Acids and Bases
Practice Test
1.
pH is defined as __________.
a.
-log [H
+
]
b.
log [H
+
]
c.
log [OH
-
]
d.
-log [OH
-
]
2.
H
2
SO
4
is a ____________.
a.
monoprotic acid
b.
monoprotic base
c.
diprotic base
d.
diprotic acid
3.
Identify a conjugate acid-base pair in the reaction NH
3
+ H
2
O ‹–› NH
4
+
+ OH
-
a.
H
2
O and NH
4
+
b.
NH
3
and OH
-
c.
H
2
O and OH
-
d.
NH
3
and H
2
O
4.
What will a nonmetallic anhydride produce in aqueous solution?
a.
base
b.
salt
c.
solid precipitate
d.
acid
5.
Which of the following cannot be a buffer?
a.
a mixture of a weak acid and a weak base
b.
a mixture of a weak acid and a strong base
c.
a mixture of a strong acid and a weak base
d.
a mixture of a strong acid and a strong base
6.
According to the BrÆnsted-Lowry theory, a base is a(n) ___________.
a.
electron pair donor
b.
electron pair acceptor
c.
hydrogen ion acceptor
d.
hydrogen ion donor
7.
Which of the following salts will produce a basic solution?
a.
Ca(NO
3
)
2
b.
KCN
c.
KBr
d.
NaCl
8.
The acid ionization constant,
K
a
, is __________ for __________ acids.
a.
largest, weak
b.
smallest, weak
c.
largest, anhydride
d.
smallest, strong
9.
Compared to strong acids, weak acids produce __________ ions and conduct electricity __________ efficiently.
a.
more, less
b.
fewer, more
c.
more, more
d.
fewer, less
10.
Neutralization is the chemical process in which ____________.
a.
hydrogen ions react with chloride ions to form hydrogen chloride
b.
sodium ions react with chloride ions to form sodium chloride
c.
hydrogen ions react with hydroxide ions to form water
d.
sodium ions react with hydroxide ions to form sodium hydroxide
11.
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
-
] = 0.50
M
c.
[H
+
] = 0.50
M
and [OH
-
] = 2.0 ´ 10
-14
M
d.
[H
+
] = 1.0 ´ 10
-7
M
and [OH
-
] = 1.0 ´ 10
-7
M
12.
When a solution has a pH of 4, what is the pOH of that solution?
a.
7
b.
4
c.
18
d.
10
13.
Calculate the pH of a solution that has a [OH
-
] = 2.50 x 10
-4
M
.
a.
10.4
b.
0.4
c.
3.6
d.
-3.6
14.
A 0.001
M
solution of HCl is ____________.
a.
a weak acid solution
b.
neutral
c.
a concentrated acid solution
d.
a dilute acid solution
15.
What is the net ionic equation for the neutralization reaction between HF and KOH?
a.
H
+
+ OH
-
→ H
2
O
b.
H
+
+ KOH → H
2
O + K
+
c.
K
+
+ F
-
→ KF
d.
HF + OH
-
→ H
2
O + F
-
16.
A substance that contains hydrogen and produces H
+
ions in aqueous solution is a(n) ________.
a.
acid
b.
salt
c.
base
d.
water
17.
Why is it possible to derive the ion product constant for water, but not for aqueous acids?
a.
Aqueous acids never reach equilibrium.
b.
At a given temperature, aqueous acids have constant concentrations.
c.
Water does not ionize completely.
d.
The concentration of pure water is constant.
18.
Calculate the pH of 0.075
M
KOH.
a.
10.4
b.
12.88
c.
11.12
d.
11.46
