In qualitative analysis, Ag+ , Hg2 2+ and Pb2+ are separated from other cations

Question

In qualitative analysis, Ag+ , Hg2 2+ and Pb2+ are separated from other cations by the addition of HCl. A)Calculate the concentration of Cl required to just begin the precipitation of AgCl in a solution having metal-ion concentrations of 0.022 M . B)Calculate the concentration of Cl required to just begin the precipitation of Hg2Cl2 in a solution having metal-ion concentrations of 0.022 M. C)Calculate the concentration of Cl required to just begin the precipitation of PbCl2 in a solution having metal-ion concentrations of 0.022 M. D)What fraction of the Pb2+ remains in the solution when the Ag+ just begins to precipitate?

Explanation / Answer

In qualitative analysis, Ag , Hg2(2 ) and Pb(2 ) are separated from other cations by the addition of HCl. Part A Calculate the concentration of Cl- required to just begin the precipitation of AgCl in a solution having metal-ion concentrations of 0.022 M. ANSWER = 8.2x10^(-9) Part B Calculate the concentration of Cl- required to just begin the precipitation of Hg2Cl2 in a solution having metal-ion concentrations of 0.022 M. ANSWER = 8.0X10^-9 Part C Calculate the concentration of Cl- required to just begin the precipitation of PbCl2 in a solution having metal-ion concentrations of 0.022 M. ANSWER = 2.3X10^(-2) Part D What fraction of the Pb(2 ) remains in the solution when the Ag just begins to precipitate? AgCl ppt's first, requiring the least amount of [Cl-] = 8.2x10^(-9) PbCl2 won't even start to ppt until much later when the [Cl-] is 2.3X10^(-2)

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