Will a precipitate of AgCl form when 0.050 mol NaCl(s) and 0.050 mol AgN0subnumber3(s) are dissolved in 500.0 milliliter of 3.0 mol/Litre NHsubnumber3 solution? (Kf for Ag(NH3)2^+ is 1.5x10^7)
Ksp for AgCl = 1.6x10^-10.© BrainMass Inc. brainmass.com October 24, 2018, 6:00 pm ad1c9bdddf
Before any reaction and after mixing the concentrations of all species are:
[Cl-]=0.1 M, [Ag+]=0.1 M, [NH3]=3 M.
First we ...
Solution includes calculations regarding the precipitate of AgCl.
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A solution contains 0.01 M Ag+, 0.04 M Hg22+ and 0.1 M Pb2+. NaCl is gradually added to precipitate the Ag+ as AgCl, the Hg22+ as Hg2Cl2, and the Pb2+ as PbCl2. Given the following Ksp values: AgCl (Ksp = 1.6 x 10-10); Hg2Cl2 (Ksp = 3.5 x 10-18); PbCl2 (Ksp = 2.4 x 10-4).
a) at what [Cl-] will precipitation of each salt begin. Start with the following UNBALANCED equations:
i) AgCl (s) --> Ag+ (aq) + Cl- (aq)
ii) Hg2Cl2 (s) --> Hg22+ (aq) + Cl- (aq)
i) PbCl2 (s) --> Pb2+ (aq) + Cl- (aq)
b) What is the concentration of Hg22+ in solution when AgCl begins to precipitate?
c) What are the concentrations of Ag+ and Hg22+ when Pb2+ begins to precipitate?
d) Discuss the suitability of fractional precipitation using NaCl for the separation of Ag+, Hg22+ and Pb2+.