exposed on continuing basis.
Example of theraputic criteria
Radiation therapy
The most efficient buffer will have
[HA] approximately equal to [A^-]
S (s) + O2 (g) → SO2 (g) What is happening here?
S gains oxygen
Write the equilibrium expression for the following H2 (g) + I2 (g) -> 2 HI (g)
[HI]^2/[H2][I2]
The general expression for the acid ionization constant for a weak acid, HA, is
[H^+][A^−]/[HA]
For each solute, identify the better solvent: water or carbon tetrachloride I2
carbon tetrachloride (CCl4)
nuclear reaction is when you're
changing # of protons & neutrons
H2 + I2 <=> 2HI
This reaction is at equilibrium
Half-life
Time required for 1/2 of given quantity of radioactive substance to undergo decay
Strong acid does what?
Transfers 100% of its protons to water
Write the equilibrium constant expression for each of the following reactions. I2(g) + Cl2(g) -> 2ICl(g)
[ICl]^2/[I2][Cl2]
What does the value of Ka tell us about the strength of an acid?
Weak acid has small value for Ka
oil requires
a nonpolar solvent
Which of the following is always a product of an acid-base neutralization reaction? a. an acid b. a base c. a salt d. no correct response
a salt
What does potassium iodide (KI) do when dissolved in water?
dissociates to potassium and iodide ions
Write balanced nuclear equations for the alpha decay of each of the following nuclides. a) 200Po84 b) Curium-240 c) 244Cm96 d) uranium-238
a) 200Po84 -> 4a2 + 196Pb82 b) 240Cm26 -> 4a2 + 236Pu94 c) 244Cm96 -> 4a2 + 240Pu94 d) 238U92 -> 4a2 + 234Th90
238U92 a) 238 is b) 92 is
a) mass number b) atomic number
in HNO3 and H2SO4
all hydrogen atoms are acidic
in NH3 and CH4
all hydrogen atoms are nonacidic
Electrolyte
anything that comes apart in solution
How do the neutron-to-proton ratios compare for stable nuclei of low atomic number and stable nuclei of high atomic number?
approx 1 to 1 ratio for low atomic numbered stable nuclei & 3 to 2 ratio for higher atomic numbered stable nuclei
polar + polar
dissolve
A solution is made by dissolving 34.0 g of NaCl in 100 g of h2O at 0°C. Based on the data in Table 8-1, should this solution be characterized as dilute or concentrated
concentrated
[for colligative property]The number of solute particles present in a solution
depends on concentration of solute present & whether solute breaks up [dissociates] into ions once in solution.
pKa is calculated
from Ka in exactly same way pH is calculated from [H3O^+]
In the process of osmosis, solvent passes through a semipermeable membrane
from a dilute solution to a more concentrated solution
in terms of electron transfer: reduction
gain of electrons
in Cu(s) + Pt^2+(aq) -> Cu^2+(aq) + 2Pt(s)
gained Pt so reduced [oxidizing agent]
the oxidizing agent does what?
gains electrons
The term radioactive nuclide designates an atom whose nucleus
is unstable
Has no effect on cell size.
isotonic
element 118, the highest-atomic-numbered laboratory-produced element, has a half-life measured in
milliseconds
Lower the pH,
more acidic
Which substance is the reducing agent in the following redox reaction? CO+H2O -> CO2 +H2 a. h2O b. CO2 c. h2 d. no correct response
no correct response
The numerical value for a colligative property is dependent on the
number of solute particles present
When the forward and reverse reaction
occur at same rate, write equation w arrow pointing in both directions.
With pH, the sum
of exponents has to be -14
Gain of oxygen
oxidized
Keq=
products/reactants
Classify each of the following reactions using one selection from the choices redox and nonredox combined with one selection from the choices combination, decomposition, displacement, exchange, and combustion 2CuO -> 2Cu + O2
redox & decomposition
H2O+H2O ⇔ H3O+ +OH- is an example of
self-ionization
Solutions can be!
separated by physical means
10^ button on calculator
shift log
what is a nonaqueous solution?
solution in which substance other than water is solvent
How do you know how far the reaction goes to the right or left?
the equilibrium constant
Why does the Reaction rate increase as the temperature of the reactants increase?
the faster particles fly around, higher the chance of effective collision
Generally, solutions are
transparent [clear]
How does energy relate to gas & bbq
won't turn to fire until light it [flame you provide is activation energy]
Acidic hydrogen atoms are!
written at front of chemical formula
is O2 soluble in water?
yes
1 M NaCl =
•1 mol NaCl/1 L solution •2 mol NaCl/2 L solution •0.5 mol NaCl/0.5 L solution
Weak acids do what?
Transfers small % of its protons to water.
define self-ionization
Water molecules in pure water interact w one another to form ions
What is the general chemical equation for Combination reaction
X + Y -> XY
What is the general chemical equation for each of the following types of chemical reactions? Displacement reaction
X + YZ -> Y + XZ
What is the correct equilibrium constant expression for the reaction 3C(g) -> A(g) + 2B(g)
[A][B]^2/[C]^3
Write the Keq of: 4NH3(g) + 7O2(g) -> 4NO2(g) + 6H2O(g)
[NO2]^4 [H2O]^6/[NH3]^4 [O2]^7
Write equilibrium constant expressions for the following reactions. 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g)
[NO]^4[H2O]^6/[NH3]^4[O2]^5
In general, it is found that the
greater the diff in solute-solvent polarity, less soluble
Strong vs weak
has nothing to do w toxicity or danger [for acids]
The reactant, O2, is an element and thus
has oxidation number of zero (rule 1).
"which produces a beta particle" =
has to be on right side
When we dissolve 1 mole of NaCl in 1 liter of water,
have 1 mole of chemical & 2 moles of charge [1 mole Na^+ & 1 mole Cl^-]
When we dissolve 1 mole of CaCl2 in 1 liter of water,
have 1 mole of chemical & 3 moles of charge [1 mole of Na^+ & 2 moles of Cl^-]
Solutions of equal osmolarity
have equal osmotic pressures.
For strong hydroxide bases,
have group IA hydroxides and group IIA hydroxides
in N2(g) + 3H2(g) <—— -> 2NH3(g) + Heat
heat is product [exothermic reaction] so adding heat shifts equilibrium to left.
Will red blood cells crenate, hemolyze, or remain unaffected when placed in 2.3%(m/v) glucose solution
hemolyze
unstable =
high energy
for therapy, you want
high energy & a short half life
Geiger counters
high energy ionizing radiation
Match each of the following statements about the dis- solving of the ionic solid NaCl in water with the term hydrated ion, hydrogen atom, or oxygen atom. A Cl− ion surrounded with water molecules
hydrated ion
Match each of the following statements about the dis- solving of the ionic solid NaCl in water with the term hydrated ion, hydrogen atom, or oxygen atom. A Na+ ion surrounded with water molecules
hydrated ion
HBr
hydrobromic acid
HCl
hydrochloric acid
Match each of the following statements about the dis- solving of the ionic solid NaCl in water with the term hydrated ion, hydrogen atom, or oxygen atom. The portion of a water molecule that is attracted to a Cl− ion
hydrogen atom
Anything with
hydrogen bonds will be soluble in water
How does water interact with sodium?
hydrogen interacts w the chlorine; oxygen interacts w the sodium
HI
hydroiodic acid
Which of the following statements concerning acidic and basic solutions is correct? a. Acidic solutions have positive ph values and basic solutions have negative ph values. b. Acidic solutions have a ph greater than 7 and basic solution have a ph less than 7. c. hydronium and hydroxide ions are present in both acidic and basic solutions. d. no correct response
hydronium and hydroxide ions are present in both acidic and basic solutions.
any base besides
hydroxide is weak
the strong bases are
hydroxides of groups IA and IIA [metal hydroxides]
Causes cells to crenate (shrink).
hypertonic
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 0.28 M in both glucose and sucrose
hypertonic
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 5.0%(m/v) NaCl solution
hypertonic
osmolarity relative to body fluids is greater than
hypertonic
osmotic effect on cells is: net flow of water out of cells
hypertonic
osmotic pressure relative to body fluids is greater than
hypertonic
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 0.92%(m/v) glucose solution
hypotonic
Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? 2.3%(m/v) glucose solution
hypotonic
osmolarity relative to body fluids is less than
hypotonic
osmotic effect on cells is: net flow of water into cells
hypotonic
Tell me something about H2(g) + I2(g) <=> HI(g)
if add more product, reaction will move toward left
How do you know if you can donate a hydrogen?
if hydrogen is written at the beginning
Crenation occurs
in concentrated sodium chloride solution [a hypertonic solution]
Hemolysis occurs
in pure water [a hypotonic solution]
Solution is a homogeneous mixture of two or more substances
in which each substance retains its chemical identity
inert
inactive
When you combine an acid and a base, there is
no conjugate acid & base bc they neutralize
At 24°C, the ion product constant for water has the value a. 1.00 × 10^−7 b. 1.00 × 10^−10 c. 1.00 × 10^−13 d. no correct answer
no correct answer
After four half-lives have elapsed, the amount of a radioactive sample that has decayed is which of the following? a. 1/4 the original amount b. 3/4 the original amount c. 1/16 the original amount d. no correct response
no correct response
For which of the following solutions is the concentration 1.0 molar? a. 3.0 moles of solute in 1.5 L of solution b. 2.0 moles of solute in 500.0 mL solution c. 1.0 mole of solute in 100.0 mL solution d. no correct response
no correct response
In a solution containing 15 mL of water and 25 mL of isopropyl alcohol a. the water is the solvent b. the alcohol is the solute c. both the water and alcohol are considered to be solvents d. no correct response
no correct response
What is the [H3O+] in a neutral solution? a. zero b. equal to 1.00 × 10^−5 c. greater than 1.00 × 10^−7 d. no correct response
no correct response
Which of the following does not affect the rate at which a solute dissolves in a solvent? a. state of subdivision of the solute b. temperature of the solvent c. stirring during the dissolving process d. no correct response
no correct response
Which of the following effects will occur if the pressure on the following equilibrium system is decreased? 2NO2(g) -> N2(g) + 2O2(g) a. NO2 concentration increases b. N2 concentration remains the same c. O2 concentration decreases d. no correct response
no correct response
Which of the following general equations is a representation for a displacement reaction? a. X + Y -> XY b. XY -> X + Y c. AX + BY -> AY + BX d. no correct response
no correct response
Which of the following statements concerning the conduction of electricity by an aqueous solution is correct? a. All electrolytes produce strongly conducting solutions. b. All nonelectrolytes produce weakly conducting solutions. c. All soluble salts produce weakly conducting solutions. d. no correct response
no correct response
Which of the following types of radioactive emissions has a mass of 2 amu? a. alpha particle b. beta particle c. gamma radiation d. no correct response
no correct response
Consider the following system at equilibrium: 2SO2(g) + O2(g) <=> 2SO3(g) How will adding a catalyst shift the equilibrium?
no effect
C6H6(g) + 3H2(g) -> C6H12(g) + heat Indicate if the following will shift the equilibrium to the right or left. Also indicate if the changes will change the value of Keq. Adding a catalyst
no effect on equilibrium or Keq
C2H4 has...
no ions
H2O2 has...
no ions
gamma ray has ?
no mass [that's how is diff from alpha & beta]
A semipermeable membrane separates two aqueous solutions at 20 degrees Celsius. Name the solution into which a net flow of water (if any will occur). Assume 100% dissociation for electrolytes, meaning ion-pairing can be ignored. solution A: 0.10 M Al(NO3)3 (aq) solution B: 0.20 M NaNO3 (aq)
no net flow
A semipermeable membrane separates two aqueous solutions at 20 degrees Celsius. Name the solution into which a net flow of water (if any will occur). Assume 100% dissociation for electrolytes, meaning ion-pairing can be ignored. solution A: 0.10 M NaCl (aq) solution B: 0.10 M KBr (aq)
no net flow
A semipermeable membrane separates two aqueous solutions at 37 degrees Celsius. For the following case, name the solution into which a net flow of water (if any) will occur. solution A: 0.20 M KCl (aq) solution B: 0.20 M NaCl (aq)
no net flow
If the colligative concentrations on each side of the membrane are equal,
no net flow of water
A substance that does not produce ions when dissolved in water
nonelectrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte a substance that forms an aqueous solution that does not conduct electricity
nonelectrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte methanol, CH3OH
nonelectrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte most molecular solutes
nonelectrolyte
Classify the following substance & description as an electrolyte or nonelectrolyte table sugar
nonelectrolyte
Sucrose(s) -> sucrose(aq)
nonelectrolyte
Hydrocarbons are
nonpolar
Is CH4 polar or nonpolar?
nonpolar
Is N2 polar or nonpolar?
nonpolar
is CCl4 polar or nonpolar? Why?
nonpolar bc symmetrical
Classify each of the following reactions using one selection from the choices redox and nonredox combined with one selection from the choices combination, decomposition, displacement, exchange, and combustion NaCl + AgNO3 -> AgCl + NaNO3
nonredox & exchange
beta particle is!
not an electron bc coming out of nucleus
Molecular ([covalent]) solutes do
not break up to produce ions in solution.
What two factors determine whether a collision between two reactant molecules will result in a reaction?
total kinetic energy of colliding reactants; collision orientation
By definition, what happens to a substance when it is oxidized?
substance loses electrons [oxidation number increases]
reducing agent aka
substance oxidized
the reducing agent and
substance oxidized are always same
oxidizing agent aka
substance reduced
Tell me what a catalyst is
substance that increases chemical reaction rate without being consumed in chemical reaction.
The solute is the
substance that is dissolved
the conjugate base [of weak acid] that buffer contains is bc they need
substance to react w & remove added acid
the weak acid that buffers contain is bc they need
substance to react w & remove added base
What's an electrolyte?
substance whose aqueous solution conducts electricity
Identify the solute and the solvent in solutions composed of the following: 4.00 g of sucrose (table sugar) and 1000 g of water
sucrose solute; water solvent
H2SO4
sulfuric acid
Classify each of the following solutions as saturated, unsaturated, or supersaturated based on the following observations. Agitation of the solution produces a large amount of solid crystals.
supersaturated
If addition of a small crystal of NaCl to an NaCl solution causes additional crystals to form then the original solution was
supersaturated
Will red blood cells swell, remain the same size, or shrink when placed in 0.92%(m/v) glucose solution
swell
Will red blood cells swell, remain the same size, or shrink when placed in 2.3%(m/v) glucose solution
swell
When red blood cells are placed in pure water,
swell up & rupture [hemolysis]
What happens in hypotonic solution?
swells or burst
in a nuclear equation, the
symbols stand for nuclei rather than atoms
no lone pairs =
symmetrical [so can't be polar]
combination reaction aka
synthesis reaction
According to Le Chatelier, concentration
system will shift away from added component [If component is removed, opposite effect occurs]
Le Châtelier's principle states that if an equilibrium is disturbed
system will shift such that equilibrium is reestablished
"determine pH"
take negative log of hydrogen ion concentration
A solution with high osmotic pressure will
take up more water [more pressure must be applied to prevent osmosis]
The "most used" radionuclide in diagnostic medicine is
technetium-99m
You can't increase
temp in humans to make reactions go faster [so we use catalysts; enzymes in humans]
Contrast how factors such as temperature, pressure, and catalysts affect reaction rate for nuclear and chemical reactions.
temp, pressure & catalysts affect chemical reaction rates but do not affect nuclear reaction rates
in a chemical reaction, Reaction rates are influenced by
temp, pressure, catalysts & reactant concentrations.
Reaction rates in chemical reactions are
temperature dependent but those in nuclear reactions are not
Reactants high, products low
tend to stay to left
in a chemical reaction, Energy changes
that accompany chemical reactions are relatively small.
the smaller the pH value
the higher the concentration of hydrogen ions
In the notation carbon-14, the number 14 is
the mass number of the carbon atom
The oxidizing agent and
the substance reduced are always same
in a chemical reaction, Elements retain
their identity in chemical reactions.
If you dissolve base in water,
then water becomes the acid
The implantation of a radionuclide in living tissue is a common procedure in
therapeutic, but not diagnostic, medicine
3 protons per molecule transferred in an acid-base reaction
triprotic acid
H3PO4 would be an example of
triprotic acid
Indicate whether each of the following statements about the general properties of solutions is true or false. A solution may contain more than one solute.
true
Indicate whether each of the following statements about the general properties of solutions is true or false. All solutions are homogeneous mixtures.
true
Indicate whether each of the following statements about the general properties of solutions is true or false. every part of a solution has exactly the same properties as every other part.
true
Is the following statement concerning a saturated solution true or false? undissolved solute may or may not be present
true
Is the following statement concerning a saturated solution true or false? undissolved solute, if present, is in equilibrium with dissolved solvent
true
true or false: Solutes remain uniformly distributed throughout the solution.
true
true or false: Solutions can contain more than one solute
true
true or false: Solutions in which both solute and solvent are in the solid state are not possible.
true
true or false: at equilibrium, reactants are still being converted to products & vice versa
true
true or false: at equilibrium, the concentrations of reactants and products remain constant
true
true or false: at equilibrium, the rates of the forward & reverse reactions are equal
true
true or false: solutions are homogeneous mixtures.
true
true or false: solutions have a variable composition.
true
true or false: to determine whether a collision between 2 reactant molecules will result in a reaction, the particles must be in the correct orientation upon impact
true
true or false: to determine whether a collision between 2 reactant molecules will result in a reaction, the particles must collide with enough energy to meet the activation energy of the reaction
true
true or false? decreasing the temperature decreases the kinetic energy of the reactants, and the reaction goes more slowly
true
true or false? increasing the amount of reactants increases the number of collisions & the reaction goes fastser
true
true or false? reactants must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur
true
true or false? the energy of a collision between atoms or molecules must be greater than or equal to the activation energy for bonds to be broken
true
in diagnostic!!
trying to figure out what's wrong
the effect of 1 mole of NaCl on colligative properties will be twice that of 1 mole of glucose bc
twice as many particles are present even tho molar amounts of solute are same
solutes are the substances that
undergo reaction when solutions are mixed [active]
Write equilibrium constant expressions for the following reactions. AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
[NaNO3]/[AgNO3][NaCl]
Write equilibrium constant expressions for the following generalized reactions. 2X(s) + 3Y(s) -> 2Z(g)
[Z]^2
Write equilibrium constant expressions for the following generalized reactions. 2X(g) + 3Y(s) -> 2Z(g)
[Z]^2/[X]^2
Write equilibrium constant expressions for the following generalized reactions. 2X(g) + 3Y(g) -> 2Z(g)
[Z]^2/[X]^2 [Y]^3
Which of the following acids contains the greatest number of acidic hydrogen atoms? a. H2SO4 b. HC3H3O3 c. HC3H5O3 d. no correct response
a
Which of the following is not a polyprotic acid? a. HCN b. H3PO4 c. H2SO4 d. no correct response
a
What does it mean to say the percent concentration is 15%(m/m) NaCl solution
there are 15g of NaCl in 100g of solution
What does it mean to say the percent concentration is 25%(m/v) sucrose solution
there are 25g of sucrose in 100 mL of solution
What does it mean to say the percent concentration is 6%(v/v) methanol solution
there are 6 mL of methanol in 100 mL of solution
If there's an acid,
there's a base [bc need base to accept proton]
Most molecular solutes do not produce ions or charged particles when dissolved in water
therefore don't allow solution to conduct electricity
How do the radionuclides used for therapeutic purposes differ from the radionuclides used for diagnostic purposes?
they are usually a or b emitters
"of"
they go together on one side
Solute is the
thing you're dissolving
Pressure has a major effect on the solubility of gases in water?
think of a can of soda
Arrhenius bases are produced
through process of dissociation
Identify the solute in: bronze (an alloy of 95% copper and 5% tin)
tin
a good buffer has
to be able to absorb acids & bases so pH doesn't change
Nonmetals tend
to gain electrons
The formula for lactic acid is preferably written as hC3h5O3 rather than as C3h6O3. explain why.
to show it is monoprotic acid
Identify which substance is oxidized and which substance is reduced in each of the following redox reactions. N2 +3H2 -> 2NH3
H2 oxidized; N2 reduced
What substances are present in the following reaction mixture when equilibrium has been obtained? 3H2 + N2 <=> 2NH3
H2, N2, NH3
Give the conjugate acid for the base below: HCO3^-
H2CO3
Identify the Bronsted-Lowry acid in the following reaction H2O + H2CO3 -> H3O^+ + HCO3^-
H2CO3
Which of the following is a Bronsted Lowy acid? H2CO3 Cl - NH3 OH -
H2CO3
A sample of 56.0 g NaBr is added to 500.0 mL of H2O. Which component represents the solvent?
H2O
Example of amphiprotic substance
H2O
Identify the Bronsted-Lowry base in the following reaction H2O + H2CO3 -> H3O^+ + HCO3^-
H2O
Which substance is reduced in the following redox reaction? CO+H2O -> CO2 +H2
H2O
in NH3 + H2O -> NH4 + OH^- what is the acid?
H2O
Which of the following is the strongest acid? a) HX,Ka = 1.0 × 10^−3 b) HY,Ka =1.0 × 10^−5 c) HZ,Ka =1.0 × 10^−7 d) all have the same strength
a
Thus a 5% NaCl solution is assumed to be
a 5%(m/m) NaCl solution.
reduction involves
a decrease in oxidation number.
What is a solution?
a homogeneous mixture
Consider the following system at equilibrium: 2SO2(g) + O2(g) <=> 2SO3(g) How will increasing the concentration of SO3 shift the equilibrium?
to the left
Consider the following system at equilibrium: 2SO2(g) + O2(g) <=> 2SO3(g) How will increasing the concentration of SO2 shift the equilibrium?
to the right
The proper assignment of oxidation numbers to the elements in the compound H2SO4 is
+1 for h, +6 for S, −2 for O
Determine the oxidation number of the indicated ele- ment in each of the following ions. N in NO3^-
+5
Determine the oxidation number of the indicated ele- ment in each of the following ions. P in PO4^3-
+5
The proper assignment of oxidation numbers to the elements in the polyatomic ion PO4^3− is
+5 for P, −2 for O
What is the oxidation number of S in each of the following molecules? SO3
+6
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? 2000 g (2.000 kg)
-0.93 degrees celsius
What is the freezing point for a solution containing 1.00 mole of glucose (a nondissociating solute) dissolved in 1.00 kg water?
-1.86 degrees celsius
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? 1000 g (1.000 kg)
-1.9 degrees celsius
What is the freezing point of the solution 3.00 moles of NaCl (an ionic compound)
-11.16 degrees celsius
What is the freezing point of an aqueous solution that contains 3.00 moles of the ionic solute CaCl2 (a deicing compound) per one kilogram of water?
-16.7 degrees celsius
Determine the oxidation number of the indicated ele- ment in each of the following ions. S in S^2-
-2
What is the oxidation number of S in each of the following molecules? H2S
-2
What is the freezing point of the solution 3.00 moles of Na3PO4 (an ionic compound)
-22.32 degrees celsius
Which member of each of the following pairs of compounds has the higher boiling point? 1.0 M NaCl or 1.0 M Na2SO4
1.0 M Na2SO4
Which member of each of the following pairs of compounds has the higher boiling point? 2.0 M glucose or 1.0 M Na2SO4
1.0 M Na2SO4
Which member of each of the following pairs of compounds has the higher boiling point? 1.0 M glucose or 1.0 M NaCl
1.0 M NaCl
If pH = 4.00 then [H3O+] =
1.0 x 10^-4
The percent-by-mass concentration of a solution containing 5.0 g of NaCl in 500.0 g of solution is
1.0% (m/m)
A 0.200 M solution of NaCl which contains 0.200 mole of NaCl would have a volume of
1.00 L
[H3O^+] [OH^-] =
1.00 x 10^-14
Determine the pH of the following solutions: 1.0 × 10^-4 M OH^-
1.00 x 10^1
What is the [OH−] in an aqueous solution in which [H3O+] is 1.00 × 10^−5?
1.00 × 10^−9
A solution of hydrogen peroxide (H2O2) in water with a volume of 70.0 mL is diluted by adding 50.0 mL of water. Calculate the solution's new concentration given the following original concentrations. (Addition of 50.0 mL of water is equivalent to adding 50.0 g of water since the density of water is 1.00 g/mL.) 2.0 M
1.17 M
A solution of hydrogen peroxide (H2O2) in water with a volume of 70.0 mL is diluted by adding 50.0 mL of water. Calculate the solution's new concentration given the following original concentrations. (Addition of 50.0 mL of water is equivalent to adding 50.0 g of water since the density of water is 1.00 g/mL.) 2.0%(m/m)
1.17% (m/m)
A solution of hydrogen peroxide (H2O2) in water with a volume of 70.0 mL is diluted by adding 50.0 mL of water. Calculate the solution's new concentration given the following original concentrations. (Addition of 50.0 mL of water is equivalent to adding 50.0 g of water since the density of water is 1.00 g/mL.) 2.0%(m/v)
1.17% (m/v)
A solution of hydrogen peroxide (H2O2) in water with a volume of 70.0 mL is diluted by adding 50.0 mL of water. Calculate the solution's new concentration given the following original concentrations. (Addition of 50.0 mL of water is equivalent to adding 50.0 g of water since the density of water is 1.00 g/mL.) 2.0%(v/v)
1.17% (v/v)
Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 563 g of NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution
1.41 x 10^1 M
Determine the final concentration of each of the following solutions after 20.0 mL of water has been added. 60.0 mL of 2.0 M NaCl solution
1.5 M
What is the osmolarity of each of the following solutions? 2.0 M KNO3
4.0 OsM
The [H3O+] concentration of a solution is 2.5 x 10^-4 Calculate the [OH^-]
4.0 x 10^-11
The [H3O+] concentration of a solution is 2.5 x 10^-9 Calculate the [OH^-]
4.0 x 10^-6
Calculate the pH for the following solutions. 1.0 x 10^-4 M H3O^+
4.00
Calculate the volume percent of solute in each of the following solutions. 20.0 mL of methyl alcohol in enough water to give 475 mL of solution
4.21% (v/v)
Determine the pKa for acetic acid, hC2h3O2, given that Ka for this acid is 1.8 × 10^-5.
4.74
Calculate the value of the equilibrium constant for the reaction N2O4(g) <=> 2NO2(g) if the concentrations of the species at equilibrium are [N2O4] = 0.213 and [NO2] = 0.0032
4.8 x 10^-5
The pKa for an acid whose Ka is 1.0 × 10^−5 is
5.0
Calculate the pH for the following solutions. 3.2 x 10^-6 M H3O^+
5.49
Calculate the molarity of 0.850 mol of Na2S in 1.50 L of solution
5.67 x 10^-1 M
Determine the molarities of the following solutions. 4.35 moles of KMnO4 are dissolved in enough water to give 750 mL of solution.
5.80 moles KMnO4/L solution
What is the osmolarity of each of the following solutions? 2.0 M Na2SO4
6.0 OsM
What is the osmolarity of each of the following solutions? 2.0 M in both KNO3 and glucose
6.0 OsM
A solution is 0.0030 M in hpO42− ion. What is this ion concentration in meq/L?
6.0 mEq/L
Which of the following solutions is hypertonic with respect to red blood cells? a. 2.0%(m/v) glucose b. 4.0%(m/v) glucose c. 6.0%(m/v) glucose d. no correct response
6.0%(m/v) glucose
Calculate the ph for each of the following solutions. [H3O+] = 1.0 × 10^−6
6.00
The ph for a solution with [h3O+] = 1.0 × 10^−6 is
6.00
Calculate the mass percent of solute in the following solutions. 2.31 g of LiBr dissolved in 35.0 g of H2O
6.19% (m/m)
What is the percent-by-mass concentration of glucose in a solution made my dissolving 5.5 g of glucose in 78.2 g of water?
6.6%
Calculate the molarity of 30.3 g of MgS in 787 mL of solution
6.82 x 10^-1 M
Indicate whether or not each of the following changes would affect the value of a system's equilibrium constant. a. removal of a reactant from the equilibrium mixture b. Decrease in the system's total pressure c. Decrease in the system's temperature d. Addition of a catalyst to the equilibrium mixture
A) no b) no c) yes d) no
Which of the following statements concerning electrolytes is correct? a. All strong acids are strong electrolytes. b. All salts are weak electrolytes. c. Some, but not all, molecular substances are strong electrolytes. d. no correct response
All strong acids are strong electrolytes
vapor-pressure lowering
Adding a nonvolatile solute to solvent lowers vapor pressure of resulting solution below that of pure solvent at same temp
Boiling point elevation
Adding a nonvolatile solute to solvent raises boiling point of resulting solution above that of pure solvent.
Cu(s) + 2AgNO3(aq) -> 2Ag(s) + Cu(NO3)2(aq) What is the oxidizing agent?
Ag^+
Cu(s) + 2AgNO3(aq) -> 2Ag(s) + Cu(NO3)2(aq) Which substance gets reduced?
Ag^+
Which of the following will have the largest effect on freezing point depression or boiling point elevation •NaCl •C2H4 •AlCl3 •H2O2
AlCl3
Equilibrium says
All reactions are reversible in theory [can go in either direction]
Write the chemical formulas for the products formed when each of the following hydrocarbons undergoes complete combustion. C6H6
CO2, H2O
Write the chemical formulas for the products formed when each of the following hydrocarbons undergoes complete combustion. CH4
CO2, H2O
Dilution formula
CSVS = CDVD
Ca -> Ca^2+
Ca loses 2 electrons [Ca is oxidized = reducing agent]
What is the missing reactant in the following decomposition reaction? ? -> CaO(s) + CO2(g)
CaCO3
CaCl2 ->
Ca^2+ + 2Cl^−
For the following reactions, indicate which substance is oxidized and which substance is reduced. Identify the oxidizing and reducing agents. Cl2 (g) + 2NaBr (aq) -> Br2 (aq) + 2NaCl (aq)
Br is oxidized [reducing agent] and Cl is reduced [oxidizing agent]
Cl2 (g) + 2NaBr (aq) -> Br2 (aq) + 2NaCl (aq) What is happening to Br and Cl here?
Br loses 1 electron; Cl gains 1 electron
Write the conjugate base of each of the following: HBr
Br^-
A proton donor
Bronsted-Lowry acid
A proton acceptor
Bronsted-Lowry base
What are the major species in solution after the reaction of hydrochloric acid and sodium hydroxide (hydrochloric acid has H+ and Cl^-) (sodium hydroxide has Na^+ and OH^-)
H2O, Na^+ and Cl^-
Label each reactant and product in this reaction as a Bronsted acid or base CH3OH + OH^- <=> CH3O^- + H2O
CH3OH [acid], OH^- [base], CH3O^- [base], H2O [acid]
For the redox reaction FeO+CO -> Fe+CO2 identify the: reducing agent
CO
For the redox reaction FeO+CO -> Fe+CO2 identify the: substance oxidized
CO
2CO(g) + O2(g) <=> 2CO2(g) if you decrease the volume of the system, how will the concentration then change to reach equilibrium?
CO goes down, O2 goes down, CO2 goes up
2CO(g) + O2(g) <=> 2CO2(g) if you increase the concentration of CO, how will the concentration then change to reach equilibrium?
CO goes down, O2 goes down, CO2 goes up
2CO(g) + O2(g) <=> 2CO2(g) if you increase the concentration of CO2, how will the concentration then change to reach equilibrium?
CO goes up, O2 goes up, CO2 goes down
Identify the solute in: CO2(g) in water
CO2
Write the chemical formulas for the products formed when each of the following hydrocarbons undergoes complete combustion. C4H10
CO2, H2O
Write the chemical formulas for the products formed when each of the following hydrocarbons undergoes complete combustion. C4H6
CO2, H2O
Cl2 -> 2Cl^-
Cl2 gains 2 electrons [Cl2 is reduced = oxidizing agent]
Identify which substance is the oxidizing agent and which substance is the reducing agent in each of the redox reactions Cl2 + 2KI -> 2KCl + I2
Cl2 oxidizing agent; KI reducing agent
Fe(s) + Cu^2+(aq) -> Fe^2+(aq) + Cu(s) Which substance gets reduced?
Cu^2+
For the triprotic acid h3pO4, the reactant in the second proton-transfer step is
H2PO4^-
Identify which substance is oxidized and which substance is reduced in each of the following redox reactions. 3H2SO3 + 2HNO3 -> 2NO + H2O + 3H2SO4
H2SO3 oxidized; HNO3 reduced
Which of the following effects will occur if the temperature of the following equilibrium system is increased? H2(g) + F2(g) -> 2HF(g) + heat a. the equilibrium shifts to the right b. hF concentration increases c. h2 and F2 concentrations increase d. no correct response
H2 and F2 concentrations increase
CO(g) + 2H2(g) <- ——> CH3OH(g) if CO increases
H2 decreases & CH3OH increases [but Keq stays constant]
HC2H3O2/C2H3O2^- common lab buffer [acetic acid/sodium acetate buffer]
Equal amounts of acetic acid [weak acid] & its weak conjugate base [acetate ion]
If reactants are high & Keq is small [< 10 - 3]
Equilibrium lies to left (not much product)
If products are high and Keq is large [larger than 103]
Equilibrium lies to right (lots of product)
ADDING REACTANT
Equilibrium shifts to product side
REMOVING PRODUCT
Equilibrium shifts to product side
INCREASING TEMPERATURE in an endothermic reaction
Equilibrium shifts to product side for an endothermic reaction
DECREASING TEMPERATURE in an exothermic reaction
Equilibrium shifts to product side for exothermic reaction
ADDING PRODUCT
Equilibrium shifts to reactant side
REMOVING REACTANT
Equilibrium shifts to reactant side
DECREASING TEMPERATURE in an endothermic reaction
Equilibrium shifts to reactant side for endothermic reaction
INCREASING TEMPERATURE in an exothermic reaction
Equilibrium shifts to reactant side for exothermic reaction
INCREASING PRESSURE
Equilibrium shifts to side that has fewest moles of gas
DECREASING PRESSURE
Equilibrium shifts to side that has greatest moles of gas
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) what is the conjugate base?
F^-
For the redox reaction FeO+CO -> Fe+CO2 identify the: substance reduced
FeO
Label each reactant and product in this reaction as a Bronsted acid or base H2Y^- + H2Z <=> H3Y + HZ^2-
H2Y^- [base], H2Z^- [acid], H3Y [acid], HZ^2- [base]
H2O is the conjugate base of
H3O^+
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) what is the conjugate acid?
H3O^+
HF + H2O <=> H3O^+ + F^- if you put OH in
H3O^+ goes down
Which acid in the choices below is an example of a triprotic acid? H3PO4 HCl HC2H3O2 H2SO4
H3PO4
Which of the following is a weak acid? HCN HCl HI HNO3
HCN
Write an equation for each of the following buffering actions. The response of HCN/CN− buffer to the addition of OH− ions
HCN + OH^- -> CN^- + H2O
Label each reactant and product in this reaction as a Bronsted acid or base HCN + NH2^- <=> CN^- + NH3
HCN [acid], NH2^- [base], CN^- [base], NH3 [acid]
Give the conjugate acid for the base below: CO3^2-
HCO3^-
Write the conjugate base of each of the following: H2CO3
HCO3^-
What is the acid in HCl + H2O → Cl^- + H3O^+
HCl
HCl + H2O -> H3O^+ + Cl
HCl + H2O is dissolving acid in water
The chemical formula for the conjugate acid of ClO^− is
HClO
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) what is the acid?
HF
Identify the Bronsted-Lowry acid in the following reaction HF + H2O -> H3O^+ + F^-
HF
Which of the following pairs is a buffer. HF and F - HCl and NaCl H2SO4 and Na2SO4 NH3 and NH4+
HF and F^-
Which pair of molecules will mix together to form a homogeneous solution? Hydrogen fluoride (HF) and water (H2O) Pentane (C5H12) and methanol (CH3OH) Benzene (C6H6) and water (H2O) Formaldehyde (CH2O) and hexane (C6H14)
HF and H2O
HF + H2O how do you know which is acid and which is base?
HF can only be acid; H2O can be either
Write the conjugate acid of each of the following: NO2^-
HNO2
For the buffer system hNO2/NO2−, do the concentra- tions of hNO2 and NO2− increase or decrease when a small amount of strong acid is added to the buffer?
HNO2 increases & NO2^- decreases
Write the chemical formula of each of the following. The conjugate acid of NO3^−
HNO3
Write the conjugate base of each of the following: H2S
HS^-
What is happening when you go from: F^- to HF
H^+ gain
What is happening when you go from: H2O to H3O^+
H^+ gain
In an Arrhenius acid-base theory context, the acidic species in an aqueous solution is the
H^+ ion
What is happening when you go from: H3O^+ to H2O
H^+ loss
What is happening when you go from: HF to F^-
H^+ loss
What is the acid ionization constant of: HA(aq) + H2O(l) ⇔ H3O+(aq) + A-(aq)
Ka = [H3O^+] [A^-]/[HA]
If [Products] is high then
Keq will be large >103
If [Reactants] is high then
Keq will be small < 10 - 3
In neutral, acidic, or basic solutions,
Kw is always 1.0 x 10^-14
In all three possible situations [neutral, acidic or basic]
Kw= 1.00 x 10^-14 = [H3O^+] x [OH^-]
M1 x V1=
M2 x V2
Write the chemical formula of each of the following. The conjugate base of HSO4^−
SO4^2-
Identify which substance is the oxidizing agent and which substance is the reducing agent in each of the redox reactions Sb2O3 + 3Fe -> 2Sb + 3FeO
Sb2O3 oxidizing agent; Fe reducing agent
Identify which substance is oxidized and which substance is reduced in each of the following redox reactions. Sb2O3 + 3Fe -> 2Sb + 3FeO
Sb2O3 reduced; Fe oxidized
Mg(s) + Cl2(g) -> Mg^2+(aq) + 2Cl^-(aq) Which substance gets oxidized?
Mg
Why is the following reaction a displacement reaction? Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
Mg displaces H
2 Mg (s) + CO2(g) -> 2 MgO (s) + C (s) You can also see this as
Mg gains oxygen [oxidized] and carbon loses oxygen [reduced]
For the following reaction, indicate which substance is oxidized and which substance is reduced. Identify the oxidizing and reducing agents. 2 Mg (s) + CO2(g) -> 2 MgO (s) + C (s)
Mg is oxidized [reducing agent] and C is reduced [oxidizing agent]
2 Mg (s) + CO2(g) -> 2 MgO (s) + C (s) What is happening to Mg and C here?
Mg loses 2 electrons; C gains 4 electrons
Activation energy is like
Minimum combined kinetic energy that colliding reactant particles must possess for their collision to result in chemical reaction
Identify the solvent in: air (a solution of 78% N2, 21% O2 and various other gases)
N2
Identify which substance is the oxidizing agent and which substance is the reducing agent in each of the redox reactions N2 +3H2 -> 2NH3
N2 oxidizing agent; H2 reducing agent
Consider the following equilibrium system. N2(g) + O2(g) <=> 2NO(g) Write the chemical equation for the forward reaction.
N2(g) + O2(g) -> 2NO(g)
For the chemical reaction N3^− + H2O -> HN3 + OH^−, the Brønsted-Lowry base is
N3^-
Give the conjugate base for the acid below: NH4^+
NH3
What is the base in H2O + NH3 → OH^- + NH4^+
NH3
in NH3 + H2O -> NH4 + OH^- what is the base?
NH3
Give the conjugate acid for the base below: NH3
NH4^+
Write the conjugate acid of each of the following: NH3
NH4^+
in NH3 + H2O -> NH4 + OH^- what is the conjugate acid?
NH4^+
Consider the reaction below. HNO3 + H2O <----> H3O+ + NO3- Which substance is the conjugate base of HNO3?
NO3^-
At a given temperature, which of the two aqueous solutions 1.0 M glucose or 1.0 M NaCl has the higher boiling point
NaCl
At a given temperature, which of the two aqueous solutions 1.0 M glucose or 1.0 M NaCl has the higher osmotic pressure
NaCl
Which of the following aqueous solutions would give rise to a greater osmotic pressure? 8.00 g of NaCl in 375 mL of solution or 4.00 g of NaBr in 155 mL of solution
NaCl
In which of the following pairs of compounds are both members of the pair strong electrolytes? a. NaOh and NaCl b. Nh3 and hCl c. NaCN and hCN d. no correct response
NaOH and NaCl
What is the base and what is the acid? NaOH + HCl -> H2O + NaCl
NaOH is base; HCl is acid
NaCl ->
Na^+ + Cl^-
in self-ionization,
Net effect is formation of equal amounts of hydronium & hydroxide ions
3Ni^2+(aq) + 2Co(s) -> 2Co^3+(aq) + 3Ni(s) Which substance gets reduced?
Ni^2+
for acid ionization constant
Notice water does not appear in equilibrium expression [pure substance]
in NH3 + H2O -> NH4 + OH^- what is the conjugate base?
OH^-
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. Carbon dioxide gas in water with P = 2 atm and T = 50°C Carbon dioxide gas in water with P = 1 atm and T = 50°C
P =2
Give the conjugate base for the acid below: HPO4^2-
PO4^3-
beta particle
Particle whose charge & mass are identical to those of electron that is emitted by certain radioactive nuclei.
Molecular Collisions [collision theory]
Particles have to collide in order to react.
Activation Energy [collision theory]
Particles have to have enough energy to react
Collision Orientation [collision theory]
Particles have to have right orientation in order to react
Keq is Concentration of products divided by concentration of reactants
Raised to power of coefficient from balanced equation
How does temperature affect chemical reaction rate?
Reaction rate increases as temp of reactants increase
Collision orientation is like
Reaction rates are sometimes very slow bc reactant molecules must be orientated in certain way for collisions to lead successfully to products
Gamma radiation effects can
Readily penetrate deeply into organs, bone & tissue
For the following reactions, indicate which substance is oxidized and which substance is reduced. Identify the oxidizing and reducing agents. S (s) + O2 (g) → SO2 (g)
S is oxidized [reducing agent] and oxygen must be reduced in this reaction
Give the formula of the conjugate base of HSO4^-
SO4^2-
Write equations for the following nuclear bombardment processes. a. Beryllium-9 is bombarded with an alpha particle, and a neutron is a product. b. Sodium-23 is bombarded with hydrogen-2, and neon-21 is a product. c. Bombardment of cadmium-113 with a small particle produces cadmium-114 and a gamma ray. d. Bombardment of a nuclide with an alpha particle produces phosphorus-30 and a neutron.
a) 9Be4 + 4a2 -> 1N0 + 12C6 b) 23Na11 + 2H1 -> 21Ne10 + 4a2 c) 113Cd48 + 1N0 -> 114Cd48 + 0Y0 d) 27Al13 + 4a2 -> 30P15 + 1N0
Classify each of the following as a property of an Arrhenius acid or the property of an Arrhenius base. a. has a sour taste b. has a bitter taste
a) Arrhenius acid b) Arrhenius base
Write a balanced equation for the dissociation into ions of each of the following soluble salts in aqueous solution. a. Ba(NO3)2 b. Na2SO4 c. CaBr2 d. K2CO3
a) Ba(NO3)2 -> Ba^2+ + 2NO3^- b) Na2SO4 -> 2Na^+ + SO4^2- c) CaBr2 -> Ca^2+ + 2Br^- d) K2CO3 -> 2K^+ + CO3^2-
Write chemical equations showing the individual proton- transfer steps that occur in aqueous solution for each of the following acids. a. h2CO3 (carbonic acid) b. h2C3h2O4 (malonic acid)
a) H2CO3 + H2O -> HCO3^- + H3O^+; HCO3^- + H2O -> CO3^2- + H3O^+ b) H2C3H2O4 + H2O -> HC3H2O4^- + H3O^+; HC3H2O4^- + H2O -> C3H2O4^2- + H3O^+
Write a balanced molecular equation for the preparation of each of the following salts, using an acid-base neutralization reaction. a. Li2SO4 (lithium sulfate) b. NaCl (sodium chloride) c. KNO3 (potassium nitrate) d. Ba3(pO4)2 (barium phosphate)
a) H2SO4 + 2LiOH -> Li2SO4 + 2H2O (b) HCl + NaOH -> NaCl + H2O (c) HNO3 + KOH -> KNO3 + H2O d) 2H3PO4 + 3Ba(OH)2 -> Ba3(PO4)2 + 6H2O
Using the acid ionization constant information given in Table 10-3, indicate which acid is the stronger in each of the following acid pairs. a. h3pO4 and hNO2 b. hCN and hF c. h2CO3 and hCO3− d. hNO2 and hCN
a) H3PO4 b) HF c) H2CO3 d) HNO2
Identify the two "active species" in each of the following buffer systems. a. hCN and KCN b. h3pO4 and Nah2pO4 c. h2CO3 and KhCO3 d. NahCO3 and K2CO3
a) HCN and CN^- b) H3PO4 and H2PO4^- c) H2CO3 and HCO3^- d) HCO3^- and CO3^2-
Identify the buffer system(s)--the conjugate acid-base pair(s)--present in a solution that contains equal molar amounts of the following: a. hCN, KCN, hClO, and NaClO2 b. h2CO3, Na2CO3, NaNO2, and hNO2
a) HCN/CN^- b) HNO2/NO2^-
The ion hCO3− is an amphiprotic ion. Write the chemi- cal equation to describe its behavior in aqueous solution when it functions as a a. Brønsted-Lowry base b. Brønsted-Lowry acid
a) HCO3^- + H2O -> H2CO3 + OH^- b) HCO3^- + H2O -> CO3^2- + H3O^+
Write a balanced chemical equation to represent each of the following acid-base neutralization reactions. a. hCl and NaOh b. hNO3 and KOh c. h2SO4 and LiOh d. Ba(Oh)2 and h3pO4
a) HCl + NaOH -> NaCl + H2O b) HNO3 + KOH -> KNO3 + H2O c) H2SO4 + 2LiOH -> Li2SO4 + 2H2O d) 2H3PO4 + 3Ba(OH)2 -> Ba3(PO4)2 + 6H2O
Write equations depicting the behavior of the following Arrhenius acids and bases in water. a. hI (hydroiodic acid) b. hClO (hypochlorous acid) c. LiOh (lithium hydroxide) d. CsOh (cesium hydroxide)
a) HI -> H^+ + I^- b) HClO -> H^+ + ClO^- c) LiOH -> Li^+ + OH^- d) CsOH -> Cs^+ + OH^-
Write chemical equations that show the indicated behavior in aqueous solution for each of the following chemical species. a) HOCl behaves as a Brønsted-Lowry acid b) NH3 behaves as a Brønsted-Lowry base c) H2PO4^− behaves as a Brønsted-Lowry acid d) CO3^2− behaves as a Brønsted-Lowry base
a) HOCl + H2O -> OCl^- + H3O^+ b) NH3 + H2O -> NH4^+ + OH^- c) H2PO4^- + H2O -> HPO4^2- + H3O^+ d) CO3^2- + H2O -> HCO3^- + OH^-
Which of the four species Cl−, hpO42−, CO32−, and h2SO3 have the following properties? a. amphiprotic b. does not hydrolyze in water c. hydrolyzes in water to give a basic solution d. can function as a buffer system component
a) HPO4^2- b) Cl^- c) HPO4^2-, CO3^2- d) HPO4^2-, CO3^2-, H2SO3
Write the formula of each of the following. a. conjugate base of h2SO3 b. conjugate acid of CN− c. conjugate base of hC2O4^− d. conjugate acid of hpO4^2−
a) HSO3^- b) HCN c) C2O4^2- d) H2PO4^-
In Arrhenius acid-base theory, what ion is responsible for the properties of a. acidic solutions b. basic solutions
a) H^+ b) OH^-
Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. hF (hydrofluoric acid) b. hC2h3O2 (acetic acid)
a) Ka= [H^+][F^-]/[HF] b) Ka = [H^+][C2H3O2^-]/[HC2H3O2]
Write a balanced chemical equation for the dissociation in water of each of the salts listed in a) NaCl b) Mg(NO3)2 c) K2S d) NH4CN
a) NaCl -> Na^+ + Cl^- b) Mg(NO3)2 -> Mg^2+ + 2NO3^- c) K2S -> 2K^+ + S^2- d) NH4CN -> NH4^+ + CN^-
What is the oxidation number of each element present in the following compounds or ions? a) SiF4 b) H2SO4 c) Na3PO4 d) Cr2O7^2−
a) Si: +4, F: -1 b) H: +1, S: -6, O: -2 c) Na: +1, P: +5, O: -2 d) Cr: +6, O: -2
Is the monoprotic acid Y or the monoprotic acid Z the stronger acid in each of the following situations? a. At equal concentrations, Y dissociates to a greater extent than Z in water. b. Ka for Z is larger than Ka for Y. c. The equilibrium position for the dissociation of Y lies farther to the right than that for Z. d. proton transfer to water occurs to a lesser extent for Z than for Y.
a) Y b) Z c) Y d) Y
Write the base ionization constant expression for the ionization of each of the following bases. In each case, the nitrogen atom accepts the proton. a. NH3 (ammonia) b. C6H5NH2 (aniline)
a) [NH4^+][OH^-]/[NH3] b) [C6H5NH3^+][OH^-]/[C6H5NH2]
Indicate whether the first listed reactant in each of the following Brønsted-Lowry acid-base reactions is func- tioning as an acid or a base. a) HF + H2O -> H3O^+ +F^− b) CN^− + H2O -> HCN + OH^− c) HCN + NO2^− -> HNO2 + CN^− d) NH3 + HNO3 -> NH4^+ + NO3^−
a) acid b) base c) acid d) base
Classify each of the following substances as an acid, a base, or a salt. a. hBr b. NaI c. Nh4NO3 d. Ba(Oh)2
a) acid b) salt c) salt d) base
Consider the following chemical system at equilibrium. CO(g) + H2O(g) + heat <=> CO2(g) + H2(g) For each of the following adjustments of conditions, indicate the effect (shifts left, shifts right, or no effect) on the position of equilibrium. a. refrigerating the equilibrium mixture b. Adding a catalyst to the equilibrium mixture c. Adding CO to the equilibrium mixture d. Increasing the size of the reaction container
a) left b) no effect c) right d) no effect
Classify each of the following acids as monoprotic, diprotic, or triprotic. a. hClO3 (chloric acid) b. hC3h5O4 (glyceric acid) c. h3C6h5O7 (citric acid) d. h3pO4 (phosphoric acid)
a) monoprotic b) monoprotic c) triprotic d) triprotic
predict whether each of the following pairs of substances could function as a buffer system in aqueous solution. a) hCl and NaCl b) hCN and KCN c) hCl and hCN d) NaCN and KCN
a) no b) yes c) no d) no
predict whether each of the following pairs of substances could function as a buffer system in aqueous solution. a. hNO3 and NaNO3 b. hF and NaF c. KCl and KCN d. h2CO3 and NahCO3
a) no b) yes c) no d) yes
Indicate whether each of the following reactions is an acid-base neutralization reaction. a. NaCl+AgNO3 -> AgCl+NaNO3 b. hNO3 + NaOh -> NaNO3 + h2O c. hBr+KOh -> KBr+h2O d. h2SO4 + pb(NO3)2 -> pbSO4 + 2hNO3
a) no b) yes c)yes d) no
What would be the expected effect of each of the following short-term, whole-body radiation exposures? a. 10 rems b. 150 rems
a) no detectable effects b) nausea, fatigue, lowered blood cell count
In each of the following changes is the reactant undergoing oxidation or reduction? (The given equation for the change is not a complete chemical equation.) a) SO2 -> SO3 b) N2O -> NO c) Cr^3+ -> Cr^2+ d) S2− -> S
a) oxidation b) oxidation c) reduction d) oxidation
Should heat be added as a reactant or as a product to each of the following equations for chemical reactions based on the given thermicity for the reaction? a. H2 + Cl2 -> 2HCl (exothermic) b. 4NO + 6H2O -> 4NH3 + 5O2 (endothermic) c. 2H2O + 2Cl2 -> 4HCl + O2 (endothermic) d. 2H2O -> 2H2 + O2 (exothermic)
a) product b) reactant c) reactant d) product
Classify each of the following reactions as a redox reac- tion or a nonredox reaction. a) 2Cu + O2 -> 2CuO b) K2O + H2O -> 2KOH c) 2KClO3 -> 2KCl + 3O2 d) CH4 +2O2 -> CO2 +2H2O
a) redox b) nonredox c) redox d) redox
Classify each of the acids as a strong acid or a weak acid. a. hClO3 (chloric acid) b. hC3h5O4 (glyceric acid) c. h3C6h5O7 (citric acid) d. h3pO4 (phosphoric acid)
a) strong acid b) weak acid c) weak acid d) weak acid
For each of the following pairs of acids, indicate whether the first member of the pair is a stronger or weaker acid than the second member of the pair. a. hNO3 and hNO2 b. hF and hBr c. h2CO3 and hClO3 d. hCN and hCl
a) stronger b) weaker c) weaker d) weaker
Classify each of the following compounds as a strong electrolyte or a weak electrolyte. a. h2CO3 b. KOh c. NaCl d. h2SO4
a) weak b) strong c) strong d) strong
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. h3pO4 b. h3pO3 c. hBr d. hC2h3O2
a) weak, triprotic b) weak, triprotic c) strong, monoprotic d) weak, monoprotic
Indicate whether or not both members of each of the following pairs of substances are salts. a. KCN and NaCN b. hCl and LiCl c. Na2SO4 and NaOh d. Al(NO3)3 and Ca(NO3)2
a) yes b) no c) no d) yes
For each of the following pairings of nuclear notations indicate whether the two members of the pair denote the same nuclide? a. nitrogen-14 and 14N7 b. Al-27 and 28Al 13 c. chlorine-35 and Cl-35 d. O-18 and (18 protons + 18 neutrons)
a) yes b) no c) yes d) no
Based on charge-balance considerations, indicate whether it would be possible to prepare solutions with each of the following total compositions. a. 75 meq Na+, 25 meq K+, 95 meq Cl−, and 5 meq NO3− b. 73 eq K+, 55 eq Cl−, and 25 eq C2h3O2− c. 750 meq Na+ and 0.750 eq Cl− d. 0.025 mole Na+, 0.025 mole Ca2+ and 0.075 mole Cl−
a) yes b) no c) yes d) yes
Indicate whether or not the two members of each of the following pairs of substances constitute a conjugate acid-base pair. a. HCl and Cl− b. Nh4+ and Nh3 c. h2CO3 and CO3^2- d. h2pO4^− and hpO4^2−
a) yes b) yes c) no d) yes
For each of the following pairings of acid and base indicate whether both the acid and the base are classified as strong? a. h2SO4 and KOh b. hCl and NaOh c. hClO4 and Sr(Oh)2 d. hF and Ba(Oh)2
a) yes b) yes c) yes d) no
Write an equation for each of the following buffering actions. a. the response of a hF/F− buffer to the addition of h3O+ ions b. the response of a h2CO3/hCO3− buffer to the addition of Oh− ions c. the response of a hCO3−/CO32− buffer to the addition of h3O+ ions d. the response of a h3pO4/h2pO4− buffer to the addition of Oh− ions
a)F^- + H3O^+ -> HF + H2O b) H2CO3 + OH^- -> HCO3^- + H2O c) CO3^2- + H3O^+ -> HCO3^- + H2O d) H3PO4 + OH^- -> H2PO4^- + H2O
The half-life of Na-24 is 15.0 hours. a. How many grams of Na-24 in a 4.00 g sample of this nuclide will have decayed after 60.0 hours? b. How many hours are required to reduce the amount of Na-24 present in a 28.0 mg sample to 7.0 mg?
a. 3.75 g b. 30.0 hours
a Bronsted-lowry base is a substance that can
accept proton [H^+ ion] from some other substance
HF(aq) + H2O(l) <=> F^-(aq) + H3O^+(aq) in this acid-base reaction, a base H2O
accepts H^+ to form its conjugate acid H3O^+
in HCl + H2O -> Cl^- + H3O^+ H2O
accepts proton
in a nuclear reaction, Energy changes that
accompany nuclear reactions are much larger than those in chemical reactions.
For endothermic chemical reactions the energy needed to break reactant chemical bonds is
greater than that released in product chemical bond formation
you use isotopic notation
for elements in nuclear reactions
in water, weak electrolytes
forms solution of few ions & mostly undissociated molecules
Effect of concentration changes
forward & reverse reaction rates adjust until are again equal & equilibrium is re-established
What statement is correct for a system at chemical equilibrium?
forward & reverse reaction rates are equal
What condition must occur when a chemical reaction is at equilibrium?
forward & reverse reactions are happening at equal rates
In Cl2(g) + 2NaBr(aq) -> Br2(aq) + 2NaCl(aq) Cl
gained; reducing agent
Indicate whether each of the following substances loses or gains electrons in a redox reaction. The oxidizing agent
gains
Indicate whether each of the following substances loses or gains electrons in a redox reaction. The substance undergoing reduction
gains
Which of the following correctly orders the three types of naturally occurring radiation in terms of increasing ability to produce ion pairs through radiation-matter interactions?
gamma, beta, alpha
Pressure is...
gas concentration
Classify each of the following events based on whether the solubility of the indicated gas will increase, decrease or stay the same air in the blood of a diver breathing compressed air that quickly surfaces
gas solubility decreases
Classify each of the following events based on whether the solubility of the indicated gas will increase, decrease or stay the same the temperature is increased
gas solubility decreases
Classify each of the following events based on whether the solubility of the indicated gas will increase, decrease or stay the same O2 in the blood of a person who is in a hyperbaric chamber
gas solubility increases
Classify each of the following events based on whether the solubility of the indicated gas will increase, decrease or stay the same the partial pressure of an anesthetic gas is increased
gas solubility increases
Classify each of the following events based on whether the solubility of the indicated gas will increase, decrease or stay the same the pressure of a gas over a solvent is increased
gas solubility increases
Only concentrations of
gases & substances in solution are written in equilibrium expression.
When put acid & base together,
get 2 products [salt & water]
How can you tell it's Redox when all nonmetals?
get more hydrogens or electrons = reduced
You need energy to
get reaction going [like gas & bbq]
mass/volume percent concentration % (m/v)
gives number of grams of solute as percentage of number of milliliters
At a given temperature, which of the two aqueous solutions 1.0 M glucose or 1.0 M NaCl has the higher freezing point
glucose
At a given temperature, which of the two aqueous solutions 1.0 M glucose or 1.0 M NaCl has the higher vapor pressure
glucose
Tell me about: 3H2 + N2 -> 2NH3
goes forward for while but eventually ammonia will break down if in closed container
Indicate whether the osmotic pressure of a 0.1 M NaCl solution will be less than, the same as, or greater than that of each of the following solutions. 0.050 M MgCl2
greater
Indicate whether the osmotic pressure of a 0.1 M NaCl solution will be less than, the same as, or greater than that of each of the following solutions. 0.1 M glucose
greater
The greater the concentration difference between the separated solutions,
greater magnitude of osmotic pressure.
A semipermeable membrane separates two aqueous solutions at 37 degrees Celsius. For the following case, name the solution into which a net flow of water (if any) will occur. solution A: 0.10 M NaCl (aq) solution B: 0.01 M NaCl (aq)
net flow is toward solution A
A semipermeable membrane separates two aqueous solutions at 20 degrees Celsius. Name the solution into which a net flow of water (if any will occur). Assume 100% dissociation for electrolytes, meaning ion-pairing can be ignored. solution A: 0.10 M CaCl2 (aq) solution B: 0.50 M CaCl2 (aq)
net flow is toward solution B
A semipermeable membrane separates two aqueous solutions at 37 degrees Celsius. For the following case, name the solution into which a net flow of water (if any) will occur. solution A: 0.10 M NaHCO3 (aq) solution B: 0.20 M NaHCO3 (aq)
net flow is toward solution B
When 2 solutions have different solute concentrations,
net flow of solvent will be toward more concentrated solution
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral [H^+] = 1.0 x 10^-7
neutral
The following value represents an aqueous solution at 25 degrees Celsius. Classify the solution as acidic, basic or neutral pH = 7.00
neutral
if H3O^+ is 1.0 x 10^-7 M and OH^- is 1.0 x 10^-7, type of solution is
neutral
pH = 7
neutral
[H3O+] = [OH-]
neutral solution
HCl + NaOH -> H2O + NaCl is
neutralization
H2SO4 +2KOH→K2SO4 +2H2O is an example of
neutralization reaction
HCl + NaOH → NaCl + H2O is an example of
neutralization reaction
When you put an acid & base together, they
neutralize each other & make water and salt as product
The explanation for how a beta particle is produced in the nucleus of a radionuclide and then ejected involves the conversion (in a complex series of steps) of a
neutron to a proton and a beta particle
For example: How many milliliters of a 5.75% (v/v) ethanol solution can be prepared from 2.25 mL of ethanol? How do you know which one to start with?
never start with the 5.75% v/v bc it's a conversion factor
for a solute to dissolve in a solvent, need to overcome solute-solute attractions & solvent-solvent attractions
new type of interaction forms [solute-solvent attractions]
HNO3
nitric acid
Identify whether or not the following set contains an acid-base conjugate pair HCl and ClO4^-
no
Indicate whether or not each of the following chemical reactions represents a combustion reaction. ( C + CO2 -> 2CO
no
Indicate whether or not product formation increases if the size of the reaction container is increased for each of the equilibrium systems in C2H4(g) + 3O2(g) <=> 2CO2(g) + 2H2O(g) + heat
no
Indicate whether or not product formation increases if the size of the reaction container is increased for each of the equilibrium systems in N2(g) + 2O2(g) + heat <=> 2NO2(g)
no
Indicate whether or not product formation increases if the size of the reaction container is increased for each of the equilibrium systems in heat + 2N2(g) + 6H2O(g) <=> 4NH3(g) + 3O2(g)
no
Indicate whether or not product formation increases w increasing temperature in each of the following equilibrium systems C2H4(g) + 3O2(g) <=> 2CO2(g) + 2H2O(g) + heat
no
Will the following combination make a buffer solution? H3PO4 and NaCl
no
Will the following combination make a buffer solution? HCl and KCl
no
Will the following increase the rate of reaction? cooling the reaction down to low temperatures
no
Will the following increase the rate of reaction? omitting the addition of a catalyst
no
Will the following increase the rate of reaction? using a solid, granular solid, instead of a finely powdered solid for a reactant
no
Does the following ion form a compound with Pb2+ that is soluble in water? Na^+
no [Pb^2+ and Na^+ cannot form a compound]
Identify whether or not the following set contains an acid-base conjugate pair H2CO3 and CO3^2-
no [bc differs by 2 hydrogens]
Does the following ion form a compound with Pb2+ that is soluble in water? Br^-
no [precipitates]
Does the following ion form a compound with Pb2+ that is soluble in water? SO4^2-
no [precipitates]
Which of the following solutions would have a lower freezing point than a solution containing 0.20 mole of glucose per kilogram of solvent? a. solution containing 0.10 mole of glucose per kilogram of solvent b. solution containing 0.10 mole of NaCl per kilogram of solvent c. solution containing 0.10 mole of MgCl2 per kilogram of solvent d. no correct response
solution containing 0.10 mole of MgCl2 per kilogram of solvent
what is an aqueous solution?
solution in which water is solvent
Solution vs Pure substance
solution is 2 or more components; pure substance is 1 component
what is a concentrated solution?
solution that contains large amount of solute relative to amount that could dissolve
unsaturated solution
solution that contains less than maximum amount of solute that can be dissolved under conditions at which solution exists
saturated solution
solution that contains maximum amount of solute that can be dissolved under conditions at which solution exists
what is a dilute solution?
solution that contains small amount of solute relative to amount that could dissolve
What is a hypertonic solution?
solution w higher osmotic pressure than that within cells
What is a hypotonic solution?
solution w lower osmotic pressure than that within cells
What is an isotonic solution?
solution w osmotic pressure equal to that within cells.
Osmosis is the movement of
solvent across semipermeable membrane
In dialysis & osmosis
solvents move toward areas of high concentration & solutes move toward areas of low concentration
Semipermeable means
some things go across but others can't
polarity of water [+ & - ends] suggests all ionic compounds would be soluble
sometimes ions in compound are more attracted to each other than to water molecules
for example; unstable nucleus readily undergoes change The change is
spontaneous emission of either energy or a particle
What physical manifestation indicates that an atom possesses an unstable nucleus?
spontaneous emission of radiation from nucleus of atom
In a reaction, if you
start w high energy & end w low, then exothermic reaction
What is chemical equilibrium?
state in which forward & reverse chemical reactions occur simultaneously at same rate
thick sheet of paper
stops alpha particles
aluminum [1 cm thick]
stops beta particles
lead and concrete [5 cm thick]
stops some gamma radiation]
Acid ionization constants give information about
strength of acid
100% or very nearly 100% of its protons are transferred to water
strong acid
HA + H2O <- ——> H3O^+ + A^- is showing
strong acid
Identify each of the following as a strong or weak acid or base. H2SO4
strong acid
Identify each of the following as a strong or weak acid or base. HBr
strong acid
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other HBr
strong acid
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other HNO3
strong acid
How does a buffer resist change in pH upon addition of a strong acid?
strong acid reacts w weak base in buffer to form weak acid which produces few H^+ ions in solution & therefore only little change in pH
Identify each of the following as a strong or weak acid or base. NaOH
strong base
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other Ba(OH)2
strong base
In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases or other NaOH
strong base
hydroxide bases are
strong bc ionic
Classify these compounds as strong electrolytes, weak electrolytes or nonelectrolytes HBr
strong electrolyte
Classify these compounds as strong electrolytes, weak electrolytes or nonelectrolytes Zn(NO3)2
strong electrolyte
HCl(s) + H2O(l) → H+ (aq) + Cl- (aq)
strong electrolyte
NaCl(s) + H2O(l) → Na+ (aq) + Cl- (aq)
strong electrolyte
Since salt is a
strong electrolyte, it is completely dissociated in solution
the Weaker the acid,
stronger its conjugate base
A solution with a ph of 12.0 is
strongly basic
The solvent is the
substance doing the dissolving
