Acids and Bases
Practice Test
1.
A substance that contains hydrogen and produces H
+
ions in aqueous solution is a
n
________.
SC.A.2.4.1
a.
water
b.
acid
c.
base
d.
salt
2.
Which of the following would force the forward reaction to completion?
CaCO
3
s
+2H
3
O
+
aq
→ Ca
2+
aq
+3H
2
O
l
+CO
2
g
SC.A.1.4.4
a.
add CO
2
to the mixture
b.
add more Ca
2+
to the mixture
c.
conduct the experiment in an open container
d.
add base to neutralize the H
3
O
+
3.
When Δ G is zero, ______________.
SC.B.1.4.7
a.
the reaction is not spontaneous
b.
the reaction has no energy
c.
the reaction is spontaneous
d.
the reaction is at equilibrium
4.
A 0.001
M
solution of HCl is ____________.
SC.A.1.4.4
a.
neutral
b.
a dilute acid solution
c.
a weak acid solution
d.
a concentrated acid solution
5.
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?
SC.A.1.4.4
a.
rate order
b.
catalyst
c.
specific rate constant
d.
instantaneous rate
6.
Name the pair that contains an incorrect formula.
a.
aluminum phosphate AlPO
4
b.
silver carbonate AgCO
3
c.
iron
II
sulfite FeSO
3
d.
magnesium hydroxide Mg
OH
2
7.
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
?
SC.A.1.4.5
a.
4.0 x 10
-15
b.
8.1 x 10
-9
c.
5.3 x 10
-12
d.
1.2 x 10
-8
8.
Compared to strong acids, weak acids produce __________ ions and conduct electricity __________ efficiently.
SC.C.2.4.5
a.
more, less
b.
more, more
c.
fewer, more
d.
fewer, less
9.
What is the formula for ammonium bromide?
a.
NH
4
Br
b.
NH
4
Br
2
c.
NH
3
Br
d.
NH
4
2
Br
10.
Which of the following is a strong base?
SC.A.1.4.5
a.
NH
3
b.
HCO
3
-
c.
HCOOH
d.
NaOH
11.
What are the individual steps in a complex reaction known as?
a.
elementary steps
b.
rate-determining steps
c.
intermediate steps
d.
complex steps
12.
Which of the solubility product expressions is incorrect?
SC.A.1.4.4
a.
K
sp
Sb
2
S
3
=
Sb
2+
3
S
3-
2
b.
K
sp
Ag
2
S
=
Ag
+
2
S
2-
c.
K
sp
CuS
=
Cu
2+
S
2-
d.
K
sp
CaF
2
=
Ca
2+
F
-
2
13.
Neutralization is the chemical process in which ____________.
a.
hydrogen ions react with hydroxide ions to form water
b.
hydrogen ions react with chloride ions to form hydrogen chloride
c.
sodium ions react with chloride ions to form sodium chloride
d.
sodium ions react with hydroxide ions to form sodium hydroxide
14.
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
15.
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?
SC.B.1.4.1
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.
16.
What is the molecular compound name for hydrazine, N
2
H
4
?
Number of atoms
Prefix
1
mono-
2
di-
3
tri-
SC.A.2.4.2
a.
trinitrogen quatrohydride
b.
trinitrogen pentahydride
c.
dinitrogen tetrahydride
d.
dinitrogen hydride
17.
What is the formula for the binary compound of aluminum and nitrogen?
SC.A.1.4.1
a.
Al
2
N
b.
AlN
c.
Al
2
N
2
d.
AlN
2
18.
pH is defined as __________.
a.
log
OH
-
b.
-log
H
+
c.
log
H
+
d.
-log
OH
-
19.
Why is it possible to derive the ion product constant for water, but not for aqueous acids?
SC.A.1.4.5
a.
Aqueous acids never reach equilibrium.
b.
The concentration of pure water is constant.
c.
Water does not ionize completely.
d.
At a given temperature, aqueous acids have constant concentrations.
20.
A molecular system that is a dynamic process with two opposing reactions balancing each other is a
n
___________.
SC.A.1.4.4
a.
unreacted set of chemicals.
b.
spontaneous reaction
c.
nonspontaneous reaction
d.
chemical equilibrium
