We’re being asked to calculate the Ksp for Mg3(PO4)2
Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds.
The dissociation of slightly soluble ionic compounds in solution is as follows:
MnNm(s) ⇌ n Mm+(aq) + m Nn–(aq)
We can construct an ICE table for this dissociation.
Remember that solids are ignored in the ICE table and Ksp expression.
The solubility of magnesium phosphate is 1.54 x 10-3 g/L (MM = 262.9 g/mol) Calculate the Ksp for Mg3(PO4)2 (REMEMBER: g/L)!!
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