Dissociation of ammonium acetate in water

On the dissociation of ammonium acetate in water. Ammonium acetate is a salt composed of ammonium ion and acetate ion. When placed in water, it dissociates.

Ammonium acetate ($NH_ {4} Ac $) in water ($H_ {2} O $) dissociates according to the following formula: $NH_ {4} Ac\ longrightarrow NH_ {4 }^{+} + Ac ^{-}$ 。 During this process, ammonium ions ($NH_ {4 }^{+}$） and acetate ions ($Ac ^ {-} $) are separated from the crystal structure of ammonium acetate and dispersed between water molecules.

However, although ammonium acetate does dissociate in water, its dissociation is not complete. The capped ammonium ion will bind to the hydroxide ion ionized by water, and the hydrolysis reaction will occur: $NH_ {4 }^{+} + H_ {2} O\ rightleftharpoons NH_ {3} · H_ {2} O + H ^{+}$ ； The acetate ion will also bind to the hydrogen ion ionized by water, and the hydrolysis reaction will occur: $Ac ^{-} + {2} O\ rightleftharpoons HAc + OH ^{-}$ 。

The mutual influence of these two hydrolysis reactions makes the dissociation of ammonium acetate in the solution inhibited, so ammonium acetate is not completely dissociated in water. Although it is a strong electrolyte, it should be completely dissociated in theory, but the existence of hydrolysis makes the dissociation situation complicated and it is difficult to achieve complete dissociation. In short, the degree of dissociation of ammonium acetate in water is restricted by hydrolysis factors and cannot be regarded as complete dissociation.