In an aqueous solution,SCN^-,Br^-,I^-,and Cl^ | vedclass

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(A) The precipitation of a salt occurs when the ionic product exceeds its solubility product $(K_{sp})$.For a given concentration of $Ag^+$ ions,the s

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$I^-$

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(A) The precipitation of a salt occurs when the ionic product exceeds its solubility product $(K_{sp})$.For a given concentration of $Ag^+$ ions,the salt with the lowest $K_{sp}$ value will reach its ionic product limit first and precipitate first.Comparing the given $K_{sp}$ values:$K_{sp}(AgI) = 1.7 	imes 10^{-16}$$K_{sp}(AgBr) = 3.5 	imes 10^{-13}$$K_{sp}(AgCl) = 1.2 	imes 10^{-10}$$K_{sp}(AgSCN) = 7.1 	imes 10^{-7}$Since $1.7 	imes 10^{-16}$ is the smallest value among the given $K_{sp}$ constants,$AgI$ will precipitate first.Therefore,$I^-$ will be the first to precipitate.

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In an aqueous solution,$SCN^-$,$Br^-$,$I^-$,and $Cl^-$ are present. Which will get precipitated first when $AgNO_3$ is added to the solution? Given that:$K_{sp}(AgCl) = 1.2 \times 10^{-10}$,$K_{sp}(AgI) = 1.7 \times 10^{-16}$,$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,$K_{sp}(AgBr) = 3.5 \times 10^{-13}$