HCN is 1 % ionized in its 0.2 M aqueous solu | vedclass

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(B) For a weak acid,the degree of ionization $\alpha$ is given by the formula $\alpha = \sqrt{\frac{K_a}{C}}$.Since $K_a$ is constant at a constant te

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$\sqrt{10} \%$

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(B) For a weak acid,the degree of ionization $\alpha$ is given by the formula $\alpha = \sqrt{\frac{K_a}{C}}$.Since $K_a$ is constant at a constant temperature,$\alpha \propto \frac{1}{\sqrt{C}}$.Therefore,$\frac{\alpha_2}{\alpha_1} = \sqrt{\frac{C_1}{C_2}}$.Given $\alpha_1 = 1 \%$,$C_1 = 0.2 \ M$,and $C_2 = 0.02 \ M$.Substituting the values: $\frac{\alpha_2}{1 \%} = \sqrt{\frac{0.2}{0.02}} = \sqrt{10}$.Thus,$\alpha_2 = \sqrt{10} \%$.

$HCN$ is $1 \%$ ionized in its $0.2 \ M$ aqueous solution. At the same temperature,what would be its percent ionization in its $0.02 \ M$ aqueous solution?

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