How many moles of sodium acetate should be ad | vedclass

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Question

(C) The Henderson-Hasselbalch equation for an acidic buffer is: $pH = pK_a + \log\frac{[Salt]}{[Acid]}$Given $pH = 5.5$,$pK_a = 4.5$,and $[Acid] = 0.1

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$1$

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(C) The Henderson-Hasselbalch equation for an acidic buffer is: $pH = pK_a + \log\frac{[Salt]}{[Acid]}$Given $pH = 5.5$,$pK_a = 4.5$,and $[Acid] = 0.1 \ M$.Substituting the values: $5.5 = 4.5 + \log\frac{[Salt]}{0.1}$$\log\frac{[Salt]}{0.1} = 5.5 - 4.5 = 1$Taking antilog on both sides: $\frac{[Salt]}{0.1} = 10^1 = 10$$[Salt] = 10 	imes 0.1 = 1 \ M$.Since the volume is $1 \ L$,the number of moles of sodium acetate required is $1 \ mol$.

How many moles of sodium acetate should be added to $1 \ L$ of a $0.1 \ M$ solution of $CH_3COOH$ to give a solution of $pH = 5.5$? (Given: $pK_a$ of $CH_3COOH = 4.5$)

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