What volume (in mL) of 0.10 , M sodium format | vedclass

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(C) The $pH$ of a buffer solution is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$ Given: $pH = 4.0$,$pK_a = 3

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$50$

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(C) The $pH$ of a buffer solution is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$ Given: $pH = 4.0$,$pK_a = 3.7$ $[Acid] = 0.05 \, M$,$Volume_{acid} = 50 \, mL$ $[Salt] = 0.10 \, M$,$Volume_{salt} = V$ Substituting the values: $4.0 = 3.7 + \log \frac{0.10 	imes V}{0.05 	imes 50}$ $0.3 = \log \frac{0.10 	imes V}{2.5}$ Since $\log 2 \approx 0.3$,we have: $2 = \frac{0.10 	imes V}{2.5}$ $0.10 	imes V = 5.0$ $V = 50 \, mL$

What volume (in $mL$) of $0.10 \, M$ sodium formate is required to be added to $50 \, mL$ of $0.05 \, M$ formic acid to prepare a buffer solution with $pH = 4.0$? (Given: $pK_a$ of formic acid $= 3.7$)

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