## Chemistry: Molecular Approach (4th Edition)

Published by Pearson

# Chapter 16 - Exercises - Page 771: 12

#### Answer

The acid ionization constant is an equilibrium constant for the ionization reaction of a weak acid. It is used to quantify the strength of a weak acid, which means: the higher the $K_a$, the stronger the acid. It is defined mathematically with this equation: Ionization: $$HA(aq) + H_2O(l) \leftrightharpoons A^-(aq)+ H_3O^+(aq)$$ $$K_a = \frac{[A^-][H_3O^+]}{[HA]}$$ It is a very important concept for the study of acid equilibrium, since it is useful to calculate the amount of $H_3O^+$ produced at equilibrium with the initial concentration of the acid or vice versa.

#### Work Step by Step

The acid ionization constant is an equilibrium constant for the ionization reaction of a weak acid. It is used to quantify the strength of a weak acid, which means: the higher the $K_a$, the stronger the acid. It is defined mathematically with this equation: Ionization: $$HA(aq) + H_2O(l) \leftrightharpoons A^-(aq)+ H_3O^+(aq)$$ $$K_a = \frac{[A^-][H_3O^+]}{[HA]}$$ It is a very important concept for the study of acid equilibrium, since it is useful to calculate the amount of $H_3O^+$ produced at equilibrium with the initial concentration of the acid or vice versa.

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