The dissociation of potassium acetate

potassium acetate ($CH_3COOK $) can be dissociated in water. The process is as follows:

$CH_3COOK\ longrightarrow K ^ ++ CH_3COO ^ - $

Potassium ions ($K ^ + $) are relatively stable and do not react significantly with water in general aqueous solution environments. However, acetate ions ($CH_3COO ^ - $) exhibit unique chemical behaviors. Since acetic acid is a weak acid, the acetate ion will bind to the hydrogen ion ($H ^ + $) ionized by water and undergo a hydrolysis reaction:

$CH_3COO ^ - + H_2O\ rightleftharpoons CH_3COOH + OH ^ - $

This reaction increases the concentration of hydroxide ions ($OH ^ - $) in the solution, which in turn makes the solution alkaline. This hydrolysis equilibrium is affected by many factors, such as the increase in temperature. According to Le Chatelier's principle, the equilibrium will move towards endothermic direction, and the hydrolysis reaction will endothermic, so the temperature rise will promote the hydrolysis of acetate ions; if acid is added to the solution, the concentration of hydrogen ions increases, and the equilibrium moves in the opposite direction, inhibiting the hydrolysis of acetate ions; if alkali is added, the concentration of hydroxide ions increases, and the equilibrium moves in the opposite direction, inhibiting hydrolysis. In short, the dissociation of potassium acetate in water and the subsequent hydrolysis of acetate ions play a key role in the properties of its solution and related chemical reactions.