Acids and Bases
Practice Test
1.
Why is it possible to derive the ion product constant for water, but not for aqueous acids?
a.
Aqueous acids never reach equilibrium.
b.
Water does not ionize completely.
c.
The concentration of pure water is constant.
d.
At a given temperature, aqueous acids have constant concentrations.
2.
What is the slowest of the elementary steps in a complex reaction called?
a.
mechanism
b.
fast step
c.
rate-limiting step
d.
propagating step
3.
A substance that contains hydrogen and produces H
+
ions in aqueous solution is a(n) ________.
a.
acid
b.
base
c.
salt
d.
water
4.
What is the net ionic equation for the neutralization reaction between HF and KOH?
a.
H
+
+ KOH → H
2
O + K
+
b.
K
+
+ F
-
→ KF
c.
HF + OH
-
→ H
2
O + F
-
d.
H
+
+ OH
-
→ H
2
O
5.
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
)/[NH
4
NO
3
]
2
b.
K
eq
= [NH
3
][NO][H
2
][O2]
c.
K
eq
= ([NH
3
][NO][H
2
][O2])/[NH
4
NO
3
]
d.
K
eq
= [NH
3
]
2
[NO]
2
[H
2
][O2]
2
6.
For the reaction, H
2
(g) + Cl
2
(g) → 2HCl(g) + heat, what will be the effect on the equilibrium constant,
K
eq
, if the pressure of the vessel is decreased at constant temperature?
a.
K
eq
increases
b.
K
eq
decreases
c.
The question cannot be answered without knowing the initial value of
K
eq
.
d.
K
eq
does not change
7.
The value of the
K
sp
for SrSO
4
is 2.8 x 10
-7
. What is the molar solubility of SrSO
4
?
a.
7.6 x 10
-7
M
b.
5.8 x 10
-13
M
c.
5.7 x 10
-3
M
d.
5.3 x 10
-4
M
8.
What is the name given to the simplest ratio of ions in an ionic compound?
a.
formula unit
b.
mole
c.
monatomic ion
d.
empirical formula
9.
The acid ionization constant,
K
a
, is __________ for __________ acids.
a.
smallest, weak
b.
largest, anhydride
c.
smallest, strong
d.
largest, weak
10.
The correct molecular compound name for H
2
O
2
is ________.
a.
hydrogen dioxide
b.
hydrogen oxide
c.
dihydrogen dioxide
d.
dihydrogen monoxide
11.
For the system, H2(g) + CO2(g) → H2O(g) + CO(g) at equilibrium, the addition of H2(g) would cause ____________.
a.
only more CO to form
b.
only more CO
2
to form
c.
only more H
2
O to form
d.
more H
2
O and CO to form
12.
Consider the following reaction in which all reactants and products are gases. 1.00 mole of A and 2.00 moles of B are placed in a 5.0—L container. After equilibrium has been established, 0.50 mole of D is present. What is the equilibrium constant for this reaction: A + 2B → 2C + D?
a.
1
b.
3
c.
0.15
d.
0.33
13.
Under what condition is the OH
-
ion concentration in water expected to be zero?
a.
never
b.
in a solution of strong acid
c.
in a solution of weak base
d.
in a solution of strong base
14.
A 0.001
M
solution of HCl is ____________.
a.
a weak acid solution
b.
a concentrated acid solution
c.
neutral
d.
a dilute acid solution
15.
Which of the following cannot be a buffer?
a.
a mixture of a strong acid and a strong 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 weak acid and a weak base
16.
If NaCl is added to a 0.010M solution of AgNO
3
in water at 25°C, what will be [Cl
-
] when precipitation of AgCl begins? The Ksp for AgCl is 1.8 x 10
-10
.
a.
1.3 x 10
-6
M
b.
1.0 x 10
-10
M
c.
1.8 x 10
-8
M
d.
1.8 x 10
-12
M
17.
Which one of the following classifications of ions in the table contains an error?
Hydroxide
OH
-
monatomic
anion
carbonate
CO
3
2-
polyatomic
anion
ammonium
NH
4+
polyatomic
cation
magnesium
Mg
2+
monatomic
cation
a.
carbonate
b.
magnesium
c.
hydroxide
d.
ammonium
18.
Calculate the pH of 0.075
M
KOH.
a.
11.12
b.
10.4
c.
11.46
d.
12.88
19.
What is the correct name for HBr in an aqueous solution?
a.
bromous acid
b.
bromic acid
c.
hydrobromic acid
d.
hydrogen bromide
20.
What is the name given to a chemical produced in one elementary step and used up in a subsequent elementary step?
a.
intermediate
b.
complex step
c.
elementary step
d.
reaction mechanism
