A solution contains Cl^{-},I^{-},and SO_{4}^{ | vedclass

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(A) $Pb^{2+}$ ion is capable of precipitating $Cl^{-}$,$I^{-}$,and $SO_{4}^{2-}$ ions as insoluble salts.$Pb^{2+} + 2Cl^{-} \longrightarrow PbCl_{2} \

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$Pb^{2+}$

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(A) $Pb^{2+}$ ion is capable of precipitating $Cl^{-}$,$I^{-}$,and $SO_{4}^{2-}$ ions as insoluble salts.$Pb^{2+} + 2Cl^{-} \longrightarrow PbCl_{2} \downarrow$ (White precipitate)$Pb^{2+} + 2I^{-} \longrightarrow PbI_{2} \downarrow$ (Yellow precipitate)$Pb^{2+} + SO_{4}^{2-} \longrightarrow PbSO_{4} \downarrow$ (White precipitate)While $Ba^{2+}$ precipitates $SO_{4}^{2-}$,it does not form insoluble precipitates with $Cl^{-}$ and $I^{-}$ in aqueous solutions.

$A$ solution contains $Cl^{-}$,$I^{-}$,and $SO_{4}^{2-}$ ions. Which of the following ions is capable of precipitating all of the above when added to this solution?

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