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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Acids generally release
H2 gas when they react
with
a. | nonmetals. | c. | active metals. | b. | semimetals. | d. | inactive metals. |
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2.
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Hydroxides of Group 1
metals
a. | are all strong
bases. | c. | are all
acids. | b. | are all weak bases. | d. | might be either strong or weak
bases. |
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3.
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What is the concentration of
H3O+ in pure
water?
a. | 10–7 M | c. | 55.4 M | b. | 0.7 M | d. | 107
M |
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4.
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What is the product of
H3O+ and
OH– concentrations in water?
a. | 10–28 | c. | 10–7 | b. | 10–14 | d. | 55.4 |
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5.
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Which expression represents the
pH of a solution?
a. | log[H3O+] | c. | log[OH–] | b. | –log[H3O+] | d. | –log[OH–] |
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6.
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A water solution whose pH is
4
a. | is always
neutral. | c. | is always
acidic. | b. | is always basic. | d. | might be neutral, basic, or
acidic. |
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7.
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If
[H3O+] = 8.26 × 10–5 M, what is the pH of the solution?
a. | 2.161 | c. | 4.083 | b. | 3.912 | d. | 8.024 |
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8.
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What is the hydroxide ion
concentration of a solution whose pH is 12.40?
a. | 2.5 × 10–2 M | c. | 8.9 × 10–2 M | b. | 4.4 × 10–2
M | d. | 1.0 × 10–1 M |
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9.
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What is the most common
oxidation number of combined oxygen?
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10.
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What are the oxidation numbers
in the compound KCl?
a. | K = 0, Cl =
0 | c. | K = +1, Cl =
–1 | b. | K = –1, Cl = +1 | d. | K = +2, Cl = –2 |
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11.
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What are the oxidation numbers
in the ion SO32–?
a. | S = +6, O =
–2 | c. | S = +4, O =
–2 | b. | S = +1, O = –1 | d. | S = 0, O = –1 |
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12.
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In the reaction F2 +
Mg → 2F– +
Mg2+, which species is oxidized?
a. | F2 only | c. | both Mg and F2 | b. | Mg only | d. | neither Mg nor F2 |
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13.
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In a redox reaction,
MnO4– is
changed to MnO42–. How many electrons must be lost or gained by
Mn?
a. | none lost or
gained | c. | one
gained | b. | one lost | d. | two gained |
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14.
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The redox equation
4H+ + N2 →
NH4+ + N is
a. | correctly
balanced. | b. | correctly balanced for number of atoms but not for
charge. | c. | correctly balanced for charge but not for number of
atoms. | d. | not balanced for number of atoms or
charge. |
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15.
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In redox
reactions,
a. | the oxidizing agent is the substance
oxidized. | b. | the reducing agent is the substance
oxidized. | c. | both oxidizing and reducing agents are
oxidized. | d. | the reducing agent is the substance
reduced. |
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16.
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Where does oxidation take place
in an electrochemical cell?
a. | the
anode | c. | the anode or the
cathode | b. | the cathode | d. | the half-cell |
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17.
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Where does reduction take place
in an electrochemical cell?
a. | the
anode | c. | the anode or the
cathode | b. | the cathode | d. | the half-cell |
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18.
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After balancing the redox
equation Cr2O72– + SO2 + H+ → Cr3+ + HSO4–
+ H2O, the coefficients, in order from left to right, are
a. | 1, 3, 5, 2, 3,
1. | c. | 2, 5, 10, 4, 5,
2. | b. | 1, 2, 4, 2, 2,
1. | d. | 2, 1, 2, 5, 1,
2. |
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