I m looking for some idea about the solubility of aluminum amalgam (Al/Hg) in acetonitrile or dichloromethane.
In the literature, only THF is used for (Al/Hg) reduction which can't be with my radicals
Thanks in advance for your feedback.
Kind regards
Not clear what you are trying to do. If you're asking about the solubility of the metals themselves in various organic solvents, the answer is that their solubility is negligible.
Are you trying to reduce Al(3+) onto a mercury electrode so that an Al amalgam is formed? In that case you of course need an aluminum salt that is at least somewhat soluble in the solvent. I suspect the presence in the solvent molecule of oxygen atoms - such as the ether oxygen in THF - will be necessary.
Dear Emanuel Cooper,
Thanks a lot for your response.
I m trying to reduce my dithiadiazoly chloride salt using (Al/Hg).
Cheers
Dear Awatef Ayadi,
While I don't know the details of this reduction reaction, I wonder whether the use of mercury is absolutely necessary. It is possible that you can perform the reduction using a gallium-based "amalgam" of aluminum. If the volumes you deal with are small (gallium is fairly expensive), it may be worth trying. Your safety officer will be happier...
See the discussion at http://www.sciencemadness.org/talk/viewthread.php?tid=11687 , which also includes a Ga-Al phase diagram.
dear Awatef Ayadi find out following link
https://link.springer.com/content/pdf/10.1007/BF02880401.pdf
Dear Pr. Emanuel Cooper thanks a lot for all this interesting information.
Dear Pr. Devidas Bhagat thanks a lot for the interesting and helpful link.
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