Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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Pure water contains
a. | water molecules only. | b. | hydronium ions only. | c. | hydroxide ions
only. | d. | water molecules, hydronium ions, and hydroxide ions. |
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2.
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Pure water partially breaks down into charged particles in a process
called
a. | hydration. | c. | self-ionization. | b. | hydrolysis. | d. | dissociation. |
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3.
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What is the concentration of H3O+ ions 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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Which expression represents the concentration of OH– ions in
solution?
a. | 10–14 – [H3O+] | c. | 10–14 ¸
[H3O+] | b. | 10–14 ´ [H3O+] | d. | [OH–] ¸ 10–14 |
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5.
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If [H3O+] of a solution is greater than
[OH–], the solution
a. | is always acidic. | c. | is always neutral. | b. | is always basic. | d. | might be acidic, basic, or
neutral. |
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6.
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What is the pH of a neutral solution at 25°C?
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7.
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The pH of a basic solution is
a. | less than 0. | c. | greater than 7. | b. | less than 7. | d. | greater than
14. |
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8.
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A water solution whose pH is 10
a. | is always neutral. | c. | is always acidic. | b. | is always basic. | d. | might be neutral, basic, or
acidic. |
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9.
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Which of the following liquids is basic?
a. | lemons | c. | milk | b. | vinegar | d. | tomatoes |
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10.
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Which of the following liquids is acidic?
a. | seawater | c. | milk of magnesia | b. | blood | d. | orange juice |
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11.
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What is the pH of a 10–5 M KOH solution?
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12.
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If [H3O+] = 1.7 ´ 10–3 M, what is the pH of the solution?
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13.
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What is the pH of a 0.027 M KOH solution?
a. | 6.47 | c. | 12.92 | b. | 12.43 | d. | 14.11 |
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14.
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How would you classify KOH in the equation below?  a. | a weak acid | c. | a weak base | b. | a strong acid | d. | a strong base |
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15.
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What is the OH– 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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16.
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The antilogarithm of a number, y, is
a. | the inverse of y. | c. | y raised to the power of
10. | b. | the square root of y. | d. | 10 raised to the power of
y. |
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17.
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What is the transition interval for bromthymol blue?
a. | pH 3.1–4.4 | c. | pH 6.2–7.6 | b. | pH 6.4–8.0 | d. | pH
8.0–10.0 |
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18.
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What is the transition interval for methyl orange?
a. | pH 3.1–4.4 | c. | pH 6.2–7.6 | b. | pH 6.4–8.0 | d. | pH
8.0–10.0 |
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19.
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Which indicator is used to study neutralizations of weak acids with strong
bases?
a. | phenolphthalein | c. | bromthymol blue | b. | methyl orange | d. | None of the
above |
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20.
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Which indicator is used to study neutralizations of strong acids with weak
bases?
a. | phenolphthalein | c. | bromthymol blue | b. | methyl orange | d. | None of the
above |
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21.
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What unknown quantity can be calculated after performing a titration?
a. | volume | c. | mass | b. | concentration | d. | density |
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22.
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During an acid-base titration, a very rapid change in pH
a. | occurs when the first addition of the known solution is made. | b. | occurs when the
amounts of H3O+ ions and OH– ions are nearly
equivalent. | c. | occurs at several points during the titration. | d. | does not occur
during titration. |
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23.
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When titrating a strong acid with a strong base, the equivalence point
a. | will be below a pH of 7.0. | c. | will be at a pH of
7.0. | b. | will be above a pH of 7.0. | d. | will be either above or below a pH of 7.0. |
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24.
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What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of
0.0904 M HNO3?
a. | 0.230 M | c. | 0.460 M | b. | 0.355 M | d. | 0.620 M |
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25.
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What is the molarity of an H2SO4 solution if 49.0 mL is
completely titrated by 68.4 mL of an NaOH solution whose concentration is 0.333 M?
a. | 0.116 M | c. | 0.465 M | b. | 0.232 M | d. | 0.880 M |
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