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Author: Subject: The unfindable reference for Acetone Dicarboxylic Acid Anhydride
Johnny Windchimes
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[*] posted on 3-2-2020 at 05:46
The unfindable reference for Acetone Dicarboxylic Acid Anhydride


Good day,

I am on the hunt for a reference for the synthesis of 1,3 Acetone dicarboxylic acid anhydride from 1940. Findlay makes reference to it as well as Casale and a number of others. According to 1950's Findlay it yields "in excellent amounts"; that's the scientist equivalent of "BAD ASS DUDE!!!!111"


Here is the reference:

R. Kaushall, J. of Indian Chem. Soc., 17, 138 (1940).



Now, before anyone says UTFSE....

Google, sci-hub, my library at Uni.... cant find it. It definitely exists, but perhaps was never digitized? I've even emailed the current Indian Chem Society about it (no response for 2 weeks now, not wholly unexpected....)

Can anyone here locate this beast? I'd even take a copy in Hindi at this point....

Thanks to all who try!~

[Edited on 3-2-2020 by Johnny Windchimes]

[Edited on 3-2-2020 by Johnny Windchimes]
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[*] posted on 3-2-2020 at 10:20


We have a section for article requests. Can you please contact Polverone or Woelen for access.
"References
Articles or books may be requested or shared in this forum. For access, please contact Polverone or woelen. "

It is def. offline.

Your Uni. should be able to get it for you for a small fee (about 5 USD) as an interlibary loan/request. If you are a student you should even have discount on loans.



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Johnny Windchimes
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[*] posted on 3-2-2020 at 11:26


Thanks I'll give that a go!
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[*] posted on 4-2-2020 at 05:08


Below is a more recent paper. Four steps 77% yield. What do you want it for?

Attachment: Acetone-Dicarboxylic-Acid-Anhydride.pdf (184kB)
This file has been downloaded 237 times

[Edited on 2/4/2020 by wg48temp9]




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Johnny Windchimes
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[*] posted on 4-2-2020 at 10:19


Hey there,

I'd very much like to stabilize it (it decomposes quickly as you may know) for storage. I've been having some issues with the various methods (From Kato 1966 & 1967 to Findlay 1950 and Casale 1987) and I think its basically my poor temperature control. That, and the ungodly "classic" synth via H2SO4 and Citric acid that I could barely handle....

Now, I do have a tube furnace and a quartz tube re: Garage Chemists SO3 Oleum synth, but I would LOVE to avoid that and have been using just 98% H2SO4 and Anhydrous Citric acid.

Oh how much hubris I had when I read 1899 Jerden and decided "pfffft I have vac distillation and a few fritted filters..... I need not a hydraulic press as per EVERY 'real' scientist who ever made 1,3 acetonedicarboxylic acid...."

Well a bunch of wasted time (days and days and days and days) later I got a nice stainless steel press and away we went.

Again, typical of my syntheses I ran out of time and came back to the quenched classic (albeit modified to avoid oleum and use instead Conc. H2SO4) reaction in the freezer and worked it up. Positive violet colour test with FeCl3 sol'n in H2O, so instead of taking the 15 minutes to do even a basic melting point on it, away we went to waste a liter of acetic anhydride.

I'm fairly sure I eventually made Citraconic Anhydride because it all melted at basically 3 - 6 degrees C. But thats a crazy guess based on a literature browse and not much else.


Onwards to the later Oxone and Cobalt & Tungstate catalyzed reactions (ragukumar2014; ordered those catalysts and awaiting their arrival), and finally ending with a slight modification of a Chinese patent (CN103288629B) involving H2O2 oxidation with a catalytic amount of conc. H2SO4 and we have a winner.

Prep scale for now as I don't want to waste any more Citric Acid, but a nice melting point of 134-136 C, and keeping it in a jar at room temp for even a few hours had it decompose into a yellow mess and build pressure in the jar (A la' Acetone and CO2).


So.... short story long, I'd like to store the next batch as the anhydride and I wanted to know what Dr. Kaushal[sic] had to say about it which spawned such rave reviews.

Cheers~!

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Johnny Windchimes
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[*] posted on 30-11-2020 at 11:42


Quote: Originally posted by Johnny Windchimes  
Hey there,

I'd very much like to stabilize it (it decomposes quickly as you may know) for storage. I've been having some issues with the various methods (From Kato 1966 & 1967 to Findlay 1950 and Casale 1987) and I think its basically my poor temperature control. That, and the ungodly "classic" synth via H2SO4 and Citric acid that I could barely handle....

Now, I do have a tube furnace and a quartz tube re: Garage Chemists SO3 Oleum synth, but I would LOVE to avoid that and have been using just 98% H2SO4 and Anhydrous Citric acid.

Oh how much hubris I had when I read 1899 Jerden and decided "pfffft I have vac distillation and a few fritted filters..... I need not a hydraulic press as per EVERY 'real' scientist who ever made 1,3 acetonedicarboxylic acid...."

Well a bunch of wasted time (days and days and days and days) later I got a nice stainless steel press and away we went.

Again, typical of my syntheses I ran out of time and came back to the quenched classic (albeit modified to avoid oleum and use instead Conc. H2SO4) reaction in the freezer and worked it up. Positive violet colour test with FeCl3 sol'n in H2O, so instead of taking the 15 minutes to do even a basic melting point on it, away we went to waste a liter of acetic anhydride.

I'm fairly sure I eventually made Citraconic Anhydride because it all melted at basically 3 - 6 degrees C. But thats a crazy guess based on a literature browse and not much else.


Onwards to the later Oxone and Cobalt & Tungstate catalyzed reactions (ragukumar2014; ordered those catalysts and awaiting their arrival), and finally ending with a slight modification of a Chinese patent (CN103288629B) involving H2O2 oxidation with a catalytic amount of conc. H2SO4 and we have a winner.

Prep scale for now as I don't want to waste any more Citric Acid, but a nice melting point of 134-136 C, and keeping it in a jar at room temp for even a few hours had it decompose into a yellow mess and build pressure in the jar (A la' Acetone and CO2).


So.... short story long, I'd like to store the next batch as the anhydride and I wanted to know what Dr. Kaushal[sic] had to say about it which spawned such rave reviews.

Cheers~!





I feel its important to update this dead thread for anyone in the far future trying to make this stuff by saying that, no, the anhydride I thought I formed was not indeed the anhydride of acetonedicarboxylic acid, as a FTIR I was able to semi-recently run at school unfortunately revealed.

Those Chinese patents don't work, or at least I could not get them to work, line for line, ACS quality reagent for reagent (ie no shortcuts were taken).

That being said, I'm totally not the worlds best anything so if anyone else can make them work, please don't keep that info to yourselves!!:D




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[*] posted on 30-11-2020 at 12:51


Well JW, if it makes you feel any better I have tried most methods including the chinese patent with H2O2 and the only one that worked was conc sulphuric and anhydrous ctric acid. But I couldn't get a decent yield of free acid from the crude product but I did discover that simply adding the crude product to excess absolute ethanol and warming slowly to the 80-82 C for a few hours gave the diethyl ester in excellant yield (about 38% based on citric acid) so I think this is the way to go since citric acid and conc sulphuric acid are cheap. I even bought a 500g jar once but once you have opened it you have only hours to use it all and the yield of 1,3-diisonitrosoacetone was still very poor at <30%. In my opinion any preparation which claims to use aqueous conditions in its preparation is total Bull S***!

There is a method that claims it is possible to convert diethyl or dimethyl citrate direct to the dialkyl acetone dicarboxylate ester. Given that citric acid is a tribasic acid and that the acid groups are not identical I can see another minefield in this route too.
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Johnny Windchimes
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[*] posted on 30-11-2020 at 13:32


Quote: Originally posted by Boffis  
Well JW, if it makes you feel any better I have tried most methods including the chinese patent with H2O2 and the only one that worked was conc sulphuric and anhydrous ctric acid. But I couldn't get a decent yield of free acid from the crude product but I did discover that simply adding the crude product to excess absolute ethanol and warming slowly to the 80-82 C for a few hours gave the diethyl ester in excellant yield (about 38% based on citric acid) so I think this is the way to go since citric acid and conc sulphuric acid are cheap. I even bought a 500g jar once but once you have opened it you have only hours to use it all and the yield of 1,3-diisonitrosoacetone was still very poor at <30%. In my opinion any preparation which claims to use aqueous conditions in its preparation is total Bull S***!

There is a method that claims it is possible to convert diethyl or dimethyl citrate direct to the dialkyl acetone dicarboxylate ester. Given that citric acid is a tribasic acid and that the acid groups are not identical I can see another minefield in this route too.


Haha yes it does, lol, I've run the Reaxys gambit on this one myself.



Also, as long as we are discussing dead Acetonedicarboxylic Acid dreams....

Heres one from circa 1899 / 1900 that DOES work using Potassium Permanganate, but you need Mercury (sub)Sulfate to precipitate the Acetonedicarboxylic acid before it over oxidizes. Not really my cup of tea....

CHIMIEORGANIQUE.—Sur 'oxydation manganique des acides citrique etmalique. Note de M. G. Denigès. 10 grams d'acide citrique ont été dissous à chaud dans 20cc's d'eau; la solutionrefroidieversi5°aétéverséedansuneliqueurpréparéeendissolvant3 grams deMn04Kdans 100 cc's d'eau chaude,refroidieensuiteài5°.» Lemélange,entouréd'eaufroide,change de teinteauboutdequelquesinstants,puisbrunitendégageantabondammentCO2. Pour avoir un bon rendement, il faut éviter, dans cette réaction, que la températuredépasse 30° à 35° C


ORGANIC CHEMISTRY. — On manganic oxidation of citric and malic acids. Note from M. G. Denigès. 10 grams of citric acid was dissolved in 20cc's of hot water; the solution cooled to 5° C was poured into a liquor prepared with 3 grams of MnO4K in 100 cc's of hot water, then cooled to 5° C The mixture, surrounded by cold water, changes color after a few moments, then browns and releases abundant CO2. To have a good yield, it is necessary to avoid, in this reaction, that the temperature exceeds 30° to 35° C.



(EDIT: I only Google translated a bit of his article, read the pages yourself for the Mercury part etc etc)

denigras 1 - Copy.jpg - 144kB denigras 2 - Copy.jpg - 141kB denigras 3 - Copy.jpg - 148kBDenigas Hg Test ADA - Copy.png - 286kB denigras 4 - Copy.jpg - 133kB



[Edited on 30-11-2020 by Johnny Windchimes]




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Johnny Windchimes
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[*] posted on 30-11-2020 at 13:43


Or.... how About this bad boy?

In eine Losung von 14 g (0,1 Mol) Malonylchlorid[2] in 30 ml Chloroform (mittels P2P5 getrocknet) wurde bei einer Temperatur von -5 bis 0° im Ganzen 3 Stunden lang (0,4 Mol/Std.) Keten eingeleitet. Die Reaktionsmasse wurde am Rückflusskiihler mit 25 ml absoluten Athanols versetzt und das Losnngsmittel nach beendeter Reaktion durch Vakuumdestillation entfernt. Durch Fraktionierung des Rückstandes wurden 18,3 g (90 %) Acetondicarbonsaure athylester vom Sdp. 105-1100 /1 mm gewonnen. Eine Zur Analyse destillierte Probe be sass einen Sdp. von 92º/0.5 mm,?D20 1,4420, d420 1,113. Das Semicarbazon derselben wies den Smp. 96° auf; die Mischschmelzpunktbestimmung mit einer authentischen Probe (Smp. 96°) ergab keine Depression. Die angefiihrten Werte entsprechen den Literaturangaben[3]translation----------

-In a solution of 14 g (0.1 mol) of malonyl chloride [2] in 30 ml of chloroform (dried using P2P5) was ketene at a temperature of -5 to 0 ° for 3 hours (0.4 mol / h) initiated. 25 ml of absolute ethanol were added to the reflux condenser, and the solvent was removed by vacuum distillation after the reaction had ended. Fractionation of the residue gave 18.3 g (90%) of acetone dicarboxylic acid, ethyl ester, bp 105-1100 / 1 mm. A sample distilled for analysis had a bp of 92 ° / 0.5 mm, ?D20 1.4420, d420 1.113. The semicarbazone thereof had a mp of 96 °; the mixed melting point determination with an authentic sample (mp. 96 °) showed no depression. The values ??given correspond to the literature data [3]



I will also add that yeah....ketene....bad....deadly....dangerous....etc....

You'll also have to forgive the previous French and German excerpts I posted; they reek of Google translate!


Source for that and even MORE obscure acetonedicarboxylic acid refs in the attached ref doc, and I threw in the Reaxys doc too because, why not?


Attachment: ADA Reaxys - Copy.pdf (1.2MB)
This file has been downloaded 66 times

Attachment: Many Pathways to Acetonedicarboxylic - Copy.pdf (2.6MB)
This file has been downloaded 91 times





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[*] posted on 30-11-2020 at 14:04


Quote:

R. Kaushall, J. of Indian Chem. Soc., 17, 138 (1940).

It is abstracted in British Chemical Abstracts, available online.
However, fortunately, needed article is also available. To save the time - the article in attachment.

Attachment: Kaushall.pdf (265kB)
This file has been downloaded 97 times





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Johnny Windchimes
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[*] posted on 30-11-2020 at 14:09


Quote: Originally posted by kmno4  
Quote:

R. Kaushall, J. of Indian Chem. Soc., 17, 138 (1940).

It is abstracted in British Chemical Abstracts, available online.
However, fortunately, needed article is also available. To save the time - the article in attachment.


WHERE WERE YOU 9 MONTHS AGO!?!

THANKS!!:D:D:D




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[*] posted on 30-11-2020 at 14:17


I am still around, but I am not sure if the article was available online 9 months ago... Entire volume 17 is available, but 16 or 18 vols. are not :P.



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Johnny Windchimes
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[*] posted on 30-11-2020 at 14:43


@ Boffis:

If its esters you seek, I'm sure you're aquianted with these fine docs:

It's doable, but looks tedious as all hell IMO....

Order of reading should be Green, Hirota, Walton I think....



Attachment: GREEN DOWEX - turhanen2019 - Copy.pdf (1.5MB)
This file has been downloaded 68 times

Attachment: Asym Monomethyl Citrate - hirota1980 - Copy.pdf (5.7MB)
This file has been downloaded 65 times

Attachment: US2848480 - Walton Patent - Copy.pdf (569kB)
This file has been downloaded 70 times





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Johnny Windchimes
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[*] posted on 30-11-2020 at 14:45


*File was too big to include above*



Attachment: Citric Acid Esters - Copy.pdf (486kB)
This file has been downloaded 69 times




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[*] posted on 5-12-2020 at 12:42


Ummm. Exotic reagent.

One might jump to the conclusion, that the Acetone Dicarboxylic Acid Anhydride, might be destined for an exotic product.

Like being reacted with an alkyl alcohol, to form the half ester. Followed by a condensation that produces a Tropanone.

A challenge.

Now, I wouldn't take on the challenge, because the reduced Tropanone. Or Tropanol, would have two centers of assymetry.

Meaning that, in the final product, four isomers would be present. Three of them, of doubtful physiological
activity.

Though perhaps I am mistaken?



[Edited on 6-12-2020 by zed]
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[*] posted on 5-12-2020 at 15:01


IIRC you can also use periodic acid to oxidize citric acid instead of oleum but the conditions are hard to get right. Jackson attached mentions production of acetaldehyde by oxidation of lactic acid for example but acetaldehyde itself degrades under the rxn conditions.

Attachment: jackson2011.pdf (3.4MB)
This file has been downloaded 65 times





[Edited on 04-20-1969 by clearly_not_atara]
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[*] posted on 7-12-2020 at 18:12


Will if tropinone, or some other analog, is what you’re after I always thought a zn(cu) couple with 1,3-dichloroacetone (or dibromo) and N-methylpyrrole would be an option. Then a hydrogenation of the double bond followed by a Claisen condensation with dialkyl carbonate. If you were so inclined. Or do the hydrogenation after the Claisen condensation. That might be a better option

8E62050E-DA71-4F3D-9F75-5BE0EA8571A3.png - 22kB

[Edited on 8-12-2020 by Opylation]
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