Formic acid has a molarity of 0.024 M in a solution.
The formic acid buffer is at a 0.1 M concentration. Accordingly, 0.1 moles of formic acid and formate will be present in a 1 L batch of the buffer solution.
Assume that n is the conjugate base of formic acid, and that m is the amount of formic acid.
0.1 = m+n
The pH of a buffer solution can be determined using the Henderson-Hasselbalch equation shown below.
pH = pKa + log (Conjugate / Acid)
Putting in the values,
4.25 = 3.75 + log (0.1-m / m)
3.16 = 0.1-m / m
m = 0.024
Thus the concentration of formic acid in solution = 0.024 / 1 L
= 0.024 M
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