What is the pH of a 0.010 M acetic acid solution? (K_a for acetic acid is 1.76 $\times$ 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 acetic acid, [H⁺] can be found using the formula [H⁺] = √(Kₐ × [CH₃COOH]). Substituting the given values, [H⁺] = √(1.76 × 10⁻⁵ × 0.010) ≈ 1.32 × 10⁻³. Therefore, pH = -log(1.32 × 10⁻³) ≈ 3.38.

What Is the PH of a 0 ×\times× 10-5

What Is the PH of a 0 $\times$ 10^-⁵