CH3COOH is a weak acid (and based on the Bronsted-Lowry definition, an acid is a proton (H+) donor. Once CH3COOH loses its proton, its conjugate base is formed).
CH3COOH(aq) + H2O(l) ⇌ CH3COO-(aq) + H3O+(aq)
(weak acid) (base) (conjugate base) (conjugate acid)
CH3COOH + H2O ⇌
Calculate the pH of a solution that is 1.00 M CH 3COOH (Ka = 1.8 x 10 -5) and 1.00 M CH 3COONa.
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