The pH of 0.1 M acetic acid is 3. The dissoc | vedclass

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(B) Given: $pH = 3$,concentration $c = 0.1 \ M = 10^{-1} \ M$.For a weak acid,the concentration of hydrogen ions is given by $[H^{+}] = 10^{-pH} = 10^

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$1.0 	imes 10^{-5}$

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(B) Given: $pH = 3$,concentration $c = 0.1 \ M = 10^{-1} \ M$.For a weak acid,the concentration of hydrogen ions is given by $[H^{+}] = 10^{-pH} = 10^{-3} \ M$.The formula for the dissociation constant $K_a$ of a weak acid is $[H^{+}] = \sqrt{K_a 	imes c}$.Squaring both sides,we get $[H^{+}]^2 = K_a 	imes c$.Substituting the values: $(10^{-3})^2 = K_a 	imes 10^{-1}$.$10^{-6} = K_a 	imes 10^{-1}$.$K_a = \frac{10^{-6}}{10^{-1}} = 10^{-5}$.

The $pH$ of $0.1 \ M$ acetic acid is $3$. The dissociation constant of the acid will be:

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