Thanks in advance to whoever is helping with this

Question

Hydroxyapatite, Ca10(PO4)6(OH)2 , has a solubility constant of K_sp = 2.34×10−59, and dissociates according to

Ca10(PO4)6(OH)2(s)↽−−⇀10Ca^2+(aq)+6PO4^3−(aq)+2OH−(aq)

Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2+ in this solution if [OH−]is fixed at 6.20×10^−4 M ?

[Ca2+]=M?

Answer 1

Ca10(PO4)6(OH)2(s)↽−−⇀10Ca^2+(aq)+6PO4^3−(aq)+2OH−(aq)

Ksp = [Ca²⁺]¹⁰[PO₄^3-]⁶[OH-]²

Let x = [Ca²⁺], then [PO₄^3-] = 0.6x

2.34x10^-59 = (x)¹⁰(0.6x)⁶(6.20x10^-4)²

6.09x10^-53 = 0.6x¹⁶

x¹⁶ = 1.01x10^-52

x = 0.0005627 M = [Ca²⁺]