On the chemical equilibrium formula for the reaction between acetic acid and barium hydroxide

Acetic acid, a weak acid, is partially ionized in water; barium hydroxide, a strong base, is also completely ionized in water. When the two meet, a neutralization reaction occurs, and the chemical equilibrium formula is the core, this formula reveals the relationship between the nature of the reaction and the amount of each substance.

When acetic acid ($CH_ {3} COOH $) reacts with barium hydroxide ($Ba (OH) _ {2} $), hydrogen ions in acetic acid combine with hydroxide ions in barium hydroxide to form water molecules, while acetate ions and barium ions remain in solution. The chemical reaction equation is: $2CH_ {3} COOH + Ba (OH) _ {2} = (CH_ {3} COO) _ {2} Ba + 2H_ {2} O $. This is the balanced equilibrium formula, which follows the law of conservation of mass, and the number of atoms of each element on the left and right sides is equal.

From an ionic perspective, the reaction is essentially a combination of hydrogen ions and hydroxide ions. Although acetic acid is a weak acid and partially ionized, when reacting with a strong base, hydrogen ions are continuously ionized to participate in the reaction. Barium hydroxide completely ionizes barium ions and hydroxide ions, and hydroxide ions combine with hydrogen ions ionized by acetic acid to form water.

Understanding this equilibrium formula is of great significance for grasping the essence of acid-base reactions. It helps us know the direction and extent of the reaction, and also provides a theoretical basis for practical applications such as chemical analysis and industrial production.

In short, the chemical equilibrium formula for the reaction of acetic acid and barium hydroxide is the key to understanding such acid-base reactions and lays the foundation for in-depth exploration of chemical reaction laws.