For a 10 M CH_3COOH solution,if K_a = 10^{- | vedclass

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(B) For a weak acid,the dissociation constant is given by $K_a = C\alpha^2$,where $C$ is the concentration and $\alpha$ is the degree of dissociation.

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$10^{-2}, 2$

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(B) For a weak acid,the dissociation constant is given by $K_a = C\alpha^2$,where $C$ is the concentration and $\alpha$ is the degree of dissociation.Given $K_a = 10^{-5}$ and $C = 10 \ M$.$10^{-5} = 10 	imes \alpha^2$ $\Rightarrow \alpha^2 = 10^{-6}$ $\Rightarrow \alpha = 10^{-3}$.The concentration of hydrogen ions is $[H^+] = C\alpha = 10 	imes 10^{-3} = 10^{-2} \ M$.The $pH$ is calculated as $pH = -\log[H^+] = -\log(10^{-2}) = 2$.

For a $10 \ M \ CH_3COOH$ solution,if $K_a = 10^{-5}$,what will be the values of $[H^{+}]$ and $pH$ respectively?

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