Chemistry Reference
In-Depth Information
19.35
Label each of the species in the following equations as
an acid or a base, and connect the conjugate pairs:
ment: Dilution of a weak base causes an increase in
percentage of ionization.
19.45
Which base in Table 19.2 has the highest hydroxide ion
concentration in 0.180 M solution?
HNO
2
(aq)
H
2
O(
/
) E NO
2
(aq)
H
3
O
(aq)
C
5
H
5
N(aq)
H
2
O(
/
) E C
5
H
5
NH
(aq)
OH
(aq)
19.36 Label each of the species in the following equations as
an acid or a base, and connect the conjugate pairs:
19.3 Autoionization of Water
19.46
Calculate the pH of a solution having each of the follow-
ing hydroxide ion concentrations:
(a)
H
3
PO
4
(aq)
OH
(aq) E H
2
PO
4
(aq)
H
2
O(
/
)
H
2
PO
4
(aq)
OH
(aq) E HPO
2
(aq)
H
2
O(
/
)
1.17
10
6
M
5.00
10
13
M
(b)
4
HPO
2
4
(aq)
OH
(aq) E PO
3
4
(aq)
H
2
O(
/
)
4.14
10
7
M
(c)
19.47
Calculate the hydronium ion concentration of a solution
having each of the following pH values:
(a) 2.000
19.37 Label each of the species in the following equations as
an acid or a base, and connect the conjugate pairs:
SO
2
3
(aq)
H
2
O(
/
) E HSO
3
(aq)
OH
(aq)
(b) 12.000
(c) 0.000
(d) 14.000 (e) 7.000
19.48
Calculate the hydroxide ion concentration of a solution
having each of the following pH values:
(a) 4.419 (b) 12.509 (c) 6.39
19.49 What is the hydroxide ion concentration of a solution
having each of the following pH values?
(a) 3.414 (b) 8.010 (c) 13.595
19.50
Calculate the pH of a solution having each of the follow-
ing hydroxide ion concentrations:
(a)
NH
4
(aq)
H
2
O(
/
) E NH
3
(aq)
H
3
O
(aq)
19.38
Label each of the species in the following equations as
an acid or a base, and connect the conjugate pairs:
HSO
4
(aq)
H
3
O
(aq) E H
2
SO
4
(aq)
H
2
O(
/
)
HSO
4
(aq)
OH
(aq) E SO
2
(aq)
H
2
O(
/
)
4
19.2 Dissociation Constants
19.39
Calculate the ammonia concentration and the ammonium
ion concentration in each of the following solutions:
(a) 0.180 mol of
6.2
10
4
M
9.93
10
8
M
(b)
4.55
10
12
M
NH
3
and 0.060 mol of
NH
4
Cl
in 1.00 L
(c)
19.51
Calculate the hydronium ion concentration of a solution
having each of the following pH values:
(a) 5.113 (b) 13.017 (c) 4.640
19.52
Calculate the pH of each of the following solutions:
(a)
of solution
(b) 0.240 mol of
NH
3
and 0.060 mol of HCl in 1.00 L of
solution
(c) Do you need to use for these calculations?
19.40 A 0.200 M solution of a weak base, represented as B, has
a hydroxide ion concentration of
K
b
6.16
10
3
M
KOH
6.74
10
5
M.
Calcu-
1.73
10
4
M
late the value of
K
b
for B. The equation for the ionization
(b)
(c)
19.53 Calculate the pH of each of the following solutions:
(a) 0.00100 M
HClO
3
of this base is
5.00
10
3
M
Ba(OH)
2
B(aq)
H
2
O(
/
) E BH
(aq)
OH
(aq)
19.41
A 0.100 M solution of a weak acid, represented as HA,
has a hydronium ion concentration of
Calculate the value of
H
2
SO
4
(b) 0.0250 M NaOH
2.50
10
5
M.
(c) 0.330 M NaCl
19.54 What is the hydroxide ion concentration of a solution
having each of the following pH values?
(a) 0.500 (b) 9.73 (c) 13.73
19.55 Calculate the pH of each of the following solutions:
(a)
(b)
19.56
Calculate the pH of each of the following solutions:
(a) 0.0100 M HBr
K
a
for HA. The equation for the
ionization of this acid is
H
2
O(
/
) E H
3
O
(aq)
A
(aq)
HA(aq)
19.42
Calculate the hydronium ion concentration of 0.350 M
formic acid,
19.43 Calculate the hydronium ion concentration of 0.100 M
phenol,
K
a
1.7
10
4
HCHO
2
.
7.15
10
3
M
HNO
3
K
a
1.3
10
10
HOC
6
H
5
.
2.42
10
3
M
Ba(OH)
2
HOC
6
H
5
(aq)
H
2
O(
/
) E OC
6
H
5
(aq)
H
3
O
(aq)
19.44
Calculate the percent ionization of pyridine, in
(a) a 1.00 M solution, (b) a 0.100 M solution, and (c) a
0.0500 M solution. Tabulate the initial concentration
of pyridine, the hydroxide ion concentration, and the
percent ionization for these cases. Explain the state-
C
5
H
5
N,
(b) 0.0100 M KOH
(c) 0.0100 M NaBr
19.57
A 0.199 M solution of a weak base, represented as B, has
a pH of 11.57. Calculate the value of
K
b
for B.
