If the solubility products of AgBrO_3 and Ag_ | vedclass

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(C) For $AgBrO_3$ (type $AB$): $K_{sp} = S^2$ $S = \sqrt{K_{sp}} = \sqrt{5.5 	imes 10^{-5}} \approx 7.41 	imes 10^{-3} \ M$. For $Ag_2SO_4$ (type $A

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$S_{AgBrO_3} < S_{Ag_2SO_4}$

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(C) For $AgBrO_3$ (type $AB$): $K_{sp} = S^2$ $S = \sqrt{K_{sp}} = \sqrt{5.5 	imes 10^{-5}} \approx 7.41 	imes 10^{-3} \ M$. For $Ag_2SO_4$ (type $A_2B$): $K_{sp} = 4S^3$ $S = \sqrt[3]{\frac{K_{sp}}{4}} = \sqrt[3]{\frac{2 	imes 10^{-5}}{4}} = \sqrt[3]{0.5 	imes 10^{-5}} = \sqrt[3]{5 	imes 10^{-6}} \approx 1.71 	imes 10^{-2} \ M$. Comparing the two values,$S_{Ag_2SO_4} > S_{AgBrO_3}$ or $S_{AgBrO_3} < S_{Ag_2SO_4}$.

If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,what is the relationship between their solubilities?

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