42) Determine the molar solubility for Pb3(PO4)2in pure water. Ksp for Pb3(PO4)2is 1.0 x 10-54. A) 4.1 x 10-28M B) 5.8 x 10-10M C) 1.1 x 10-11M D) 6.2 x 10-12M E) 1.0 x 10-54M 43) Determine the molar solubility of BaF2in a solution containing 0.0750 M LiF. Ksp(BaF2) = 1.7 × 10-6. 44) Give the equation for a saturated solution in comparing Q with Ksp. 45) A solution containing AgNO3is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp(AgCl) = 1.77 × 10-10. 46) A solution containing CaCl2is mixed with a solution of Li2C2O4to form a solution that is 3.5 × 10-4M in calcium ion and 2.33 × 10-4 M in oxalate ion. What will happen once these solutions are mixed? Ksp(CaC2O4) = 2.3 × 10-9. A) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. B) Nothing will happen Ksp> Q for all possible precipitants. C) A precipitate will form as calcium oxalate is not soluble to any extent. D) A precipitate will form since Q > Kspfor calcium oxalate. E) There is not enough information to determine. 47) A solution contains 0.021 M Cl⁻and 0.017 M I⁻. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10-6, Ksp(CuI) = 5.1 × 10-12. 48) Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.
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- Fall '09
- pH, NH3