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A weak acid with $\mathrm{p} K_a 5.9$ and weak base with $\mathrm{p} K_b 5.8$ are mixed in equal proportions. $\mathrm{pH}$ of the resulting solution is
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The correct answer is:
$7.05$
$\mathrm{pH}$ of the resultant solution is given by,
$\begin{aligned} \mathrm{pH} & =7+\frac{1}{2}\left(\mathrm{pK}_a-\mathrm{p} K_b\right)=7+\frac{1}{2}(5.9-5.8) \\ \mathrm{pH} & =7.05\end{aligned}$
$\begin{aligned} \mathrm{pH} & =7+\frac{1}{2}\left(\mathrm{pK}_a-\mathrm{p} K_b\right)=7+\frac{1}{2}(5.9-5.8) \\ \mathrm{pH} & =7.05\end{aligned}$
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