chem b
To reduce the amount of CO2 that escapes from a bottle of carbonated beverage when you open the cap, you should ________.
Put the bottle in a refrigerator for several hours before opening the cap.
What happens if the solvent-solute attraction is greater than the solute-solute attraction when two substances are mixed?
The solute particles are pulled apart and dispersed throughout the particles of the solvent, which holds the particles of the solute in solution.
KClO3
potassium and chlorate oxyanion formula
The state in which the processes of distribution and recrystallization of a solute occur at the same rate is called ___________.
solution equilibrium
Many ionic compounds are ___________ because they completely ionize in water to create a solution with charged ions that can act as an electrical conductor.
strong electrolytes
A solution that contains more solute that would normally dissolve at a particular temperature and pressure is a(n) ________ solution.
supersaturated
molar mass
the mass of one mole of a substance
excess reactant
the reactant that is not completely used up in a chemical reaction
A kind of decomposition reaction that requires heat is ______.
thermal
The general rule for determining solubility is:
"like dissolves like"
A chemist can use thermochemistry to do the following: a. tell how much __________ is transferred in chemical reactions and physical changes. b. predict whether certain substances will __________ with each other. c. predict the __________ of reactions. d. predict what kinds of will __________ occur.
(heat), (react), (rates), (reaction)
Na2O2 - oxidation number of Na - oxidation number of O - name in the systematic nomenclature - name in Stock system
- (+1) - (-1) - sodium peroxide - not Stock name since sodium only has one oxidation state
Na2O - oxidation number of Na - oxidation number of O - name in the systematic nomenclature - name in Stock system
- (+1) - (-2) - disodium dioxide - not Stock name since sodium only has one oxidation state
Strontium and chlorine combine to form a binary ionic compound. - oxidation number of Sr - oxidation number of Cl - oxidation number of O - chemical formula - name in the systematic nomenclature - name in Stock system
- (+2) - (-1) -
A single displacement reaction will be:
- A + BC → AC + B - a reaction in which one element displaces a similar element in a compound. - A +BC → BA +C
A double-displacement reaction will be:
- AB + CD → AD + CB - a chemical reaction in which two aqueous compounds exchange ions to produce two new compounds.
What are the equations for the chemical reactions that took place when the acids reacted with active metals?
- Cu(s) + HCl → nothing happened - Mg(s) + 2HCl(aq) → MgCl2 (aq)+ H2↑ - Zn(s) + 2HCl(aq) → ZnCl2 (aq)+ H2↑
Barium and phosphate oxyanions bond to form an ionic compound. - oxidation number of Ba - oxidation number of P - oxidation number of O - chemical formula - name in the systematic nomenclature
- (+2) - (+5) - (-2) - Ba3(PO4)2 - barium phosphate
Magnesium and sulfur react to form a binary ionic compound. - oxidation number of magnesium - oxidation number of sulfur - chemical formula - name in the systematic nomenclature - name in Stock system
- (+2) - (-2) - MgS - magnesium sulfide - magnesium(II) sulfide
Phosphorus and bromine react to form a molecular compound. (+3) - oxidation number of phosphorus: - oxidation number of bromine - chemical formula - name in the systematic nomenclature - name in Stock system
- (+3) - (-1) - PBr3 - phosphorus tribromide - phosphorus(III) bromide
PCl3 - oxidation number of phosphorus - oxidation number of chlorine - name in the systematic nomenclature - name in Stock system
- (+3) - (-1) - phosphorus trichloride - phosphorus(III) chloride
Phosphorus and bromine react to form a molecular compound. (+5) - oxidation number of phosphorus: - oxidation number of bromine - chemical formula - name in the systematic nomenclature - name in Stock system
- (+5) - (-1) - PBr5 - phosphorus pentabromide - phosphorus(V) bromide
Some physical processes that chemical thermodynamics studies are: Select all that apply.
- Dissolution - Changes of State
Would wet hands be better conductors than dry hands? Why or why not?
Wet hands would be better conductors since salts dissolve in water.
Which will dissolve faster: 25 g of CuSO4 in powder or 25 g of CuSO4 in one crystal? Why?
25 g of CuSO4 in powder have larger surface area
What is the balanced equation for the burning of hydrogen in oxygen?
2H2(g)+O2(g)→ 2H2O(l)
What is the reverse equation of the burning of hydrogen in oxygen?
2H2O(l) + Energy → O2(g) + 2H2(g)
Identify the decomposition reaction(s):
2NaClO3(s) → 2NaCl(s) +3O2(g)
For a particular lab experiment, you need 150 mL of a 2.50 M solution of ammonium nitrate. How many grams of NH4NO3 will you need for the solution?
30.0 g
molar mass: C2H6
30.0688 g/mol
You have 500 mL of a 4.00 M solution of KNO3 from a previous experiment, but now you need 250 mL of a 0.500 M concentration of the same solution. How much of the stock solution will you need to make the dilute solution?
31 ML
Calculate the percentage of composition of each element in the compound: CO
42.88 % C 57.12 % O
molar mass: KOH
56.1056 g/mol
molar mass: NaCl
58.443 g/mol
Calculate the percentage of composition of each element in the compound: KOH
69.69% K 28.52% O 1.80% H
If you choose to titrate a weak acid with a strong base, the acid -base indicator should work in _______ range
7.0-9.0
Calculate the percentage of composition of each element in the compound: C2H6
79.89% C 20.11% H
Identify the double displacement(s)
Al(NO3)3(aq)+3NaOH(aq)→Al(OH)3(aq)+3NaNO3(s)
In 1919, a German chemist named ________ proposed a new nomenclature for naming chemical compounds that uses Roman numerals to indicate the oxidation number of the first element in the compound.
Alfred Stock
A solution has a pH of 11.00. Calculate the [H3O+] of the solution.
[H3O+]= 1.0x10-11
A nitric acid solution (HNO3) has a molar concentration of 0.00044 M. Calculate the [H3O+], [OH-] and the pH of the solution. Remember that Kw= 1.0x10-14M2
[H3O+]= 4.4x10-4, [OH-]=2.3x10-11M, pH 3.36
hydrogen halide
a binary molecular compound composed of hydrogen and a halogen
hydride
a binary molecular compound made up of hydrogen and a main group element
decomposition reaction
a chemical reaction in which a single compound undergoes a chemical reaction to produce two or more simpler substances
combustion reactio
a chemical reaction in which a substance combines with an oxidizer (usually oxygen) and releases energy in the form of light and heat
single-displacement reaction
a chemical reaction in which one element displaces a similar element in a compound
double-displacement reaction
a chemical reaction in which two aqueous compounds exchange ions to produce two new compounds
synthesis reaction
a chemical reaction in which two or more substances combine to form a new compound
electrolysis
a chemical reaction that occurs when an electric current is passed through an electrolyte to bring about a decomposition reaction
binary ionic compound
a compound formed from one monatomic cation and one monatomic anion
binary molecular compound
a compound whose molecule consists of two atoms that share electrons to form a covalent bond
mole ratio
a conversion factor that compares the number of moles of one substance with the number of moles of another substance
thermal decomposition
a decomposition reaction in which heat is required
catalytic decomposition
a decomposition reaction that requires a catalyst
volumetric flask
a large flask with only one marking that precisely indicates a specific volume; used to prepare solutions with specific concentrations
activity series
a list that ranks elements according to the ease with which they undergo certain chemical reactions
covalent network solid
a network of covalently bonded atoms that forms a crystal lattice
oxidation number
a numerical value assigned to each element to indicate the number of electrons that might be lost, gained, or shared by an atom of that element when it bonds with an ion or an atom of another element to form a compound
oxyanion
a polyatomic ion that contains oxygen
precipitate
a solid product that settles out of an aqueous solution as a result of a reaction between aqueous reactants
aqueous solution
a solution in which the solvent is water
Reviewing the three types of mixtures, solutions, colloids, and suspensions, you can say that a solution is different from the others in that:
a solution is homogeneous and has particles that are less than 1 nm in diameter
unsaturated solution
a solution that contains less solute than a saturated solution
supersaturated solution
a solution that contains more solute than what would normally dissolve at a particular temperature and pressure
saturated solution
a solution that contains the maximum amount of solute that will dissolve at a particular temperature and pressure; a solution that has reached solution equilibrium
catalyst
a substance that alters the rate of a chemical reaction without being consumed in the reaction
empirical formula
a symbolic representation of a chemical compound that uses element symbols and subscripts to indicate the smallest whole-number ratio of each kind of atom in a chemical compound
systematic nomenclature
a system for naming inorganic binary compounds that uses the names of the two elements or ions in the compound with prefixes to indicate how many atoms or ions are contributed to each molecule or formula unit
Stock system
a system for naming inorganic binary compounds that uses the systematic names for compounds, but uses a Roman numeral to indicate the oxidation state of the first element in the compound
semipermeable membrane
a thin barrier that permits the passage of some particles but restricts the passage of other particles
A(n) ___ is an ionic compound formed by a cation bonded to an oxyanion that has one or more hydrogen atoms.
acid salt
You can increase the rate of dissolution by _________ a solution or by increasing the _________ of the solvent, both of which cause the dissolved solute particles to dissolve faster.
agitating temperature
You are given a sample of an unknown aqueous substance. After performing several tests on the compound, you discover that it turns blue litmus paper red and that reacts with sodium hydroxide (NaOH), which is a base, to form a salt (NaCl) and water. As a result, you conclude the unknown substance to be:
an acid
binary acid
an acid composed of only two elements: hydrogen and one highly electronegative element, such as a halogen
oxyacid
an acid that contains hydrogen, oxygen, and a third element, which is usually a nonmetal
formula equation
an expression of a chemical reaction that uses chemical formulas and symbols to represent the identity and physical state of each reactant and product in the chemical reaction
chemical equation
an expression of a chemical reaction that uses chemical formulas, symbols, and coefficients to represent the identity, physical state, and molar amount of each reactant and product in the chemical reaction
word equation
an expression of a chemical reaction that uses words and symbols to represent the identity of each reactant and product in the chemical reaction
acid salt
an ionic compound formed by a cation bonded to an oxyanion that has one or two hydrogen atoms
oxidizer
any substance that causes another substance to lose electrons
nonelectrolyte
any substance that does not ionize when dissolved
polarity
any substance that does not ionize when dissolved
electrolyte
any substance that ionizes when dissolved or melted to become an electrical conductor
When a substance is dissolved in water (the solvent), a(n) ____ solution is created.
aqueous
BaO
barium and oxygen formula
A(n) ___ is composed of only two elements, hydrogen and one highly electronegative element, such as a halogen.
binary acid
One monatomic cation and one monatomic anion =
binary ionic compound
The ___________________ is the boiling-point elevation of a solvent in a one molal solution of a nonvolatile, nonelectrolyte solute.
boiling-point elevation
_________ is a solution that can resist changes in pH.
buffer
identify nonelectrolyte
c2h5oh ccl4 c12h22o11
CaCl2
calcium and chlorine formula
Ca3N2
calcium nitride
What is the measurement of enthalpy changes caused by chemical reactions, changes of state, or the formation of a solution?
calorimetry
A kind of decomposition reaction that requires a catalyst is ______.
catalytic
What kind of enthalpy does a bomb calorimeter measure?
combustion
The measure of the amount of solute in a given amount of solvent is the _________ of the solution.
concentration
The compound that is formed after an acid loses a proton and is now a proton acceptor is called ________.
conjugate acid
The compound that is formed after accepting a proton from a base and is now a proton donor is called ________.
conjugate base
Also called the law of ________ of energy, the first law of thermodynamics states that the total amount of energy in a thermodynamic system remains constant.
conservation
The correct way to name a copper cation with a charge of +2 is ______.
copper (II)
A covalent network solid is a network of covalently bonded atoms that forms a _______.
crystal lattice
According to the rules for the systematic nomenclature for naming binary compounds, the correct name for the compound with the chemical formula B2F4 would be:
diboron tetrafluoride
During the process of _______________ the solute maybe completely ionized, partially ionized, or it may remain intact.
dissolution
The rapid release of a dissolved gas from a liquid is called __________.
effervescence
Which one is not a colligative property?
electrolyte solubility
Lewis acid
electron pair acceptor
The point at which the color of the acid-base indicator changes color in an acid-base titration is called the _____________
end point
If the sum of the energy required to dissolve a solute is greater than the energy released when the solute is solvated, then the enthalpy of solution is _________ and the final temperature of the solution is lower than its temperature before dissolution.
endothermic
The total amount of energy in a thermodynamic system is called ___________.
enthalpy
The net energy change when a solute is dissolved in a solution is called _________.
enthalpy of solution
Also called the law of ________ is the second law of thermodynamics, which states that for any thermodynamic system not in thermodynamic equilibrium, energy will move to increase entropy.
entropy
The point at which both substances in a titration exist in chemically equivalent amounts is called the __________________.
equivalence point
A negative value for the enthalpy of solution, ΔHsol, indicates a(n) _________ process.
exothermic
The amount of energy that is transferred when one mole of a compound is formed from its component elements in their standard states is the standard molar enthalpy of _______________.
formation
Increasing the temperature will permit more of a solid or liquid solute to be dissolved in a liquid solvent but the opposite is true of __________ dissolved in liquids.
gases
identify weak electrolyte
h2co3 nh3 hgcl2
identify strong electrolyte
h2so4 NaOH nh4no3 hbr nacl hcl
When calcium chloride dissolves in water, it recrystallizes as a(n) __________, with the chemical formula CaCl2 • 2H2O.
hydrate
A(n) ___ is a binary molecular compound made up of hydrogen and a main group element.
hydride
If hydrogen bromide (a hydrogen halide) is dissolved in water, what is he name of the binary acid that is produced?
hydrobromic acid
The gas that is liberated when an acid reacts with an active metal is _____.
hydrogen
A binary molecular compound composed of hydrogen and halogen is a(n) ___.
hydrogen halide
The general name for an ionic compound composed of a cation from a base bonded to an anion produced by an acid is a(n) ___.
hydrogen halide
__________ are liquids completely insoluble in each other.
immiscibles
Solubility is determined by the molecular or ionic structures of the solute and the solvent, and by the _________ that hold together the particles of each substance.
intermolecular forces
The ______________ of water is the product of the concentration of hydronium ions and the concentration of hydroxide ions in water.
ionization constant
The equation below shows the product of the hydronium and hydroxide concentrations in water and is called the __________ of water. Kw = [H3O+] [OH-] = (1.0 * 10^-7 M) (1.0 * 10^-7 M) = 1.0 * 10^-14 M^2
ionization constant
A combustion reaction will be:
is a chemical reaction in which a substance combines with an oxidizer (usually oxygen) and releases energy in the form of light and heat
PbSO4
lead (II) and a sulfate oxyanion formula
The _______ is used up in a chemical reaction and causes the reaction to stop.
limiting reactant
LiBr
lithium and bromine formula
While working in your garage, you accidentally spilled battery acid on the floor. You remembered from chemistry that a strong base would neutralize the acid. Which of the substances would work best to neutralize the acid?
lye
MgCO3
magnesium and carbonate oxyanion formula
MgCl2
magnesium chloride
titration
method of determining the concentration of a solution of unknown concentration by adding a controlled and measured amount of a solution of known concentration until a desired chemical reaction occurs
The boiling-point elevation of a solvent in a one molal solution of a nonvolatile, nonelectrolyte solute is the ________________.
molal boiling-point constant
The _____________ is the freezing-point depression of a solvent in a one molal solution of a nonvolatile, nonelectrolyte solute.
molal freezing-point constant
The concentration of a solution expressed by the number of moles of solute per liter of solution is called _________.
molarity
What is the name of the oxyacid that forms (NO3-) oxyanions when it breaks down?
nitric acid
Compounds that do not ionize at all in solution are called __________.
nonelectrolytes
Answer the question using the equation: HCl(aq)+H2O(l)→H+(aq)+Cl-(aq)+H2O(l)→H3O+(aq)+Cl-(aq) Which product is a Lewis base?
not: H3O+
In this equation, which substance is a strong Brønsted-Lowry base? HClO4(aq)+H2O(l)→H3O+(aq)+ ClO4-(aq)
not: HClO4
In this equation, which substance is a weak Brønsted-Lowry conjugate acid? HClO4(aq)+H2O(l)→H3O+(aq)+ ClO4-(aq)
not: HClO4 ClO4-
When an element forms more than one oxyanion, the ion with the greater _____ is given the suffix -ate.
number of oxygen atoms
__________ is the movement of a solvent, usually water, through a(n) __________ membrane from a region of lower solute concentration to a region of higher solute concentration.
osmosis semipermeable
A(n) _____ is any substance that will cause another substance to lose electrons.
oxidizer
A(n) ___ is an acid that contains hydrogen, oxygen, and a third element, which is usually a nonmetal.
oxyacid
Is hydrofluoric acid a binary acid or an oxyacid? How can you tell?
oxyacid, it end on -ic
The negative of the common logarithm of the hydronium concentration of a solution is __________ but the negative logarithm of the hydroxide concentration of a solution is __________
pH pOH
As a rule, solvents consisting of polar molecules will dissolve substances that are ________.
polar
The degree of contrast between two opposing forces is called _________.W
polarity
KI
potassium iodide
KMnO4
potassium permanganate
colligative properties
properties that depend on the concentration of a solute in a solution but not on the identity of the solute
Brønsted-Lowry base
proton acceptor
The standard molar enthalpy of ________________ is the amount of heat transferred when the number of moles of reactants specified in a chemical equation is completely converted into products in their standard states.
reaction
The formation of crystals by particles of a solute that had previously dissolved from a crystal is called ____________.
recrystallization
immiscible
referring to liquids that are completely insoluble in each other
miscible
referring to liquids that are soluble in each other in any proportion
A solution that contains the maximum amount of solute that can dissolve at a particular temperature and pressure is a(n) ________ solution.
saturated
What can you summarize about the use of acid-base indicators?
An acid-base indicator is used to identify the presence of an acid or base. These indicators exhibit different colors depending on the solution that they are in. They are especially useful when completing titrations to determine the molarity of an unknown substance.
Why does an electrolyte depress the freezing point of a solvent more than a nonelectrolyte?
An electrolyte contributes more particles to the solution than a nonelectrolyte.
Which substance(s) is a Lewis acid?
Cl-
The following compounds are nonelectrolytes that are soluble in water. Which statement below is true of the colligative properties of these compounds? acetic acid CH3COOH glycerol C3H5(OH)3 sucrose C12H22O11 urea CH4N2O
Each compound would have the same colligative properties.
______ is a symbolic representation of a chemical compound that uses element symbols and subscripts to indicate the smallest whole-number ratio of each kind of atom in a chemical compound.
Empirical formula
HCl(aq)+H2O(l)→H+(aq)+Cl-(aq)+H2O(l)→H3O+(aq)+Cl-(aq) Which reactant is a Lewis base?
H2O
In this equation, which substance is a strong Brønsted-Lowry acid? HClO4(aq)+H2O(l)→H3O+(aq)+ ClO4-(aq)
H2O
You are given a sample of an unknown aqueous substance. After performing several tests on the compound, you discover that it turns blue litmus paper red and that reacts with sodium hydroxide (NaOH), which is a base to form a salt (NaCl) and water. As a result, you conclude the unknown substance to be:
H2O
Identify the synthesis reaction(s):
H2O(l)+SO3(l)→H2SO4(aq)
HCl(aq)+H2O(l)→H+(aq)+Cl-(aq)+H2O(l)→H3O+(aq)+Cl-(aq) Which substance(s) is a Lewis acid-base complex?
H3O+
Which of the following solutes would be the best substance to produce a solution that could be placed in an instant hot pack? Review table B-9.
HI
Based on the percentage of composition and molar mass of each of the following compounds, determine the empirical and chemical formulas A compound consists of 5.93% H and 94.07% O. The mass of one mole of the compound is 34.0146g.
HO empirical formula H2O2 molecular formula
Which law states that the overall enthalpy change in a reaction is the same whether it occurs in one step or a series of steps?
Hess's
How does the mathematical ratio translate to relative amounts expressed in the balanced equation?
In the balanced equation, there are two moles of hydrogen gas and one mole of oxygen gas. This corresponds to the 2:1 ratio for the volume of gas produced.
Ca (calcium)
Ionic Formula: Charge: +2
Al (aluminum)
Ionic Formula: Al3+ Charge: +3
Ba (barium)
Ionic Formula: Ba2+ Charge: +2
Cl (chloride)
Ionic Formula: Cl- Charge: -1
F (flouride)
Ionic Formula: F- Charge: -1
I (iodine)
Ionic Formula: I- Charge: -1
K (potassium)
Ionic Formula: K+ Charge: +1
Li (lithium)
Ionic Formula: Li1+ Charge: +1
Mg (magnesium)
Ionic Formula: Mg2+ Charge: +2
Nitride
Ionic Formula: N3- Charge: -3
Na (sodium)
Ionic Formula: Na1+ Charge: +1
O (oxide)
Ionic Formula: O2- Charge: -2
P (phosphide)
Ionic Formula: P3- Charge: -3
S (sulfide)
Ionic Formula: S2- Charge: -2
Zn (zinc)
Ionic Formula: Zn2+ Charge: 2+
What types of substances would definitely be good conductors?
Ionic substances would be good conductors since they dissolve in water and form ions.
In 1782 a French chemist named ________ proposed a systematic nomenclature for naming chemical compounds.
Louis-Bernard Guyton de Morveau
Identify the single displacement reaction(s):
Mg(s)+2HCl (aq)→MgCl2+H2(g)
__________ are liquids soluble in each other in any proportion.
Miscibles
_________ is the concentration of a solution expressed by the number of moles of solute per kilogram of solvent.
Molality
Which of the following is NOT an oxyanion?
NH4
Based on the percentage of composition and molar mass of each of the following compounds, determine the empirical and chemical formulas. A compound consists of 57.48% Na, 40% O, and 2.52% of H. The mass of one mole of the compound is 39.9971g.
NaOH empirical formula NaOH molecular formula
If 50 mL of acetic acid is added to 100 mL of water at 60°C, will it produce a saturated solution? Why, or why not?
No, acetic acid is completely miscible in water so no amount of solute will ever produce a saturated solution.
The best mixture of antifreeze and water is 50% antifreeze, 50% water. The cooling system in your car has a mixture of 6.00L water and 6.00 L ethylene glycol (antifreeze). The molality of the solution is 17.9m. The chemical formula of antifreeze is C2H6O2 and its density is 1.1132 g/cm3. If the summer temperatures rise and the coolant reaches a temperature of 108°C, will it boil?
No, it would boil at 109.13°C
A solution containing 94.4 mL of carbon tetrachloride, CCl4, dissolved in 250.0 mL of nitrobenzene, C6H5NO2, was placed in the freezer, which dropped the temperature to 0°C. Did the solution freeze at that temperature? If so, at what temperature? The density of CCl4 is 1.59g/cm3. The density of C6H5NO2 is 1.2 g/cm3.
No, it would freeze at -16.61°C.
NaNO3
Sodium and nitrate oxyanion formula
Why does tap water conduct electricity but distilled water does not?
Tap water contains dissolved metals and other substances that can act as conductors, but distilled water does not have these dissolved substances.
What happens to the equilibrium between hydronium ions, hydroxide ions and water in a neutral solution when a base is added?
The equilibrium shifts to reduce the hydronium concentration.
Why are colligative properties different when a volatile solute is used?
The evaporation of the solute increases the vapor pressure. The increased vapor pressure prevents the solute from elevating the boiling point or depressing the freezing point of the solvent.
Which one is not a rule for naming binary molecular compounds in the systematic nomenclature?
The first name of the molecule or compound is given a prefix to indicate the number of atoms it contributes to the compound, even if it is only one (mono-).
When performing an acid-base titration, why is it important to swirl the solution?
The indicator will not diffuse evenly throughout the solution and you may get a false reading.
Based on your observations of the electrolysis apparatus, where do the oxide ions go?
The negative oxide ions collect at the positive electrode.
In the electrolysis apparatus, where do the hydrogen ions go?
The positive hydrogen ions collect at the negative electrode.
______________ is the branch of chemistry that studies the heat transfers that accompany chemical or physical changes.
Thermochemistry
What can you conclude happens to strong acids and bases when placed in water?
They dissolve into ions in water.
By what means did scientists arrive at the conclusion that water ionizes to contribute additional hydronium ions to a solution?
They learned how to measure the amount of ions in a solution by carefully measuring the amount of electric current that could be conducted through solutions with electrolytes.
According to the rules for the systematic nomenclature for naming binary compounds, the correct name for the compound with the chemical formula SiS2 would be:
silicon disulfide
NaOH
sodium hydroxide
The Stock system of naming compounds uses the ______ name of the compound without prefixes with a Roman numeral after the first name of the compound to indicate its _____ number.
systematic; oxidation
osmotic pressure
the amount of external pressure required to stop osmosis
molal boiling-point constant
the boiling-point elevation of a solvent in a one-molal solution of a nonvolatile, nonelectrolyte solute
molality
the concentration of a solution expressed by the number of moles of solute per kilogram of solvent
molarity
the concentration of a solution expressed by the number of moles of solute per liter of solution
oxidation state
the condition under which an oxidation number is applied to an element
Which of the following is NOT a decomposition reaction?
the decomposition of a non-metal oxidizer
percentage yield
the difference between the actual yield and the theoretical yield of a chemical reaction expressed as a percentage
boiling point elevation
the difference between the boiling point of a pure solvent and the boiling point of a solution of a nonelectrolyte in the same solvent
freezing point depression
the difference between the freezing temperature of a pure solvent and the freezing point of a solution of a nonelectrolyte in the same solvent
Which of the following is NOT a single-displacement reaction?
the displacement of hydrogen to form a molecular compound
recrystallization
the formation of crystals by particles of a solute that had previously dissolved from a crystal
molal freezing-point constant
the freezing-point depression of a solvent in a one-molal solution of a nonvolatile, nonelectrolyte solute
salt
the general term for an ionic compound composed of a cation from a base bonded to an anion produced by an acid
theoretical yield
the maximum amount of product that could be produced in a chemical reaction under ideal conditions
concentration of a solution
the measure of the amount of solute in a given amount of solvent; expressed as molarity or molality
actual yield
the measured quantity of a product that is obtained from a chemical reaction
osmosis
the movement of a solvent, usually water, through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration
pOH
the negative logarithm of a solution's hydroxide concentration of a solution
pH
the negative of the common logarithm of a solution's hydronium concentration
enthalpy of solution
the net energy change when a solute is dissolved in a solution
percentage composition
the percentage by mass of each element in a compound
equivalence point
the point at which both substances in a titration exist in chemically equivalent amounts
end point
the point at which the color of the acid-base indicator changes color in an acid-base titration
common logarithm
the power to which 10 must be raised to equal a specific number
disproportionation
the process in which a substance acts as both an oxidizing agent and a reducing agent in the same reaction
oxidation
the process in which an atom or ion experiences an increase in oxidation state
dissolution
the process of dissociating a solute into smaller particles by a solvent to produce a solution
solvation
the process whereby particles of a solvent completely surround the particles of a solute and hold them in solution
ionization constant of water
the product of the concentration of hydronium ions and the concentration of hydroxide ions in water
effervescence
the rapid release of a dissolved gas from a liquid
limiting reactant
the reactant that is used up in a chemical reaction and causes the reaction to stop
dissociation
the separation of a molecular compound into smaller molecules or separate elements, or the separation of an ionic compound into separate ions
solution equilibrium
the state in which the processes of dissolution and recrystallization of a solute occur at the same rate
composition stoichiometry
the study of the relationship between the quantities of the elements in a compound
stoichiometry
the study of the relationships between the quantities of elements in compounds or the quantities of elements and compounds in chemical reactions
reaction stoichiometry
the study of the relationships between the quantities of reactants and products involved in chemical reactions
Which of the following is NOT a kind of synthesis reaction?
the synthesis of hydrogen from the reaction of an acid with a metal
The condition under which an oxidation number is applied to an element is called its ___ state.
theoretical
___ is a numerical value assigned to each element to indicate the number of electrons that might be lost, gained, or shared by an atom of that element when it bonds with an ion or an atom of another element to form a compound.
theoretical yield
Chemical ___________ is the study of the relationship between heat and work within chemical reactions or physical changes of state.
thermodynamics
ionize
to break up a substance into individual cations and anions; to become an ion by gaining or losing electrons
A solution that contains less solute than it could dissolve at a particular temperature and pressure is a(n) ________ solution.
unsaturated
Freezing-point depression and boiling-point elevation result from a decrease in _______ pressure.
vapor
To prepare solutions with specific concentrations, you need a(n) _________ flask, which is a large flask with only one marking that precisely indicates a specific volume.
volumetric
Some ionic compounds are ___________ because they partially ionize in solution.
weak electrolytes
Identify the combustion reaction(s):
2C8H18(l)+25O2(g)→16CO2(g)+18H2O(l)
molar mass: CO
28.0101 g/mol
molar mass: Na2SO4
142.0422 g/mol
Which of the following apply to Hess's law? Select all that apply.
- If a reaction contains intermediate steps, the overall enthalpy change of the reaction is equal to the sum of the enthalpy changes of the intermediate steps. - Thermochemical equations may be reversed, if necessary, to calculate unknown enthalpies, as long as the sign of the enthalpy value also changes. - To find the enthalpy of formation of a compound, you can use the enthalpy changes of reactions that involve the elements that make up the compound, even if those reactions are not necessarily intermediate steps in the production of that compound. - Known enthalpy changes can be combined to calculate unknown enthalpies of reaction.
Strontium and chlorine combine to form an ionic compound. Select the formula that would be correct and the possible names using both the systematic nomenclature system and the Stock system. Select all that apply.
- SrCl2 - strontium(II) chloride
Why is it important to know the temperature of the water when dealing with ions in an aqueous solution?
- Temperature affects the concentration of water. - Water at a higher temperature will produce more ions than water at a lower temperature. - The ionization constant of water is usually given at 25 °C.
A synthesis reaction will be:
- a chemical reaction in which two or more substances combine to form a new compound - A + B → AB
A decomposition reaction will be:
- a reaction in which a single compound undergoes a chemical reaction to produce two or more simpler substances - AB → A + B
The basic types of reactions are
- double displacement - decomposition - synthesis - combustion - single displacement
You can increase the rate of dissolution by: Select all that apply.
- increasing the temperature - increasing the surface area - agitating the solution
When you work a stoichiometry calculation, you should set up and work the problem in a(n) _____ manner.
- orderly - systematic
Which ones are decomposition reactions?
- thermal - catalytic - electrolysis
Oxidation numbers help chemists:
- write chemical formulas - name compounds - balance chemical equations
What is the freezing point of a solution of 498mL of water (solute) dissolved in 2.50 L of ethanol (solvent), C2H5OH? The density of C2H5OH is 0.789g/cm3. (Remember that water has a density of 1.0 g/cm3.)
-142 C
The best mixture of antifreeze and water is 50% antifreeze with 50% water. The cooling system in your car has a mixture of 6.00 L water and 6.00 L ethylene glycol (antifreeze). The molality of the solution is 17.9m. The chemical formula of ethylene glycol (antifreeze) is C2H6O2 and its density is 1.1132 g/cm3. At what temperature would this mixture freeze?
-33.3°C
The names of monatomic anions are formed by using the first syllable of the chemical name of the element and adding the suffix _____.
-ide
A 2.00 L bottle of Dr Pepper contains 225 g of sucrose, C12H22O11. What is the molality of that solution?.
.329 M
What is the molarity of a 250.0 mL aqueous solution that contains 18.7 g of AgNO3?
0.440 M
A 1.0M solution is one that contains:
1.0 liter of solution that contains 1.0 mole of solute
At equilibrium, 1.0L of H2O produces ______ mole of hydronium ions.
1.0 x 10-7
Which of these solutions are saturated?
128 g of KI at 0°C 8.22 g of Ba(OH)2 at 40°C
What is the boiling point of a solution of 76 g of water dissolved in 500 mL of acetic acid, CH3COOH? The density of CH3COOH is 1.049 g/cm3
142.5 C
Winter is coming and it's time to make sure you have the right amount of antifreeze in your car. The best mixture of antifreeze and water is 50% antifreeze with 50% water. The cooling system in your car has a mixture of 6.00 L water with 6.00 L of ethylene glycol (antifreeze). What is the molality of that solution?
17.9m
molar mass: H20
18.0152 g/mol
You have a stock solution consisting of 2.5L of 6.00 M MgSO4. However, you need 225 mL of a 0.500 M solution. How will you dilute the solution, and how much of the stock solution will you need?
18.8 mL
What is the mathematical ratio of the volume of oxygen created to the volume of hydrogen created?
1:2
For every unit of oxygen collected, how many units of hydrogen gas were collected?
2
Which of these solutions are unsaturated?
2.00 g of PbCl2 at 80°C 100.2 g of NaNO3 at 60°C 75.5 g of LiCl at 20°C
What is the molarity of a 750.0 mL aqueous solution that contains 117 g of NaCl?
2.67 M
