If the K_a for cyanoacetic acid is 3.5 times | vedclass

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(D) The salt of a weak acid and a strong base undergoes anionic hydrolysis.For a salt of a weak acid and a strong base,the hydrolysis constant $K_h$ i

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$7.559 	imes 10^{-6}$

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(D) The salt of a weak acid and a strong base undergoes anionic hydrolysis.For a salt of a weak acid and a strong base,the hydrolysis constant $K_h$ is given by $K_h = \frac{K_w}{K_a}$.Given $K_w = 1.0 	imes 10^{-14}$ and $K_a = 3.5 	imes 10^{-3}$,we have $K_h = \frac{1.0 	imes 10^{-14}}{3.5 	imes 10^{-3}} \approx 2.857 	imes 10^{-12}$.The degree of hydrolysis $h$ is given by the formula $h = \sqrt{\frac{K_h}{C}}$,where $C$ is the concentration of the salt.Given $C = 0.05 \ M$,we have $h = \sqrt{\frac{2.857 	imes 10^{-12}}{0.05}} = \sqrt{5.714 	imes 10^{-11}} = \sqrt{57.14 	imes 10^{-12}} \approx 7.559 	imes 10^{-6}$.

If the $K_a$ for cyanoacetic acid is $3.5 \times 10^{-3}$,what is the degree of hydrolysis for a $0.05 \ M$ solution of sodium cyanoacetate?

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