MCQ
What is the $pH$ of a $10^{-4}\, M\,OH^-$ solution at $330\,K$, if $K_w$ at $330\,K$ is $10^{-13.6}$ ?
- A$4$
- B$9$
- C$10$
- ✓$9.6$
✓
Answer
Correct option: D.
$9.6$
d
Given at $330\,K$
Given at $330\,K$
${K_w} = {10^{ - 13.6}}$
i.e. $p{K_w} = pH + pOH$
$\because \,pOH = - \log [O{H^ - }]$
$13.6 = pH + pOH$
$pOH = - \log \,{10^{ - 4}}$
$13.6 = pH + 4$
$\therefore \,pH = 13.6 - 4$
$ = 9.6$
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