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Question

(B) The solubility of a sparingly soluble salt like $AgBr$ decreases in the presence of a common ion due to the common ion effect.$AgBr(s) \rightlefth

Vedclass · Accepted Answer

$0.1 \, M \, CaBr_2$

Vedclass · Answer

(B) The solubility of a sparingly soluble salt like $AgBr$ decreases in the presence of a common ion due to the common ion effect.$AgBr(s) ightleftharpoons Ag^+(aq) + Br^-(aq)$.In $0.1 \, M \, CaBr_2$,the concentration of $Br^-$ ions is $0.2 \, M$ $(2 	imes 0.1 \, M)$.In $0.1 \, M \, NaBr$,the concentration of $Br^-$ ions is $0.1 \, M$.In $0.1 \, M \, AgNO_3$,the concentration of $Ag^+$ ions is $0.1 \, M$.Since the common ion concentration is highest in $0.1 \, M \, CaBr_2$ $([Br^-] = 0.2 \, M)$,the solubility of $AgBr$ will be the minimum in this solution.

The solubility of $AgBr$ is minimum in:

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