Honors Chemistry
Chapter 12 Quiz
Name _________________________
Period _____ Date __________
1) Choose the statement below that is TRUE.
A) A solution will form between two substances if the solute-solvent interactions are of
comparable strength to the solute-solute and solvent-solvent interactions.
B) A solution will form between two substances if the solute-solvent interactions are small
enough to be overcome by the solute-solute and solvent-solvent interactions.
C) A solution will form between two substances if the solute-solute interactions are strong
enough to overcome the solvent-solvent interactions.
D) A solution will form between two substances only if the solvent-solvent interactions are
weak enough to overcome the solute-solvent interactions.
E) None of the above are true.
2) Choose the situation below that would result in a ΔHsolution near 0.
A) When |ΔHsolvent| >> |ΔHsolute|
B) When |ΔHsolute| > |ΔHhydration|
C) When |ΔHsolute| < |ΔHhydration|
D) When |ΔHsolute| is close to |ΔHhydration|
E) There isn't enough information to determine.
3) Choose the situation below that would result in an exothermic ΔHsolution.
A) When |ΔHsolute| > |ΔHhydration|
B) When |ΔHsolute| is close to |ΔHhydration|
C) When |ΔHsolute| < |ΔHhydration|
D) When |ΔHsolvent| >> |ΔHsolute|
E) There isn't enough information to determine.
4) Dynamic equilibrium can be defined as
A) rate of dissolution = rate of deposition
B) rate of dissolution < rate of deposition
C) rate of dissolution > rate of deposition
D) rate of bubbling > rate of dissolving
E) rate of evaporating > rate of condensing
5) A solid can be purified through what technique?
A) recrystallization
B) dilution
C) dissolution
D) boiling
E) melting
6) Identify the compound whose solubility is least affected by temperature.
A) Na2SO4
D) KClO3
E) NaCl
B) K2Cr2O7
C) KNO3
7) Which of the following statements is TRUE?
A) In general, the solubility of a solid in water decreases with increasing temperature.
B) In general, the solubility of a gas in water decreases with increasing temperature.
C) The solubility of a gas in water usually increases with decreasing pressure.
D) The solubility of an ionic solid in water decreases with increasing temperature.
E) None of the above statements are true.
8) Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.2 atm. The
Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm.
A) 0.15 M
C) 0.65 M
E) 0.29 M
B) 0.57 M
D) 0.18 M
9) Give the term for the amount of solute in moles per kilogram of solvent.
A) molality
D) mole percent
B) molarity
E) mass percent
C) mole fraction
10) Which of the following concentration units are temperature dependent?
A) mole fraction
D) molarity
B) molality
E) none of the above.
C) mass percent
11) Identify the colligative property.
A) vapor pressure lowering
B) freezing point depression
C) boiling point elevation
D) osmotic pressure
E) all of the above
12) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the
molarity of the HCl, if the solution has a density of 1.20 g/mL.
A) 7.79 M
C) 12.8 M
E) 13.9 M
B) 10.7 M
D) 9.35 M
13) A 1.00 L sample of water contains 0.0036 g of Cl- ions. Determine the concentration of chloride
ions in ppm if the density of the solution is 1.00 g/mL.
A) 2.8 ppm
C) 3.6 ppm
E) 5.4 ppm
B) 7.2 ppm
D) 1.8 ppm
14) Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6) in
250.0 mL of water. The vapor pressure of pure water at 25°C is 23.8 torr.
A) 70.8 torr
C) 23.1 torr
E) 7.29 torr
B) 72.9 torr
D) 22.9 torr
15) The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of
sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? K b
(water) = 0.512°C/m.
A) 261 g sucrose
C) 762 g sucrose
E) 130. g sucrose
B) 528 g sucrose
D) 223 g sucrose
16) Give the reason that antifreeze is added to a car radiator.
A) The freezing point is lowered and the boiling point is elevated.
B) The freezing point is elevated and the boiling point is lowered.
C) The freezing point and the boiling point are elevated.
D) The freezing point and the boiling point are lowered.
E) None of the above.
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17) Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing
osmotic pressure.
I. 0.011 M sucrose
II. 0.00095 M glucose
III. 0.0060 M glycerin
A) I > III > II
B) I > II > III
C) II > III > I
D) III > I > II
E) II > I > III
18) Choose the aqueous solution with the lowest vapor pressure. These are all solutions of
nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.
A) 0.120 m C2H6O2
D) 0.030 m LiC2H3O2
E) They all have the same vapor
B) 0.040 m (NH4)2SO4
pressure.
0.060
m
K
CO
C)
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19) Identify the classification of milk.
A) aerosol
B) solid aerosol
C) foam
D) emulsion
E) solid emulsion
20) What happens to a supersaturated solution of potassium acetate once it is cooled and a
small crystal of solid potassium acetate is added?
21) Give the preparation of rock candy.
22) Define osmosis.
23) Calculate the osmotic pressure, in torr, of a solution containing 3.00 mg of a sugar (342
g/mole) in 15.0 mL of water at 25°C.
24) Define a colloid.
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Δ Hsol’n = Δ Hsolute + Δ Hsolvent + Δ Hmix
Δ Hsol’n = - Δ Hlattice energy + Δ Hsolvent + Δ Hmix
Δ Hsol’n = Δ Hhydration + Δ Hmix
Henry’s Law: Sgas = kHPgas
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Raoult’s Law: Psolvent in solution = csolvent∙P°
vapor pressure lowering
ΔP = Pºsolvent − Psolution = csolute  Pºsolvent
Raoult’s Law for Volatile Solute: Ptotal = Psolute + Psolvent
Where Psolute = csoluteP°solute and Psolvent = csolventP°solvent
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Freezing Point Depression: (FPsolvent – FPsolution) = ΔTf = mKf
Boiling Point Elevation: (BPsolution – BPsolvent) = ΔTb = mKb
Δ Tf = i∙m∙Kf

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