Express the relationship between K_{sp} and s | vedclass

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(A) The dissociation of $Ca_3(PO_4)_2$ in water is represented as:$Ca_3(PO_4)_2(s) \rightleftharpoons 3Ca^{2+}(aq) + 2PO_4^{3-}(aq)$If the solubility

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$K_{sp} = 108S^5$

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(A) The dissociation of $Ca_3(PO_4)_2$ in water is represented as:$Ca_3(PO_4)_2(s) \rightleftharpoons 3Ca^{2+}(aq) + 2PO_4^{3-}(aq)$If the solubility of the salt is $S \ mol/L$,then the concentration of ions at equilibrium is:$[Ca^{2+}] = 3S$$[PO_4^{3-}] = 2S$The solubility product expression is:$K_{sp} = [Ca^{2+}]^3 [PO_4^{3-}]^2$Substituting the values:$K_{sp} = (3S)^3 (2S)^2$$K_{sp} = (27S^3) (4S^2)$$K_{sp} = 108S^5$

Express the relationship between $K_{sp}$ and solubility $(S)$ for the salt $Ca_3(PO_4)_2$.

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