The Ksp of PbCO3 and MgCO3 are 1.5 X 10-15 and 1X10-15 respectively at 298 K. The concentration of Pb+2 ions in a saturated solution containing MgCO3 and PbCO3 is – (a)1.5 X10-4 (b)3X10-8 (c)2X10-8 (d)2.5X10-8

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The Ksp of PbCO3 and MgCO3 are 1.5 X 10-15 and 1X10-15 respectively at 298 K. The concentration of Pb+2 ions in a saturated solution containing MgCO3 and PbCO3 is – (a)1.5 X10-4 (b)3X10-8 (c)2X10-8 (d)2.5X10-8

Chemistry
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Hey what do u think the answer is ?
I think that the ans is option (c). Not really sure about it though ..........
how did you find it?

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I didn't this was the ans given in my book ……………….. Since quite a few ans in that book have proven to be incorrect I am not really positive that this is the right ans. If I knew the solution to the question I wouldn't be asking for it on openstudy
Yea I didn't get any of the answers.What is your strategy to solve the problem?
Well for starters Haha \[PbCO _{3} (Aq) --> Pb ^{2+} + CO _{3}^2- \] \[K _{sp} = [x][x] = [Pb ^{2+}][CO _{3}^2-]\] \[MgCO _{3}--> Mg _{2+} + CO _{3}^2-\] \[K _{sp} = [x][x] = Mg ^{2+} CO _{3}^2- \]
well done the PbCO3 (s) it is insoluble, that is the reason you dont include in the Ksp, the ions are (aq) PbCO3(s)−−>Pb2+(aq)+CO23−(aq) then we have the common ion CO23−(aq) effect in the solubility
@Cuanchi thanks for pointing that out.. i forgot most of the solubility rules, but I never saw a problem where we are given two Ksp values

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