We got this interesting lab today in AP Chem. Pretty much, you have to figure out the formula for copper chloride (unknown whether it's I or II) by devising your own procedure. The only hint you're given is that you can use .1 mol AgNO3. There is only 1.5g copper chloride.
I was thinking that you could mix the silver nitrate with the copper chloride so that silver chloride would precipitate. You can filter that out, mass it, and then find the mass of the Cl. I'm not sure what to do with the copper nitrate, though. I suppose you could figure out the volume of the c chloride sample, and from there find the density. I have a feeling that it'll have something to do with the limiting reactant... or I'm making stuff up that sounds good to me
Hmm... we'll hopefully talk about this more in class.
The point of this post is
not for you to tell me the answer, but rather to tell me if I'm on the right track. And if that offends your delicate academic sensibilities, so be it.