The solubility of Ba_3(AsO_4)_2 (molar mass = | vedclass

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(B) The solubility $s$ in $g/L$ is calculated as: $s = (6.9 	imes 10^{-2} \ g / 100 \ mL) 	imes (1000 \ mL / 1 \ L) = 0.69 \ g/L$. Convert solubilit

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$1.08 	imes 10^{-13}$

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(B) The solubility $s$ in $g/L$ is calculated as: $s = (6.9 	imes 10^{-2} \ g / 100 \ mL) 	imes (1000 \ mL / 1 \ L) = 0.69 \ g/L$. Convert solubility to $mol/L$: $s = 0.69 \ g/L / 690 \ g/mol = 10^{-3} \ mol/L$. The dissociation of $Ba_3(AsO_4)_2$ is: $Ba_3(AsO_4)_2(s) ightleftharpoons 3Ba^{2+}(aq) + 2AsO_4^{3-}(aq)$. $K_{sp} = [Ba^{2+}]^3 [AsO_4^{3-}]^2 = (3s)^3 (2s)^2 = 27s^3 	imes 4s^2 = 108s^5$. Substituting $s = 10^{-3}$: $K_{sp} = 108 	imes (10^{-3})^5 = 108 	imes 10^{-15} = 1.08 	imes 10^{-13}$.

The solubility of $Ba_3(AsO_4)_2$ (molar mass $= 690 \ g/mol$) is $6.9 \times 10^{-2} \ g/100 \ mL$. What is the value of its $K_{sp}$?

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