vano - 8-9-2021 at 11:26
Hi, i bought lots of BeO(in hand), but I have no idea what to do with it. If anyone has an interesting idea, tell me and I will gladly do it.
[Edited on 8-9-2021 by vano]
AvBaeyer - 8-9-2021 at 18:10
I suggest that you make yourself knowledgeable in the toxicity of beryllium and its compounds. This element and its compounds are extremely toxic.
There is plenty of information via a Google search.
Please take care.
AvB
vano - 8-9-2021 at 22:37
Yes I have read a lot about beryllium and its compounds, I used to use metal to make its compounds, this is not the first time. I was just wondering
if anyone had any good ideas. thanks!
woelen - 8-9-2021 at 23:48
First try to dissolve some of the BeO in dilute acid (e.g. 20% HCl, H2SO4, or HNO3). I hope that this is possible. If needed, apply heating until the
solution is near boiling. BeO can be notoriously inert and very difficult to dissolve in any acid. It depends on how strongly it is heated/calcined
during its production.
If dissolving in dilute acids does not work, then you may have more success in hot concentrated H2SO4 (at 300 C), or molten anhydrous NaHSO4 (which is
very hot), or maybe even molten NaOH, but the latter three options are very corrosive and dangerous to handle. You also will need suitable vessels for
that.
If you cannot dissolve it in dilute aqueous acids, then in my opinion it will hardly be interesting for chemistry experiments. Too much risk in
working with the molten salts or 300 C conc. H2SO4.
And indeed, beware of berylliuym toxicity. Once you have some of the BeO dissolved, you have a very toxic brew!
vano - 9-9-2021 at 02:57
Thank woelen! It's fact that It's cancinated at low temperature, below 500°C, if cancinated temperature is higher you know oxide is very inert. This
two jar are exactly same and oxide is quite reactive i can dissolve it in acids and bases very easily. I'm going to buy HF to make some
fluoroberylattes.
Bedlasky - 9-9-2021 at 06:30
Woelen: Product from BeO + conc. H2SO4 will be anhydrous BeSO4, which is insoluble (soluble is only tetrahydrate).
vano - 9-9-2021 at 06:57
Why it's insoluble? It's hard to make hydrated salt from anhydrous in solution?
[Edited on 9-9-2021 by vano]
Bedlasky - 10-9-2021 at 08:15
I don't know why. I read it in book. Sometimes isn't easy to make hydrated salt from anhydrous one. Anhydrous chromium sulfate is also insoluble in
water.
https://woelen.homescience.net/science/chem/exps/raw_materia...
vano - 10-9-2021 at 10:29
Maybe reason is simple, but It's strange without reason. Thank!
teodor - 22-12-2021 at 08:00
"An apparently unique property of beryllium is its tendency to form so-called "basic" derivatives of a number of organic acids"
The scan from "Inorganic Synthesis, Volume III, Audrieth, 1950" is attached.
Attachment: img-211222164749.pdf (385kB)
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