Name: ______________________
Class: _________________
Date: _________
ID: A
chpt 15 review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Which of the following is primarily responsible for holding water molecules together in the liquid state?
a. dispersion forces
b. hydrogen bonds
c. ionic bonds
d. polar covalent bonds
____
2. Which atom in a water molecule has the greatest electronegativity?
a. one of the hydrogen atoms
b. both hydrogen atoms
c. the oxygen atom
d. There is no difference in the electronegativities of the atoms in a water molecule.
____
3. What is primarily responsible for the surface tension of water?
a. dispersion forces
b. hydrogen bonding
c. ionic attractions
d. covalent bonding
____
4. Which is responsible for the high thermal energy required to melt ice?
a. covalent bonding
b. dispersion forces
c. hydrogen bonding
d. ionic attractions
____
5. A solution has which of the following properties?
a. Gravity separates its parts.
b. The top layer is different in composition than the bottom layer.
c. The average diameter of its solute particles usually is less than 1 nm.
d. A filter can remove the solute.
____
6. What occurs in solvation?
a. Solute ions separate from solvent molecules.
b. Solvent molecules surround solute ions.
c. Solvent molecules bind covalently to solute molecules.
d. Ionic compounds are formed.
____
7. Which of these compounds is likely to have very low solubility in water?
a. NaCl
b. HCl
c. CF 4
d.
CuSO 4
1
Name: ______________________
____
____
ID: A
8. Which compound would you expect to be soluble in the nonpolar solvent carbon disulfide?
a. H 2 O
b.
CI 4
c.
d.
NaCl
SnS 2
9. What type of compound is always an electrolyte?
a. polar covalent
b. nonpolar covalent
c. ionic
d. network solid
____ 10. Which of the following compounds conducts electricity only in the molten state?
a. sodium bromide
b. magnesium sulfate
c. calcium hydroxide
d. barium sulfate
____ 11. Which of the following compounds is an electrolyte in aqueous solution?
a. methanol
b. sugar
c. carbon tetrachloride
d. sodium hydroxide
____ 12. Which of the following are weak electrolytes in water?
a. ionic compounds that partially dissociate in water
b. ionic compounds that are soluble
c. polar compounds that ionize
d. nonpolar compounds that do not ionize
____ 13. Which of the following compounds is a strong electrolyte?
a. ammonia
b. acetic acid
c. sucrose
d. potassium sulfate
____ 14. Which of these materials is a hydrate?
a. baking soda
b. saltwater
c. Epsom salt
d. sugar
____ 15. Which of the following mixture types can be filtered to remove solute?
a. suspensions only
b. colloids only
c. suspensions and colloids
d. suspensions and solutions
2
Name: ______________________
____ 16. An
a.
b.
c.
d.
ID: A
emulsion is which type of mixture?
suspension
colloid
solution
gaseous
____ 17. Which of these statements is correct?
a. Particles can be filtered from a suspension.
b. A solution is heterogeneous.
c. A colloidal system does not exhibit the Tyndall effect.
d. The particles in a colloidal system are affected by gravity.
____ 18. Which of the following usually makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles
____ 19. What is the solubility of silver nitrate if 11.1 g can dissolve in 5.0 g of water at 20°C?
2.2 g
a.
at 20°C
100 g H 2 O
b.
45 g
at 20°C
100 g H 2 O
c.
22.2 g
at 20°C
100 g H 2 O
d.
222 g
at 20°C
100 g H 2 O
____ 20. Which of the following generally occurs as temperature increases?
a. Solubility of a solid solute decreases.
b. Solubility of a solid solute increases.
c. Solubility of a solid solute remains the same.
d. Molarity of a solid solute doubles.
____ 21. Which phrase correctly describes the effect of pressure on the solubility of a gas in a liquid?
a. proportional to the square root of the pressure of the gas above the liquid
b. directly proportional to the pressure of the gas above the liquid
c. inversely proportional to the pressure of the gas above the liquid
d. unrelated to the pressure of the gas above the liquid
____ 22. What happens to the solubility of a gas in a liquid if the partial pressure of the gas above the liquid
decreases?
a. The solubility decreases.
b. The solubility increases.
c. The solubility remains the same.
d. The solubility cannot be determined.
3
Name: ______________________
ID: A
____ 23. What is the concentration of a solution that contains 6 moles of solute in 2 liters of solution?
a. 6M
b. 12M
c. 7M
d. 3M
____ 24. In which of the following is the solution concentration expressed in terms of molarity?
10 g of solute
a.
1000 gof solution
10 g of solute
b.
1000 mL of solution
10 mL of solute
c.
1 L of solution
10 mol of solute
d.
1 L of solution
____ 25. Which of the following operations yields the number of moles of solute?
a. molarity × moles of solution
b. molarity × liters of solution
c. molarity × mass of solution
d. moles of solution ÷ volume of solution
____ 26. What is the number of moles of solute in 250 mL of a 0.4M solution?
a. 0.1 mol
b. 0.16 mol
c. 0.62 mol
d. 1.6 mol
____ 27. What mass of Na 2 SO 4 is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g)
a.
b.
c.
d.
178
284
356
710
g
g
g
g
____ 28. Which of the following is unchanged when a solution is diluted by the addition of solvent?
a. volume of solvent
b. mass of solvent
c. number of moles of solute
d. molarity of solution
____ 29. To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI
solution. What is the molarity of the new solution?
a. 180M
b. 2.8M
c. 0.35M
d. 0.18M
4
Name: ______________________
ID: A
____ 30. What measures are used to calculate the percent by volume of a solution?
a. mass of solute and volume of solvent
b. mass of solute and volume of solution
c. volume of solute and volume of solvent
d. volume of solute and volume of solution
____ 31. If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of
solute in solution?
a. 8.0 g
b. 50 g
c. 80 g
d. 800 g
____ 32. In which of the following is concentration expressed in percent by volume?
10 mL of solute
a.
× 100%
100 mL of solvent
10 mL of solute
b.
× 100%
100 mL of solution
10 g of solute
c.
× 100%
100 mL of solvent
10 g of solute
d.
× 100%
100 mL of solution
____ 33. Which of the following is a colligative property of a solution?
a. boiling point elevation
b. melting point elevation
c. vapor pressure increase
d. freezing point increase
____ 34. Which of the following is an expression of molality?
10 mol of solute
a.
1 kg of solvent
10 mol of solute
b.
1 L of solution
10 mol of solute
c.
1 L of solvent
10 mol of solute
d.
1 kg of solution
____ 35. To
a.
b.
c.
d.
which of the following variables is change in boiling point directly proportional?
molarity of solution
molality of solution
percent by volume of solution
percent (mass/mass) of solution
5
ID: A
chpt 15 review
Answer Section
MULTIPLE CHOICE
1. ANS: B
PTS: 1
DIF: L1
REF: p. 489
OBJ: 15.1.1 Identify the factor that causes the high surface tension, low vapor pressure, and high
boiling point of water.
BLM: comprehension
2. ANS: C
PTS: 1
DIF: L1
REF: p. 489
OBJ: 15.1.1 Identify the factor that causes the high surface tension, low vapor pressure, and high
boiling point of water.
BLM: comprehension
3. ANS: B
PTS: 1
DIF: L2
REF: p. 490
OBJ: 15.1.1 Identify the factor that causes the high surface tension, low vapor pressure, and high
boiling point of water.
BLM: comprehension
4. ANS: C
PTS: 1
DIF: L2
REF: p. 492
OBJ: 15.1.2 Describe the structure of ice.
BLM: application
5. ANS: C
PTS: 1
DIF: L1
REF: p. 494
OBJ: 15.2.1 Identify the types of substances that dissolve most readily in water.
BLM: comprehension
6. ANS: B
PTS: 1
DIF: L1
REF: p. 495
OBJ: 15.2.1 Identify the types of substances that dissolve most readily in water.
BLM: comprehension
7. ANS: C
PTS: 1
DIF: L2
REF: p. 494
OBJ: 15.2.1 Identify the types of substances that dissolve most readily in water.
BLM: application
8. ANS: B
PTS: 1
DIF: L2
REF: p. 495
OBJ: 15.2.1 Identify the types of substances that dissolve most readily in water.
BLM: application
9. ANS: C
PTS: 1
DIF: L1
REF: p. 496
OBJ: 15.2.2 Explain why all ionic compounds are electrolytes.
BLM: knowledge
10. ANS: D
PTS: 1
DIF: L2
REF: p. 496
OBJ: 15.2.2 Explain why all ionic compounds are electrolytes.
BLM: comprehension
11. ANS: D
PTS: 1
DIF: L2
REF: p. 497
OBJ: 15.2.2 Explain why all ionic compounds are electrolytes.
BLM: application
12. ANS: A
PTS: 1
DIF: L2
REF: p. 497
OBJ: 15.2.2 Explain why all ionic compounds are electrolytes.
BLM: application
13. ANS: D
PTS: 1
DIF: L2
REF: p. 497
OBJ: 15.2.2 Explain why all ionic compounds are electrolytes.
BLM: application
14. ANS: C
PTS: 1
DIF: L1
REF: p. 499
OBJ: 15.2.3 Explain why hydrates easily lose and regain water.
BLM: knowledge
1
ID: A
15. ANS:
OBJ:
BLM:
16. ANS:
OBJ:
BLM:
17. ANS:
OBJ:
BLM:
18. ANS:
OBJ:
BLM:
19. ANS:
OBJ:
BLM:
20. ANS:
OBJ:
BLM:
21. ANS:
OBJ:
BLM:
22. ANS:
OBJ:
BLM:
23. ANS:
OBJ:
24. ANS:
OBJ:
BLM:
25. ANS:
OBJ:
BLM:
26. ANS:
OBJ:
27. ANS:
OBJ:
28. ANS:
OBJ:
BLM:
29. ANS:
OBJ:
BLM:
30. ANS:
OBJ:
BLM:
31. ANS:
OBJ:
BLM:
A
PTS: 1
DIF: L1
REF: p. 504 | p. 505
15.3.1 Distinguish between a suspension and a solution.
knowledge
B
PTS: 1
DIF: L1
REF: p. 507
15.3.2 Identify how to distinguish a colloid from a suspension and a solution.
knowledge
A
PTS: 1
DIF: L2
REF: p. 494 | p. 504 | p. 505 | p. 506
15.3.2 Identify how to distinguish a colloid from a suspension and a solution.
application
A
PTS: 1
DIF: L1
REF: p. 519
16.1.1 Identify the factors that affect how fast a substance dissolves.
knowledge
D
PTS: 1
DIF: L2
REF: p. 521
16.1.3 Describe the factors that affect the solubility of a substance.
analysis
B
PTS: 1
DIF: L2
REF: p. 521
16.1.3 Describe the factors that affect the solubility of a substance.
comprehension
B
PTS: 1
DIF: L2
REF: p. 523
16.1.3 Describe the factors that affect the solubility of a substance.
comprehension
A
PTS: 1
DIF: L1
REF: p. 523 | p. 524
16.1.3 Describe the factors that affect the solubility of a substance.
knowledge
D
PTS: 1
DIF: L1
REF: p. 526
16.2.1 Calculate the molarity of a solution.
BLM: analysis
D
PTS: 1
DIF: L2
REF: p. 538
16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
application
B
PTS: 1
DIF: L2
REF: p. 538
16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
comprehension
A
PTS: 1
DIF: L2
REF: p. 527
16.2.1 Calculate the molarity of a solution.
BLM: analysis
D
PTS: 1
DIF: L3
REF: p. 526
16.2.1 Calculate the molarity of a solution.
BLM: analysis
C
PTS: 1
DIF: L1
REF: p. 528
16.2.2 Describe the effect of dilution on the total moles of solute in solution.
knowledge
D
PTS: 1
DIF: L2
REF: p. 528 | p. 529
16.2.2 Describe the effect of dilution on the total moles of solute in solution.
analysis
D
PTS: 1
DIF: L1
REF: p. 529
16.2.3 Express solution concentration as a percent by volume or percent by mass.
knowledge
A
PTS: 1
DIF: L2
REF: p. 531
16.2.3 Express solution concentration as a percent by volume or percent by mass.
analysis
2
ID: A
32. ANS: B
PTS: 1
DIF: L2
REF: p. 530
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: comprehension
33. ANS: A
PTS: 1
DIF: L1
REF: p. 534
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: knowledge
34. ANS: A
PTS: 1
DIF: L2
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: application
35. ANS: B
PTS: 1
DIF: L1
REF: p. 540
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to
molality.
BLM: knowledge
3