The reaction of ammonium acetate dissolved in water
Ammonium acetate ($CH_ {3} COONH_ {4} $) is a strong electrolyte, which is completely ionized after dissolving in water: $CH_ {3} COONH_ {4}\ longrightarrow CH_ {3} COO ^{-} + NH_ {4 }^{+}$ 。

Water has a weak ionization equilibrium: $H_ {2} O\ rightleftharons poH ^{+} + O H ^{-}$ 。

$CH_ {3} COO ^ {-} $will bind water-ionized $H ^{+}$ ， hydrolysis reaction: $CH_ {3} COO ^{-} + H_ {2} O\ rightleftharpoons CH_ {3} COOH + OH ^{-}$ ；$ NH_ {4 }^{+}$ will bind water-ionized $OH ^{-}$ ， hydrolysis reaction: $NH_ {4 }^{+} + H_ {2} O\ rightleftharpoons NH_ {3}\ cdot H_ {2} O + H ^{+}$ 。

Since the ionization constants of acetic acid and ammonia monohydrate are similar, the degree of hydrolysis of $CH_ {3} COO ^ {-} $and $NH_ {4 }^{+}$ in ammonium acetate solution is equivalent, and the solution is close to neutral. The total hydrolysis ionic equation is: $CH_ {3} COO ^{-} + NH_ {4 }^{+} + H_ {2} O\ rightleftharons poons CH_ {3} COOH + NH_ {3}\ cdot H_ {2} O $. This reaction is reversible and there is a hydrolytic equilibrium. When conditions such as temperature, concentration, etc. are changed, the equilibrium will shift. Heating will promote the hydrolysis of ammonium acetate, and dilution with water will also promote its hydrolysis.