2 compounds are able to precipitate in this solution. Cl- combines with either Pb2+ or Ag+. Now let us look at dissociation reactions for both.
PbCl2(s)⇌Pb2+(aq) + 2 Cl- (aq)
AgCl(s)⇌Ag+(aq) + Cl- (aq)
A solution is 0.15 M in both Pb2+ and Ag+. If Cl– is added to this solution, what is [Ag+] when PbCl2 begins to precipitate?
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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.