Equal volumes of 0.5 N acetic acid and 0.5 | vedclass

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Question

(C) The mixture of acetic acid and sodium acetate acts as an acidic buffer. The $pH$ of the solution can be calculated using the Henderson-Hasselbalch

Vedclass · Accepted Answer

$4.75$

Vedclass · Answer

(C) The mixture of acetic acid and sodium acetate acts as an acidic buffer. The $pH$ of the solution can be calculated using the Henderson-Hasselbalch equation: $pH = pK_{a} + \log \frac{[	ext{salt}]}{[	ext{acid}]} = pK_{a} + \log \frac{[	ext{sodium acetate}]}{[	ext{acetic acid}]}$ Since equal volumes of solutions with equal normality are mixed,the concentrations of the salt and acid in the final mixture remain equal,i.e.,$[	ext{sodium acetate}] = [	ext{acetic acid}]$. Therefore,$pH = pK_{a} + \log(1) = pK_{a} + 0$. Given $pK_{a} = 4.75$,the $pH$ of the resultant solution is $4.75$.

Equal volumes of $0.5 \ N$ acetic acid and $0.5 \ N$ sodium acetate are mixed. What is the $pH$ of the resultant solution? $(pK_{a}$ of acetic acid $= 4.75)$

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