578. If 0. 581 gram of magnesium hydroxide (MM 58. 3) is added to 1 8. If gram of magnesium hydroxide (MM 58.3) is added to 1.00L of water, will it all dissolve? (Ksp = 8.9 x 10-12)Below what pH would the solution be buffered so that it does all dissolve?
589. Calculate the concentration of NH4+ from ammonium chloride required to prevent the precipitation of Ca(OH)2 in a liter of solution that contains 0.10 mole of ammonia and 0.10 mole of calcium ion.
5910. If 50. mL of 0. 012M barium chloride are mixed with 25 mL of 1 10. If 50. mL of 0.012M barium chloride are mixed with 25 mL of 1.0 x 10-6M sulfuric acid, will a precipitate form?HINT: use the concentration quotient “Q” as we used it before
60You have a aqueous solution of Zn2+ and Pb2+ both 0. 0010 M You have a aqueous solution of Zn2+ and Pb2+ both M. Both form insoluble sulfides. Approximately what pH will allow maximum precipitation of one ion and leave the other in solution?[Ksp ZnS = 2.5 x 10-22][Ksp PbS = 7 x 10-29]
68You need to familiarize yourself with “typical” complex ions, Appendix K
69Note that a formation constant reflects the stability of the complex.
7013. Calculate the equilibrium constant for AgI(s) + 2NH3(aq) <===>[Ag(NH3)2]+(aq) + I-(aq)
7114. Will 5.0 mL of 2.5 M NH3 dissolve 0.0001 mole AgCl?
7215. A solution is prepared by adding 0. 10 mole Ni(NH3)6Cl2 to 0 15. A solution is prepared by adding 0.10 mole Ni(NH3)6Cl2 to 0.50 L of 3.0 M NH3. Calculate the [Ni(NH3)62+] and [Ni2+] in the solution.