The pH of a solution that contains 0.818 M acetic acid (K_a = 1.76 × 10^-5)and 0.182 M sodium acetate is __________. A)4.102 B)5.407 C)8.593 D)8.370 E)9.898

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Quizplus · Accepted Answer

The solution is a buffer, and the pH can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]). Here, pKa = -log(1.76 × 10^-5) ≈ 4.755, [A-] = 0.182 M, and [HA] = 0.818 M. Substituting these values gives pH ≈ 4.755 + log(0.182/0.818) ≈ 4.102.

The PH of a Solution That Contains 0