Multiple Choice
Identify the
choice that best completes the statement or answers the question.
|
|
|
1.
|
A solution contains an equal amount of hydrogen ion and hydroxide ions.
This solution would be considered?
a. | neutral solution | c. | acidic solution | b. | basic solution | d. | saline solution |
|
|
|
2.
|
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. | Ammonia is an acid, and vinegar is a
base. | c. | Ammonia is a base, and vinegar is an acid. | d. | Both of the
chemicals are bases. |
|
|
|
3.
|
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. | 2.5 x 10-3 | b. | 5.0 x
10-2 | d. | 1.0 x
1010 |
|
|
|
4.
|
What is the pH of 0.300 M of NaOH?
|
|
|
5.
|
What is the base ionization constant expression, K b, for
ammonia? NH3 (aq) + H2O
(l) D NH4+ (aq)
+OH- (aq)
|
|
|
6.
|
What is the formula for the following name: Sulfous Acid
|
|
|
7.
|
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 entire container will become solid because the solution is
supersaturated. | c. | The solute will begin to dissolve because the solution is
unsaturated. | d. | The solution will become supersaturated. |
|
|
|
8.
|
What is the pH of a 1.0 x 10-5 M HCl solution?
|
|
|
9.
|
In the reaction
HSO4-(aq) + H2O
(l) D H3O+(aq) +
SO42-(aq),
an acid- conjugate base pair is
a. | HSO4-(aq) and
SO42-(aq) | c. | SO42-(aq) and
H3O+(aq) | b. | HSO4-(aq) and
H2O(l) | d. | SO42-(aq) and
H2O(l) |
|
|
|
10.
|
What is the pH of a solution whose hydroxide ion concentration,
[OH-], is 1.0 x 10-3 M?
|
|
|
11.
|
What is the formula for phosphoric acid?
|
|
|
12.
|
Calculate the pH of a 0.325 M acetic acid
(HC2H3O2) solution. Ka = 1.8 x
10-5
a. | 5.23 | c. | 0.488 | b. | 4.74 | d. | 2.62 |
|
|
|
13.
|
What is the name for the following: HNO3
a. | Nitric Acid | c. | Nitrous Acid | b. | Hydronitric Acid | d. | Hydronitrate
Acid |
|
|
|
14.
|
Hydrochloric acid is a strong, highly corrosive acid. What is the pOH of a
0.037500 M HCl solution?
a. | 12.574 | c. | 1.733 | b. | 1.433 | d. | 12.270 |
|
|
|
15.
|
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. | H2PO4-1(aq) | d. | H3O+ (aq)
|
|
|
|
16.
|
How many milliliters of 18.4 M H2SO4 are needed to prepare
600.0 mL of a 0.10 M H2SO4 solution?
a. | 7.5 mL | c. | 3.3 mL | b. | 4.6 mL | d. | 4.0 mL |
|
|
|
17.
|
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. | 0.0433 M | d. | 0.0325 M |
|
|
|
18.
|
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 10-7
M | b. | 4.6 x 10-7 M | d. | 2.2 x 10-1 M |
|
|
|
19.
|
A substance has a hydroxide concentration of 0.00761 M. This solution
would be considered a
a. | basic | c. | neutral | b. | saline | d. | acidic |
|
|
|
20.
|
Which statement below best descibes what happens when sodium chloride,
NaCl, is dissolved in water?
a. | The NaCl separates into uncharged Na and Cl. | b. | The NaCl reacts with
water to form NaH and HCl. | c. | The NaCl react with water to form NaOH and
Cl2. | d. | The NaCl separates into Na+ and Cl-
ions. |
|
|
|
21.
|
Which of the following would represent the reaction the occurs between
hydrobromic acid and potassium hydroxide?
a. | HBr + KOH " KBr + H2O | c. | HBr +
H2O " KBr + KOH | b. | KBr + H2O
" HBr + KOH | d. | KOH + H2O " KBr +
HBr |
|
|
|
22.
|
Which equation represents a neutralization reaction?
a. | H2CO3(aq) " CO2(g) +
H2O(l) | b. | 2H2(g)
+ O2(g) "
2H2O(l) | c. | H2SO4(aq) +2NaOH(aq)"Na2SO4(aq)+2H2O(l) | d. | 2Al(OH)3(s) "
Al2O3(s) + 3H2O(l) |
|
|
|
23.
|
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 acts as a proton (H+) donor. | b. | Water has a 2:1
ratio of hydrogen to oxygen. | c. | Water acts as a proton (H+)
acceptor. | d. | Water contains hydrogen atoms. |
|
|
|
24.
|
Which of the following would be considered an Arrhenius Base?
|
|
|
25.
|
The pH of milk is 6.4. Based on this information, which of the following
statements best describes milk?
a. | It is slightly acidic. | c. | It is slightly basic. | b. | It is very
basic. | d. | It is very
acidic. |
|
|
|
26.
|
Of the four different laboratory solutions, which would exhibit the most
acidic behavior?
a. | pH = 11 | c. | pH = 3 | b. | pH = 7 | d. | pH = 5 |
|
|
|
27.
|
The covalent bond between H and O in a water molecule are polar because
a. | O is more electronegative that H | c. | H is more electronegative than
O | b. | O and H are equally electronegative | d. | water molecules are
cohesive |
|
|
|
28.
|
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. | polar | b. | Both polar and nonpolar | d. | neither polar nor
nonpolar |
|
|
|
29.
|
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. | A Base | c. | An acid | b. | Deionized water | d. | An Indicator |
|
|
|
30.
|
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. | Lemon Juice | b. | Pure Water | d. | Ammonia |
|
|
|
31.
|
How many moles of H2SO4 are needed to prepare 5.0 liters
of a 2.0 M solution of H2SO4
a. | 2.5 mol | c. | 5.0 mol | b. | 10 mol | d. | 20 mol |
|
|
|
32.
|
A solution is always
a. | heterogeneous. | c. | composed of only two phases. | b. | homogeneous. | d. | in the liquid phase. |
|
|
|
33.
|
A weak acid will produce a strong ______________
a. | conjugate acid | c. | base | b. | acid | d. | conjugate base |
|
|
|
34.
|
The picture below depicts an unknown substance. The unknown substance a. | must be a non-electrolyte. | b. | must be a strong
electrolyte. | c. | remains unknown because there is not enough information. | d. | must be a weak
electrolyte. |
|
|
|
35.
|
Consider the picture below: Which statement accurately describes the picture? a. | B would be considered the solute because it is getting dissolved by
A. | b. | B would be the solution because it is getting
dissolved. | c. | A would be considered the solute because
it is getting dissolved by B. | d. | A would be considered the solvent
because it is getting dissolved by B. |
|
|
|
36.
|
Why is water considered amphoteric?
a. | Water acts as a base. | b. | Water acts as both an acid and a
base. | c. | Water doesn’t react with any substance. | d. | Water acts as an
acid. |
|