Hydroxylapalite. Ca_10(PO_4)_6(OH)_2, has a solubility constant of K_sp = 2.34 times 10^-59, and dissociates according to...
"Hydroxyapatite, Cao(PO)(OH),, has a solubility constant of Ksp = 2.34 x 10-59, and dissociates according to Ca,(PO)(OH),(s) = 10 Ca2+ (aq) + 6 PO (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 6.50 x 10-M?
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 6.20×10−6 M ? [Ca2+]=
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 ?
Need help!! The molar solubility of Ba_3(PO_4)_2 is 6.5 times 10^-7 M. Calculate K_sp for Ba_3(PO_4)_2. For Pbl_2 K_sp = 8.7 times 10^-9. Calculate the molar solubility of PbI_2 in 0.100 M Cal_2.
A particular saturated solution of calcium phosphate, Ca_3(PO_4)_2 has [Ca^2+] = 2.01 times 10^-8 M and [PO_4^3] = 1.60 times 10^-5 M. (a) Calculate the K_sp for Ca_3(PO_4)_2? (b) What happens to the concentration of PO_4^3- if a little amount of CaCO_3, is added into this solution?
Write a solubility product constant expression, K_sp, for an equilibrium in a saturated aqueous solution of the slightly soluble salts Magnesium fluoride, MgF_2 Zinc phosphate, Zn_3(PO_4)_2 Chromium(II) hydroxide, Cr(OH)_3 Strontinum sulfate, SrSO_4. Calculate the solubility in g/L for calcium carbonate, CaCO_3, in pure water given the K_sp = 2.8 times 10^-9. Calculate the solubility in g/L for CaCO_3, in 0.050 M Na_2CO_3.
Saturated Ca(OH)_2 solution in pure water means that [OH-] = 2 times solubility [Ca2+] = 2 times solubility [OH-] = solubility [OH-] = solubility/2
Calculate the K_sp for hydroxide if the solubility of Sr(OH)_2 in pure water is 2.1 times 10^1 g/L. 1.16 times 10^-1 1.60 times 10^-2 1.42 times 10^1 6.40 times 10^-3 7.70 times 10^-33
Need help The solubility of Zinc phosphate, Zn_3(PO_4)_2 is 5.91 times 10^-6 g in 100 ml of water. What is the solubility product of zinc phosphate? Zn_3(PO_4)_2 Zn + PO_4
The solubility products for a series of hydroxides are BiOOH K_sp = 4.0 times 10^-10 = [BiO^+][OH^-] Be(OH)_2 K_sp = 7.0 times 10^-22 Tm(OH)_3 K_sp = 3.0 times 10^-24 Hf(OH)_4 K_sp = 4.0 times 10^-26 Which hydroxide has a. the lower molar solubility in H_2 O b. the lowest molar solubility in solution that is 0.30 in NaOH?