Steam - 18-7-2014 at 17:49
Ok, so this may be a dumb question but upon looking at all the procedures fro making Cu(II) acetylsalicylate not one used an organic solvent to
dissolve the ASA. Would it be possible to avoid aqueous conditions while producing Cu(II) acetylsalicylate?
For example, could you potentially heat the ASA into it liquid state (165 C I think? which is below the decomposition temperature of the complex ) and
then add the copper salt?
I am trying to substitute one of the acetylsalicyates with a fatty salicylate ester (which is in a liquid state) if this helps.
TheChemiKid - 18-7-2014 at 19:51
Why didn't you add this to the existing Copper acetylsalicylate thread?
Steam - 19-7-2014 at 04:31
Didnt want to bring it back from the dead!
TheChemiKid - 19-7-2014 at 06:13
Ok, fine with me. 
Oscilllator - 19-7-2014 at 16:45
I don't understand whta you are trying to achieve here. If your fatty salicylate ester is a liquid, then why do you need to melt normal ASA?
As for conducting the reaction in an organic medium - go try it! Dissolve some ASA in an organic solvent, along with a copper(II) compound (perhaps
the nitrate, as the sulfate is fairly insoluble in most organic solvents). Mix the two together, and observe the results 
.
Going out and conducting experiments like this for yourself is an important part of chemistry. Just sitting round trying to find a previous example of
your reaction working often turns out to be way less time effective than just going out and doing it yourself.