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(B) The solubility of a sparingly soluble salt like $AgCl$ is governed by the common ion effect. According to the solubility product principle,$K_{sp}

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Water

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(B) The solubility of a sparingly soluble salt like $AgCl$ is governed by the common ion effect. According to the solubility product principle,$K_{sp} = [Ag^+][Cl^-]$. When a common ion ($Ag^+$ or $Cl^-$) is present in the solution,the equilibrium shifts to the left,decreasing the solubility of the salt. In $0.1 \, M \, AgNO_3$,there is a common ion $Ag^+$. In $0.1 \, M \, NaCl$ and $0.1 \, M \, KCl$,there is a common ion $Cl^-$. In pure water,there are no common ions present. Therefore,the solubility of $AgCl$ is highest in pure water compared to the other solutions containing common ions.

In which of the following is the solubility of $AgCl$ maximum?

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