Chapter 15:
Acids and Bases React
Practice Test
1.
22.5 mL of 0.122 M HCl neutralizes 30.0 mL of a KOH solution. What is the molarity of the KOH solution?
a.
0.00445 M
b.
0.163 M
c.
0.0915 M
d.
1.08 M
Hint
2.
What volume of 0.0500 M HNO
3
is required to neutralize 52.6 mL of 0.250 M LiOH?
a.
263 mL
b.
525 mL
c.
52.6 mL
d.
10.5 mL
Hint
3.
Acid-base reactions are usually __________________ reactions.
a.
combustion
b.
double-displacement
c.
synthesis
d.
decomposition
Hint
4.
Which of these compounds is NOT used in antacids?
a.
NaHCO
3
b.
Mg(OH)
2
c.
KOH
d.
CaCO
3
Hint
5.
A solution of known molarity used in an acid-base titration is known as a/an _______________.
a.
standard solution
b.
indicator
c.
aliquot
d.
hetergeneous solution
Hint
6.
What is the base in the reaction HI + H
2
O
H
3
O + I
-
?
a.
Isub>2
b.
H
2
O
c.
H
3
O
+
d.
HI
Hint
7.
According to the Bronsted-Lowry definition, an acid is a _______________.
a.
electron donor
b.
hydrogen-ion donor
c.
electron acceptor
d.
hydrogen-ion acceptor
Hint
8.
What is the net ionic equation for the reaction of a hydrogen carbonate antacid with hydrochloric acid?
a.
HCO
3
-
(aq) + H
+
(aq)
H
2
O(l) + CO
2
(g)
b.
H
2
CO
3
(aq) + 2HCl(aq)
2H
2
O(l) + CO
2
(g) + Cl
-
(aq)
c.
HCO
3
-
(aq) + HCl(aq)
H
2
O(l) + CO
2
(g) + Cl
-
(aq)
d.
HCO
3
-
(aq) + H
+
(aq)
H
2
CO
3
(g)
Hint
9.
This is the formula for the spectator ion in the reaction between hydrobromic acid and ammonia.
a.
Br
-
b.
H
3
O
+
c.
NH
3
d.
HBr
Hint
10.
A __________ is a substance that resists changes in pH when moderate amounts of acids or bases are added.
a.
buffer
b.
hydronium
c.
spectator ion
d.
hydroxide
Hint
11.
What is the net ionic equation for the reaction between hydrocyanic acid and sodium hydroxide?
a.
H
+
(aq) + OH
-
(aq)
H
2
O(l)
b.
HCN(aq) + NaOH(aq)
H
2
O(l) + NaCN(aq)
c.
HCN(aq) + OH
-
(aq)
H
2
O(l) + CN
-
(aq)
d.
H
3
O
+
(aq) + OH
-
(aq)
2H
2
O(l)
Hint
12.
Which of these combinations will NOT make an acid-base buffer?
a.
HCN/KCN
b.
NaOH/NaCl
c.
NH
3
/NH
4
NO
3
d.
HC
2
H
3
O
2
/NaC
2
H
3
O
2
Hint
13.
The complete neutralization of a weak acid with a strong base produces a _______________ solution.
a.
acidic
b.
basic
c.
neutral
d.
cold
Hint
14.
Along with water, the compound produced in most acid-base reactions is _____________.
a.
sodium hydroxide
b.
carbon dioxide
c.
a salt
d.
barium oxide
Hint
15.
Buffers maintain the pH of human blood near _____.
a.
7.4
b.
12.5
c.
6.8
d.
1
Hint
16.
An acid-base reaction is called a __________ reaction.
a. neutralization
b. combustion
c. synthesis
d. single-replacement
Hint
17.
What will be the acid-base condition of the solution when ammonium citrate is dissolved in water?
a.
neutral
b.
The acid-base condition cannot be determined.
c.
acidic
d.
basic
Hint
18.
Ions that are present in a solution but that do not participate in the reaction are called ________________.
a.
reactants
b.
products
c.
spectator ions
d.
gases
Hint
19.
One of the best acid-base indicators to use for a strong acid-strong base titration is ______________.
a.
methyl red
b.
phenolphthalein
c.
bromothymol blue
d.
thymol blue
Hint
20.
H
+
(aq) + OH
-
(aq)
H
2
O(l) is the _____________ equation for a strong acid-strong base neutralization reaction.
a.
complete ionic
b.
net ionic
c.
formula
d.
reverse
Hint
