Problem: A solution is 0.025 M in Pb2+. What minimum concentration of Cl- is required to begin to precipitate PbCl2? For PbCl2, Ksp = 1.17 x 10–5.

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PbCl2 (s)  Pb2+ (aq) + 2 Cl- (aq)


Ksp =[Pb2+][Cl-]2[Cl-] =Ksp[Pb2+]


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Problem Details

A solution is 0.025 M in Pb2+. What minimum concentration of Cl- is required to begin to precipitate PbCl2? For PbCl2, Ksp = 1.17 x 10–5.

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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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hamad's class at HAWAII HILO.