Write a solubility product constant, Ksp, equilibrium expression for the following ionic solid. Assume A is a metal ion and B is an anion. For example, for CaCO3(s): Ksp = [Ca2+][CO32-] A4B1(s): Ksp = [A+]x[B-]y What is the value of x?

Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?

Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?

Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?

Consider a 2.0-L aqueous solution of 4.17 M NH3, where 21.0 g of NH4Cl are dissolved. To this solution, 4.8 g of CaCl2 are added. (a) What is [OH-] before CaCl2 is added? (b) Will a precipitate form? (c) What is [Ca2+] after equilibrium is established?

Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.

Phosphoric acid dissociates to form phosphate anion and hydroniumcation. The K, for this reaction is 4.5 x 10 13. Choose the correct equation which expresses this reaction. 4.5 x 1013 - ([PO4³] × [H3O*J³ ) / ( [H3PO4] × [H2O] ) 4.5 x 1013 - ( [PO4®] × [H3O*] ) / [H3PO4] 4.5 x 1013 = ( [PO,³] × [H3O*]³ ) / [H3PO4] 4.5 x 1013 = [H3PO4) / ([PO4®] x [H3D*j$ ) Question 14 5 pts Cheesethe e for the loulmeler

Which of the following compounds will have the highest molar solubility in pure water? O Fe(OH)3, Ksp 2.79 x 10- -39 O ZnS, Ksp 2.0 x 10 - 25 ZnSe, Ksp 3.6 x 10–26 O PbS, Ksp = 9.04 × 10-29 O Ag2 S, Ksp 6.0 × 10-51

What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of CuNO3 to a solution of CN-? The final volume of the solution was 1.00 L and the concentration of CN- was 2.7046 M before equilibrium was established.Cu+(aq) + 2CN-(aq)↔[Cu(CN)2]-(aq) Kf = 1.00e16

Suppose 60.0 mL of 0.100 M Pb(NO3)2 is added to 30.0 mL of 0.150 M KI. How many grams of Pbl2 will be formed? Mass Pbl₂ = 1.037 Hint [K+] Your answer is correct. [1] What will be the molar concentrations of all the ions in the mixture after equilibrium has been reached? Record all answers to three (3) significant figures. Your answer is partially correct. [Pb²+] 0.05 i 0.05 g [NO3] 0.13 0.067 M M 3 3 M