Dissociation constant of an acid HA is 1 × {10^{ - 5}} . pH of 0.1 molar solution of acid wi

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6-2.Equilibrium-II (Ionic Equilibrium)

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The dissociation constant of an acid $HA$ is $1 \times {10^{ - 5}}$. The $pH$ of $0.1$ molar solution of the acid will be

A

$5$

B

$4$

C

$3$

D

$1$

Solution

(c) $HA$ $ \rightleftharpoons $ ${H^ + } + {A^ – }$

$[{H^ + }] = 0.1\,\,M$; ${[{H^ + }]^2} = {K_a} \times C$

$[{H^ + }] = \sqrt {{K_a} \times C} = \sqrt {1 \times {{10}^{ – 5}} \times 0.1} = \sqrt {{{10}^{ – 6}}} $

$[{H^ + }] = {10^{ – 3}}M;\,\,pH = 3$

Standard 11

Chemistry

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