Question:
What is the pH of $10^{-2}M$ aqueous solution of aniline at 298 K?}
What is the pH of $10^{-2}M$ aqueous solution of aniline at 298 K?}
Show Hint
For weak bases:
\[
[OH^-]=\sqrt{K_bC}
\]
followed by
\[
pH=14-pOH
\]
Updated On: Jun 17, 2026
- 7.3
- 7.4
- 9.4
- 8.3
Show Solution
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The Correct Option is D
Solution and Explanation
Concept:
For a weak base,
\[
[OH^-]=\sqrt{K_bC}
\]
Step 1: Calculate hydroxide ion concentration.
\[ [OH^-] = \sqrt{(4\times10^{-10})(10^{-2})} \] \[ = \sqrt{4\times10^{-12}} \] \[ =2\times10^{-6} \]
Step 2: Find pOH.
\[ pOH = -\log(2\times10^{-6}) \] \[ =6-0.3 \] \[ =5.7 \]
Step 3: Calculate pH.
\[ pH=14-5.7 \] \[ pH=8.3 \] \[ \boxed{8.3} \]
Step 1: Calculate hydroxide ion concentration.
\[ [OH^-] = \sqrt{(4\times10^{-10})(10^{-2})} \] \[ = \sqrt{4\times10^{-12}} \] \[ =2\times10^{-6} \]
Step 2: Find pOH.
\[ pOH = -\log(2\times10^{-6}) \] \[ =6-0.3 \] \[ =5.7 \]
Step 3: Calculate pH.
\[ pH=14-5.7 \] \[ pH=8.3 \] \[ \boxed{8.3} \]
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