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MHT-CET : Chemistry Entrance Exam

MHT - CET : Chemistry - Ionic Equilibria Page 5

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17.

Hydrolysis

 

Hydrolysis of Salt:
The reaction in which the anions or the cations or both of a salt react with water to produce acidity or basicity is called hydrolysis.

  • Degree of Hydrolysis (h):
    The fraction of total number of moles of the salt which has undergone hydrolysis at equilibrium is called the degree of hydrolysis of the electrolyte.
  • Hydrolysis Constant (kh):
    The equilibrium constant of the hydrolysis equilibrium of a salt is called hydrolysis constant of the salt.

    Salts of strong acid and strong base do not undergo hydrolysis.
  • Degree of Hydrolysis of Strong Acid and Weak Base:

Kh = h2C

or

h =

h = degree of hydrolysis

\ h

C = Concentration, mol dm-3

Kh = Hydrolysis constant

  • Weak Acid - Strong Base:

Kh = h2C

or

h =

h = degree of hydrolysis

\ h

C = Concentration, mol dm-3

Kh = Hydrolysis constant

  • Weak Acid - Weak Base:

Kh

=

h2<

h

=



 

 

18.

Relation Between Hydrolysis Constant, Dissociation Constant of Acid and Ionic Product of Water

 

For weak acid - strong base:

    

Kh =

Kw

Ka

For strong acid - weak base:

 

Kh =

Kw

Kb

For weak acid - weak base:

 

Kh =

Kw

Ka Kb

 

where

Kw = ionic product of water

 

Kh = hydrolysis constant
Ka and Kb = dissociation constant for an acid and base respectively.

 

 

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