Acids and Bases
Practice Test
1.
A molecular system that is a dynamic process with two opposing reactions balancing each other is a(n) ___________.
a.
chemical equilibrium
b.
nonspontaneous reaction
c.
spontaneous reaction
d.
unreacted set of chemicals.
2.
Compared to strong acids, weak acids produce __________ ions and conduct electricity __________ efficiently.
a.
fewer, more
b.
more, less
c.
fewer, less
d.
more, more
3.
Which of the following is the formula for nitric acid?
Formula
Acid Name
H
2
SO
3
Sulfurous acid
H
2
SO
4
Sulfuric acid
a.
HN
b.
HNO
2
c.
HNO
d.
HNO
3
4.
What is the name given to a chemical produced in one elementary step and used up in a subsequent elementary step?
a.
elementary step
b.
reaction mechanism
c.
intermediate
d.
complex step
5.
How many grams of MgF
2
will dissolve in 150 mL of 0.100
M
NaF solution? Ksp for MgF
2
is 6.4 x 10
-9
.
a.
1.0 x 10
-5
g
b.
4.1 x 10
-6
g
c.
6.4 x 10
-7
g
d.
6.0 x 10
-6
g
6.
H
2
SO
4
is a ____________.
a.
monoprotic acid
b.
monoprotic base
c.
diprotic base
d.
diprotic acid
7.
What is the equilibrium constant expression for the following reaction?
2NH
4
NO
3
(s) → 2NH
3
(g) + 2NO(g) + H
2
(g) + 2O
2
(g)
a.
K
eq
= [NH
3
]
2
[NO]
2
[H
2
][O2]
2
b.
K
eq
= ([NH
3
]
2
[NO]
2
[H
2
][O2]
2
)/[NH
4
NO
3
]
2
c.
K
eq
= ([NH
3
][NO][H
2
][O2])/[NH
4
NO
3
]
d.
K
eq
= [NH
3
][NO][H
2
][O2]
8.
For the reaction, 2SO
2
(g) + O
2
(g) → 2SO
3
(g) + heat, at equilibrium, what will be the effect on the net amount of SO
3
present if the temperature of the container is increased?
a.
The concentration of SO
3
remains the same.
b.
The concentration of SO
3
increases.
c.
This question cannot be answered without knowing the value of Keq.
d.
The concentration of SO
3
decreases.
9.
A 0.001
M
solution of HCl is ____________.
a.
a dilute acid solution
b.
a weak acid solution
c.
a concentrated acid solution
d.
neutral
10.
For the reaction, 2SO
2
(g) + O
2
(g) → 2SO
3
(g) at equilibrium, what will be the effect on the net amount of SO
3
present if the volume of the container is increased?
a.
The concentration of SO
3
will increase.
b.
The concentration of SO
3
will decrease.
c.
The concentration of SO
3
will remain the same.
d.
This question cannot be answered without knowing the value of Keq.
11.
What kind of ion is iodide (I
-
)?
a.
polyatomic anion
b.
polyatomic cation
c.
monatomic anion
d.
monatomic cation
12.
A solution of pH = 2.1 would be described as __________.
a.
slightly acidic
b.
distinctly basic
c.
slightly basic
d.
distinctly acidic
13.
What is the correct name for H
2
SO
3
in an aqueous solution?
a.
hydrosulfuric acid
b.
hydrosulfic acid
c.
sulfuric acid
d.
sulfurous acid
14.
Sulfate (SO
4
2-
) is a ____________.
a.
monatomic cation
b.
polyatomic anion
c.
monatomic anion
d.
polyatomic cation
15.
What quantity is defined by the change in concentration of a component in a chemical reaction divided by the change in time of the reaction?
a.
rate order
b.
catalyst
c.
specific rate constant
d.
instantaneous rate
16.
What is the net ionic equation for the neutralization reaction between HF and KOH?
a.
K
+
+ F
-
→ KF
b.
HF + OH
-
→ H
2
O + F
-
c.
H
+
+ KOH → H
2
O + K
+
d.
H
+
+ OH
-
→ H
2
O
17.
Neutralization is the chemical process in which ____________.
a.
sodium ions react with hydroxide ions to form sodium hydroxide
b.
hydrogen ions react with chloride ions to form hydrogen chloride
c.
hydrogen ions react with hydroxide ions to form water
d.
sodium ions react with chloride ions to form sodium chloride
18.
The molar solubility for BaCO
3
is 9.0 x 10
-5
M
at 25°C. What is the solubility product constant,
K
sp
, for BaCO
3
?
a.
8.1 x 10
-9
b.
4.0 x 10
-15
c.
1.2 x 10
-8
d.
5.3 x 10
-12
19.
Which of the following is a weak acid?
a.
HF
b.
HNO
3
c.
HCl
d.
HClO
4
20.
Calculate the pH of a solution that has a [OH
-
] = 2.50 x 10
-4
M
.
a.
-3.6
b.
3.6
c.
0.4
d.
10.4
