Consider the dissociation equilibrium of acetic acid: . If a small amount of solid sodium acetate () — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

The addition of $CH_3COONa$ provides common acetate ions ($CH_3COO^-$), shifting the reaction backward. This consumes $H^+$ and forms more unionized $CH_3COOH$, so unionized concentration increases (making B incorrect). Because $[H^+]$ drops, the pH increases. The equilibrium constant $K_a$ depends only on temperature, so it strictly remains unchanged.