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The concentration of $[{H^ + }]$ and concentration of $[O{H^ - }]$ of a $ 0.1$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $ = 1 \times {10^{ - 14}}]$
$2 \times {10^{ - 3}}$ $M$ and $5 \times {10^{ - 12}}$ $M$
$1 \times {10^3}\;M\;{\rm{and}}\;3 \times {10^{ - 11}}M$
$0.02 \times {10^{ - 3}}\;M\;{\rm{and}}\;5 \times {10^{ - 11}}M$
$3 \times {10^{ - 2}}\;M\;{\rm{and}}\;4 \times {10^{ - 13}}M$
Solution
(a) Given that
Concentration of solution $ =0.1$
Degree of ionisation $ = 2\% = \frac{2}{{100}} = 0.02$
Ionic product of water $ = 1 \times {10^{ – 14}}$
Concentration of $[{H^ + }]$= Concentration of solution $\times$ degree of ionisation $ = 0.1 \times 0.02 = 2 \times {10^{ – 3}}M$
Concentration of $[O{H^ – }] = \frac{{{\rm{Ionic product of water}}}}{{[{H^ + }]}}$
$ = \frac{{1 \times {{10}^{ – 14}}}}{{2 \times {{10}^{ – 3}}}} = 0.5 \times {10^{ – 11}} = 5 \times {10^{ – 12}}M$.
