Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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What is the concentration of OH– ions in pure water?
a. | 10–7 M | c. | 55.4 M | b. | 0.7
M | d. | 107
M |
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2.
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What is the product of H3O+ ion and OH–
ion concentrations in water?
a. | 10–28 | c. | 10–7 | b. | 10–14 | d. | 55.4 |
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3.
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Which expression represents the concentration of H3O+ ions
in solution?
a. | 10–14 – [OH–] | c. | 10–14 ¸
[OH–] | b. | 10–14 ´ [OH–] | d. | [OH–] ¸ 10–14 |
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4.
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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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5.
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What is the pH of a neutral solution at 25°C?
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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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Which of the following liquids is acidic?
a. | seawater | c. | milk of magnesia | b. | blood | d. | orange juice |
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8.
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To calculate the pH of a solution whose [OH–] is
known, first calculate
a. | [H3O+]. | c. | antilog[H3O+]. | b. | log[OH–]. | d. | [H2O]. |
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9.
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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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10.
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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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11.
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What is the pH of a 0.001 62 M NaOH solution?
a. | 3.841 | c. | 9.923 | b. | 5.332 | d. | 11.210 |
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12.
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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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13.
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How would you classify CH 3COOH in the equation below?    a. | a weak acid | c. | a weak base | b. | a strong acid | d. | a strong base |
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14.
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What is the hydronium ion concentration of a solution whose pH is 4.12?
a. | 4.4 ´ 10–8 M | c. | 6.4 ´ 10–5 M | b. | 5.1 ´
10–6 M | d. | 7.6
´ 10–5 M |
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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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Indicators are classified into three types according to
a. | their molar mass. | c. | their color. | b. | their polarity. | d. | the pH at which they change
color. |
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18.
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What is the transition interval for phenol red?
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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What is the transition interval for phenolphthalein?
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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20.
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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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21.
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In an acid-base titration,
a. | base is always added to acid. | b. | acid is always added to
base. | c. | base is added to acid or acid is added to base. | d. | None of the
above |
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22.
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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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23.
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An acid-base titration is carried out by monitoring
a. | temperature. | c. | pressure. | b. | pH. | d. | density. |
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24.
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When titrating a weak 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. | cannot be determined by pH. |
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25.
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What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely
titrated by 15.3 mL of 0.247 M H2SO4?
a. | 0.0101 M | c. | 0.0402 M | b. | 0.0201 M | d. | 0.0805 M |
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