Barium acetate dissolves in water
Now there is barium acetate, and when it is placed in water, it will dissolve and change. Barium acetate, according to the chemical formula, is $ (CH_ {3} COO) _ {2} Ba $. When it enters water, the water molecules are active and interact with barium acetate.

Barium acetate has a strong electrolyte. Its dissociation state in water is as follows: $ (CH_ {3} COO) _ {2} Ba\ stackrel {H_ {2} O }{=\!=\!=} Ba ^ {2 + } + 2CH_ {3} COO ^{-}$ 。 Among them, barium ion $ (Ba ^ {2 +}) $and acetate ion $ (CH_ {3} COO ^ {-}) $are free between water molecules and evenly dispersed.

Acetate ion, because acetic acid is a weak acid, acetate in water has a tendency to combine with hydrogen ion $ (H ^ {+}) $ionized by water. For water, weak ionization, $H_ {2} O\ rightleftharpoons H ^{+} + O H ^{-}$ 。 Acetate ions combine with hydrogen ions to form acetate molecules $ (CH_ {3} COOH) $, which shifts the ionization equilibrium of water to the right, and the concentration of hydroxide ions $ (OH ^ {-}) $gradually increases, so the solution becomes weakly alkaline. This process, although the degree of hydrolysis of acetate is small, it has an impact on the properties of the solution. Barium ions, on the other hand, are relatively stable in water and do not undergo such hydrolysis reactions with water. Barium acetate dissolves in water, and there is both dissociation of strong electrolytes and hydrolysis of acetate ions. The two are related to each other and together affect the composition and properties of the solution.