Consider the dissociation equilibrium of acetic acid: . If a small amount of solid sodium acetate () is dissolved in this solution, which of the following statements are correct according to Le Chatel

Question

Consider the dissociation equilibrium of acetic acid: $CH_3COOH \rightleftharpoons CH_3COO^- + H^+$. If a small amount of solid sodium acetate ($CH_3COONa$) is dissolved in this solution, which of the following statements are correct according to Le Chatelier's principle?

Prashant Kotian · Accepted Answer

Correct answer: A,C,D. The addition of provides common acetate ions (), shifting the reaction backward. This consumes and forms more unionized , so unionized concentration increases (making B incorrect). Because drops, the pH increases. The equilibrium constant depends only on temperature, so it strictly remains unchanged.

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