Question

The Ksp of calcium sulfate, CaSO4, is 9.0 × 10-6. What is the concentration of CaSO4 in a saturated solution? A. 3.0 × 10-3 Molar B. 9.0 × 10-3 Molar C. 3.0 × 10-6 Molar D. 9.0 × 10-6 Molar

Answer 1

Answer: The concentration of
`CaSO_4` in a saturated solution is
`3.0* 10^(-3)M`

Step-by-step explanation:

Solubility product is defined as the equilibrium constant in which a solid ionic compound is dissolved to produce its ions in solution. It is represented as
`K_(sp)`

The equation for the ionization of
`CaSO_4` is given as:

`K_(sp)` of
`CaSO_4` =
`9.0* 10^(-6)`

By stoichiometry of the reaction:

1 mole of
`CaSO_4` gives 1 mole of
`Ca^(2+)` and 1 mole of
`SO_4^(2-)`

When the solubility of
`CaSO_4` is S moles/liter, then the solubility of
`Ca^(2+)` will be S moles\liter and solubility of
`SO_4^(2-)` will be S moles/liter.

`K_(sp)=[Ca^(2+)][SO_4^(2-)]`

`9.0* 10^(-6)=[s][s]`

`9.0* 10^(-6)=s^2`

`s=3.0* 10^(-3)M`

Thus concentration of
`CaSO_4` in a saturated solution is
`3.0* 10^(-3)M`