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- A1) Estimate the solubility of CaF2(aq) [in units of MICROmolar] in the presence of 0.156 molar CaCl2(aq). A2) Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.831 molar AlF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.]ST5G.2 - Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.701 molar AIF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.] Type your answer..For the reaction aA(aq) + bB(1) cC(g) + dD(aq) the equilibrium constant, K, can be written as Pc- [D]d [A]a K= The equilibrium constant is unitless because the units always mathematically cancel when the pressure is expressed in torr and concentration is expressed in molality. each quantity is a dimensionless ratio of the actual concentration or pressure divided by standard state concentration or pressure. pressure and concentration are unitless quantities. taking each pressure or concentration to its coefficient power cancels out the units.
- A sparingly soluble salt silver phosphate, Ag3PO4, is in equilibrium with its ions in solution according to the following equation A93PO4(s) = 3 Ag*(aq) + PO (aq) Write an expression for Ksp of Ag;PO4 The solubility of silver phosphate, Ag;PO4, at 25°C is 1.59 x 10 mol/L. What is the Ksp for the silver phosphate at 25°C?= 1.2 X 1018 1. Calculate the molar solubility and the mass solubility for Hg2Cl2, given the following solubility reaction and Ksp value. Hg,Cl, (s) = Hg.* (aq) + 2 Cl- KspWhat is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Kgp of AGCI = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70×107? Express your answer in decimal notation rounded to three significant figures.
- Copper(I) ions in aqueous solution react with NH, (aq) according to Cut (aq) + 2 NH, (аq) — Си(NH, ); (aq) 3 6.3 х 1010 - Calculate the solubility (in g-L-!) of CuBr(s) (Ksp = 6.3 × 10-9) in 0.72 M NH, (aq). solubility of CuBr(s): g/LFor the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium? ....... J/mol The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 68 oC is Keq = 401,568. (b) What is the standard reaction Gibbs energy of this reaction?.....J/molCalculate the solubility of copper(I) sulfide (Cu2S, Ksp = 2.26 × 10−48) in a 0.010 M CuC2H3O2(aq) solution. (C2H3O2− = acetate)
- Consider an amphoteric hydroxide, M(OH)₂ (s), where M is a generic metal. M(OH)₂ (s) = M² (aq) + 2OH(aq) K»p = 2 X 10-16 M(OH)₂ (s) + 2OH(aq) = [M(OH), 1²(aq) K₁ = 0.06 Estimate the solubility of M(OH), in a solution buffered at pH = 7.0, 10.0, and 14.0. solubility at pH=7.0 solubility at pH= 10.0 solubility at pH=14.0 2.0 x10-2 2 x10-8 2 x10-16 Incorrect M M MCalculate the molar solubility of lithium phosphate, Li;PO4, given that the Kp of lithium phosphate is 2.37 x 10-11.app.101edu.co Question 16 of 25 A 185.0 mL sample of 1.200 M Pb(NO3), is mixed with 139.50 mL of 1.500 M NaCl, and the PbCl, precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr2 precipitate is also collected and dried. What is the mass (in grams) of the PbBr2 precipitate, assuming the yield in each precipitation step is 100%? 1 3 6. 8. 6. +/- 2. LO