[elementcollector1]

John Cuthber, on 5 January 2012 - 06:48 PM, said:

Unless you can tell me what oxidant you plan to use for step 5 ("Oxidise this resulting solution to produce Pr2 O(SO4)3(?)")
you are talking nonsense.
Also "you are no worse off than you were to begin with. " is only true if you don't value your time (strictly speaking, someone else's time) and didn't pay for the materials you wasted.

I'd guess H₂O₂.
"Someone else's time?" "materials you wasted?" Brother, I'm experimenting with my stuff, not someone else's. I paid for everything, and do this in my free time.
Even if I do get a precipitate containing both metals, then it would still be in the (III) oxidation state. If that's true, then I can probably just re-dissolve in HCl or H₂SO₄.
Again, no matter how much speculating is done on whether or not it will work, it all comes down to the actual experiments, which I'm perfectly willing to sacrifice my materials and free time to do. Now, it's just a matter of coming up with the easiest way to do it.

[elementcollector1]

Just tested the oxalic acid + magnet chloride today, and found myself with a greenish-gray precipitate. This is not neodymium oxalate, but could it be the oxide? Something else entirely?