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blogfast25
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Quote: Originally posted by Wizzard  | Here's some reference Be(SO)4 for you guys 
This was made from high-purity 98% sulfuric and high purity Beryllium lump, some fraction of a g of metal, to yeild around 1.5g of the salt.
I did not write down measurements... But it's close. The bottle is 1" and the salt is a bit hygroscopic to the point of deliquiesence.
[Edited on 3-13-2013 by Wizzard] |
Nice crystals, Wizz.
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woelen
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I also have some BeSO4 and this salt is not that hygroscopic. Maybe wizzard's product is so hygroscopic due to remains of H2SO4. I uploaded a picture
of my BeSO4.4H2O to wikipedia:
http://en.wikipedia.org/wiki/File:Beryllium_sulfate_4_hydrat...
The compound is not that interesting. I did some small experiments with the BeSO4 (the picture shown on Wikipedia is all I have, so my amount is very
limited). Its aqueous chemistry resembles that of aluminium sulfate. A flocculent precipitate of beryllium hydroxide can be made from this. This
redissolves in strongly alkaline solutions, similar to aluminium hydroxide, which dissolves in strongly alkaline solutions.
[Edited on 13-3-13 by woelen]
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blogfast25
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woelen: did you buy this BeSO4.4H2O in the photo?
It's true that it's a fairly ordinary compound and that Be2+ aqeuous chemistry is much more like Al3+ than Mg2+. But considering how many hoops I had
to jump through to obtain it from raw Beryl, I'm still quite glad I obtained it all the same. Once I've got a little more I'll probably go for
(NH4)2BeF4, the precursor to BeF2.
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Wizzard
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@blogfast - Thanks!
@woelen - That may be the case - There was a bit excess sulfuric acid present, and also a bit of undissolved Be! Over the course of about a year in a
plastic (barely sealed) container, they became a bit 'slimey', like they had just been taken from water.
One neat thing is they have some dispersion, like a diamond.. It's rather hard to capture. Perhaps I'll grow some larger crystals from my present
stock.
If only my hot plate wasn't dead 
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AndersHoveland
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What about trying to dissolve the beryl in boiling concentrated phosphoric acid ?
It can attack glass and fused quartz, though the reaction may take some time.
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blogfast25
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| Quote: Originally posted by AndersHoveland | What about trying to dissolve the beryl in boiling concentrated phosphoric acid ?
It can attack glass and fused quartz, though the reaction may take some time. |
Literature shows that untreated, raw Beryl is extremely acid-insoluble. Alkali fusion (the easiest method on a gram scale) and vitrification
by melting followed by extreme quenching are the most common treatments, to render it acid-soluble.
Beryl’s structure appears to be a bit of a solid solution of beryllia and alumina in silica, that kind of explains it.
I haven’t found any references to treatment with boiling conc. H3PO4 but that doesn't mean there aren't any.
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Admagistr
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Czech professor of Inorganic chemistry, Milbauer described a great method of separating Be from Al via the double salt - potassium beryllium oxalate.
I will look for the information and write down the details.
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chloric1
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| Quote: Originally posted by woelen | I expect molten KF/KHF2 will do the job, but this is really nasty stuff. Not something to try at home in my opinion.
Btw, your results, although not very encouraging at the moment, are interesting. They demonstrate that BeO indeed is a dificult material to treat
mechanically and chemically. I have finely powdered pure BeO and this has proven to be extremely inert, but as I wrote before, I only tried dissolving
in all kinds of hot aqueous concentrated solutions. I did not try any melts.
[Edited on 10-1-13 by woelen] |
General Chemistry by Linus Pauling mentions a process of reacting beryl with molten barium chloride yielding barium aluminosilicate and beryllium
chloride
Fellow molecular manipulator
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