A weak monoprotic acid of 0.1, M, ionizes to 1% in solution. What will be pH of solution

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6-2.Equilibrium-II (Ionic Equilibrium)

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A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution

A

$1$

B

$2$

C

$3$

D

$11$

Solution

(c) $[{H^ + }] = C\,.\,\alpha $

$[{H^ + }] = 0.1 \times \frac{1}{{100}} = {10^{ – 3}}$

$pH$ $ = – \log \,\,[{H^ + }] = – \log \,{10^{ – 3}} = 3$

Standard 11

Chemistry

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