A solution contains 0.036 M0.036 M Ag+Ag+ and 0.013 M0.013 M Pb2+.Pb2+. If you add Cl−,Cl−,...

A solution contains 0.036 M0.036 M Ag+Ag+ and 0.013 M0.013 M Pb2+.Pb2+. If you add Cl−,Cl−, AgClAgCl and PbCl2PbCl2 will begin to precipitate.

What is the concentration of Cl−Cl− required, in molarity, when AgClAgCl precipitation begins?

concentration of Cl−=Cl−=

What is the concentration of Cl−Cl− required, in molarity when AgClAgCl precipitation is 99.99% complete?

concentration of Cl−=Cl−=

What is the concentration of Cl−Cl− required, in molarity when PbCl2PbCl2 precipitation begins?

concentration of Cl−=Cl−=

What is the concentration of Cl−Cl− required, in molarity when PbCl2PbCl2 precipitation is 99.99% complete?

concentration of Cl−=Cl−=

Finally, give the Cl−Cl− concentration range in which Ag+Ag+ can be completely separated from Pb2+Pb2+ by precipitation.

Give the lowest Cl−Cl− concentration for the separation of Ag+Ag+ from Pb2+.Pb2+.

concentration of Cl−=Cl−=

Give the highest Cl−Cl− concentration for the separation of Ag+Ag+ from Pb2+.Pb2+.

concentration of Cl−=Cl−=

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Expert Solution

queen_honey_blossom answered 1 year ago

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