What is the pH of an aqueous solution that contains 0.183 M sodium formate (NaCHO₂) and 0.300 M in formic acid?
K _a(HCHO₂) = 1.8×10^{- 4}

Question

What is the pH of an aqueous solution that contains 0.183 M sodium formate (NaCHO₂) and 0.300 M in formic acid? K _a(HCHO₂) = 1.8×10^{- 4}

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(1.8×10^-4) = 3.74, [A-] = 0.183 M, and [HA] = 0.300 M. Substituting these values gives pH = 3.74 + log(0.183/0.300) = 3.53.

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