Question:medium
What is the pH of a \(10^{-4}\ \mathrm{M\ OH^-}\) solution at 330 K, if \(K_w\) at 330 K is \(10^{-13.6}\) ?
What is the pH of a \(10^{-4}\ \mathrm{M\ OH^-}\) solution at 330 K, if \(K_w\) at 330 K is \(10^{-13.6}\) ?
Show Hint
Find \([H^+]\) from \(K_w = [H^+][OH^-]\) at 330 K, then take \(-\log\).
Updated On: Oct 31, 2026
- 4
- 9.0
- 10
- 9.6
Show Solution
The Correct Option is D
Solution and Explanation
Use \(\mathrm{pH} + \mathrm{pOH} = \mathrm{p}K_w\).
\(\mathrm{pOH} = -\log(10^{-4}) = 4\) and \(\mathrm{p}K_w = 13.6\) at 330 K.
\(\mathrm{pH} = 13.6 - 4 = 9.6\).
Answer: (4) 9.6
\(\mathrm{pOH} = -\log(10^{-4}) = 4\) and \(\mathrm{p}K_w = 13.6\) at 330 K.
\(\mathrm{pH} = 13.6 - 4 = 9.6\).
Answer: (4) 9.6
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