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Sloan [31]
3 years ago
6

Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 x 10^-59. Solid hydroxylapatite is dissolved in water

to form a saturated solution. What is the concentration of Ca+2 in this solution if [OH-] is somehow fixed at 5.30 x 10-6 M?
Chemistry
1 answer:
nadezda [96]3 years ago
3 0

Answer:

The concentration of [Ca²⁺] is 8.47 x 10⁻³ M

Explanation:

We consider the solubility of hydroxyapatite,

Ca₁₀(PO₄)₆(OH)₂ ⇔ 10Ca²⁺ + 6PO₄³⁻ + 2 OH⁻

Assumed that there is <em>a</em> mol of hydoxyapatite disolved in water, yielding <em>10a</em> mol Ca²⁺ of  and <em>6a</em> mol of PO₄³⁻

We also have Ksp equation,

Ksp = [Ca²⁺]¹⁰ x [PO₄³⁻]⁶ x [OH⁻]² = 2.34 x 10⁻⁵⁹

     ⇔  10a¹⁰ x 6a⁶ x (5.30 x 10⁻⁶)² = 2.24 x 10⁻⁵⁹

     ⇔  60a¹⁶                                    = 2.24 x 10⁻⁵⁹ / 5.30 x 10⁻¹²

     ⇔  a¹⁶                                         = 0.007 x 10⁻⁴⁷ = 7 x 10⁻⁵⁰

     ⇔  a                                           = \sqrt[16]{7 . 10^{-50} } =  8.47 x 10⁻⁴

Hence,

[Ca²⁺] = 10<em>a</em> = 8.47 x 10⁻³ M

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