Hydroxyapatite, Ca,(PO,),(OH),, has a solubility constant of Ksp = 2.34 × 10-5º, and dissociates according to Ca1, (PO,),(OH),(s) = 10 Ca²+(aq) + 6 PO}-(aq) + 2 OH¯(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 7.40 × 10-4 M? 4.81 x10¬6 [Ca**] = M Incorrect

Hydroxyapatite, Ca,(PO,),(OH),, has a solubility constant of Ksp = 2.34 × 10-5º, and dissociates according to Ca1, (PO,),(OH),(s) = 10 Ca²+(aq) + 6 PO}-(aq) + 2 OH¯(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 7.40 × 10-4 M? 4.81 x10¬6 [Ca**] = M Incorrect

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.CCP

See similar textbooks

Similar questions

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Hydroxyapatite, Ca,(PO,),(OH),, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according to Ca10 (PO,),(OH),(s) = 10 Ca²+(aq) + 6 PO (aq) + 2 OH¯(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 5.30 x 10-4 M? [Ca²*] = M
Hydroxyapatite, Ca,(PO)(OH)₂, has a solubility constant of K-2.34 x 10-59, and dissociates according to Cao (PO)(OH)₂ (s) = 10 Ca² (aq) + 6PO (aq) + 2OH(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+ in this solution if JOH is fixed at 8.30 x 10M? |Ca²1 M
Hydroxyapatite, Ca,(PO4),(OH)₂, has a solubility constant of Ksp = 2.34 x 10-59, and dissociates according to Cao (PO)(OH)₂ (s)10 Ca2 (aq) + 6PO (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 3.40 x 10-4 M? [Ca²+] = M
Hydroxyapatite, Ca₁(PO)(OH)₂, Ca₁(PO4)(OH)₂ (s) ⇒ 10 Ca² ¹(aq) + 6PO³(aq) + 2OH(aq) has a solubility constant of Ksp = 2.34 × 10-5⁹, and dissociates according to 10 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 x 10-4 M?
(c) 1.0cm^3 0.25 moldm^-3 potassium chromate(VI), K2CrO4, is added as an indicator. At the end-point, all the silver chloride has been precipitated in the 52.5cm^3 solution. A slight excess of silver ions causes a red-brown precipitate of silver chromate(VI) to form. 2Ag + (aq) + CrO4 2- (aq) - - > Ag2CrO4 (s) (i) The solubility product of silver chloride is: Ksp = 2.0 ×10^-10 mol^2 dm^-6 Use this value to explain why [Ag+] = 1.41 × 10^-5 moldm^-3 at the end point.
When the sparingly soluble salt BACO, is dissolved in water, the following simultaneous equilibria apply: BACO; Ba" + co, co,- + H;0 HCO," + OH Employing mass- and charge-balance equations, the following relationship can be obtained for a saturated solution of BaCO, in water: Kyp = [Ba*"][CO,²] = 5.1 × 10* K, = [OH"][ HCO;"JM CO,²] = 2.1 x 10* (Ba**j° - K,K, [Ba"]" –- K, = 0 sp Find the concentration of free Ba" in the saturated solution.
Calculate the solubility of calcium carbonate water temperature of 5 °C; at that temperature, Ksp = 8.1 x 10^-9 for CaCO3, Ka = 2.8 x 10^-11 for HCO3-, and Kw = 2.0 x 10^-14.
The mineral pyrite, FeS2(s), can incorporate large amounts of arsenic. The dissolution of arsenic-rich pyrite can therefore release arsenic into groundwater (i.e., pyrite dissolution can be written as FeS2(s) = Fe2+ + S22-). What equation would you use to calculate whether pyrite in an aquifer will dissolve or precipitate?
estion 1 of 3 > General Chemistry 4th Edition McQuarrie Rock Gallogly Copper(I) ions in aqueous solution react with NH₂ (aq) according to Cut (aq) + 2NH₂ (aq) Cu(NH3)2(aq) Kf = 6.3 x 1010 Calculate the solubility (in g.L-¹) of CuBr(s) (Ksp = 6.3 x 10-2) in 0.87 M NH3(aq). solubility of CuBr(s): 2.50 x10-3 University Science Books presented by Macmillan Learning Incorrect g/L
You look at the solubility of Ca(OH)2 in water (Ksp = 4 x 10–10). You wait until the system reaches equilibrium and then add Cr(C2H3O2)3. (Ksp = 6.7 x 10–31 for Cr(OH)3). Would affect do you think would occur to the solubility? (increase, decrease, stay the same) Show this through a calculation (Note: Two equilibria must be considered).
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 9.60×10−4 M ?