# Chemistry

posted by .

Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according to

Ca10(PO4)6(OH)2(s) --> 10Ca2+(aq) + 6PO43-(aq) + 2OH-(aq)

Solid hydroxylapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2 in this solution if [OH–] is somehow fixed at 7.30 × 10-6 M?

I am confused as to how to solve for x with such large exponents

• Chemistry -

Ca10(PO4)6(OH)2 ==> 10Ca^2+ + 6PO4^3- + 2OH^-
I would substitute
(Ca^2+) = 10x
(PO4^3-) = 6x
(OH^-) = 2x + 7.3E-6
Ksp = (Ca^2+)^10(PO4^3-)^6(OH^-)^2
Ksp = (10x)^10(6x)^6(2x + 7.3E-6)^2
Solve for x. You want x = (Ca^2+).

• Chemistry -

Thank you. I think I understand how to set it up.

## Similar Questions

1. ### chemistry

If the concentration of Pb^2+ is known to be roughly 2.1 x 10 to the power of -9 mol/L within a saturated solution of Pb(PO4)2, calculate the Ksp of Pb3(PO4)2?
2. ### chemistry

If the concentration of Pb2+ is found to be 2.3 x 10-9 mol/L in a saturated solution of Pb3(PO4)2, what is the Ksp of Pb3(PO4)2 ?
3. ### chemistry

If the concentration of Pb2+ is found to be 2.3 x 10-9 mol/L in a saturated solution of Pb3(PO4)2, what is the Ksp of Pb3(PO4)2 ?
4. ### Chemistry

Write the balanced equation and solubility product expression for the solubility equilibrium of Mn3(PO4)2: i thought the answer was Mn3(PO4)2 (s) = Mn^2+(aq) + (PO4)2 ^3- (aq) but that's not right. then for the Ksp expression i thought …
5. ### Chemistry

Write the balanced equation and solubility product expression for the solubility equilibrium of Mn3(PO4)2: i thought the answer was Mn3(PO4)2 (s) = Mn^2+(aq) + (PO4)2 ^3- (aq) but that's not right. then for the Ksp expression i thought …

What is the molar solubility of barium phosphate in a 0.282M barium acetate solution?
7. ### Chemistry

Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according to Ca10(PO4)6(OH)2(s) --> 10Ca2+(aq) + 6PO43-(aq) + 2OH-(aq) Solid hydroxylapatite is dissolved in water to form a saturated …
8. ### Chemistry

Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 × 10^-59. Solid hydroxylapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2 in this solution if [OH–] is somehow …
9. ### Chemistry - Posted for Rudy

Posted by Rudy on Sunday, January 26, 2014 at 7:24pm. Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according to Ca10(PO4)6(OH)2(s) --> 10Ca2+(aq) + 6PO43-(aq) + 2OH-(aq) Solid …