What is the pH of a 0.375 M solution of benzoic acid? Ka = 6.3 × 10^-5

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Quizplus · Accepted Answer

The pH of a weak acid solution can be calculated using the formula: pH = -log[H⁺], where [H⁺] is the concentration of hydrogen ions. For benzoic acid, we use the expression for the acid dissociation constant (Ka): Ka = [H⁺][A⁻]/[HA]. Assuming x is the concentration of H⁺ ions, Ka = x²/(0.375 - x). Solving for x using the given Ka value, we find x ≈ 0.00485 M. Thus, pH = -log(0.00485) ≈ 2.3.

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