Name__________________
AP Chapter 14
1. 70 grams of a certain solute is dissolved in 100 grams
of water, which has a freezing point depression of 1.858
K/m. The solution's freezing point is now 265.568 K.
What is the molar mass of this solute?
A) 123 g/mol
C) 167 g/mol
E) 200 g/mol
B) 140 g/mol
D) 175 g/mol
2. A solution of Na + ions would be best represented by
which picture?
A)
Date____________
5. A clear, colorless liquid in a beaker in a hood is heated at
a constant rate. The liquid begins to boil at 110 ° C. The
boiling temperature gradually increases to 115 ° C, at
which time the heating is discontinued. The material in
the beaker is probably a
A)
B)
C)
D)
E)
pure element
pure compound
a colloid
heterogeneous solution
homogeneous solution
6. The table below summarizes the result as 0.10 M
solutions are mixed.
B)
Which substance is a precipitate in this experiment?
A) KCl
C) NaCl
E) Cd(OH) 2
7. Which of the following dissolves in water to form an
ionic solution?
C)
A) O2
C) KMnO4
E) CH 4
B) SiO2
D) C12H22O11
8. As temperature increases, solubility of which of the
following decreases?
D)
A) NH3
C) NaNO3
E) KI
3. Which compound has the highest conductivity?
C) 0.18
D) 0.90
A)
B)
C)
D)
E)
C6H 6, benzene
CH 3Cl, chloromethane
C2H5OH, ethanol
C2H5COOH, propanoic acid
C5H10O5, fructose
10. What is the percent composition of a solution where 60.
g of a 10% salt solution in water is mixed with 40. g of
a 20% solution of the same salt? All are mass percents
B) H2O
D) HNO 3
4. What is the mole fraction of HF in a 10.% (by mass)
solution?
A) 0.090 B) 0.10
B) NH 4Cl
D) KCl
9. Of the following organic compounds, which is LEAST
soluble in water at 298 K?
E)
A) HF
C) CaSO 4
E) Pb(OH)2
B) NaCN
D) Zn(NO 3) 2
E) 0.91
A) 8%
B) 14%
C) 15%
D) 16%
E) 30%
11.If 149 grams of Ca(OH)2 is dissolved in 500 mL of
water, what are the resulting concentrations of calcium
2+ and hydroxide ions?
Ca2+ OH –
A)
B)
C)
D)
E)
2 M
2 M
4 M
8 M
4M
2 M
4 M
4 M
4 M
8M
12. An aqueous solution of concentrated HBr contains 48%
HBr (MM = 80.9) by mass. The density of the solution
is 1.50 g•mL –1. What is the molarity of the HBr
solution?
A) 5.9 M
C) 11.4 M
E) 40.0 M
B) 8.9 M
D) 18.5 M
What is the molarity of concentrated HCl?
B) 3.3 M
D) 9.9 M
14. Which statement accounts for the facts that:
I. Hydrogen chloride in a nonpolar solvent does not
conduct electricity.
II. A water solution of hydrogen chloride, HCl, is an
excellent conductor of electricity.
A)
B)
C)
D)
Water is an electrolyte.
Hydrogen chloride ionizes in water.
Hydrogen chloride is a nonelectrolyte.
Hydrogen chloride releases electrons in water
solutions.
E) Chlorine is a strong reducing agent.
15. A one mole solid sample of acetic acid (molecular wt.=
60 g/mol) is dissolved in 1.0 L of water to create a 1.0
molar solution. Which of the following would be the
best procedure for determining the molality of the
solution?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
The normality of the solution decreases.
The mole fraction of the solution increases.
The molarity of the solution remains the same.
The solution's molality does not change.
The density of the solution does not change.
17. How many milliliters of 11.5-molar HCOOH must be
diluted to obtain 23 L of 2.0-molar HCOOH?
A) 1000 mL
C) 3000 mL
E) 5000 mL
Finding the volume of the solute
Calculating the mass of the solvent
Determining the specific heat of the solution
Finding the normality of the solution
Multiplying the molarity value by a factor of a
thousand
B) 2000 mL
D) 4000 mL
18. How many milliliters of 4.5-M H2CO 3 must be diluted
to obtain 12.0L of 3.0-M H2CO 3?
A) 2000 mL
C) 4000 mL
E) 12000 mL
13.
A) 0.82 M
C) 6.8 M
E) 12.5 M
16. A student raises the temperature of an aqueous solution
of KBr from 313K to 363K. Which of the following
statements is true?
B) 2500 mL
D) 8000 mL
19. How many milliliters of 9.0-molar H 2CO 3 must be
diluted to obtain 3.0 L of 6.0-molar H 2CO 3?
A) 2000 mL
C) 1050 mL
E) 475 mL
B) 1175 mL
D) 575 mL
20. The weight of HC2H3O2 (molecular weight 60.0) in
20.0 milliliters of a 2.50-molar solution is
A) 2.50 grams
C) 6.00 grams
E) 30.0 grams
B) 3.00 grams
D) 25.0 grams
21. The weight of HNO 3 (molecular weight 63.0) in 40.0
milliliters of 5.00-molar solution is
A) 5.6 g
C) 10.4 g
E) 13.1 g
B) 8.7 g
D) 12.6 g
22. A 50.0 mL aliquot of a sulfuric acid solution was
treated with barium chloride and the resulting BaSO 4
was isolated and weighed. If 0.667 g of BaSO 4 was
obtained, what was the molarity of the H 2SO 4?
A) 0.00700 M
C) 0.0572 M
E) 1.43 M
B) 0.0286 M
D) 0.114 M
23. 1.0 mole of KCl(aq) is added to which solution to
produce a precipitate?
A) Ag+
B) Zn2+
C) Li +
D) Co2+
E) Ca2+
24. What is the [H3O+] in a solution formed by adding 60.0
mL of water to 40.0 mL of 0.040 M KOH?
A) 3.7 × 10 –15 M
C) 4.6 × 10 –11 M
E) 2.7 × 10 –7 M
B) 6.2 × 10–13 M
D) 3.1 × 10 –9 M
25. The salt Na2CO 3 undergoes hydrolysis to produce a
basic solution. What is the [OH–] in 0.100 M Na2CO 3?
A) 2.5 × 10 –3 M
C) 6.5 × 10 –3 M
E) 9.6 × 10 –5 M
B) 4.2 × 10–3 M
D) 7.2 × 10 –5 M
26. What is the percent by mass of NH 3CO 3 (molar mass 77. g) in a 2.0 M solution that has a
density of 1.1 g/mL?
A) 1.4% B) 2.6% C) 14.% D) 20.% E) 26.%
27. What is the molarity of a solution of NaF that is 14.%
solute by mass and has a density of 1.20 g/mL?
A) 0.50 M
C) 2.0 M
E) 4.0 M
B) 1.0 M
D) 3.0 M
28. What is the density of a 1.0 M solution of C 5H10O2 that
is 7.5% C5H10O2 by mass?
A) 1.0 g/mL
C) 3.0 g/mL
E) 1.4 g/mL
B) 0.50 g/mL
D) 1.5 g/mL
29. How much water must be added to 300. mL of a 7.00 M
HCl solution to reduce the concentration to 4.20 M?
A) 50.0 mL
C) 150. mL
E) 400. mL
B) 100. mL
D) 200. mL
30. When 110. grams of Mg(ClO4) 2 (molar mass of 220. g)
is dissolved in enough water to make 500. milliliters of
solution, what are the concentrations of the Mg 2+ and
ClO4– ions respectively?
A)
B)
C)
D)
E)
0.500 M and 1.00 M
0.500 M and 0.500 M
1.00 M and 1.00 M
1.00 M and 0.500 M
1.00 M and 2.00 M
31. CaSO 4 is LEAST soluble in which 0.5 Molar solution?
A) Ca(NO 3) 2
C) Fe(SO4)
E) NH 3
B) Fe 2(SO 4)3
D) Cr(SO4) 2
32. I. CH3–CH 2–CH 2–CH 3 II. OH–CH2–CH 2–CH 3 III.
OH–CH 2–CH 2–OH
Arrange these three chemicals in the order of
decreasing solubility
A) III < I < II
C) I < II < III
E) III < II < I
B) II < I < III
D) I < III < II
33. Aqueous solutions of sugar (C6H12O6), NaCl, and HCl
are all 10% solute by mass. Which represents them in
order of increasing molarity?
A)
B)
C)
D)
E)
HCl < NaCl < C6H 12O 6
NaCl < C 6H12O6 < HCl
C6H12O6 < HCl < NaCl
C6H12O6 < NaCl < HCl
NaCl < HCl < C6H12O6 34. Given that a solution is 10% glucose by mass, what
other information is needed to determine the molarity
of the solution?
I. The molar mass of glucose
II. The density of the solution
III. The temperature of the solution
A) I only
C) I and II
E) I, II, and III
B) III only
D) I and III
35. When 1 L of 1.0 M PbCl 2(aq) is mixed with 1 L of 2.0 M H2SO4(aq), what is the resulting concentration of
Pb2+?
A) 0.00 M
C) 2.00 M
E) 4.00 M
B) 1.00 M
D) 3.00 M
36. The vapor pressure of acetic acid is 200. mmHg at 80.0 o
C. What is the vapor pressure at 80.0oC of a solution
containing 0.250 mol of a non volatile substance
dissolved in 6.50 mol of acetic acid?
A) 193. mmHg
C) 207. mmHg
E) 214. mmHg
B) 200. mmHg
D) 186. mmHg
37. What is the vapor pressure of a 20.0% by mass solution
of C 6H14NO 5 (molar mass 180.) in water at 29ºC
(vapor pressure of pure water at 29.0ºC is 30.0 torr)?
A) 0.700 torr
C) 30.0 torr
E) 70.0 torr
B) 29.3 torr
D) 30.7 torr
38. A solution of a nonvolatile molecular solute in benzene
is prepared. Which describes what happens to the
freezing point, boiling point, and vapor pressure of the
solution compared to pure benzene?
A) Freezing point and boiling point increase, vapor
pressure decreases
B) F.P. and B.P. decrease, V.P. increases
C) F.P. decreases, V.P. and B.P. increase
D) F.P. and V.P. increase, B.P. decreases
E) F.P. and V.P. decrease, B.P. increases
39. Potassium Chloride, KCl, is less effective than an equal
mass of sodium chloride, NaCl, for raising the boiling
point of water because
A)
B)
C)
D)
E)
KCl is less soluble in water than NaCl.
KCl dissociates into fewer ions than the NaCl.
KCl(s) has a lower boiling point than NaCl(s).
KCl has a larger formula mass than NaCl.
NaCl forms hydrogen bonds and KCl does not.
40. What is the boiling point elevation if 29.0 g of KF is
dissolved in 500. g of a compound that has a Kb = 2.00ºC molal–1 ?
A) 2.00ºC
C) 8.00ºC
E) 20.0ºC
B) 4.00ºC
D) 10.0ºC
41. To find its molar mass, 6.00 g of a compound was
dissolved in 100. g of a compound that has a Kf =
6.00ºC molal –1. If the freezing point was lowered by
2.00ºC, what is the molar mass of the compound?
A) 2.00 g
C) 20.0 g
E) 200.g
B) 18.0 g
D) 180. g
42. When 228. g of K 2C2O2 (molar mass 144. g) is
dissolved in enough water to make 500.mL of solution,
what are the concentrations of the K+ and C2O22– ions
respectively?
A) 2.00 M and 4.00 M B) 4.00 M and 2.00 M
C) 4.00 M and 4.00 M D) 4.00 M and 8.00 M
E) 8.00 M and 4.00 M
43. Which of the following would have the highest boiling
point?
A)
B)
C)
D)
E)
a 1.5 M solution of AlCl 3
a 2.0 M solution of NaCl
a 2.5 M solution of Na2S
a 3.0 M solution of C 6H12O6
a 3.0 M solution of HCl
44. Which of the following would increase the boiling point
of a pure liquid in an open container?
I. Dissolving 1 mol of any solid solute into the liquid
II. Moving the liquid and container to a higher altitude
III. Increasing the number of moles of liquid in the
container
A) I only
C) III only
E) I, II, and III
B) II only
D) I and III only
45. As the concentration of HCl in aqueous solution
increases, which of the following decreases?
A)
B)
C)
D)
E)
Osmotic pressure
Boiling point
Temperature
Freezing point
Electrical conductivity
46. Which of the following aqueous solutions has the
lowest freezing point?
A)
B)
C)
D)
E)
0.10 M Magnesium Chloride: MgCl 2
0.10 M Sodium Phosphate: Na3PO 4
0.10 M Lithium Chloride: LiCl
0.10 M Hydrobromic acid: HBr
0.20 M fructose: C5H10O5
47. Why does a 1-molal solution of table salt (NaCl) have a
lower freezing point than a 1-molal solution of sugar
(C 6H12O6)?
A) Molecules of table salt are smaller than the
molecules of sugar.
B) Molecules of table salt have stronger bonds than
molecules are sugar.
C) Table salt is ionic and dissociates in water, sugar
does not.
D) Table salt contains metallic atoms, sugar does not.
E) Solid table salt has a different crystalline structure
than sugar.
48. The molality of a solution of an unknown non-ionic
solute can be determined by which of the following?
A)
B)
C)
D)
E)
Density of the solution
Temperature of the solution
BECAUSE
Freezing point depression of the solution
II. the atmospheric pressure decreases as the altitude
increases.
Volume of the solution
Mass of the solution
49. Base your answer to the following question on the types
of solids given below.
(A) A metallic solid
(B) A molecular solid with hydrogen bonds (C) A molecular solid with non-polar molecules
(D) A network solid
(E) An ionic solid
For solutions of equal molality, which would generally
have the greatest freezing point depression?
A) A
B) B
C) C
D) D
A)
B)
C)
D)
BECAUSE
II. the addition of antifreeze lowers the vapor pressure
of the water.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
explanation of I
53. I. An aqueous salt solution is a good conductor of
electricity
BECAUSE
II. the solution contains positive and negative ions.
A)
B)
C)
D)
BECAUSE
II. water has stronger intermolecular bonds.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
54. I. Addition of a non-volatile solute to a solvent causes
the freezing point of the solution to be lowered
E) I and II are BOTH TRUE and II IS a correct
explanation of I
51. I. At standard pressure, water has a higher boiling point
than alcohol
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
E) E
50. I. Addition of antifreeze to water lowers the freezing
point of the solution A)
B)
C)
D)
52. I. Water boils at a higher temperature at low altitudes
than at high altitudes
BECAUSE
II. the solute is always molecular.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
55. I. Antifreeze dissolved in water elevates the freezing
point
BECAUSE
58. Which graph represents the relationship between
solubility and temperature of most gases, such as NH3 ,
in water?
A)
B)
C)
D)
II. the antifreeze molecules prevent the water molecules
from crystallizing.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
E)
56. I. Ammonia gas will escape from a saturated water
solution when heated
BECAUSE
II. the solubility of gases decreases when the
temperature increases.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
57. When the two aqueous solutions of CoCl 2 and NaOH
are mixed, a precipitate forms.
CoCl2(aq) + NaOH(aq) ® Precipitate + Ions
What is the formula of the precipitate?
A) NaCl
C) NaOH
E) NaCl2
59. Which is the correct net ionic equation for the reaction
between water solutions of ammonium sulfide, (NH4 ) 2
S, and lead (II) nitrate, Pb(NO 3) 2?
A) Pb2+(aq) + S2–(aq) ® PbS(s)
B) NH 4+(aq) + NO3–(aq) ® NH 4NO 3(s)
C) 2 NH 4+(aq) + S2–(aq) + Pb2+(aq) + 2NO3–(aq) ® PbS(s) + 2 NH4+(aq) + 2 NO3–(aq)
D) 2 NH 4+(aq) + S2–(aq) + Pb2+(aq) + 2 NO3–(aq) ® 2 NH4NO3(s) + S2–(aq) + Pb2+(aq)
E) 2 NH 4+(aq) + S2–(aq) + Pb2+(aq) + 2 NO3–(aq) ®
PbS(s)
60. Note the chart of interactions of equal volumes of
various 0.100 M aqueous solutions. (Symbols of
elements or ions have been replaced by capital letters,
and soluble products are indicated.) What is the formula
of the precipitate?
B) CoCl2
D) Co(OH) 2
A) AX
B) BY
C) CX
D) DY
E) XY
Answer Key
AP Chemistry Solutions
1.
D
37.
B
2.
E
38.
E
3.
D
39.
D
4.
A
40.
A
5.
E
41.
D
6.
E
42.
E
7.
C
43.
C
8.
A
44.
A
9.
A
45.
D
10.
B
46.
B
11.
E
47.
C
12.
B
48.
C
13.
D
49.
E
14.
B
50.
D
15.
B
51.
E
16.
D
52.
E
17.
D
53.
E
18.
D
54.
A
19.
A
55.
B
20.
B
56.
E
21.
D
57.
D
22.
C
58.
A
23.
A
59.
A
24.
B
60.
A
25.
B
26.
A
27.
E
28.
E
29.
D
30.
E
31.
B
32.
E
33.
A
34.
A
35.
A
36.
A