(A) For a weak acid $HA$,the degree of dissociation $\alpha$ is very small,so $(1 - \alpha) \cong 1$. The formula for the degree of dissociation is $\

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(A) For a weak acid $HA$,the degree of dissociation $\alpha$ is very small,so $(1 - \alpha) \cong 1$. The formula for the degree of dissociation is $\alpha = \sqrt{\frac{K_{a}}{c}}$. Given $K_{a} = 1.0 \times 10^{-5}$ and $c = 0.1 \ M$. Substituting the values: $\alpha = \sqrt{\frac{1.0 \times 10^{-5}}{0.1}} = \sqrt{1.0 \times 10^{-4}} = 10^{-2}$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)pH of weak Acids and weak Bases

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Calculate $\alpha$ for $0.1 \ M$ acetic acid $(K_{a} = 1.0 \times 10^{-5})$.

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A
$10^{-2}$
B
$10^{-3}$
C
$10^{-4}$
D
$10^{-5}$

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Calculate $\alpha$ for $0.1 \ M$ acetic acid $(K_{a} = 1.0 \times 10^{-5})$.

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