Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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A weak acid will produce a strong ______________
a. | conjugate base | c. | conjugate acid | b. | acid | d. | base |
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2.
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The covalent bond between H and O in a water molecule are polar because
a. | O and H are equally electronegative | c. | water molecules are
cohesive | b. | O is more electronegative that H | d. | H is more electronegative than
O |
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3.
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A solution is always
a. | in the liquid phase. | c. | homogeneous. | b. | composed of only two
phases. | d. | heterogeneous. |
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4.
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How many milliliters of 18.4 M H2SO4 are needed to prepare
600.0 mL of a 0.10 M H2SO4 solution?
a. | 4.6 mL | c. | 3.3 mL | b. | 4.0 mL | d. | 7.5 mL |
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5.
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In the reaction
HSO4-(aq) + H2O
(l) D H3O+(aq) +
SO42-(aq),
an acid- conjugate base pair is
a. | SO42-(aq) and
H3O+(aq) | c. | SO42-(aq) and
H2O(l) | b. | HSO4-(aq) and
H2O(l) | d. | HSO4-(aq) and
SO42-(aq) |
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6.
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What is the conjugate base of the acid H 3PO 4? H3PO4
(aq) + H2O (l) D
H3O+ (aq) +
H2PO4-1(aq) a. | H2O (l) | c. | OH-1 | b. | H3O+ (aq) | d. | H2PO4-1(aq) |
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7.
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Which of the following would represent the reaction the occurs between
hydrobromic acid and potassium hydroxide?
a. | KOH + H2O " KBr + HBr | c. | HBr +
H2O " KBr + KOH | b. | KBr + H2O
" HBr + KOH | d. | HBr + KOH " KBr +
H2O |
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8.
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Calculate the pH of a 0.325 M acetic acid
(HC2H3O2) solution. Ka = 1.8 x
10-5
a. | 2.62 | c. | 4.74 | b. | 0.488 | d. | 5.23 |
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9.
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The pH of milk is 6.4. Based on this information, which of the following
statements best describes milk?
a. | It is very acidic. | c. | It is very basic. | b. | It is slightly basic. | d. | It is slightly
acidic. |
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10.
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Matt is testing whether ammonia and vinegar are acids or bases. Litmus
paper helps determine whether a chemical is an acid or a base. A drop of ammonia turns the
litmus paper blue, and a drop of vinegar turns the litmus paper red. What can be deduced from
Matt’s experiment? a. | Both of the chemicals are acids. | b. | Both of the chemicals are
bases. | c. | Ammonia is a base, and vinegar is an acid. | d. | Ammonia is an acid,
and vinegar is a base. |
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11.
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Hydrochloric acid is a strong, highly corrosive acid. What is the pOH of a
0.037500 M HCl solution?
a. | 12.574 | c. | 1.433 | b. | 1.733 | d. | 12.270 |
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12.
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Why is water considered amphoteric?
a. | Water doesn’t react with any substance. | b. | Water acts as an
acid. | c. | Water acts as a base. | d. | Water acts as both an acid and a
base. |
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13.
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Which of the following would be considered an Arrhenius Base?
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14.
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The equation below shows ammonia dissolving in water. NH3 (aq) + H2O (l) D NH4+(aq) +
OH-(aq)
Why is water considered an acid when ammonia is dissolved in
it? a. | Water contains hydrogen atoms. | b. | Water acts as a proton (H+)
donor. | c. | Water has a 2:1 ratio of hydrogen to oxygen. | d. | Water acts as a
proton (H+) acceptor. |
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15.
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Of the four different laboratory solutions, which would exhibit the most
acidic behavior?
a. | pH = 3 | c. | pH = 11 | b. | pH = 5 | d. | pH = 7 |
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16.
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What is the name for the following: HNO3
a. | Nitrous Acid | c. | Hydronitric Acid | b. | Nitric Acid | d. | Hydronitrate
Acid |
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17.
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Cameron neutralized a solution of HCl with a solution of NaOH. What would be
best to add to this reaction to determine when HCl was completely neutralized by NaOH?
a. | An Indicator | c. | Deionized water | b. | A Base | d. | An acid |
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18.
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What is the formula for phosphoric acid?
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19.
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A stock solution of NaOH is found to have a pH of 10.0. What is the
[H+] for the solution?
a. | 1.0 x 10-10 | c. | 1.0 x 1010 | b. | 5.0 x
10-2 | d. | 2.5 x
10-3 |
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20.
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A substance has a hydroxide concentration of 0.00761 M. This solution
would be considered a
a. | acidic | c. | saline | b. | basic | d. | neutral |
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21.
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What is the formula for the following name: Sulfous Acid
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22.
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A glass of cola
was spilled on the carpet. Most colas are acidic with a pH usually between 2. Based on
the pH shown above, which of the following substances could best be used to neutralize the spilled
cola? a. | Baking Soda | c. | Ammonia | b. | Lemon Juice | d. | Pure Water |
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23.
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How many moles of H2SO4 are needed to prepare 5.0 liters
of a 2.0 M solution of H2SO4
a. | 20 mol | c. | 10 mol | b. | 2.5 mol | d. | 5.0 mol |
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24.
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What is the pH of a solution whose hydroxide ion concentration,
[OH-], is 1.0 x 10-3 M?
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25.
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Which statement below best descibes what happens when sodium chloride,
NaCl, is dissolved in water?
a. | The NaCl react with water to form NaOH and Cl2. | b. | The NaCl reacts with
water to form NaH and HCl. | c. | The NaCl separates into uncharged Na and
Cl. | d. | The NaCl separates into Na+ and Cl-
ions. |
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26.
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A solution is made in the below test tube by adding solute particles until no
more will dissolve after stirring. What will happen if more solute is added to the
solution? a. | The additional solute will settle to the bottom of the container because the solution
is saturated. | b. | The solute will begin to dissolve because the solution is
unsaturated. | c. | The entire container will become solid because the solution is
supersaturated. | d. | The solution will become supersaturated. |
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27.
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An unknown substance dissolves readily in water but not in benzene (a nonpolar
solvent). Molecules of what type are present in the unknown substance?
a. | nonpolar | c. | Both polar and nonpolar | b. | polar
| d. | neither polar nor
nonpolar |
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28.
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What is the pH of a 1.0 x 10-5 M HCl solution?
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29.
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The picture below depicts an unknown substance. The unknown substance a. | must be a weak electrolyte. | b. | remains unknown because there is not enough
information. | c. | must be a non-electrolyte. | d. | must be a strong
electrolyte. |
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30.
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What is the pH of 0.300 M of NaOH?
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31.
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Determine the molarity of a solution containing 6.76 g BaCl2 in 750.0
mL of solution.
a. | 0.00901 M | c. | 0.0244 M | b. | 0.0325 M | d. | 0.0433 M |
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32.
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Which equation represents a neutralization reaction?
a. | 2Al(OH)3(s) "
Al2O3(s) + 3H2O(l) | b. | H2CO3(aq) "
CO2(g) + H2O(l) | c. | 2H2(g) + O2(g) "
2H2O(l) | d. | H2SO4(aq) +2NaOH(aq)"Na2SO4(aq)+2H2O(l) |
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33.
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A solution contains an equal amount of hydrogen ion and hydroxide ions.
This solution would be considered?
a. | saline solution | c. | acidic solution | b. | neutral solution | d. | basic solution |
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34.
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Consider the picture below: Which statement accurately describes the picture? a. | B would be the solution because it is getting
dissolved. | b. | B would be considered the solute because
it is getting dissolved by A. | c. | A would be considered the solvent
because it is getting dissolved by B. | d. | A would be considered the solute because
it is getting dissolved by B. |
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35.
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A solution contains a hydroxide ion concentration 4.6 x 10-8 M.
What is the hydrogen ion concentration in this solution?
a. | 1.6 x 10-7 M | c. | 2.2 x 10-1
M | b. | 4.6 x 10-7 M | d. | 2.2 x 10-7 M |
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36.
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What is the base ionization constant expression, K b, for
ammonia? NH3 (aq) + H2O
(l) D NH4+ (aq)
+OH- (aq)
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