A solution is 0.1 M with respect to AcOH and | vedclass

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(C) The solution contains a weak acid $AcOH$ and its salt $AcONa$,forming a buffer solution. $AcONa$ is a strong electrolyte and dissociates completel

Vedclass · Accepted Answer

$0.3$

Vedclass · Answer

(C) The solution contains a weak acid $AcOH$ and its salt $AcONa$,forming a buffer solution. $AcONa$ is a strong electrolyte and dissociates completely: $AcONa \rightarrow Na^+ + Ac^-$. Since the concentration of $AcONa$ is $0.2 \ M$,the concentration of $Ac^-$ ions from the salt is $0.2 \ M$. $AcOH$ is a weak acid and dissociates as: $AcOH \rightleftharpoons H^+ + Ac^-$. Because of the common ion effect,the dissociation of $AcOH$ is suppressed,and the total concentration of $Ac^-$ is approximately equal to the concentration of $Ac^-$ from the salt. Therefore,$[Ac^-] \approx 0.2 \ M$.

$A$ solution is $0.1 \ M$ with respect to $AcOH$ and $0.2 \ M$ with respect to $AcONa$. What is the concentration of $Ac^-$? (Given $x = 0.2$)

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