On the addition of a solution containing CrO_ | vedclass

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(C) The solubility product $(K_{sp})$ values for the chromates of alkaline earth metals are in the order: $K_{sp}(CaCrO_4) > K_{sp}(SrCrO_4) > K_{sp}(

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$BaCrO_4$

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(C) The solubility product $(K_{sp})$ values for the chromates of alkaline earth metals are in the order: $K_{sp}(CaCrO_4) > K_{sp}(SrCrO_4) > K_{sp}(BaCrO_4)$.Since $BaCrO_4$ has the lowest $K_{sp}$ value,it requires the lowest concentration of $CrO_4^{2-}$ ions to exceed its solubility product.Therefore,$BaCrO_4$ will precipitate first upon the addition of $CrO_4^{2-}$ ions to the solution containing these cations.The reaction is: $Ba^{2+}(aq) + CrO_4^{2-}(aq) 	o BaCrO_4(s) \downarrow$ (Yellow precipitate).

On the addition of a solution containing $CrO_4^{2-}$ ions to a solution containing $Ba^{2+}$,$Sr^{2+}$,and $Ca^{2+}$ ions,the precipitate obtained first will be of

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