Answer:
b. Ksp = 2,39×10⁻⁵
Step-by-step explanation:
For the equilibrium:
CaSO₄(s) ⇌ Ca²⁺(aq) + SO₄²⁻(aq)
The solubility product constant is defined as:
![ksp = [Ca^(2+)] [SO_(4)^(2-)]](https://img.qammunity.org/2020/formulas/chemistry/high-school/9iuq70mwdmnkq23ro836wdpmlckx14sjmd.png)
-The concentration of CaSO₄ is not taken into account because is a solid that has an activity of 1.-
As the concentration of both Ca²⁺(aq) and SO₄²⁻(aq) were 4,89×10⁻³ M
The ksp is:
4,89×10⁻³ M × 4,89×10⁻³ M =
b. Ksp = 2,39×10⁻⁵
I hope it helps!