What is the pH of a buffer that contains 0.15 M CH₃COOH and 0.10 M NaCH₃COO (K_a = 1.8 × 10^-5)?

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Quizplus · Accepted Answer

The pH of a buffer can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the acid. Given that Ka = 1.8 × 10^-5, pKa = -log(1.8 × 10^-5) ≈ 4.74. Substituting the given concentrations into the equation gives pH = 4.74 + log(0.10/0.15) ≈ 4.57.

What Is the PH of a Buffer That Contains 0