(C) Given: $pH = 3$,Concentration $(C) = 0.1 \ M = 10^{-1} \ M$.We know that $[H^{+}] = 10^{-pH} = 10^{-3} \ M$.For a weak acid $HQ$,the degree of dis

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(C) Given: $pH = 3$,Concentration $(C) = 0.1 \ M = 10^{-1} \ M$.We know that $[H^{+}] = 10^{-pH} = 10^{-3} \ M$.For a weak acid $HQ$,the degree of dissociation $(\alpha)$ is given by $\alpha = \frac{[H^{+}]}{C} = \frac{10^{-3}}{10^{-1}} = 10^{-2}$.The ionization constant $K_a$ is given by the formula $K_a = C \alpha^{2}$.Substituting the values: $K_a = (0.1) \times (10^{-2})^{2} = 10^{-1} \times 10^{-4} = 10^{-5}$.

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

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The $pH$ of a $0.1 \ M$ solution of the acid $HQ$ is $3$. The value of the ionization constant,$K_a$ of the acid is:

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A
$3 \times 10^{-1}$
B
$1 \times 10^{-3}$
C
$1 \times 10^{-5}$
D
$1 \times 10^{-7}$

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6-2.Equilibrium-II (Ionic Equilibrium)

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pH of weak Acids and weak Bases

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The $pH$ of a $0.1 \ M$ solution of the acid $HQ$ is $3$. The value of the ionization constant,$K_a$ of the acid is:

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