An aqueous solution contains SCN^{-},Br^{-},I | vedclass

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(A) The precipitation of a salt occurs when the ionic product exceeds its solubility product constant $(K_{sp})$. For a series of salts with the same

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$I^{-}$

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(A) The precipitation of a salt occurs when the ionic product exceeds its solubility product constant $(K_{sp})$. For a series of salts with the same stoichiometry ($1:1$ ratio),the salt with the lowest $K_{sp}$ value will precipitate first upon the addition of a common ion. Comparing the given values: $K_{sp}(AgSCN) = 7.1 	imes 10^{-7}$ $K_{sp}(AgCl) = 1.2 	imes 10^{-10}$ $K_{sp}(AgBr) = 3.5 	imes 10^{-13}$ $K_{sp}(AgI) = 1.7 	imes 10^{-16}$ Since $K_{sp}(AgI)$ is the smallest,$AgI$ will precipitate first.

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