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Ionic equilibrium
Ionic equilibrium
1.
Degree of dissociation or ionization
=
For strong electrolytes
1, for weak electrolyte
< < 1
2.
Ostwald's dilution law
For a weak electrolyte of type A
+
B
-
dissociation constant, k =
or
=
Where C = Concentration
K – Dissociation constant
V = Volume
3.
For weak monobasic acids
=
for weak non acidic bases
=
K
a
= dissociation constant of weak acid
K
b
= dissociation constant of weak base
4.
Relative strength of two acids
5.
Ionic product of water, Kw =
or
= 10
-14
at 25°C
6.
pH =
pKw = pH + pOH = 14 at 25°C
and pKa + pKb = 14
where pKa = - log Ka and pKb = - log Kb
7.
If the solubility of a salt like A
2
B
3
is S mol L
-1
, then
Solubility product Ksp = (2s)
2
(3s)
3
= 108 s
5
8.
pH of an acidic buffer is given by Henderson equation
pH = pKa + log
pH of a basic buffer is given by
pOH = pKb + log
and then pH = 14 - pOH.
9.
Buffer capacity =
or
=
10.
For salts of weak acid and strong base hydrolysis constant, K
h
=
Degree of hydrolysis h =
=
pH =
11.
For salts of strong acid and weak base
K
h
=
H =
pH =
12.
For salts of weak acid and weak base
hydrolysis constant K
h
=
pH =
13.
In case of salt of weak acid and weak base, nature of medium hydrolysis is decided as :
(i) If K
a
= K
b
(medium will be neutral)
(ii) If K
a
> K
b
(medium will be acidic)
(iii) If K
a
< K
b
, (medium will be basic)
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