Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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Which
of the following is an electrolyte? a. | sodium chloride | c. | water | b. | sugar | d. | glass | | | | |
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2.
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A
substance whose water solution does NOT conduct a current is a(n) a. | polar
substance. | c. | electrolyte. | b. | nonelectrolyte. | d. | ionic substance. | | | | |
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3.
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Which
of the following does NOT increase the rate of dissolving a solid in water? a. | raising the
temperature | c. | using larger
pieces of solid | b. | stirring | d. | crushing the solid | | | | |
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4.
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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 | | | | |
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5.
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If
the amount of solute present in a solution at a given temperature is less than the maximum amount
that can dissolve at that temperature, the solution is said to be a. | saturated. | c. | supersaturated. | b. | unsaturated. | d. | concentrated. | | | | |
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6.
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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. | | |
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7.
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The
solubility of a solute depends on a. | the nature of the solute and the temperature of the
solvent. | b. | the nature of the solute only. | c. | the temperature
of the solvent only. | d. | neither the nature of the solute nor the temperature of the
solvent. | | |
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8.
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The
solubility of gases in liquids a. | always increases with increasing
pressure. | b. | sometimes increases with increasing
pressure. | c. | always decreases with increasing
pressure. | d. | does not depend on pressure. | | |
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9.
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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 | | | | |
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10.
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What
is the molality of a solution that contains 5.10 mol KNO3 in 4.47 kg
water? a. | 0.315
m | c. | 1.02
m | b. | 0.779 m | d. | 1.14 m | | | | |
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11.
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How
many moles of HCl are present in 0.70 L of a 0.33 M HCl solution? a. | 0.23
mol | c. | 0.38
mol | b. | 0.28
mol | d. | 0.47
mol | | | | |
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12.
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How
many milliliters water are needed to make a 0.171 M solution that contains 1.00 g of
NaCl? a. | 100
mL | c. | 171
mL | b. | 1000
mL | d. | 17.1
mL | | | | |
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13.
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A
solution of sugar in water has a density of 1.05 g/cm3. If you have 75 mL of
the
solution, and if the solution is 8.1% sugar, how many grams of sugar are there in
the
solution?
a. | 63.8 g sugar | c. | 60.8 g sugar | b. | 6.4 g
sugar
| d. | 6.1 g
sugar
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14.
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What
is the boiling point change for a solution containing 0.328 moles of naphthalene (a nonvolatile,
nonionizing compound) in 250. g of liquid benzene? (Kb = 2.53°C/m for benzene)
a. | 3.32°C
| c. | 7.41°C
| b. | 1.93°C
| d. | 4.31°C
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15.
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Which of the
following aqueous solutions has the highest boiling point?
a. | 1.0 m NaOH
| c. | 1.0 m
Na2SO4 | b. | 1.0 m
NH4NO3
| d. | 1.0 m
KC2H3O2 | | | | |
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16.
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What
is the approximate freezing-point depression of a 0.010 m aqueous CaCl2
solution? a. | –0.019ºC | c. | –0.056ºC | b. | –0.037ºC | d. | –0.074ºC | | | | |
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17.
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Which
of the following pairs of solutions produce a precipitate when combined? a. | KOH and
NH4Cl | c. | Na2SO4 and KCl | b. | Fe(NO)3 and KCl | d. | NH4Cl and AgNO3 | | | | |
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18.
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Which
solute is present in aqueous solution mostly as molecules rather than as ions? a. | a weak
electrolyte | c. | a
nonelectrolyte | b. | a strong electrolyte | d. | a covalent electrolyte | | | | |
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19.
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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. | | |
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20.
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Why
is vapor-pressure lowering a colligative property? a. | It depends on
the concentration of a nonelectrolyte solute and does not depend on solute
identity. | b. | It depends on the concentration of an electrolyte solute and
does not depend on solute identity. | c. | It depends on the concentration of a nonelectrolyte solute and
on solute identity. | d. | It depends on the concentration of an electrolyte solute and on
solute identity. | | |
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21.
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What
is the approximate freezing-point depression of a 0.050 m aqueous Na2SO4
solution? a. | –0.11ºC | c. | –0.22ºC | b. | –0.28ºC | d. | –0.39ºC | | | | |
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22.
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Compared with a 0.01 m sugar solution, a 0.01 m MgCl2
solution has a. | the same
freezing-point depression. | b. | about twice the freezing-point
depression. | c. | about three times the freezing-point
depression. | d. | about four times the freezing-point
depression. | | |
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23.
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When
a 20.0-g sample of an unknown compound is dissolved in 500. g of benzene, the freezing point of the
resulting solution of 3.77°C. The freezing point of pure benzene is 5.48°C and Kf for
benzene is 5.12°C/m. Calculate the molar mass of the unknown compound a. | 120. g/mol
| c. | 100. g/mol
| b. | 140. g/mol
| d. | 80.0 g/mol
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Problem
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24.
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Muriatic acid is often used to remove rust. A solution of muriatic acid, HCl, reacts
with Fe2O3 deposits on industrial equipment. How many liters of 5.50 M HCl
would be needed to react completely with 439 g Fe2O3?
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25.
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Suppose you need to prepare 1000. mL of 0.100 m HCl(aq), and all you have on hand is
0.500 m HCl(aq). What volume of the 0.500 m solution should be diluted to 1000. mL to give the
desired 0.100 m HCl(aq) solution?
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