@Romz
I got this question wrong too. Since you seem to understand it now, do you mind explaining how the stuff in the procedure that precipitates out later is considered LESS soluble? The post to which you were referring (see above) doesn't really go into details about that.
It just doesn't seem intuitive to me. If something is really that insoluble, it should precipitate first.
Not a problem! Took me long to understand it as well.
If you've got your TBR next to you, flip to and look at Pages 195-197 of the first book of General Chemistry.
The principle they're applying here is that seen in Ion exchange chromatography and its actually a very subtle nuance.
WHY I GOT THIS QUESTION WRONG:
I
thought we had a solution of our anions and we were adding lead (Pb 2+) and watching for which one would precipitate out first. THIS IS WRONG. Re-read the experiment again.
WHY THIS QUESTION IS RIGHT:
Upon re-reading the experiment again, we'll notice that they were sequentially reacting the
products with a new set of reactants to see which one would form a precipitate. For example, in reaction #1-->#2, they DO NOT completely filter away Reaction Compound A. Instead, they react it with KI to form a new precipitate PbI. That is to say:
PbSO4 (Compound A) + KI <----> PbI2 + Whatever. Looking at this reaction, we see that between PbSO4 and PbI2, PbI2 is less soluble than PbSO4, hence it forms a precipitate. This chain of reactions continues downstream until the experiment ends. (PbI2 more soluble than PbCO3). Hence CO3 is the least soluble. To refer back to my earlier suggestion, this is the theory behind ion exchange chromatography, in which we elute the more soluble compound initially attached in the matrix through a metathesis reaction to form a more insolube compound not containing our desired anion/cation.
I hope this makes it more clear. IMO this is a GREAT MCAT passage testing our ability to really understand what's going on rather than hastily applying theory. They fooled me too - hopefully it doesn't happen again
.