Chapter 15 Items
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1. The intermolecular forces between particles in a liquid can involve all of the following except
a. London dispersion forces.
c. dipole-dipole attractions.
b. hydrogen bonding.
d. gravitational forces.
2.
a.
b.
c.
d.
The intermolecular forces between particles are
weaker in solids than in liquids.
stronger in gases than in solids.
equal in strength in gases and in liquids.
stronger in liquids than in gases.
3.
a.
b.
c.
d.
Which of these best describes vaporization?
the process by which a liquid changes to a gas
the process by which a solid changes to a gas
Both (a) and (b)
Neither (a) nor (b)
4. Which term best describes the process by which particles escape from the surface of a nonboiling liquid and enter the gas
state?
a. sublimation
c. surface tension
b. evaporation
d. aeration
5.
a.
b.
c.
d.
The difference between crystalline and amorphous solids is determined by
temperature changes.
pressure when the substances are formed.
amount of order in particle arrangement.
strength of molecular forces.
6.
a.
b.
c.
d.
Compared with a crystalline solid, the particles in an amorphous solid
occur in a random pattern.
occur in a definite, three-dimensional arrangement.
consist of molecular sheets.
have a more complex unit cell.
7. Water in air is an example of which solute-solvent combination?
a. gas-liquid
c. liquid-liquid
b. liquid-gas
d. gas-gas
8. Carbon dioxide dissolved in water is an example of which solute-solvent combination?
a. gas-liquid
c. liquid-liquid
b. liquid-gas
d. cannot be determined
9. Sugar dissolved in water is an example of which solute-solvent combination?
a. gas-liquid
c. solid-liquid
b. liquid-liquid
d. liquid-solid
10. Which mixture is made up of the smallest particles?
a. milk
c. shaving cream
b. salt water
d. muddy water
11. Which mixture contains visible particles that settle out unless the mixture is stirred?
a. a colloid
c. a solution
b. a homogeneous mixture
d. a suspension
12. A metal solution is a(n)
a. colloid.
b. alloy.
c.
d.
suspension.
emulsion.
13. A substance whose water solution is a good conductor of electricity is a(n)
a. nonelectrolyte.
c. nonpolar substance.
b. electrolyte.
d. solute.
14. Which of the following is an electrolyte?
a. sodium chloride
b. sugar
c.
d.
pure water
glass
15. Which of the following does not increase the rate of dissolving a solid in water?
a. raising the temperature of the water
b. stirring the solution
c. using larger pieces of solid
d. crushing the solid
16. Increasing the surface area of the solute
a. increases the rate of dissolution.
b. decreases the rate of dissolution.
c. has no effect on the rate of dissolution.
d. can increase, decrease, or have no effect on the rate of dissolution.
17. Which of the following will dissolve most rapidly?
a. sugar cubes in cold water
c. powdered sugar in cold water
b. sugar cubes in hot water
d. powdered sugar in hot water
18. In a solution at equilibrium,
a. no dissolution occurs.
b. the rate of dissolution is less than the rate of crystallization.
c. the rate of dissolution is greater than the rate of crystallization.
d. the rate of dissolution and the rate of crystallization are equal.
19. "Like dissolves like" is a very general rule used for predicting whether
a. one substance will form a solution with another.
b. one substance will react with another.
c. a reaction will reach equilibrium.
d. a mixture will contain two or three phases.
20. Which of the following is an example of a polar solvent?
a. carbon tetrachloride
c. water
b. benzene
d. gasoline
21. What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution?
a. 0.0132 M
c. 0.459 M
b. 0.0253 M
d. 1.363 M
22. What is the molality of a solution that contains 5.10 mol KNO3 in 4.47 kg water? (molar mass of KNO3 = 101.11 g/mol)
a. 0.315 m
c. 1.02 m
b. 0.779 m
d. 1.14 m
23. What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution? (molar mass of NaCl = 58.44 g/mol)
a. 0.535 M
c. 8.56 M
b. 2.14 M
d. 31.3 M
24. What is the molality of a solution that contains 31.0 g HCl in 5.00 kg water? (molar mass of HCl = 36.46 g/mol)
a. 0.062 m
c. 0.170 m
b. 0.425 m
d. 15.5 m
25. How many moles of HCl are present in 0.70 L of a 0.33 M HCl solution? (molar mass of HCl = 36.46 g/mol)
a. 0.23 mol
c. 0.38 mol
b. 0.28 mol
d. 0.47 mol
26. The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water. How much NaCl is in the solution?
(molar mass of NaCl = 58.44 g/mol)
a. 2.00 g
c. 117 g
b. 89.3 g
d. 224 g
27. An NaOH solution contains 1.90 mol of NaOH, and its concentration is 0.555 M. What is its volume? (molar mass of NaOH =
40.00 g/mol)
a. 0.623 L
c. 1.05 L
b. 0.911 L
d. 3.42 L
28. What mass of water must be used to make a 1.35 m solution that contains 8.20 mol of NaOH? (molar mass of NaOH = 40.00
g/mol)
a. 6.07 kg
c. 11.1 kg
b. 7.44 kg
d. 14.5 kg
29. How many milliliters of a 0.171 M solution contain 1.00 g of NaCl? (molar mass of NaCl = 58.44 g/mol)
a. 100. mL
c. 171 mL
b. 1000. mL
d. 17.1 mL
30. Pure liquids boil at higher temperatures under high pressures than they do under low pressures, because —
a. liquid molecules are closer together at higher pressures
b. it takes a higher temperature for the vapor pressure to equal the higher external pressure
c. vapor molecules are farther apart at higher pressures
d. the vapor diffuses more rapidly at higher pressures
31. Which one of the following statements is false?
a. Gases are generally more soluble in water under high pressures than under low pressures.
b. As temperature increases, the solubilities of solids in water increase.
c. Water dissolves many ionic solutes because of its ability to hydrate ions in solution.
d. Many solids dissolve more quickly in a cold solvent than in a warm solvent.
32. The solubility of a gas in a liquid would be increased by
a. the addition of an electrolyte.
b. the addition of an emulsifier.
c. agitation of the solution.
d. an increase in its partial pressure.
33. A saturated solution can become supersaturated under which of the following conditions?
a. It contains electrolytes.
b. A heated saturated solution is allowed to cool.
c. More solvent is added.
d. More solute is added.
34. Molarity is expressed in units of
a. moles of solute per liter of solution.
b. liters of solution per mole of solute.
c. moles of solute per liter of solvent.
d. liters of solvent per mole of solute.
35. What mass of NaOH is contained in 2.5 L of a 0.010 M solution?
a. 0.010 g
b. 1.0 g
c. 2.5 g
d. 0.40 g
36. A phase diagram relates the state of matter, pressure, and
a. temperature.
b. volume.
c. mass.
d. weight.
37. On a phase diagram, the point at which all equilibrium lines join is the
a. melting point.
b. boiling point.
c. critical point.
d. triple point.
38. If energy as heat is removed, most liquids will eventually
a. freeze.
b. burn.
c. evaporate.
d. diffuse.
39. The process of changing from a solid to a gas is known as
a. condensation.
b. sublimation.
c. deposition.
d. vaporization.
Use this figure to answer the following questions.
40. A solution containing 35 g of Li2SO4 dissolved in 100 g of water is heated from 10°C to 90°C. According to information in the
figure, this temperature change would result in
a. an additional 5 g of Li2SO4 in solution.
b. an additional 30 g of Li2SO4 in solution.
c. 5 g of Li2SO4 precipitate.
d. no change in Li2SO4 concentration.
41. According to saturation curves shown in the figure, which of the following solutions is supersaturated?
a. 40 g of NaCH3COO in 100 g of water at 40°C
b. 140 g of NaCH3COO in 100 g of water at 80°C
c. 80 g of NaCH3COO in 100 g of water at 40°C
d. 80 g of NaCH3COO in 200 g of water at 40°C
42. In 100 mL of cold water, 35 g of NaCl will dissolve, but 70 g will not. This observation implies that
a. solubility depends on temperature.
b. in order to dissolve more NaCl, you must increase the pressure.
c. solubility depends on the amounts of solute and solvent present.
d. NaCl is not easily hydrated.
Match the letter on the diagram with the term for that point or region.
43. Critical point
44. Vapor
45. Normal freezing point
46. Triple point
47. Solid
48. Normal boiling point
49. Liquid
50. Critical pressure
Chapter 15 Items
Answer Section
MULTIPLE CHOICE
1. D
2. D
3. C
4. B
5. C
6. A
7. B
8. A
9. C
10. B
11. D
12. B
13. B
14. A
15. C
16. A
17. D
18. D
19. A
20. C
21. B
Solution:
22. D
Solution:
23. A
Solution:
24. C
Solution:
25. A
Solution:
26. C
Solution:
27. D
Solution:
28. A
Solution:
29. A
Solution:
30. B
31. D
32. D
33. B
34. A
35. B
36. A
37. D
38. A
39. B
40. A
41. A
42. C
SHORT ANSWER
43. C
44. E
45. G
46. A
47. D
48. F
49. B
50. H