In which of the following solvents will AgBr | vedclass

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(B) The solubility of $AgBr$ is governed by its solubility product constant $(K_{sp})$.In the presence of $NaBr$ or $HBr$,the common ion effect $(Br^-

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$10^{-3} \ M \ NH_4OH$

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(B) The solubility of $AgBr$ is governed by its solubility product constant $(K_{sp})$.In the presence of $NaBr$ or $HBr$,the common ion effect $(Br^-)$ significantly decreases the solubility of $AgBr$.In pure water,$AgBr$ has a low solubility.In $NH_4OH$,$Ag^+$ ions react with $NH_3$ to form a stable complex ion,$[Ag(NH_3)_2]^+$,according to the reaction: $AgBr(s) + 2NH_3(aq) \rightleftharpoons [Ag(NH_3)_2]^+(aq) + Br^-(aq)$.This complex formation removes $Ag^+$ ions from the solution,shifting the equilibrium to the right and significantly increasing the solubility of $AgBr$ compared to the other solvents.

In which of the following solvents will $AgBr$ have the highest solubility?

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