By controlling the pH of an aqueous solution it is possible to control the formation of a precipitate (the solid form) for a slightly soluble ionic compounds. As an example, consider an aqueous solution with [Zn2+] = 2.3 x 10^-4 M. Note that the solubility product for zinc hydroxide (Zn(OH)2) is Ksp = 4.1 x 10^-17. a) At what value for pH will Zn(OH)2 solid first form? b) What percent of the initial concentration of Zn2+ ion will have formed solid at pH = 9.00?

4. Unlike most silver salts, silver fluoride is very soluble in water. AgF(s) Ag (aq) + F(aq) AgCl(s) Ag (aq) + Cl(aq) a) Calculate the molar solubility of silver fluoride. Keq = 183.8 Keq = 1.8 x 10-10 b) What is the pH of a concentrated solution of silver fluoride? c) Provide an explanation for the difference in solubility between silver fluoride and silver chloride.

The solubility product constant of calcium sulfate, CaSO4CaSO4, is 7.10×10−57.10×10−5. Its molar mass is 136.1 g/molg/mol. How many grams of calcium sulfate can dissolve in 49.0 LL of pure water?

The Solubility Product Constant for calcium sulfide is 8.0 × 10-6. The molar solubility of calcium sulfide in a 0.262 M potassium sulfide solution is M.

Determine the molar solubility for Cd₂(PO) by constructing an ICE table, writing the solubility constant expression, and solving for molar solubility. The value of Ksp for Cd₂(PO) is 2.5 × 10:³³. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) +x 1.000 + 3x Assume the solution already contains 0.500 M NPO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 1 +2x 1.500 + x Cd (PO),(s) 0.500 +3x 1.500 + 2x -0.500 0.500 + x 2 1.500 + 3x 1.000 0.500 + 2x 3 Cd²+ (aq) -1.000 3 0.500 + 3x + 1.500 1.000 + x 2 PO³(aq) RESET NEXT -1.500 1.000 + 2x

The Solubility Product Constant for silver iodide is 1.5 x 10-16. The molar solubility of silver iodide in a water solution is M.

A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar solubility of magnesium hydroxide?

What is the molar solubility of silver carbonate (Ag2CO3) in water? The solubility-product constant for Ag2CO3 is 8.1 x 10-12 at 25 °C.

The Ksp of magnesium carbonate, MgCO3, is 6.82 × 106. Calculate the molar solubility, S, of this compound. M S =

If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility =  mol/L