1. What is the density of a 1.0 M solution of C5H10O2 that is
7.5% C5H10O2 by mass?
(A) 1.0 g/mL
(D) 1.5 g/mL
(B) 0.50 g/mL
(E) 1.4 g/mL
(C) 3.0 g/mL
2. 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
(D) 18.5 M
(B) 8.9 M
(E) 40.0 M
(C) 11.4 M
3. 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
(D) 3.0 M
(B) 1.0 M
(E) 4.0 M
(C) 2.0 M
4. 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
(D) D
(B) B
(E) E
(C) C
5. 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
(D) I and III
(B) III only
(E) I, II, and III
(C) I and II
6. 1.0 mole of KCl(aq) is added to which solution to
produce a precipitate?
(A) Ag+
(D) Co2+
(B) Zn2+
(E) Ca2+
+
(C) Li
7. Which of the following would have the highest boiling
point?
(A) a 1.5 M solution of AlCl3
(B) a 2.0 M solution of NaCl
(C) a 2.5 M solution of Na2S
(D) a 3.0 M solution of C6H12O6
(E) a 3.0 M solution of HCl
8. 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
(D) 3.1 × 10–9 M
–13
(B) 6.2 × 10 M
(E) 2.7 × 10–7 M
(C) 4.6 × 10–11 M
9. CaSO4 is LEAST soluble in which 0.5 Molar solution?
(A) Ca(NO3)2
(B) Fe2(SO4)3
(C) Fe(SO4)
(D) Cr(SO4)2
(E) NH3
10. I. CH3–CH2–CH2–CH3
II. OH–CH2–CH2–CH3
III. OH–CH2–CH2–OH
Arrange these three chemicals in the order of decreasing
solubility
(A) III < I < II
(D) I < III < II
(B) II < I < III
(E) III < II < I
(C) I < II < III
11. 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
(D) I and III only
(B) II only
(E) I, II, and III
(C) III only
12. 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
(D) 180. g
(B) 18.0 g
(E) 200.g
(C) 20.0 g
13. When 110. grams of Mg(ClO4)2 (molar mass of 220. g) is
dissolved in enough water to make 500. mililiters of
solution,
what are the concentrations of the Mg2+ and ClO
–
ions
respectively?
4
(A) 0.500 M and 1.00 M
(D) 1.00 M and 0.500 M
(B) 0.500 M and 0.500 M (E) 1.00 M and 2.00 M
(C) 1.00 M and 1.00 M
17. A solution of Na+ ions would be best represented by
which picture?
(A)
14.
(B)
What is the molarity of concentrated HCl?
(A) 0.82 M
(D) 9.9 M
(B) 3.3 M
(E) 12.5 M
(C) 6.8 M
15. As temperature increases, solubility of which of the
following decreases?
(A) NH3
(B) NH4Cl
(C) NaNO3
(D) KCl
(E) KI
(C)
16. Of the following organic compounds, which is LEAST
soluble in water at 298 K?
(A) C6H6, benzene
(B) CH3Cl, chloromethane
(C) C2H5OH, ethanol
(D) C2H5COOH, propanoic acid
(E) C5H10O5, fructose
(D)
(E)
18. When 228. g of K2C2O2 (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
(D) 4.00 M and 8.00 M
(B) 4.00 M and 2.00 M
(E) 8.00 M and 4.00 M
(C) 4.00 M and 4.00 M
19. The weight of HC2H3O2 (molecular weight 60.0) in 20.0
milliliters of a 2.50-molar solution is
(A) 2.50 grams
(D) 25.0 grams
(B) 3.00 grams
(E) 30.0 grams
(C) 6.00 grams
20. What is the vapor pressure of a 20.0% by mass solution
of C6H14NO5 (molar mass 180.) in water at 29ºC (vapor
pressure of pure water at 29.0ºC is 30.0 torr)?
(A) 0.700 torr
(D) 30.7 torr
(B) 29.3 torr
(E) 70.0 torr
(C) 30.0 torr
21. 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) Water is an electrolyte.
(B) Hydrogen chloride ionizes in water.
(C) Hydrogen chloride is a nonelectrolyte.
(D) Hydrogen chloride releases electrons in water
solutions.
(E) Chlorine is a strong reducing agent.
22. What is the mole fraction of HF in a 10.% (by mass)
solution?
(A) 0.090
(D) 0.90
(B) 0.10
(E) 0.91
(C) 0.18
23. Why does a 1-molal solution of table salt (NaCl) have a
lower freezing point than a 1-molal solution of sugar
(C6H12O6)?
(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.
24. The salt Na2CO3 undergoes hydrolysis to produce a basic
solution. What is the [OH–] in 0.100 M Na2CO3?
(A) 2.5 × 10–3 M
(D) 7.2 × 10–5 M
(B) 4.2 × 10–3 M
(E) 9.6 × 10–5 M
(C) 6.5 × 10–3 M
25. A student rasies the temperature of an aqueous solution
of KBr from 313K to 363K. Which of the following
statements is true?
(A) The normality of the solution decreases.
(B) The mole fraction of the solution increases.
(C) The molarity of the solution remains the same.
(D) The solution's molality does not change.
(E) The density of the solution does not change.
26. 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
(D) 175 g/mol
(B) 140 g/mol
(E) 200 g/mol
(C) 167 g/mol
27. The molality of a solution of an unknown non-ionic
solute can be determined by which of the following?
(A) Density of the solution
(B) Temperature of the solution
(C) Freezing point depression of the solution
(D) Volume of the solution
(E) Mass of the solution
28. 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) Finding the volume of the solute
(B) Calculating the mass of the solvent
(C) Determining the specific heat of the solution
(D) Finding the normality of the solution
(E) Multiplying the molarity value by a factor of a
thousand
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
(D) 200. mL
(B) 100. mL
(E) 400. mL
(C) 150. mL
30. 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) 2 M
2M
(B) 2 M
4M
(C) 4 M
4M
(D) 8 M
4M
(E) 4 M
8M
31. Which of the following aqueous solutions has the lowest
freezing point?
(A) 0.10 M Magnesium Chloride: MgCl2
(B) 0.10 M Sodium Phosphate: Na3PO4
(C) 0.10 M Lithium Chloride: LiCl
(D) 0.10 M Hydrobromic acid: HBr
(E) 0.20 M fructose: C5H10O5
32. What is the percent by mass of NH3CO3
(molar mass 77. g) in a 2.0 M solution that has a density
of 1.1 g/mL?
(A) 1.4%
(D) 20.%
(B) 2.6%
(E) 26.%
(C) 14.%
33. The weight of HNO3 (molecular weight 63.0) in 40.0
milliliters of 5.00-molar solution is
(A) 5.6 g
(D) 12.6 g
(B) 8.7 g
(E) 13.1 g
(C) 10.4 g
34. As the concentration of HCl in aqueous solution
increases, which of the following decreases?
(A) Osmotic pressure
(D) Freezing point
(B) Boiling point
(E) Electrical conductivity
(C) Temperature
35. A 50.0 mL aliquot of a sulfuric acid solution was treated
with barium chloride and the resulting BaSO4 was
isolated and weighed. If 0.667 g of BaSO4 was obtained,
what was the molarity of the H2SO4?
(A) 0.00700 M
(D) 0.114 M
(B) 0.0286 M
(E) 1.43 M
(C) 0.0572 M
36. When 1 L of 1.0 M PbCl2(aq) is mixed with 1 L of
2.0 M H2SO4(aq), what is the resulting concentration of
Pb2+?
(A) 0.00 M
(D) 3.00 M
(B) 1.00 M
(E) 4.00 M
(C) 2.00 M
37. How many milliliters of 9.0-molar H2CO3 must be
diluted to obtain 3.0 L of 6.0-molar H2CO3?
(A) 2000 mL
(D) 575 mL
(B) 1175 mL
(E) 475 mL
(C) 1050 mL
38. The vapor pressure of acetic acid is 200. mmHg at 80.0o
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
(D) 186. mmHg
(B) 200. mmHg
(E) 214. mmHg
(C) 207. mmHg
39. 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
(D) 10.0ºC
(B) 4.00ºC
(E) 20.0ºC
(C) 8.00ºC
40. How many milliliters of 11.5-molar HCOOH must be
diluted to obtain 23 L of 2.0-molar HCOOH?
(A) 1000 mL
(D) 4000 mL
(B) 2000 mL
(E) 5000 mL
(C) 3000 mL
41. 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) pure element
(D) heterogeneous solution
(B) pure compound
(E) homogeneous solution
(C) a colloid
42. 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
43. The table below summarizes the result as 0.10 M
solutions are mixed.
Which substance is a precipitate in this experiment?
(A) KCl
(B) NaCN
(C) NaCl
(D) Zn(NO3)2
(E) Cd(OH)2
44. 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
(A) 8%
(D) 16%
(B) 14%
(E) 30%
(C) 15%
45. Aqueous solutions of sugar (C6H12O6), NaCl, and HCl
are all 10% solute by mass. Which represents them in
order of increasing molarity?
(A) HCl < NaCl < C6H12O6
(B) NaCl < C6H12O6 < HCl
(C) C6H12O6 < HCl < NaCl
(D) C6H12O6 < NaCl < HCl
(E) NaCl < HCl < C6H12O6
47. Potassium Chloride, KCl, is less effective than an equal
mass of sodium chloride, NaCl, for raising the boiling
point of water because
(A) KCl is less soluble in water than NaCl.
(B) KCl dissociates into fewer ions than the NaCl.
(C) KCl(s) has a lower boiling point than NaCl(s).
(D) KCl has a larger formula mass than NaCl.
(E) NaCl forms hydrogen bonds and KCl does not.
46. Which compound has the highest conductivity?
(A) HF
(B) H2O
(C) CaSO4
(D) HNO3
(E) Pb(OH)2
48. Which of the following dissolves in water to form an
ionic solution?
(A) O2
(B) SiO2
(C) KMnO4
(D) C12H22O11
(E) CH4
49. How many milliliters of 4.5-M H2CO3 must be diluted to
obtain 12.0L of 3.0-M H2CO3?
(A) 2000 mL
(D) 8000 mL
(B) 2500 mL
(E) 12000 mL
(C) 4000 mL
Answer Key
1.
E
30.
E
2.
B
31.
B
3.
E
32.
A
4.
E
33.
D
5.
A
34.
D
6.
A
35.
C
7.
C
36.
A
8.
B
37.
A
9.
B
38.
A
10.
E
39.
A
11.
A
40.
D
12.
D
41.
E
13.
E
42.
E
14.
D
43.
E
15.
A
44.
B
16.
A
45.
A
17.
E
46.
D
18.
E
47.
D
19.
B
48.
C
20.
B
49.
D
21.
B
22.
A
23.
C
24.
B
25.
D
26.
D
27.
C
28.
B
29.
D