(D) $CH_3COOH \rightleftharpoons H^{+} + CH_3COO^{-}$ $K_a = \frac{[H^{+}][CH_3COO^{-}]}{[CH_3COOH]} = \frac{[H^{+}]^2}{[CH_3COOH]}$ $[H^{+}] = \sqrt{

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(D) $CH_3COOH \rightleftharpoons H^{+} + CH_3COO^{-}$ $K_a = \frac{[H^{+}][CH_3COO^{-}]}{[CH_3COOH]} = \frac{[H^{+}]^2}{[CH_3COOH]}$ $[H^{+}] = \sqrt{K_a \times [CH_3COOH]}$ $[H^{+}] = \sqrt{2 \times 10^{-5} \times 0.05}$ $[H^{+}] = \sqrt{10^{-6}} = 10^{-3} \ M$ $pH = -\log[H^{+}]$ $pH = -\log(10^{-3}) = 3$

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

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The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

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A
$2$
B
$11$
C
$10^{-3}$
D
$3$

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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 $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

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