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DalisAndy
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Could one use permagnetic acid, and/or carbonatic acid? And why would Oxalic acid easier? I'm just curious
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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blogfast25
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'permagnetic acid'? That's either an Error 101 or a Googlewhack. 
You mean permanganetic acid. "HMnO<sub>4</sub>". Doesn't REALLY exist. Potassium permanganate + sulphuric acid would work but NO ONE would
do it like that.
You mean carbonic acid. That's soda water, basically. Do YOU think that would work? (Hint: NO!)
The oxalates of Nd and Fe are basically insoluble. It's a recipe for stalled reaction/big mess.
Go down the hardware store and get some 'muriatic acid' (HCl) or toilet drainer (H2SO4).
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DalisAndy
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Quote: Originally posted by blogfast25  |
'permagnetic acid'? That's either an Error 101 or a Googlewhack.
You mean permanganetic acid. "HMnO<sub>4</sub>". Doesn't REALLY exist. Potassium permanganate + sulphuric acid would work but NO ONE would
do it like that.
You mean carbonic acid. That's soda water, basically. Do YOU think that would work? (Hint: NO!)
The oxalates of Nd and Fe are basically insoluble. It's a recipe for stalled reaction/big mess.
Go down the hardware store and get some 'muriatic acid' (HCl) or toilet drainer (H2SO4). |
http://i.word.com/imedical/permanganic%20acid
It does by the way
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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Brain&Force
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Making permanganic acid is an extremely difficult endeavor, and it's not even stable for long in water. The use of oxalic acid works by complexing the
iron away as the soluble tris(oxalato)ferrate(III) complex as the neodymium precipitates as the normal oxalate.
At the end of the day, simulating atoms doesn't beat working with the real things...
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blogfast25
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A word of advice: medical dictionaries aren't the beez knees for looking up chemical stuff, you know?  <=== that's a picture of a doctor in cool shades, nodding approvingly, BTW...
[Edited on 26-5-2015 by blogfast25]
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blogfast25
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| Quote: Originally posted by Brain&Force | | Making permanganic acid is an extremely difficult endeavor, and it's not even stable for long in water. The use of oxalic acid works by complexing the
iron away as the soluble tris(oxalato)ferrate(III) complex as the neodymium precipitates as the normal oxalate. |
Errrmmm... except that oxalic acid won't oxidise Fe to Fe(III). So that separation method I proposed (and which works) only works AFTER the Fe has
been oxidised to Fe(III).
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DalisAndy
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| Quote: Originally posted by blogfast25 | | Quote: Originally posted by Brain&Force | | Making permanganic acid is an extremely difficult endeavor, and it's not even stable for long in water. The use of oxalic acid works by complexing the
iron away as the soluble tris(oxalato)ferrate(III) complex as the neodymium precipitates as the normal oxalate. |
Errrmmm... except that oxalic acid won't oxidise Fe to Fe(III). So that separation method I proposed (and which works) only works AFTER the Fe has
been oxidised to Fe(III). |
So using sulfric then oxalic would separate the Neodynium? Since Fe is in the +2 oxidation state
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
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elementcollector1
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It would, as I can attest to, but now you have to deal with the neodymium oxalate. So far, mine's resisted H2SO4, HCl, and even
a mix of H2SO4 and NaNO3. Good luck to ya.
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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MrHomeScientist
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Once again I'd recommend you read this thread in its entirety. Many of your questions have been answered right here. I know it's long; It's a
complicated process. It's worth it to learn as much about it as possible if you're serious about pursuing this project.
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DalisAndy
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Does neodymium and other rare earths have black light florescent properties?
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
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blogfast25
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Also in the thread.
Also here:
http://en.wikipedia.org/wiki/Neodymium%28III%29_chloride
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aga
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Has anyone successfully isolated Nd yet ?
There is a tiny vial of Neodymium Sulphate somewhere in the lab as i recall ...
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blogfast25
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| Quote: Originally posted by aga | Has anyone successfully isolated Nd yet ?
There is a tiny vial of Neodymium Sulphate somewhere in the lab as i recall ... |
Compound yes (sulphate), metal no. Re. latter, MrHomeScientist is the 'Amundsen' of that race here on SM.
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aga
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Huh ?
I followed some instructions in this thread around page 4000 or so and have had some nice lilac powder in a vial for many months.
That sample even survived the last Cull (to get the vials back) as the colour is rather nice.
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blogfast25
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Listen, I've had 3 Chimay's and I'm not drunk yet. Try and keep up! 
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aga
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In a universe far, far a way, a long, long time ago, ISTR that it began with some magnets in an acid ...
One appears to have made NdSO4 simply following something (i forgot what) in this thread.
Lilac powder awaiting further instructions.
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blogfast25
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There are two Nd sulphates. One's nice ruby red crystals, the other a sandy, lilac powder. We don't know what causes the difference. Be a trailblazer!
Hint: I think it's hydration. Not sure though... The easiest way would be to determine sulphate content of both 'varieties'.
[Edited on 27-5-2015 by blogfast25]
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j_sum1
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1. Leave in vial to look pretty.
2. Start work on Lanthanum from pool phosphate remover.
3. Obtain another vial with pretty crystals.
4. Copy mrhomescientist's beautiful and highly effective apparatus
5. Come in second with a better yield on the Nd race
6. Win the La race.
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aga
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7. Get some more beers and just post nonsense.
Ok. sounds like a Plan.
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blogfast25
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8. Look up protocol for BaSO4 gravimetry
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elementcollector1
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I would also like to add that the pink oxalate seems completely resistant to a mixture of elemental bromine and sulfuric acid as well.
Running out of ideas to dissolve this thing...
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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blogfast25
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| Quote: Originally posted by elementcollector1 | I would also like to add that the pink oxalate seems completely resistant to a mixture of elemental bromine and sulfuric acid as well.
Running out of ideas to dissolve this thing... |
Random chemical mixing won't get you anywhere. There's nothing bromine can do here.
Calcine the oxalate to oxide. Then treat with boiling 95 % (at least) H2SO4. Or fuse with NaHSO<sub>4</sub>.
[Edited on 28-5-2015 by blogfast25]
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DalisAndy
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| Quote: Originally posted by blogfast25 |
There are two Nd sulphates. One's nice ruby red crystals, the other a sandy, lilac powder. We don't know what causes the difference. Be a trailblazer!
Hint: I think it's hydration. Not sure though... The easiest way would be to determine sulphate content of both 'varieties'.
[Edited on 27-5-2015 by blogfast25] |
Ummm if they are crystals, shape can be determined by dissolving them and letting them solidify on a sting. Like borax ornaments
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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DalisAndy
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| Quote: Originally posted by blogfast25 | | Quote: Originally posted by elementcollector1 | I would also like to add that the pink oxalate seems completely resistant to a mixture of elemental bromine and sulfuric acid as well.
Running out of ideas to dissolve this thing... |
Random chemical mixing won't get you anywhere. There's nothing bromine can do here.
Calcine the oxalate to oxide. Then treat with boiling 95 % (at least) H2SO4. Or fuse with NaHSO<sub>4</sub>.
[Edited on 28-5-2015 by blogfast25] |
Dude, oxalates decompose easily. Go look it up, like I did today. or you could use Lithium in ethanol (or what ever non-polar solvent you have). or
when in doubt electrolysis, of it's sulphate form.
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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DalisAndy
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I don't get why we haven't created a location to consolidate knowledge for projects? I mean like log all expirements done, so others can test it
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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