A 2.0 L solution contains [Ag+] = 0.100 M and [Pb(2+)] = 0.100 M (Ksp = 1.8 * 10^(-10) for AgCl and Ksp = 1.8 * 10(-5) for PbCl2). Explain the metals are selectively precipitated by adding NaCl. Presume no volume changes.
(a) Explain at what [Cl^(-)] will each salt begin to precipitate?
(b) Explain what percent of the Ag+ has precipitated before the PB^(2+) begins to precipitate?
(c) Explain how many grams of NaCl must be added to precipitate a maximum amount of AgCl before any PbCl2 begins to precipitate?