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JEE Mains · Chemistry · STD 11 - 6.2. Equilibrium - II (icon Equilibrium)
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 \(10\)
- D \(9.6\)
Answer & Solution
Correct Answer
(D) \(9.6\)
Step-by-step Solution
Detailed explanation
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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