Matching
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Match each item with the correct statement below. a. | Henry's
law | d. | supersaturated
solution | b. | immiscible | e. | concentration | c. | saturated
solution | | | | |
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1.
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describes liquids that are insoluble in one another
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2.
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solution containing maximum amount of solute
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3.
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solution containing more solute than can theoretically dissolve at a given
temperature
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4.
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measure of the amount of solute dissolved in a specified quantity of
solvent
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Match each item with the correct statement below. a. | boiling point
elevation | d. | molarity | b. | molality | e. | freezing point depression | c. | mole
fraction | | | | |
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5.
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number of moles of solute dissolved in 1 L of solution
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6.
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a
colligative property related to the fact that ice will form at higher temperatures in the Great Lakes
than in the ocean
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7.
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a
colligative property related to a decrease in the vapor pressure of a solution
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8.
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number of moles of solute dissolved in 1 kg of solvent
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9.
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ratio
of moles of solute in solution to total number of moles of both solvent and solute
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Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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10.
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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 | | |
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11.
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What
is the maximum amount of KCl that can dissolve in 200 g of water?
(The solubility
of KCl is 34 g/100 g H2O at 20 C.) a. | 17
g | c. | 68
g | b. | 34
g | d. | 6800
g | | | | |
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12.
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If a
crystal added to an aqueous solution causes many particles to come out of the solution, the original
solution was ____. a. | unsaturated | c. | an emulsion | b. | saturated | d. | supersaturated | | | | |
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13.
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Which
of the following substances is less soluble in hot water than in cold water? a. | CO | c. | NaNO | b. | NaCl | d. | KBr | | | | |
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14.
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Which
of the following occurs as temperature increases? a. | Solubility decreases. | c. | Solubility remains the same. | b. | Solubility
increases. | d. | Molarity
doubles. | | | | |
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15.
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The
solubility of a gas in a liquid is ____. 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 | | |
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16.
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What
is the molarity of a solution that contains 6 moles of solute in 2 liters of
solution?
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17.
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In
which of the following is the solution concentration expressed in terms of molarity?
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18.
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Which
of the following operations yields the number of moles of solute? a. | molarity  moles of solution | c. | molarity  mass of
solution | b. | molarity  liters of
solution | d. | moles of
solution  volume of solution | | | | |
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19.
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What
is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
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20.
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What
is the number of moles of solute in 250 mL of a 0.4M solution? a. | 0.1
mol | c. | 0.62
mol | b. | 0.16
mol | d. | 1.6
mol | | | | |
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21.
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What
is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of
solute = 26 g/mol) a. | 1.5M | c. | 2.1M | b. | 2.2M | d. | 0.0022M | | | | |
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22.
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What
mass of sucrose, C H O , is
needed to make 500.0 mL of a 0.200M solution? a. | 34.2
g | c. | 17.1
g | b. | 100
g | d. | 68.4
g | | | | |
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23.
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How
many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M
NaBr? a. | 25
mL | c. | 100
mL | b. | 50
mL | d. | 150
mL | | | | |
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24.
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The
volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____. a. | 0.128
mL | c. | 281
mL | b. | 7.8
mL | d. | 362
mL | | | | |
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25.
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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 | c. | 0.35M | b. | 2.8M | d. | 0.18M | | | | |
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26.
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If
the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in
solution? a. | 0.5
mL | c. | 5.0
mL | b. | 1.25
mL | d. | 12.5
mL | | | | |
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27.
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In
which of the following is concentration expressed in percent by volume? a. | 10%
(v/v) | c. | 10%
(m/m) | b. | 10% (m/v) | d. | 10% | | | | |
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28.
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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 | c. | 80 g | b. | 50 g | d. | 800 g | | | | |
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29.
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The
volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____. a. | 372
mL | c. | 248
mL | b. | 40.0
mL | d. | 580
mL | | | | |
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30.
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In
which of the following is concentration expressed in percent by volume?
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31.
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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 | | | | |
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32.
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Colligative properties depend upon the ____. a. | nature of the
solute | c. | number of solute
particles in a solution | b. | nature of the solvent | d. | freezing point of a solute | | | | |
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33.
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Which
of the following is an expression of molality?
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Essay
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34.
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Discuss the phenomenon of supersaturation. Indicate how crystallization can be
initiated in a supersaturated solution.
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35.
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Explain on a particle basis how the addition of a solute affects the boiling point,
the freezing point, and the vapor pressure of the solvent.
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