Problem: 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?

FREE Expert Solution

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)


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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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Selective Precipitation concept. If you need more Selective Precipitation practice, you can also practice Selective Precipitation practice problems.

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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.