If the solubility products of AgBrO_3 and Ag_ | vedclass

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(B) For $Ag_2SO_4$: $Ag_2SO_4 ightleftharpoons 2Ag^{+} + SO_4^{2-}$.$K_{sp} = (2S)^2(S) = 4S^3$.Given $K_{sp} = 2 	imes 10^{-5}$,so $4S^3 = 2 	ime

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$S_{AgBrO_3} < S_{Ag_2SO_4}$

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(B) For $Ag_2SO_4$: $Ag_2SO_4 ightleftharpoons 2Ag^{+} + SO_4^{2-}$.$K_{sp} = (2S)^2(S) = 4S^3$.Given $K_{sp} = 2 	imes 10^{-5}$,so $4S^3 = 2 	imes 10^{-5} \implies S^3 = 0.5 	imes 10^{-5} = 5 	imes 10^{-6}$.$S = \sqrt[3]{5 	imes 10^{-6}} \approx 1.71 	imes 10^{-2} \ mol/L$.For $AgBrO_3$: $AgBrO_3 ightleftharpoons Ag^{+} + BrO_3^-$.$K_{sp} = S^2$.Given $K_{sp} = 5.5 	imes 10^{-5}$,so $S = \sqrt{5.5 	imes 10^{-5}} \approx 7.42 	imes 10^{-3} \ mol/L$.Comparing the two,$S_{AgBrO_3} (7.42 	imes 10^{-3}) Thus,the correct option is $B$.

If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,the relationship between the solubilities of these can be correctly represented as

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