(A) For a weak acid,the dissociation constant $K_a$ is related to the degree of dissociation $\alpha$ and concentration $C$ by the formula: $K_a = \al

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(A) For a weak acid,the dissociation constant $K_a$ is related to the degree of dissociation $\alpha$ and concentration $C$ by the formula: $K_a = \alpha^2 C$. Given $K_a = 10^{-5}$ and $C = 0.1 \ M$. Substituting the values: $10^{-5} = \alpha^2 \times 0.1$. $\alpha^2 = \frac{10^{-5}}{0.1} = 10^{-4}$. $\alpha = \sqrt{10^{-4}} = 0.01$. Percentage dissociation = $\alpha \times 100 = 0.01 \times 100 = 1 \%$.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium pH of weak Acids and weak Bases

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What is the percentage dissociation of $0.1 \ M$ acetic acid (in $\%$)? $(K_a = 10^{-5})$

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A
$1$
B
$10$
C
$0.1$
D
$0.01$

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2 Equilibrium: Ionic Equilibrium

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pH of weak Acids and weak Bases

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What is the percentage dissociation of $0.1 \ M$ acetic acid (in $\%$)? $(K_a = 10^{-5})$

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