MCQ
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
- A$1$
- B$2$
- ✓$3$
- D$11$
✓
Answer
Correct option: C.
$3$
(c) $[{H^ + }] = C\,.\,\alpha $
$[{H^ + }] = 0.1 \times \frac{1}{{100}} = {10^{ - 3}}$
$pH$ $ = - \log \,\,[{H^ + }] = - \log \,{10^{ - 3}} = 3$
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