(B) The degree of dissociation $(\alpha)$ of the weak acid $(HA)$ is $1 \% = 0.01$. For a weak acid,the dissociation constant $(K_{a})$ is given by t

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(B) The degree of dissociation $(\alpha)$ of the weak acid $(HA)$ is $1 \% = 0.01$. For a weak acid,the dissociation constant $(K_{a})$ is given by the formula: $K_{a} = C \alpha^2$. Given concentration $(C) = 0.5 \ M$ and $\alpha = 0.01$. Substituting the values: $K_{a} = 0.5 \times (0.01)^2$. $K_{a} = 0.5 \times (10^{-2})^2 = 0.5 \times 10^{-4}$. $K_{a} = 5 \times 10^{-1} \times 10^{-4} = 5 \times 10^{-5}$.

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

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At $27^{\circ} C$,the degree of dissociation of a weak acid $(HA)$ in its $0.5 \ M$ aqueous solution is $1 \%$. Its $K_{a}$ value is approximately:

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A
$5 \times 10^{-4}$
B
$5 \times 10^{-5}$
C
$5 \times 10^{-6}$
D
$5 \times 10^{-8}$

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2 Equilibrium: Ionic Equilibrium

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pH of weak Acids and weak Bases

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At $27^{\circ} C$,the degree of dissociation of a weak acid $(HA)$ in its $0.5 \ M$ aqueous solution is $1 \%$. Its $K_{a}$ value is approximately:

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