Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO₂H) and 0.230 mol of sodium formate (NaCO₂H) in water sufficient to yield 1.00 L of solution. The K_aof formic acid is 1.77 × 10^-⁴. A) 3.54 B) 10.46 C) 2.09 D) 3.95 E) 2.30

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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(1.77 × 10^-4) = 3.75, [A-] = 0.230 M, and [HA] = 0.370 M. Thus, pH = 3.75 + log(0.230/0.370) = 3.54.

Calculate the PH of a Solution Prepared by Dissolving 0