🤓 Based on our data, we think this question is relevant for Professor Jiang's class at UHD.

We’re being asked to **determine the K _{sp} value given that the solubility of Cd_{3}(PO_{4})_{2} is 1.2 x 10^{-7 }mo/L **

Recall that ** K_{sp}** is an equilibrium constant related to slightly soluble ionic compounds.

The dissociation of **Cd _{3}(PO_{4})_{2}** in solution is as follows:

Cd_{3}(PO_{4})_{2}_{(s)} ⇌ 3 Cd^{2+}_{(aq)} + 2 PO_{4}^{3-}_{(aq)}

We can construct an ** ICE table** for this dissociation.

Remember that solids are ignored in the ICE table and K_{sp} expression.

Given that the solubility of Cd_{3}(PO_{4})_{2} is 1.2 x 10^{-7} mol/L what is its K_{sp} value? Note: the formula mass of Cd_{3}(PO_{4})_{2} is 527 g/mol.