Problem 17.21
Part A
Calculate the pH of a buffer that is 0.13 M in lactic acid and 0.11 M in sodium lactate.
Express your answer using two decimal places.
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Part B
Calculate the pH of a buffer formed by mixing 85 mL of 0.13 M lactic acid with 95 mL of 0.16 M sodium lactate.
Express your answer using two decimal places.
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The solution to both of these requires the use of the
Henderson-Hasselbalch equation:
pH = pKa + log([A^-]/[HA])
We also need the pKa of lactic acid (not given in the
problem):
Acidity (pKa) 3.86
pH = pKa + log([A^-]/[HA])
pKa = 3.86
[A^-] = [sodium lactate] = 0.11 M .
[HA] = [lactic acid] = 0.13 M
pH = 3.79
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