Nicotinic acid (K_a = 10^{-5}) is represented | vedclass

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(A) The concentration of the solution $C$ is given by $C = \frac{n}{V} = \frac{0.1 \ mol}{2 \ L} = 0.05 \ M$. For a weak acid,the dissociation constan

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$1.4$

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(A) The concentration of the solution $C$ is given by $C = \frac{n}{V} = \frac{0.1 \ mol}{2 \ L} = 0.05 \ M$. For a weak acid,the dissociation constant $K_a$ is related to the degree of dissociation $\alpha$ by the formula $K_a = C \alpha^2$ (assuming $\alpha Substituting the values: $10^{-5} = 0.05 	imes \alpha^2$. $\alpha^2 = \frac{10^{-5}}{0.05} = 2 	imes 10^{-4}$. $\alpha = \sqrt{2 	imes 10^{-4}} = 1.414 	imes 10^{-2}$. The percentage of dissociation is $\alpha 	imes 100 = 1.414 	imes 10^{-2} 	imes 100 = 1.414 \% \approx 1.4 \%$.

Nicotinic acid $(K_a = 10^{-5})$ is represented by the formula $HNiC$. Calculate the percentage of dissociation in a solution containing $0.1 \ mol$ of nicotinic acid in $2 \ L$ of solution.

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