Determine the molar solubility for $Cd_3(PO_4)_2$ by constructing an ICE table, writing the solubility constant expression, and solving for molar solubility. The value of Ksp for $Cd_3(PO_4)_2$ is 2.5 x $10^{-33}$. Complete Parts 1-3 before submitting your answer.
Assume the solution already contains 0.500 M $Na_3PO_4$. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.
$Cd_3(PO_4)_2(s) \rightleftharpoons 3Cd^{2+}(aq) + 2PO_4^{3-}(aq)$
Using the values from the ICE table (Part 1), construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one tile. Do not combine terms.
$K_{sp} = $
$= 2.5 \times 10^{-33}$
Determine the molar solubility for $Cd_3(PO_4)_2$ by constructing an ICE table, writing the solubility constant expression, and solving for molar solubility. The value of Ksp for $Cd_3(PO_4)_2$ is 2.5 x $10^{-33}$. Complete Parts 1-3 before submitting your answer.
Based on your ICE table and Ksp expression, determine the molar solubility.
$S_{Cd_3(PO_4)_2} = \text{____} M$
