Salt hydrolysis
It is reaction of the cation or the anion or both the ions of the salt with water to produce the acidic or basic solution. Hydrolysis is reverse of neutralization.
![935_Salts.png](https://www.expertsmind.com/../CMSImages/935_Salts.png)
(1) Hydrolysis constant : The general equation for the hydrolysis of a salt (let it be BA), ![1702_Salts1.png](https://www.expertsmind.com/../CMSImages/1702_Salts1.png)
Applying the law of chemical equilibrium, we can get
, here K is equilibrium constant.
Since water is present in very large excess in the aqueous solution, its concentration [H2O] may be regarded as constant so,
![814_Salts3.png](https://www.expertsmind.com/../CMSImages/814_Salts3.png)
where Kh is called the hydrolysis constant.
(2) Degree of hydrolysis : It is defined as the fraction (or percentage) of the total salt which is hydrolysed at the equilibrium. For instance, if 90% of a salt solution is hydrolysed, it's the degree of hydrolysis and is 0.90% or as 90%. It is generally represented by h.
![2182_Salts4.png](https://www.expertsmind.com/../CMSImages/2182_Salts4.png)
Types of salt
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Exp. for Kh
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Exp. for h
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Exp. for pH
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(i) Salt of weak acid and strong base
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Kh=Kw / Ka
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![2481_Salts5.png](https://www.expertsmind.com/../CMSImages/2481_Salts5.png)
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pH=- [log Kw+log Ka- log C]
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(ii) Salt of strong acid and weak base
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Kh=Kw / Kb
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![1387_Salts6.png](https://www.expertsmind.com/../CMSImages/1387_Salts6.png)
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pH=- [log Kw- log Kb+ log C]
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(iii) Salt of weak acid and weak base
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|
![1798_Salts7.png](https://www.expertsmind.com/CMSImages/1798_Salts7.png)
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pH=- [log Ka+ log Kw- log Kb]
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(iv) Salts of the strong acids and strong bases do not undergo hydrolysis (they undergo only the ionization process) hence the resulting aqueous solution is neutral in nature.
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