Example I A peracetic acid solution was prepared by reacting 90% hydrogen peroxide with glacial acetic acid, the two reactants being used in a mole
ratio of 1: 1.5 in the manner described by Greenspan in J. Am. Chem. Soc. 68, 907, using nitric acid as catalyst instead of the sulfuric acid catalyst
described in that paper. The nitric acid was employed in an amount corresponding to 1% of total volume of reactants. The resulting peracetic acid 40%
solution was then used in the preparation of mercuric acetate as follows.
In an all-glass apparatus consisting of a twoneck flask equipped with reflux condenser, to prevent evaporation losses, and stirrer were placed 24 g.
of metallic mercury to which were added 48 ml. of glacial acetic acid. The mercury was slurried up in the acid by means of the stirrer and then there
was added in one batch 18.8 g. of the above described peracetic acid solution, this amount corresponding to a 10% ex cess, calculated on a total
active oxygen basis, over the stoichiometric amount required. Agitation of the reaction mixture was continued for approximately 12 hours at room
temperature, after which time a copious amount of insoluble mercurous acetate had formed.
The flask with its contents was then heated on a waterbath until the precipitated, insoluble mercurous acetate was dissolved by transformation into
soluble mercuric acetate. There was no trace of metallic mercury or other insoluble residue. The solution was then cooled to precipitate the mercuric
acetate, which was recovered by filtering off the liquid phase.
The product analyzed 61.7% Hg. It was readily soluble in water. Total weight of mercuric acetate recovered was 37.8 g., indicating a practically
theoretical yield.
Example II In another test preparation of mercuric acetate was carried out exactly as described in Example I, but very vigorous stirring was provided
for by using a high efiiciency stirrer. Agitation of the reaction mixture was continued for 2 hours at room temperature. The flask with its contents
was then brought to reflux temperature. After 15 minutes of refluxing, the precipitated, insoluble mercurous acetate had been completely dissolved by
transformation into the soluble mercuric acetate. There was no trace of metallic mercury or other insoluble residue. The solution was then cooled to
precipitate the mercuric acetate, which was recovered by filtering off the liquid phase.
The product obtained analyzed 61.4% Hg. It was readily soluble in water. Total weight of mercuric acetate recovered was 37.6 g., indicating a
practically theoretical yield.
[Edited on 10-5-2018 by TheVoid]ninhydric1 - 9-5-2018 at 21:06
What are you planning to use these acetates for?TheVoid - 9-5-2018 at 21:52
I have an amount of both elements on hand that i would like to consume in a fashion that might later be useful.
I also wanted to try an Al amalgam using gallium, and will probably run a mercury amalgam for comparison.
I don't see why it shouldn't work for gallium i was just wondering if anyone has a reason.ninhydric1 - 10-5-2018 at 07:14
It could be that the reaction is exceedingly slow with gallium. Gallium requires strong acids such as sulfuric and nitric acid to be dissolved, albeit
slowly. Have you tried heating the gallium,/peracetic acid mixture for a few days?TheVoid - 10-5-2018 at 20:09
Have you tried heating the gallium,/peracetic acid mixture for a few days?
sorry I haven't actually tried to run the reaction yet i am still planning, that is a good idea though. I have a friend who specializes in this type
of chemistry i will have to ask them.
