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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In
any dilute aqueous solution at SATP, if a significant concentration of hydroxide ions is found to be
present, then a. | the solution pH
value must be extremely low. | b. | the concentration of hydronium ions must be extremely
low. | c. | no other ions
are likely to be present in the solution. | d. | the solution’s Kw value will be
significantly increased. | | |
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2.
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Excess zinc is placed in each of two beakers that contain equal volumes of
0.15 mol/L hydrofluoric acid (in beaker “A”) and 0.10 mol/L hydrochloric acid (in
beaker “B”). When reaction is complete in both beakers, it will be observed that zinc
reacts a. | more rapidly in
beaker A, and to the same extent as in beaker B. | b. | more rapidly in
beaker A, and to a greater extent than in beaker B. | c. | more slowly in
beaker A, and to the same extent as in beaker B. | d. | more slowly in
beaker A, and to a greater extent than in beaker B. | | |
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3.
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The
conjugate acid of H2BO3–(aq), is a. | HBO32–(aq) | b. | H3BO3(aq) | c. | BO33–(aq) | d. | H2O(l) | | |
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4.
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The
hydrogen sulfite ion, HSO3–, is a. | an amphiprotic
entity. | b. | the conjugate acid of carbonic acid. | c. | a weak acid, but
a strong base. | d. | more likely to gain a proton than to lose one, in aqueous
solution. | | |
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5.
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Equal
volumes of aqueous solutions with equal concentrations of hydrogen carbonate ion and of dihydrogen
phosphate ion are prepared, and then mixed. The substance that acts as an acid in the predominant
Brønsted-Lowry acid-base reaction that occurs, is a. | H3PO4(aq) | b. | H2PO4–(aq) | c. | HCO3–(aq). | d. | H2O(l) | | |
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6.
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Assume that the following mixtures of solutions all involve equal volumes and equally
concentrated entities. In which case are products favored at equilibrium? a. | HSO3–(aq) and
H3PO4(aq) | b. | H2PO4–(aq) and
C6H5O73–(aq) | c. | HCO3–(aq) and
HPO42–(aq) | d. | H2CO3(aq) and
CN–(aq) | | |
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7.
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In
Ka calculations, a simplifying assumption may often be made that the equilibrium
concentration of the acid is not significantly less than the initial concentration. This assumption
holds true for which of the following acid solutions at SATP? a. | 1.00 mol/L
HClO4(aq) | b. | 1.00 mol/L
H3PO4(aq) | c. | 0.100 mol/L CH3COOH(aq) | d. | 0.0500 mol/L
C6H5COOH(aq) | | |
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Completion
Complete each sentence or
statement.
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8.
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A
0.020 mol/L solution of HNO3(aq) at SATP will have a hydroxide ion amount concentration
(expressed in scientific notation) of a.b ´ 10–cd mol/L. The values of a, b, c, and
d are ___, ___, ___, and ___.
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9.
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A
0.10 g sample of pure solid calcium hydroxide is dissolved to make 1.0 L of aqueous solution at SATP.
The pH of this solution will be ____.
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10.
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A
student is given a 0.200 mol/L aqueous solution of an unknown monoprotic acid. The solution pH is
measured to be 4.00. From this evidence, the percent reaction (ionization) of this acid with water is
calculated to be ____%.
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11.
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At a
given temperature, the pH of a 0.100 mol/L solution of hydrofluoric acid is measured to be 2.08. From
this evidence, the numerical value of Ka for HF(aq) at this temperature is
calculated to be ____ ´ 10–4 .
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12.
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The
hydronium ion concentration in a 1.00 mol/L solution of citric acid,
H3C6H5O7(aq), will be ____ mmol/L at SATP.
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13.
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If
the Ka for an acid is 7.3 ´ 10–4, the Kb for the
conjugate base of this acid (assuming both values are at SATP) will be a.b ´
10–cd mol/L. The values of a, b, c, and d are ___, ___, ___, and
___..
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14.
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The
equilibrium hydroxide ion concentration of a prepared 0.200 mol/L solution of lithium acetate is
found to be 1.2 ´ 10–5 mol/L, at temperature t. The
Kb of aqueous acetate ion, when calculated from this evidence, is a.b ´
10–cd mol/L. The values of a, b, c, and d are ___, ___, ___, and
___.
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15.
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In a
1.00 mol/L aqueous solution of potassium hydrogen carbonate, the amount concentration of aqueous
hydroxide ion should be ___ ´ 10–4 mol/L.
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