The neutralization of aqueous acetic acid and aqueous barium hydroxide
There is now a solution of acetic acid ($CH_3COOH $) dissolved in water, and a solution of barium hydroxide ($Ba (OH) _2 $) dissolved in water. Acetic acid partially ionizes in water, and its ionization equation is $CH_3COOH\ rightleftharpoons CH_3COO ^ - + H ^ + $. Barium hydroxide is a strong base and completely ionizes in water. Its ionization equation is $Ba (OH) _2 = Ba ^ {2 + } + 2 ^ OH - $.

When the two meet, $H ^ + $combines with $OH ^ - $to form water, and $CH_3COO ^ - $and $Ba ^ {2 +} $exist in solution. The ionic reaction equation is: $2CH_3COOH + Ba ^ {2 + } + 2 OH ^ - = Ba ^ {2 + } + 2CH_3COO ^ - + 2H_2O $, and the ionic reaction on both sides is $CH_3COOH + OH ^ - = CH_3COO ^ - + H_2O $.

This neutralization reaction is the interaction of acid and base, which weakens the acidity and alkalinity of the solution and tends to be neutral. Heat is released during the reaction, which is an exothermic reaction. Looking at its macroscopic performance, the temperature of the solution may appear to rise. The final solution, if the two just react completely, is barium acetate ($Ba (CH_3COO) _2 $). Barium acetate is a strong base and weak acid salt, which hydrolyzes in water, making the solution slightly alkaline.