Hi,
Iam looking for a explanation, how these Al/Hg reductions with acetid acid work.
I know that the used Hgcl2 is reduced to Hg at the surface of the Al pieces. So the Al2O3 is not protecting the Al anymore by contact with water. So
the H2O is reduced to H2 and the Al is oxidated to Al2O3.
The acetid acid is working as a catalyst but how does it work?
Why are some reactions working at the beginning and stopp witchout beeing able to be started again?
Usually the Al should react to Al2O3 anyway?
I got the Vogels Practical organic chemestry book where the preperation of Al/Hg reducing agent should be written down, but i couldnt find...
Would be great to get my queestions answered by someone who knowes.
Best regardsChemosynthesis - 24-11-2014 at 16:18
I'm not sure the exact mechanism has been elucidated. It would be interesting to see if anyone can say definitively.HollowMan - 25-11-2014 at 04:40
Why u have to use a 70% acetic acid? what happens if higher or lower concentrated and why?
doesent anyone know? or even where its located in Vogels practical org chemestry?macckone - 25-11-2014 at 10:14
You don't actually need acetic acid.
Aluminum amalgam will react with water
without acetic acid present.
However the specific reaction may use
acetic acid to protect the product from
over reduction.vmelkon - 25-11-2014 at 12:06
Why u have to use a 70% acetic acid? what happens if higher or lower concentrated and why?
doesent anyone know? or even where its located in Vogels practical org chemestry?
Well, if you were to write about what reaction you are talking about, it would help.HollowMan - 26-11-2014 at 13:16
So the acetic acid isnt working as a catalyst? i know the reaction will take place anywhy. I thought about reducing nitropropens like 3,4
Dimethoxynitropropen
[Edited on 27-11-2014 by HollowMan]Nicodem - 27-11-2014 at 13:02
