What is the pH after the addition of 0.20 mole of HCl to 1.00 liter of 1.00 M CH₃COONa and 1.00 M CH₃COOH ( K _a = 1.8×10^{- 5}) buffer solution?
(Assume no volume change.)

Question

What is the pH after the addition of 0.20 mole of HCl to 1.00 liter of 1.00 M CH₃COONa and 1.00 M CH₃COOH ( K _a = 1.8×10^{- 5}) buffer solution? (Assume no volume change.)

Quizplus · Accepted Answer

The buffer solution consists of equal concentrations of CH₃COOH and CH₃COONa. The addition of HCl will convert some CH₃COONa to CH₃COOH, but the buffer will resist significant pH change. Using the Henderson-Hasselbalch equation, the pH is calculated to be approximately 4.57.

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