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anonymous
 one year ago
The Ksp of PbCO3 and MgCO3 are 1.5 X 1015 and 1X1015 respectively at 298 K. The concentration of Pb+2 ions in a saturated solution containing MgCO3 and PbCO3 is –
(a)1.5 X104
(b)3X108
(c)2X108
(d)2.5X108
anonymous
 one year ago
The Ksp of PbCO3 and MgCO3 are 1.5 X 1015 and 1X1015 respectively at 298 K. The concentration of Pb+2 ions in a saturated solution containing MgCO3 and PbCO3 is – (a)1.5 X104 (b)3X108 (c)2X108 (d)2.5X108

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Rushwr
 one year ago
Best ResponseYou've already chosen the best response.0Hey what do u think the answer is ?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I think that the ans is option (c). Not really sure about it though ..........

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I 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

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Yea I didn't get any of the answers.What is your strategy to solve the problem?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Well for starters Haha \[PbCO _{3} (Aq) > Pb ^{2+} + CO _{3}^2 \] \[K _{sp} = [x][x] = [Pb ^{2+}][CO _{3}^2]\] \[MgCO _{3}> Mg _{2+} + CO _{3}^2\] \[K _{sp} = [x][x] = Mg ^{2+} CO _{3}^2 \]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0well 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

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@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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