🤓 Based on our data, we think this question is relevant for Professor Jiang's class at UHD.
We’re being asked to determine the Ksp value given that the solubility of Cd3(PO4)2 is 1.2 x 10-7 mo/L
Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds.
The dissociation of Cd3(PO4)2 in solution is as follows:
Cd3(PO4)2(s) ⇌ 3 Cd2+(aq) + 2 PO43-(aq)
We can construct an ICE table for this dissociation.
Remember that solids are ignored in the ICE table and Ksp expression.
Given that the solubility of Cd3(PO4)2 is 1.2 x 10-7 mol/L what is its Ksp value? Note: the formula mass of Cd3(PO4)2 is 527 g/mol.