What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? K_a = 1.8 × 10^-5 A) 4.49 B) 4.64 C) 4.85 D) 5.00 E) 5.52

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Quizplus · Accepted Answer

The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]). Here, pKa = -log(1.8 × 10^-5) = 4.74. The concentration of the acetate ion [A-] is 0.35 M and the concentration of acetic acid [HA] is 0.45 M. Plugging these values into the equation gives: pH = 4.74 + log(0.35/0.45) = 4.64.

What Is the PH of a Buffer That Consists of 0.45