What is the pH of a weak dibasic acid,that is | vedclass

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(C) For a dibasic acid $H_2A$,the dissociation is $H_2A \rightleftharpoons 2H^+ + A^{2-}$.Given concentration $C = M/100 = 0.01 \ M$.Degree of dissoci

Vedclass · Accepted Answer

$3.397$

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(C) For a dibasic acid $H_2A$,the dissociation is $H_2A ightleftharpoons 2H^+ + A^{2-}$.Given concentration $C = M/100 = 0.01 \ M$.Degree of dissociation $\alpha = 2 \% = 0.02$.Since the acid is dibasic,the concentration of $H^+$ ions is $[H^+] = 2 	imes C 	imes \alpha$.$[H^+] = 2 	imes 0.01 	imes 0.02 = 0.0004 \ M = 4 	imes 10^{-4} \ M$.$pH = -\log[H^+] = -\log(4 	imes 10^{-4}) = 4 - \log(4) = 4 - 0.602 = 3.398$.Thus,the $pH$ is approximately $3.397$.

What is the $pH$ of a weak dibasic acid,that is $2 \%$ dissociated in its $M/100$ solution at $298 \ K$?

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