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

Hydroxyapatite, 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)+6PO3−4(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 1.40×10−6 M ?

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Solubility equilibrium Cao (PO,), (OH)2 (s) żłocz (aq) +6PƠ-(aq)-20H-(aq) Solublityproduct, K,Po[o-23410 ICE table for the solubility equilibrium Cao (PO), (OH)2 (s) 2 1 0Ca2+ (aq) + 6PCr (aq) + 2OH-(aq) 1.40×10-6 Initi al concentrati ons (M) Change +10s +6s Equilibrium (M) 10s 6s 40x106 +2s Solubility product, Kp Ca 2.34x10- (10s) (6s) (1.40x10+2s -6 We can assume that 1.40 10-0 +2s 1.40 10 2.34x10-3 (10s) (6s) (140x10 2.34>< 10-9-4.6656x 10:16) (1.40x 10-6 234 10-59 4.6656×1014)(1.40×10-6) 2.34 x10-9 4.6656x10*)(1.40x106 S 16 - 1.41x103 M From the ICE table, concentration of Ca,! Ca | 10s 10( 1.41×10-4 M) = 1.41×10-3 M

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