Chapter 19:
Acids and Bases
Practice Test
1.
According to the BrØnsted-Lowry theory, a base is a(n) ___________.
a.
hydrogen ion acceptor
b.
electron pair acceptor
c.
electron pair donor
d.
hydrogen ion donor
Hint
2.
Calculate the H
+
ion and OH
-
ion concentrations in a 0.50
M
solution of HBr.
a.
[H
+
] = 1.0 × 10
-7
M
and [OH
-
] = 1.0 × 10
-7
M
b.
[H
+
] = 0.50
M
and [OH
-
] = 0.50
M
c.
[H
+
] = 0.50
M
and [OH
-
] = 2.0 × 10
-14
M
d.
[H
+
] = 0.50
M
and [OH
-
] = 2.0
M
Hint
3.
Which of the following compounds is not a salt?
a.
FeCl
2
b.
K
2
SO
4
c.
Mg(OH)
2
d.
BaCrO
4
Hint
4.
Which visual indicator would you choose to titrate HCl with NaOH? Acid Range Color pH Range Basic Range Color
a.
yellow 6.5 – 7.8 purple
b.
blue 3.4 – 4.6 yellow
c.
colorless 8.3 – 9.9 red
d.
pink 1.2 – 2.8 yellow
Hint
5.
What is the concentration of hydrogen ions in a solution that has a pH of 4.32?
a.
6.2 × 10
-4
M
b.
5.1 × 10
-4
M
c.
8.6 × 10
-5
M
d.
4.8 × 10
-5
M
Hint
6.
Which of the following is not a conjugate acid-base pair?
a.
H
2
O and OH
-
b.
H
3
O
+
and OH
-
c.
HCl and Cl
-
d.
HNO
3
and NO
3
-
Hint
7.
Calculate the pH of 0.075
M
KOH.
a.
11.12
b.
11.46
c.
12.88
d.
10.4
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.
At 298 K, pure water has a pH of __________.
a.
7
b.
0
c.
-14
d.
14
Hint
10.
A 0.001
M
solution of HCl is ____________.
a.
a concentrated acid solution
b.
a weak acid solution
c.
a dilute acid solution
d.
neutral
Hint
11.
When HClO
4
ionizes in water, ClO
4
-
is the ______________.
a.
conjugate acid
b.
conjugate base
c.
base
d.
acid
Hint
12.
pH is defined as __________.
a.
-log [OH
-
]
b.
-log [H
+
]
c.
log [H
+
]
d.
log [OH
-
]
Hint
13.
Neutralization is the chemical process in which ____________.
a.
hydrogen ions react with chloride ions to form hydrogen chloride
b.
sodium ions react with hydroxide ions to form sodium hydroxide
c.
sodium ions react with chloride ions to form sodium chloride
d.
hydrogen ions react with hydroxide ions to form water
Hint
14.
Calculate the pH of a solution that has a [OH
-
] = 2.50 × 10
-4
M
.
a.
10.40
b.
-3.60
c.
0.4
d.
3.6
Hint
15.
Which of the following salts will produce a basic solution?
a.
KCN
b.
NaCl
c.
Ca(NO
3
)
2
d.
KBr
Hint
16.
Which of the following cannot be a buffer?
a.
a mixture of a weak acid and a strong base
b.
a mixture of a weak acid and a weak base
c.
a mixture of a strong acid and a strong base
d.
a mixture of a strong acid and a weak base
Hint
17.
Which of the following is a strong base?
a.
HCOOH
b.
NH
3
c.
NaOH
d.
HCO
3
Hint
18.
Under what condition is the OH
-
ion concentration in water expected to be zero?
a.
in a solution of strong base
b.
in a solution of weak base
c.
never
d.
in a solution of strong acid
Hint
19.
Which of the following is the strongest base according to the BrØnsted-Lowry theory?
a.
I
-
b.
N
3
-
c.
Cl
-
d.
F
-
Hint
20.
A substance that contains hydrogen and produces H
+
ions in aqueous solution is a(n) ________.
a.
acid
b.
water
c.
salt
d.
base
Hint
