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(C) The precipitation of a salt occurs when the ionic product exceeds its solubility product $(K_{sp})$. For a salt $AgX$,the precipitation starts whe

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$AgI, AgBr, AgCl$

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(C) The precipitation of a salt occurs when the ionic product exceeds its solubility product $(K_{sp})$. For a salt $AgX$,the precipitation starts when $[Ag^{+}] = \frac{K_{sp}(AgX)}{[X^{-}]}$. Given $[Cl^{-}] = [Br^{-}] = [I^{-}] = 1 	imes 10^{-8} \ M$. For $AgCl$: $[Ag^{+}] = \frac{1.8 	imes 10^{-10}}{10^{-8}} = 1.8 	imes 10^{-2} \ M$. For $AgBr$: $[Ag^{+}] = \frac{5 	imes 10^{-13}}{10^{-8}} = 5 	imes 10^{-5} \ M$. For $AgI$: $[Ag^{+}] = \frac{8.3 	imes 10^{-17}}{10^{-8}} = 8.3 	imes 10^{-9} \ M$. Since the concentration of $Ag^{+}$ required for precipitation is lowest for $AgI$,it will precipitate first,followed by $AgBr$,and finally $AgCl$. The order of precipitation is $AgI > AgBr > AgCl$.

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