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Author: Subject: Could I have accidentally made dimethyl sulfate?
Tetra
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[*] posted on 11-1-2017 at 08:21
Could I have accidentally made dimethyl sulfate?


Hi, all.
Got bored and started to make Trimethyl Borate, but got interrupted after I added (more than needed) H2SO4 to some Methanol to dry it. I just remembered that the reaction of MeOH and conc. H2SO4 makes Dimethyl Sulfate, which is something I do NOT want to mess with...
I'm currently at a different location than my MeOH + H2SO4 mixture (Closed container), and I want to know: should I be worried about potentially having to handle DMSA when I get back [I want to avoid doing this], can I just proceed with the reaction, and can I dispose of it safely? (That is, if there was any formed?)

~A-N3

=(.PNG - 8kB

Edit: Descriptive title

[Edited on 1-12-2017 by zts16]
thx

[Edited on 12-1-2017 by Tetra]
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violet sin
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[*] posted on 11-1-2017 at 18:26


How concentrated was your acid...

Wikipedia- "Me2SO4 has been produced commercially since the 1920s. A common process is the continuous reaction of dimethyl ether with sulfur trioxide.[7]
(CH3)2O + SO3 → (CH3)2SO4"
----
That doesn't sound like just putting draincleaner in MeOH for a while. But hey, this isn't anything I have read up on either.

Looking around, the mildest condition found listed was 30'C MeOH with CuCl2 catalyst and SO2 bubbled through. Mentioned : http://chemistry.mdma.ch/hiveboard/chemistrydiscourse/000216...

Someone else might be more helpful here, but at least I got some random reading for the day

[Edited on 12-1-2017 by violet sin]




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[*] posted on 11-1-2017 at 20:36


It won't make any appreciable amount of dimethyl sulfate. It might form a little methyl bisulfate, but the equilibrium of MeOH + H2SO4 = MeHSO4 + H2O greatly favors the left.



As below, so above.
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Tetra
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[*] posted on 12-1-2017 at 05:12


Great, thanks guys.
Sin, the concentration was ~96-97/8 %.
Meta, that makes me feel better, haha. The Methyl Bisulfate sounds easier to handle.
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