Modified True/False
Indicate
whether the sentence or statement is true or false. If false, change the identified word or
phrase to make the sentence or statement true.
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1.
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Measuring the concentration of cholesterol in blood is an example of quantitative
analysis. ____________________
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2.
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A
solution is concentrated if it has a relatively small quantity of solute per unit volume of
solution. ____________________
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3.
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The
concentration of a solution may be expressed as a percentage V/W if it is composed of a liquid
solute and a liquid solvent. ____________________
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4.
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Adding more solvent to a solution changes the amount of solute in the solution.
____________________
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5.
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The
following balanced equation has the mole ratio: 2 mol CO(g) : 1 mol O2(g) :
2 mol CO2(g). ____________________
2 CO(g)
+ O2(g) ® 2 CO2(g)
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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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6.
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The
molar concentration of a solution that contains 0.25 mol sucrose in 2.5 L of solution
is a. | 0.1
mol/L | c. | 10
mol/L | b. | 0.01 mol/L | d. | 100 mol/L | | | | |
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7.
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The
amount of NaOH(aq) in 0.250 L of a 3.0-mol/L solution is a. | 0.25
mol | c. | 1.0
mol | b. | 0.75
mol | d. | 1.5
mol | | | | |
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8.
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According to the Safe Drinking Water Act, the maximum permitted concentration of lead
in public drinking water is 0.05 ppm. Therefore, according to the Act, the maximum permitted mass of
lead in 1 L of public drinking water is a. | 0.05 mg | c. | 5 mg | b. | 0.5 mg | d. | 0.5 g | | | | |
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9.
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When
75 mL of 0.15-mol/L HCl(aq) is diluted with distilled water to a final volume of
150 mL, the concentration of HCl(aq) is reduced to a. | 0.12
mol/L | c. | 0.050
mol/L | b. | 0.10 mol/L | d. | 0.075 mol/L | | | | |
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10.
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What
amount of chlorine gas reacts with 0.752 mol phosphorus, P4(s), in the reaction described
by the following balanced equation?
P4(s) + 6 Cl2(g) ® 4
PCl3(l) a. | 0.501 mol | c. | 4.51 mol | b. | 35.0
mol | d. | 2.47
mol | | | | |
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11.
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What
amount of lithium nitride, Li3N(s), is produced when 15.0 g of lithium,
Li(s), reacts with excess nitrogen gas according to the following balanced chemical
equation?
6 Li(s) + N2(g) ® 2
Li3N(s) a. | 5.00 mol | c. | 0.720 mol | b. | 25.2
mol | d. | 4.99
mol | | | | |
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12.
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What
mass of copper is consumed when 15.0 g of nitric oxide, NO(g), is produced according
to the following balanced equation?
3 Cu(s) + 8 HNO3(aq)
®
3 Cu(NO3)2(aq) + 4 H2O(l) + 2
NO(g) a. | 15.0
g | c. | 47.6
g | b. | 22.5
g | d. | 192
g | | | | |
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13.
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What
mass of oxygen gas is required to combust 81.2 g of methane, CH4(g), completely according
to the following balanced chemical equation?
CH4(g) + 2 O2(g) ® CO2(g) + 2
H2O(l) a. | 814 g | c. | 203 g | b. | 406
g | d. | 324
g | | | | |
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14.
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What
mass of silicon oxide, SiO2(s), may form when 81.4 g of silicon reacts with excess oxygen
according to the following balanced chemical equation?
Si(s)
+ O2(g) ® SiO2(s) a. | 250
g | c. | 174
g | b. | 375
g | d. | 81.4
g | | | | |
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Completion
Complete each sentence or
statement.
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15.
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The
____________________ of a solution is a ratio of the quantity of solute to the quantity of
____________________.
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16.
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Hydrogen peroxide may be purchased at most pharmacies as a 3% V/V aqueous solution.
The V/V notation indicates that two ____________________ are mixed to make the
solution.
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17.
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In
laboratory chemistry, the concentration of solutions is more commonly expressed in
____________________ concentration units.
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18.
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Two
parts per million of fluoride ions in drinking water corresponds to 2 g of fluoride ions in
____________________ L of drinking water.
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19.
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The
concentration of a solution may be decreased by adding more ____________________.
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20.
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____________________ is a part of chemistry that deals with the relationships between
quantities in chemical reactions.
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21.
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To
predict the masses of reactants and products in a reaction, always begin with a ____________________
equation for the reaction.
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22.
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The
mole ratio is the ratio of the ____________________ of reactants and products in a chemical
reaction
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