fusso
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extracting AlCl3 from aq using organic solvent?
AlCl3 anhydrous is soluble in CCl4, CHCl3 according to wiki hence I speculate it should also be soluble in DCM.
Is it possible to extract anhydrous AlCl3 from aq soln using DCM?
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diddi
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AlCl3 decomposes in (aq) AlCl3 + H2O = copious rapid evolution of HCl (g)
Beginning construction of periodic table display
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fusso
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That only occur when u heat it up to 1xx deg.
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Chemi Pharma
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@Fusso, you're misunderstanding the solubility of anhydrous AlCl3 in dry organic halogenated solvents as a lewis acid with AlCl3 dissolved in an
aquous solution.
At first, when you add anhydrous AlCl3 to water, it gives aluminium chloride hydroxide (H3Al2Cl3O3) and HCl. Even the hexahydrate AlCl3.6H2O you can't
extract from aquous solution with DCM or so, needing to add an excess of concentrated HCl to the aquous aluminium chloride hydroxide and freezing the
solution to 0ºC to precipitate crystals of AlCl3.6H2O.
If you're looking for an easy way to get anhydrous AlCl3, try to obtain it by the dry destilatiion of a mix between zinc chloride and aluminium
powder.
ChemPlayer made a video about that at you tube, but he actually were banned from there. Perhaps you can looking for these videos at bitchute instead:
https://www.bitchute.com
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fusso
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Quote: Originally posted by Chemi Pharma  | @Fusso, you're misunderstanding the solubility of anhydrous AlCl3 in dry organic halogenated solvents as a lewis acid with AlCl3 dissolved in an
aquous solution.
At first, when you add anhydrous AlCl3 to water, it gives aluminium chloride hydroxide (H3Al2Cl3O3) and HCl. Even the hexahydrate AlCl3.6H2O you can't
extract from aquous solution with DCM or so, needing to add an excess of concentrated HCl to the aquous aluminium chloride hydroxide and freezing the
solution to 0ºC to precipitate crystals of AlCl3.6H2O.
If you're looking for an easy way to get anhydrous AlCl3, try to obtain it by the dry destilatiion of a mix between zinc chloride and aluminium
powder.
ChemPlayer made a video about that at you tube, but he actually were banned from there. Perhaps you can looking for these videos at bitchute instead:
https://www.bitchute.com |
But can anhydrous ZnCl2 be made in a home lab setting?
[Edited on 24/05/18 by fusso]
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Chemi Pharma
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Yeah!
Otherwise AlCl3, anhydrous zinc chloride can be made from aquous ZnCl2, just evaporating the solution and drying the solid in a stove at 200ºC. ZnCl2
powder is very hygroscopic.
Aquous zinc Chloride is made from dissolving zinc into dilute HCl. Be careful with the hydrogen liberation, cause is highly explosive.
Anyway, I don't know where you live, but anhydrous zinc chloride is often dirty cheap and sold by any chemical supplier, even on the internet.
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fusso
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| Quote: Originally posted by Chemi Pharma | Yeah!
Otherwise AlCl3, anhydrous zinc chloride can be made from aquous ZnCl2, just evaporating the solution and drying the solid in a stove at 200ºC. ZnCl2
powder is very hygroscopic.
Aquous zinc Chloride is made from dissolving zinc into dilute HCl. Be careful with the hydrogen liberation, cause is highly explosive.
Anyway, I don't know where you live, but anhydrous zinc chloride is often dirty cheap and sold by any chemical supplier, even on the internet.
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I asked the synthesis method because I saw this on wiki:
When hydrated zinc chloride is heated, one obtains a residue of Zn(OH)Cl e.g.[27]
ZnCl2·2H2O → ZnCl(OH) + HCl + H2O
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Chemi Pharma
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Yes, I see now I was wrong. Evaporating the solution will only give the trihydrate, which will decompose if heated into hydroxy chloride.
But don't give up. You can heat the trihydrate with NH4Cl in a stream of HCl to obtain the anhydrous form. There are other ways to obtain anhydrous
ZnCl2. Look at this page: http://zinc.atomistry.com/zinc_chloride.html
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Nicodem
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Thread Moved
27-5-2018 at 12:17 |
AJKOER
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Two points, your atomistry reference on paths to ZnCl2 also suggests "and by the action of chlorine on zinc oxide."
Research confirms my suspicion that this is not only a reported path to ZnCl2 but possibly also Cl2O. Here is an old reference, to quote:
"An excess of chlorine, in acting on a solution of bleaching powder, may also give chlorine monoxide, because calcium carbonate also gives chlorine
monoxide under the action of chlorine. This reaction may be brought about by treating freshly precipitated calcium carbonate with a stream of chlorine
in water: 2Cl2+CaCO3=CO2+CaCl2+Cl2O. From this we may conclude that, although carbonic anhydride displaces hypochlorous anhy dride, it may be itself
displaced by an excess of the latter.
Therefore, if such oxides as those of zinc or mercury be shaken up in water, and chlorine be passed through the turbid liquid,” a reaction occurs
which may be expressed in the following manner 2HgO + 2Cl2 = Hg2OCl2 + Cl2O. In this case, a compound of mercury oxide with mercury chloride, or the
so-called mercury oxychloride, is obtained: Hg2OCl3 = HgO + HgCl2. This is insoluble in water, and is not affected by hypochlorous anhydride, so that
the solution will contain hypochlorous acid only, but the greater part of it splits up into the anhydride and water.”
Source: 'The Principles of Chemistry', Volume 1, Part 2 by Dmitry Ivanovich Mendeleyev, pages 479 to 480. Link: https://books.google.com/books?id=GR1LAQAAMAAJ&pg=PA479&...
The second point is Atomistry.com is a copyrighted composition of old chemical journals on which the copyright has expired. As such, most of the
material is dated and the reader should also check with more recent sources.
[Edited on 7-6-2018 by AJKOER]
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