[MangoPlant]

Hello. I was just wondering if someone could confirm whether my reasoning is correct or point to some flaws?

Given that PbCO₃  is less soluble than PbI₂, and that precipitates are formed when either CO₃^2- or I^- ions are added to a aqueous solution of Pb²⁺, what would happen if CO₃^2- ions were added to a mixture of PbI₂ crystals in a large beaker of water?

My reasoning: Since PbCO₃ is less soluble than PbI₂ the CO₃^2- ions would react with whatever few Pb²⁺ are formed from the very little dissociation of PbI₂ and precipitate out as PbCO₃, which will shift the equilibrium of PbI₂ to the right (into it's dissociated ions), and if enough CO₃^2- ions are added eventually the equilibrium will keep shifting and all of the PbI₂ will disappear.

[Corribus]

Your general reasoning seems sound. 

[408]

This is exactly what will happen.

[MangoPlant]

Thanks Corribus and 408.