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.
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