What is the solubility product `(K_(sp))` of calcuim phosphate in pure water ? [S=molar solubility]

Options

A. `108 S^(5)`
B. `72 S^(3)`
C. `6 S^(5)`
D. `121 S^(2)`

Answer

A

Explanation

`:'` Solubility product `(K_(sp))=x^(x).y^(y).s^(x+y)`
where, x and y are number of `Ca^(2+)` and `PO_(4)^(3-)` ions in 1 L of pure water respectively.
i.e. In `Ca_(2)(PO_(4))_(3)`
Here, `x=2` and `y=3`
Therefore, `K_(sp)=2^(2).3^(3)S^(2+3)`
`K_(sp)=108 S^(5)` and option (a) is the correct answer.