Redox Reactions
Practice Test
1.
Calculate the pH of 0.075
M
KOH.
a.
12.88
b.
10.4
c.
11.12
d.
11.46
2.
A 0.001
M
solution of HCl is ____________.
a.
neutral
b.
a concentrated acid solution
c.
a weak acid solution
d.
a dilute acid solution
3.
Which of these is a product of the first step in the ionization of phosphoric acid, H
3
PO
4
?
a.
PO
4
b.
HPO
4
c.
H
3
PO
4
d.
H
2
PO
4
4.
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 ´ 10
-14
M
b.
[H
+
] = 0.50
M
and [OH
-
] = 2.0
M
c.
[H
+
] = 0.50
M
and [OH
-
] = 0.50
M
d.
[H
+
] = 1.0 ´ 10
-7
M
and [OH
-
] = 1.0 ´ 10
-7
M
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.
When the following equation is balanced what is the coefficient of Sn?
Sn + HNO
3
→ SnO
2
+ NO
2
+ H
2
O
a.
3
b.
4
c.
1
d.
2
7.
When a solution has a pH of 4, what is the pOH of that solution?
a.
18
b.
7
c.
10
d.
4
8.
Which of the following reactions is a redox reaction?
a.
CaBr
2
(aq) + H
2
SO
4
(aq) → CaSO
4
(s) + 2HBr(aq)
b.
2Al(s) + 3H
2
SO
4
(aq) → Al
2
(SO
4
)
3
(aq) + 3H
2
(g)
c.
H
+
(aq) + OH
-
(aq) → H
2
O(l)
d.
2KBr(aq) + Pb(NO
3
)
2
(aq) → 2KNO
3
(aq) + PbBr
2
(s)
9.
A balanced reaction that shows only the oxidation process is a ___________.
a.
half-reaction
b.
balanced chemical equation
c.
single-replacement reaction
d.
synthesis reaction
10.
Which of the solubility product expressions is incorrect?
a.
K
sp
(CaF
2
) = [Ca
2+
][F
-
]
2
b.
K
sp
(Ag
2
S) = [Ag
+
]
2
[S
2-
]
c.
K
sp
(Sb
2
S
3
) = [Sb
2+
]
3
[S
3-
]
2
d.
K
sp
(CuS) = [Cu
2+
][S
2-
]
11.
Balance the following ionic equation. What is the coefficient of the reducing agent in this reaction?
Fe
2+
(aq) + MnO
4
-
(aq) + H
+
(aq) → Fe
3+
(aq) + Mn
2+
(aq) + H
2
O(l)
a.
5
b.
8
c.
4
d.
1
12.
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 strong acid
c.
never
d.
in a solution of weak base
13.
Which of the following types of reactions do not usually involve redox?
a.
synthesis
b.
decomposition
c.
double-replacement
d.
single-replacement
14.
When Δ G is zero, ______________.
a.
the reaction is at equilibrium
b.
the reaction is spontaneous
c.
the reaction has no energy
d.
the reaction is not spontaneous
15.
The acid ionization constant,
K
a
, is __________ for __________ acids.
a.
smallest, weak
b.
largest, anhydride
c.
smallest, strong
d.
largest, weak
16.
Neutralization is the chemical process in which ____________.
a.
sodium ions react with chloride ions to form sodium chloride
b.
sodium ions react with hydroxide ions to form sodium hydroxide
c.
hydrogen ions react with chloride ions to form hydrogen chloride
d.
hydrogen ions react with hydroxide ions to form water
17.
What is the equilibrium constant expression for the following reaction?
H
2
+ I
2
‹–› 2HI
a.
K
eq
= [H
2
][I
2
]/ [HI]
2
b.
K
eq
= [HI]
2
/[H
2
][I
2
]
c.
K
eq
= [HI]
2
/[H]
2
[I]
2
d.
K
eq
= [2HI]/ /[H
2
][I
2
]
18.
What is the net change in oxidation number of iodine in the following ionic reaction?
2MnO
4
-
+ I
-
+ H
2
O → 2MnO
2
+ IO
3
-
+ 2OH
-
a.
2
b.
3
c.
1
d.
6
