What is the $\mathrm{pH}$ of a $10^{-4} \mathrm{M} \mathrm{OH}^{-}$solution at $330 \mathrm{~K}$, if $\mathrm{K}_{\mathrm{w}}$ at $330 \mathrm{~K}$ is $10^{-13.6}$ ?

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Aicharya · Accepted Answer

Given at $330 \mathrm{~K}$ $ \begin{aligned} \mathrm{K}_w & =10^{-13.6} \ 	ext { i.e. } \quad \mathrm{pK}_w & =\mathrm{pH}+\mathrm{pOH} \ \because \quad \mathrm{pOH}^2 & =-\log \left[\mathrm{OH}^{-}ight] \ 13.6 & =\mathrm{pH}+\mathrm{pOH} \ \mathrm{pOH} & =-\log 10^{-4} \ 13.6 & =\mathrm{pH}+4 \ 	herefore \quad \mathrm{pH} & =13.6-4 \ & =9.6 \end{aligned} $

What is the $\mathrm{pH}$ of a $10^{-4} \mathrm{M} \mathrm{OH}^{-}$solution at $330 \mathrm{~K}$, if…

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