Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 1. A substance that does not dissolve in a solvent is said to be: c. miscible d. soluble a. insoluble b. immiscible
____ 2. An example of a suspension is: a. blood b. gelatin c. milk d. muddy water
____ 3. A _____ contains the maximum amount of dissolved solute for a given amount of solvent. a. saturated c. suspended b. supersaturated
____ 4. _____ solutions are very unstable. a. saturated b. supersaturated d. unsaturated c. suspended d. unsaturated
____ 5. A water solution containing an unknown quantity of a nonelectrolyte solute has a freezing point of –0.21ºC.
What is the molal concentration of the solution if K f
= –1.86ºC/m? a. 0.11 m c. 1.11 m d. 1.12 m b. 0.12 m
____ 6. What does NOT change when a solution is diluted by the addition of solvent? a. volume of solvent c. number of moles of solute d. molarity of solution b. mass of solvent
____ 7. Which of the following is NOT a colligative property of a solution? a. boiling point elevation c. vapor pressure lowering b. supersaturation d. freezing point depression
____ 8. Illustrated is a phenomenon know as the: a. Brownian effect b. Colloidal effect c. Suspension effect d. Tyndall effect
____ 9. A solute depresses the freezing point because the solute ____. a. is colder than the solvent

b. disrupts crystal formation of the solvent c. tends to sink to the bottom of the solution d. has bigger molecules than the solvent
____ 10. What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved? a. 2.0
M c. 0.40
M b. 10 M d. 4.0
M
____ 11. More solute can be dissolved in a _____ solution: a. saturated b. supersaturated c. suspended d. unsaturated
____ 12. Colligative properties depend on a. the identity of the solute particles. b. the concentration of the solute particles. c. the physical properties of the solute particles. d. the boiling point and freezing point of the solution.
____ 13. A substance that dissolves in a solvent is said to be: a. insoluble b. immiscible c. miscible d. soluble
____ 14. What is the approximate freezing-point depression of a 0.020 m aqueous NaBr solution? a. –0.0093ºC b. –0.019ºC c. –0.037ºC d. –0.074ºC
____ 15. The image illustrates what is formed from a _____ solution. a. saturated b. supersaturated
____ 16. The liquid illustrated is an example of a/an: c. suspended d. unsaturated

a. colloid b. suspension c. solution d. solvent
____ 17. A heterogeneous mixture of intermediate sized particles is a: a. colloid b. solute c. solvent d. suspension
____ 18. A mixture containing particles that settle out if left undisturbed is a: a. colloid b. solute c. solvent d. suspension
____ 19. Two liquids that are soluble in each other in any proportion are said to be: a. insoluble b. immiscible c. miscible d. soluble
____ 20. Two liquids that can be mixed together but separate shortly after are: a. immiscible b. insoluble c. miscible d. soluble
____ 21. A _____ solution contains more dissolved solute than a saturated solution at the same temperature. a. saturated b. supersaturated c. suspended d. unsaturated
Completion
Complete each statement.
22. The type of solution formed by creek water after heavy rain is called ____________________.
23. A substance that does not dissolve in a solvent is said to be ____________________ in that solvent.
24. The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure is called ____________________.
25. The process of surrounding solute particles with solvent particles to form a solution is called
____________________.
26. A measure of the amount of solute dissolved in a specific amount of solvent or solution is called the
____________________ of the solution.
Short Answer
27. Why does a soft drink lose its fizz after it has been opened and left with a lid on the container?

28. Calculate the molarity of the solution.
29. What is the relationship between temperature and solubility of substances?
30. Calculate the moles of camphor dissolved in phenol. The molar mass of camphor is 152 g/mol.
31. The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure is called ____________________.
32. The temperature difference between a solution’s freezing point and a pure solvent’s freezing point is called the _______________.
33. The temperature difference between a solution’s boiling point and a pure solvent’s boiling point is called the
_______________.
34. In the lab, a chemist adds 3.6 grams of sodium chloride to 100.0 g of water. What is the molarity of the solution?

Problem
35. Calculate the moles of camphor dissolved in 1.32 L of phenol. The molarity of the solution is 6.01 M.
36. What is the freezing point depression of a solution containing 1.29 m of solute dissolved in water? The K f
of water is -1.86°C/ m .
37. If a 4.2 M solution contains 5.1 mol of solute, what is the volume of the solution?
38. What is the boiling point elevation of a solution containing 0.949 m of sucrose in 100.0 g of water? The molal elevation constant of water is 0.512°C/ m .
39. What is the molarity of a solute solution that contains 0.781 mol of in 3.5 L of a solution?
40. Calculate the molarity of a solution if 3.55 mol of solute is dissolved in 2.30 L of solution

MULTIPLE CHOICE
1. ANS: A
2. ANS: D
3. ANS: A
4. ANS: B
5. ANS: A
6. ANS: C
7. ANS: B
8. ANS: D
9. ANS: B
10. ANS: B
11. ANS: D
12. ANS: B
13. ANS: D
14. ANS: D
15. ANS: B
16. ANS: A
17. ANS: A
18. ANS: D
19. ANS: C
20. ANS: A
21. ANS: B
COMPLETION
22. ANS: suspension
23. ANS: insoluble
24. ANS: solubility
25. ANS: solvation
26. ANS: concentration
SHORT ANSWER
27. ANS: The fizz is dissolved carbon dioxide which has been dissolved into the drink at a pressure much higher than atmospheric pressure. Opening the container and leaving it exposed to air at normal pressure causes the dissolved carbon dioxide to escape into the air. The loss of carbon dioxide causes the drink to lose its fizz.
28. ANS: 0.4 M
29. ANS: The relationship between temperature and solubility varies from one solute to another. The solubility increases in most substances with an increase in temperature, but in a few substances, the solubility decreases with an increase in temperature.

30. ANS: 0.0522 mol
31. ANS: Solubility
32. ANS: Freezing Point Depression
33. ANS: Boiling Point Elevation
34. ANS: 077 mol NACL / .1000 kg H
2
0 = .77 mol/kg
PROBLEM
35. ANS: 0.0522 mol
36. ANS: 2.40 °C
37. ANS: 1.21 L
38. ANS: Boiling point elevation 0.256°C.
39. ANS: 0.22 M
40. ANS: 1.54 M