Hydrolysis Equation of Ammonium Acetate
Ammonium acetate ($CH_ {3} COONH_ {4} $) is a weak acid and alkali salt, which will undergo hydrolysis reaction in aqueous solution. The ionic equation for its hydrolysis is: $CH_ {3} COO ^{-} + NH_ {4 }^{+} + H_ {2} O\ rightleftharpoons CH_ {3} COOH + NH_ {3}\ cdot H_ {2} O $.

From the hydrolysis equation, it can be seen that the acetate ion ($CH_ {3} COO ^ {-} $) binds to the hydrogen ion ($H ^{+}$）， ammonium ion ($NH_ {4 }^{+}$） binds to the water ionized hydroxide ion ($OH ^{-}$）， to promote the positive ionization equilibrium of water. Since the ionization constants of acetic acid and ammonia monohydrate are similar, the ammonium acetate solution is basically neutral. This hydrolysis reaction is a reversible reaction. When the hydrolysis equilibrium is reached, the concentration of each substance remains relatively stable. In practice, factors such as temperature and concentration will affect the hydrolysis equilibrium. When the temperature increases, the equilibrium moves towards endothermic hydrolysis; when the concentration of ammonium acetate increases, the hydrolysis equilibrium moves forward, but the degree of hydrolysis decreases.