The dissociation equation of ammonium acetate
ammonium acetate ($CH_ {3} COONH_ {4} $) will dissociate in aqueous solution, and the dissociation equation is: $CH_ {3} COONH_ {4}\ rightleftharpoons CH_ {3} COO ^ {-} + NH_ {4 }^{+}$ 。

The acetate ion ($CH_ {3} COO ^ {-} $) will undergo hydrolysis reaction and combine with the water-ionized hydrogen ion ($H ^ {+} $), $CH_ {3} COO ^ {-} + H_ {2} O\ rightleftharpoons CH_ {3} COOH + OH ^ {-} $; Ammonium ion ($NH_ {4 }^{+}$） will also hydrolyze and combine with the water-ionized hydroxide ion ($OH ^ {-} $), $NH_ {4} ^ {+} + H_ {2} O\ rightleftharpoons NH_ {3}\ cdot H_ {2} O + H ^{+}$ 。 Due to the similar ionization constants of acetic acid and ammonia monohydrate, ammonium acetate solutions are close to neutral. The dissociation and hydrolysis of ammonium acetate is of great significance in many chemical systems. For example, in the configuration of buffer solutions and some chemical reactions involving ion balance, the presence of ammonium acetate will have a significant impact on the pH and ion concentration of the system. The dissociation process follows the principle of chemical equilibrium. When external conditions such as temperature and concentration change, the dissociation equilibrium will move accordingly to reach a new equilibrium state.