emistry R122 dy Assignment 3 Solubility Equilibria How many grams of Ca3(PO4)2 will dissolve in a) 2.0L of pure water? b) 500 mL of 1.0M Ca(N03)2? %3D Ksp for Ca3(PO4)2 = 2.0 x 10-29 is the [Cr3+] in a saturated solution of Cr(
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- How many grams of PbF2 (molar mass = 245.2) will dissolve in 300 mL of 0.30 M NaF solution? The Ksp for PbF2 is 2.69e-08.Toxic Cr(VI) can be precipitated from an aqueous solution by bubbling SO2 through the solution. How much SO2 is required to treat 3.00x10^8L of 4.00x10^-2 mM Cr(VI)? 2CrO4^-2 + 3SO2 + 4H^+ —> Cr2(SO4)3 + 2H2O ___kgCalculate the solubility in grams per 100 ml H2O for La(IO3)3 (s), Ksp= 6.1*10^-12 BaF2 (s), Ksp= 1.8 *10^-7 CaCO3 (s), Ksp=5.0*10^-9 assuming density of water is 1 g/cc
- (a) Explain why Mg(OH)2 precipitates when CO32- ion isadded to a solution containing Mg2+. (b) Will Mg(OH)2precipitate when 4.0 g of Na2CO3 is added to 1.00 L of asolution containing 125 ppm of Mg2+?25c. At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0068 M. You have found Ksp to be 1.6 × 10⁻⁹. If solid In₂(SO₄)₃ is added to a solution that already contains 0.150 M In(NO₃)₃, what will the new solubility of the solid be?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 ?
- What is the solubility (in g/L) for PbBr2(s) in a 1.00 L solution that has 251 g Pb(NO3)2 already dissolved in it? The Ksp for PbBr2 is 5.67 × 10-6. If you need more room, use a second sheet.If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 9.14e-08 g of Sc(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Sc(OH)3.Ksp = (c) The Ksp of Cu3(PO4)2 at 25 oC is 1.40e-37. What is the molar solubility of Cu3(PO4)2?solubility = mol/LThe Ksp for SrF2 is 2.8 × 10–9 . What mass of SrF2 will dissolve in 5.00 × 102 L of an aqueous solution?
- Silver carbonate has a Ksp = 9.05×10-10 and a solubility of 0.0006093 M in water. Solid silver carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×10-10 M? [AgNO3] = ____ MCalculate the solubility of solid Ca3(PO4)2 (Ksp=1.3×10^-32) in a 0.20 M Na3PO4 solution.If 28.70 mL of 0.0200 M KMnO4 is required to titreate a 0.250 g sample of K3[Fe(C2O4)3]x3H20, what is the percent C2O42- in the complex?