Could someone please explain this question to me please.
The colourless aqueous solution of a white solid sample formed a precipitate with an acidified aqueous solution of lead (II) nitrate. what is the possible identity of the original solution of this sample?
a) copper (II) sulfate
b) Barium chloride
c) Sodium sulfate
d) silver chloride
Could you please explain how you disprove the incorrect options.
Thx =]
This answer is incomplete. I'll ask that someone else finish it off because I'm not sure how to incorporate the acidification. I've started it off in the meantimeSince we know that all nitrates are soluble, there is no way that the precipitate formed could've involved the nitrate ion.
Hence, we consider substances involving the lead ion Pb
2+ which are insoluble. Problem is that both PbSO
4 AND PbCl
2 are insoluble!
Begin a process of elimination.
D) is the first one to go. This is because AgCl is also insoluble. Since silver chloride is insoluble, it cannot have been the aqueous solution.
A) is the second one to go. The presence of the Cu
2+ ion means that the solid would've been blue, when clearly it is white.
The last bit is the hard one.