100 mL of 0.1 M HA (weak acid) and 100 mL of 0.2 M NaA are mixed. What is the pH of resultant solution? ( $\mathrm{K}_{\mathrm{a}}$ of HA is $10^{-5} ; \log 2=0.3$ )

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Aicharya · Accepted Answer

$\mathrm{pH}=\mathrm{pK}_{\mathrm{a}}+\log \frac{[	ext { Salt }]}{[	ext { Acid }]}$ $\begin{aligned} & \mathrm{pH}=5+\log \frac{[0.2]}{[0.1]} \quad\left[\mathrm{pK}_{\mathrm{a}}=-\operatorname{log\mathrm {K}_{\mathrm {a}}=-\operatorname {log}10^{-5}=5]}ight. \ & \mathrm{pH}=5+\log 2 \ & \mathrm{pH}=5+0.3 \ & \mathrm{pH}=5.3\end{aligned}$

100 mL of 0.1 M HA (weak acid) and 100 mL of 0.2 M NaA are mixed. What is the pH of resultant solution? (…

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