The pK_a of an equimolar mixture of sodium ac | vedclass

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(C) The $pH$ of a buffer solution is calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log\frac{[Salt]}{[Acid]}$.Since the mixture is

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$4.74$

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(C) The $pH$ of a buffer solution is calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log\frac{[Salt]}{[Acid]}$.Since the mixture is equimolar,the concentration of the salt (sodium acetate) is equal to the concentration of the acid (acetic acid),so $\frac{[Salt]}{[Acid]} = 1$.Substituting the values: $pH = 4.74 + \log(1)$.Since $\log(1) = 0$,we get $pH = 4.74 + 0 = 4.74$.

The $pK_a$ of an equimolar mixture of sodium acetate and acetic acid is $4.74$. What is the $pH$ of the solution?

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