Chem Exam 3

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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

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.

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?

What is the highest-atomic-numbered naturally occurring element?

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

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

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

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

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

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

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

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

Which of the following ions cannot be present in a salt? a. Na+ b. SO4^2− c. OH− d. no correct response

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

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

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

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

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

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

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, 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

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

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

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.

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