Problem: 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.

FREE Expert Solution

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)

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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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