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$1 \times 10^{-3}$ mole of $\mathrm{HCl}$ is added to a buffer solution made up of $0.01 \mathrm{M}$ acetic acid and 0.01 M sodium acetate. The final pH of the buffer will be (given, $\mathrm{p} K_{a}$ of acetic acid is 4.75 at $\left.25^{\circ} \mathrm{C}\right)$
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Verified Answer
The correct answer is:
4.66
$\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}^{+} \longrightarrow \mathrm{CH}_{3} \mathrm{COOH}$
$$
\begin{aligned}
\mathrm{pH}=& \mathrm{pK}_{a}+\log \frac{(\text { salt })}{(\text { acid })}=4.75+\log \frac{0.009}{0.011} \\
&=4.66
\end{aligned}
$$
$$
\begin{aligned}
\mathrm{pH}=& \mathrm{pK}_{a}+\log \frac{(\text { salt })}{(\text { acid })}=4.75+\log \frac{0.009}{0.011} \\
&=4.66
\end{aligned}
$$
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