Research on the pH of ammonium acetate solution
There are currently 0.1 M ammonium acetate solutions, and the study of their pH value is quite important. Ammonium acetate is a salt of weak acid acetic acid and weak alkali ammonia water.

The ionization constant of acetic acid is similar to that of ammonia water. When ammonium acetate is dissolved in water, both acetate and ammonium ions are hydrolyzed. The hydrolysis of acetate ions makes the solution alkaline, and the hydrolysis equation is: $CH_3COO ^ - + H_2O\ rightleftharpoons CH_3COOH + OH ^ - $; the hydrolysis of ammonium ions makes the solution acidic, and the hydrolysis equation is: $NH_4 ^ ++ H_2O\ rightleftharpoons NH_3\ cdot H_2O + H ^ +$ 。

However, due to their similar ionization constants, the degree of hydrolysis between the two is equivalent, and they inhibit each other. Therefore, the 0.1M ammonium acetate solution is almost neutral, and its pH is about 7. This is based on the principle of chemical equilibrium and salt hydrolysis. In many chemical experiments and practical applications, clarifying the pH properties of 0.1 M ammonium acetate solution is helpful to accurately control the reaction conditions and achieve the desired experimental purpose.