The pH of 0.01 M solution of acetic acid is | vedclass

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Question

(A) Given,$pH$ of $0.01 \ M \ CH_3COOH$ solution $= 5.0$. Concentration,$C = 0.01 \ M = 10^{-2} \ M$. We know that $[H^{+}] = 10^{-pH} = 10^{-5} \ M$.

Vedclass · Accepted Answer

$1 	imes 10^{-5} \ M, 1 	imes 10^{-8}$

Vedclass · Answer

(A) Given,$pH$ of $0.01 \ M \ CH_3COOH$ solution $= 5.0$. Concentration,$C = 0.01 \ M = 10^{-2} \ M$. We know that $[H^{+}] = 10^{-pH} = 10^{-5} \ M$. For a weak acid,the dissociation constant $K_a$ is given by the formula: $[H^{+}] = \sqrt{K_a \cdot C} \implies [H^{+}]^2 = K_a \cdot C$. Therefore,$K_a = \frac{[H^{+}]^2}{C} = \frac{(10^{-5})^2}{10^{-2}} = \frac{10^{-10}}{10^{-2}} = 10^{-8}$. Thus,the values are $[H^{+}] = 1 	imes 10^{-5} \ M$ and $K_a = 1 	imes 10^{-8}$.

The $pH$ of $0.01 \ M$ solution of acetic acid is $5.0$. What are the values of $[H^{+}]$ and $K_a$ respectively?

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