Dissociation Constants Of Inorganic Acids And Bases
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1
2DISSOCIATION CONSTANTS OF INORGANIC ACIDS AND BASES
The data in this table are presented as values of pK
, defined as
can be calculated from the equation
a
the negative logarithm of the acid dissociation constant K
for the
a
−
+
reaction
OH
NH
4
K
=
K
/
K
=
b
water
a
[
]
NH
BH
B
+ H
3
–
+
= 1.01 × 10
where K
at 25 °C. Note that pK
+ pK
= pK
.
–14
Thus pK
= –log K
, and the hydrogen ion concentration [H
] can
+
water
a
b
water
a
a
All values refer to dilute aqueous solutions at zero ionic strength
be calculated from
at the temperature indicated. The table is arranged alphabetically
by compound name.
+
−
H
B
K
=
a
[
]
BH
Reference
In the case of bases, the entry in the table is for the conjugate acid;
1. Perrin, D. D., Ionization Constants of Inorganic Acids and Bases in
e.g., ammonium ion for ammonia. The OH
concentration in the
–
Aqueous Solution, Second Edition, Pergamon, Oxford, 1982.
system
NH
+ H
O
NH
+ OH
+
–
3
2
4
Name
Formula
Step
t/°C
pK
a
Aluminum(III) ion
Al
25
5.0
+3
Ammonia
NH
25
9.25
3
Arsenic acid
H
AsO
1
25
2.26
3
4
2
25
6.76
3
25
11.29
Arsenious acid
H
AsO
25
9.29
2
3
Barium(II) ion
Ba
25
13.4
+2
Boric acid
H
BO
1
20
9.27
3
3
2
20
>14
Calcium(II) ion
Ca
+2
25
12.6
Carbonic acid
H
CO
1
25
6.35
2
3
2
25
10.33
Chlorous acid
HClO
25
1.94
2
Chromic acid
H
CrO
1
25
0.74
2
4
2
25
6.49
Cyanic acid
HCNO
25
3.46
Germanic acid
H
GeO
1
25
9.01
2
3
2
25
12.3
Hydrazine
N
H
25
8.1
2
4
Hydrazoic acid
HN
25
4.6
3
Hydrocyanic acid
HCN
25
9.21
Hydrofluoric acid
HF
25
3.20
Hydrogen peroxide
H
O
25
11.62
2
2
Hydrogen selenide
H
Se
1
25
3.89
2
2
25
11.0
Hydrogen sulfide
H
S
1
25
7.05
2
2
25
19
Hydrogen telluride
H
Te
1
18
2.6
2
2
25
11
Hydroxylamine
NH
OH
25
5.94
2
Hypobromous acid
HBrO
25
8.55
Hypochlorous acid
HClO
25
7.40
Hypoiodous acid
HIO
25
10.5
Iodic acid
HIO
25
0.78
3
Lithium ion
Li
25
13.8
+
Magnesium(II) ion
Mg
25
11.4
+2
Nitrous acid
HNO
25
3.25
2
Perchloric acid
HClO
20
-1.6
4
Periodic acid
HIO
25
1.64
4
Phosphoric acid
H
PO
1
25
2.16
3
4
8-40
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