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Which of the following statements are true for a solution saturated with AgCl and AgBr if their solubilities in mol per litre in separate solution are x andy mole respectively:

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$[{Ag}^{+}] = [{Br}^{-}] \times [{Cl}^{-}]$

$[{Cl}^{-}] > [Br]$

$[{Br}^{-}] > y$

$[{Ag}^{+}] = x + y$

answer is B.

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Detailed Solution

AgCl is more soluble than AgBr. The ion concentration for a salt in a solution will be in equilibrium. so among the available choices,

Hence, $[{Cl}^{-}] > [Br]$ Ag is common.

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