Chapter 19:
Acids and Bases
Practice Test
1.
A substance that contains hydrogen and produces H
+
ions in aqueous solution is a(n) ________.
a.
salt
b.
water
c.
acid
d.
base
Hint
2.
Which of the following is a strong base?
a.
HCOOH
b.
HCO
3
c.
NH
3
d.
NaOH
Hint
3.
Calculate the pH of 0.075
M
KOH.
a.
11.12
b.
12.88
c.
11.46
d.
10.4
Hint
4.
Under what condition is the OH
-
ion concentration in water expected to be zero?
a.
in a solution of strong acid
b.
in a solution of weak base
c.
in a solution of strong base
d.
never
Hint
5.
A 0.001
M
solution of HCl is ____________.
a.
a dilute acid solution
b.
a concentrated acid solution
c.
a weak acid solution
d.
neutral
Hint
6.
A solution of pH = 2.1 would be described as __________.
a.
distinctly basic
b.
slightly acidic
c.
slightly basic
d.
distinctly acidic
Hint
7.
Which of the following compounds is not a salt?
a.
BaCrO
4
b.
FeCl
2
c.
Mg(OH)
2
d.
K
2
SO
4
Hint
8.
Which one of the following could not be a BrØnsted-Lowry acid?
a.
H
3
O
+
b.
H
2
O
c.
NH
4
+
d.
BF
3
Hint
9.
Which of the following cannot be a buffer?
a.
a mixture of a weak acid and a weak base
b.
a mixture of a strong acid and a strong base
c.
a mixture of a strong acid and a weak base
d.
a mixture of a weak acid and a strong base
Hint
10.
Calculate the pH of a solution that has a [OH
-
] = 2.50 × 10
-4
M
.
a.
3.6
b.
-3.60
c.
0.4
d.
10.40
Hint
11.
Which visual indicator would you choose to titrate HCl with NaOH? Acid Range Color pH Range Basic Range Color
a.
blue 3.4 – 4.6 yellow
b.
pink 1.2 – 2.8 yellow
c.
yellow 6.5 – 7.8 purple
d.
colorless 8.3 – 9.9 red
Hint
12.
Neutralization is the chemical process in which ____________.
a.
sodium ions react with chloride ions to form sodium chloride
b.
hydrogen ions react with hydroxide ions to form water
c.
hydrogen ions react with chloride ions to form hydrogen chloride
d.
sodium ions react with hydroxide ions to form sodium hydroxide
Hint
13.
pH is defined as __________.
a.
log [H
+
]
b.
log [OH
-
]
c.
-log [OH
-
]
d.
-log [H
+
]
Hint
14.
When a solution has a pH of 4, what is the pOH of that solution?
a.
4
b.
10
c.
7
d.
18
Hint
15.
According to the BrØnsted-Lowry theory, a base is a(n) ___________.
a.
electron pair donor
b.
hydrogen ion acceptor
c.
electron pair acceptor
d.
hydrogen ion donor
Hint
16.
What is the concentration of hydrogen ions in a solution that has a pH of 4.32?
a.
8.6 × 10
-5
M
b.
5.1 × 10
-4
M
c.
6.2 × 10
-4
M
d.
4.8 × 10
-5
M
Hint
17.
At 298 K, pure water has a pH of __________.
a.
0
b.
7
c.
14
d.
-14
Hint
18.
H
2
SO
4
is a ____________.
a.
monoprotic acid
b.
diprotic acid
c.
diprotic base
d.
monoprotic base
Hint
19.
When HClO
4
ionizes in water, ClO
4
-
is the ______________.
a.
conjugate acid
b.
conjugate base
c.
base
d.
acid
Hint
20.
Calculate the H
+
ion and OH
-
ion concentrations in a 0.50
M
solution of HBr.
a.
[H
+
] = 0.50
M
and [OH
-
] = 2.0
M
b.
[H
+
] = 0.50
M
and [OH
-
] = 2.0 × 10
-14
M
c.
[H
+
] = 1.0 × 10
-7
M
and [OH
-
] = 1.0 × 10
-7
M
d.
[H
+
] = 0.50
M
and [OH
-
] = 0.50
M
Hint
