The pK_a value for acetic acid at the experim | vedclass

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(B) Given: $pK_a = 5$,so $K_a = 10^{-5}$.Concentration $C = 0.1 \ M = 10^{-1} \ M$.$K_w = 10^{-14}$.For a salt of a weak acid and a strong base,the de

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$1 	imes 10^{-2} \%$

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(B) Given: $pK_a = 5$,so $K_a = 10^{-5}$.Concentration $C = 0.1 \ M = 10^{-1} \ M$.$K_w = 10^{-14}$.For a salt of a weak acid and a strong base,the degree of hydrolysis $\alpha_h$ is given by:$\alpha_h = \sqrt{\frac{K_h}{C}} = \sqrt{\frac{K_w}{K_a \cdot C}}$$\alpha_h = \sqrt{\frac{10^{-14}}{10^{-5} \cdot 10^{-1}}} = \sqrt{\frac{10^{-14}}{10^{-6}}} = \sqrt{10^{-8}} = 10^{-4}$.Percentage hydrolysis = $\alpha_h 	imes 100 = 10^{-4} 	imes 100 = 10^{-2} \%$.

The $pK_a$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1 \ M$ sodium acetate solution will be:

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