1. Hydrolysis  dissociation with water  reaction with water
Hydrolysis can be defined as the reaction of a chemical subtance with water.
Acid + water  ionize / dissociated into ions
Base + water  ionize / dissociated into ions
Salts + water  ionize (do not hydrolyzed)
 ionize & hydrolyzed
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10. Salts do not hydrolyzed  salts from a strong acid and strong base
 The ions of salts which come from a strong acid and strong base do not react to water.
 pH the solution of the salts theoretically is equal to seven
(pH = 7)
NaCl  Na+ + Cl-
Na+ + H2O  do not react
Cl- + H2O  do not react
HCl  H Cl-
a weak conjugate base
A strong acid
HCN  H CN-
a strong conjugate base
A weak acid
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11. 2. Salts will be hydrolyzed partially
Salts from a weak acid and strong base  pH > 7
sallts from a strong acid and weak base  pH < 7
NaCN (aq)  Na+ + CN-
Na+ + H2O  do not react
CN- + H2O  HCN + OH-  Hydrolysis reaction from NaCN salt , produce OH- ion
NH4Cl (aq)  NH Cl-
NH H2O  NH4OH + H+  Hydrolysis reaction from NH4Cl salt , produce H+ ion
Cl H2O  do not react
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12. 3. Salts will be hydrolyzed completely
from a weak acid and a weak base  All ions of salts from a weak acid and a weak base can react with water to produce both H+ and OH- ions, so the property of the solution is determined by equilibrium constant of the weak acid and weak base produced.
Ex:
NH4CN (aq)  NH CN-
NH H2O  NH4OH + H+
CN H2O  HCN + OH-
NH4+ + CN- + H2O  NH4OH + HCN  Hydrolysis reaction from NH4CN salt
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13. NH4CN (aq)  NH4+ + CN- pH > 7  Ka < Kb pH = 7  Ka = Kb
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