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  4. What is the pH of a 10-4 M OH- solution at 330K, if Kw at 330K is 10-13.6?

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Q. What is the $pH$ of a $10^{-4}\, M\, OH^-$ solution at $330K$, if $K_w$ at $330K$ is $10^{-13.6}$?

JEE MainJEE Main 2013Equilibrium

Solution:

Given at $330\, K$
$K_{w}=10^{-13.6}$
i.e. $PK_{w}=pH+pOH$
$\because pOH = -log \left[OH^{-}\right]$
$13.6 = pH+pOH$
$pOH = - log\,10^{-4}$
$13.6=pH+4$
$\therefore pH = 13.6-4$
$=9.6$