The solubility product of calcium phosphate is defined as

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$K_{sp} = {[{Ca}^{2 +}]}^{2} {[{PO}_{4}^{3 -}]}^{3}$

$K_{sp} = [{Ca}^{2 +}] [{PO}_{4}^{3 -}]$

$K_{sp} = {[{Ca}^{2 +}]}^{3} {[{PO}_{4}^{3 -}]}^{2}$

$K_{sp} = \frac{[{Ca}^{2 +}] [{PO}_{4}^{3 -}]}{[{Ca}_{3} {({PO}_{4})}_{2}]}$

answer is C.

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Detailed Solution

The solubility product of calcium phosphate is defined as $K_{sp} = {[{Ca}^{2 +}]}^{3} {[{PO}_{4}^{3 -}]}^{2}$ .

The concentration of the ions in a saturated solution that are in equilibrium with the solid substance is known as the solubility product, or Ksp, of an ionic compound.

Hence the option C is correct.

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