Klute
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Synthesis of gamma-nonalactone (Coconut aroma)
This is a very easy preparation of gamma-nonalactone, or 4-pentyl-gamma-butyrolactone, a naturally occuring aroma.
The downside is that it starts from heptaldehyde, which isn't available to nayone... I gues it could be made by oxidizing heptanol by TEMPO-mediated
reactions, but you still need to find the alcohol...
The reaction is composed of two steps:
-malonic synthesis of a b,gamma-unsaturated acid
-intramolecular cylization to the lactone.
Sorry, no photos this time, my camera is broken for the moment...
Preparation of the unsaturated acid
4.16g (40 mmol) of malonic acid where charged in a 250mL 3-neck RBF equipped with a condenser, an addition funnel, a thermometer and magnetic
stirring.
5,6 mL (40 mmol) of heptaldehyde were added, followed by 8mL triethylamine (60 mmol). the addition of the amine caused some milkyness to appear as the
malonic acid dissolved, and quickly gave place to a clear, colorless solution. The mixture was heated to 100-110°C for 1H.
The now slight yellow limpid solution was transfered to an seperating funnel, and the flask rinced with 2x20mL Et2O. An aqueous layer dropped out.
40mL of 4N HCl were then added, and the layers shaken. The slightly opaque yellow ethereal layer was then washed with 2x10mL dH2O.
40mL 1.25N NaOH were then added, the aqueous layer turning light redish, and the organic staying light yellow. The aq. was seperated, and the organic
washed with 2x10mL dH2O.
The solution was washed with 2x10mL Et2O, and acidified with 40mL 4N HCl, a red/purple oily compound crashing out. The acid was extracted with 3x20mL
Et2O, washed with 20mL brine, and dried over Na2SO4.
The solvent was then removed, leaving 4.7g (30,13 mmol, 75,33%) of light amber oil, single spot by TLC (Pet ether:AcOEt 6:4, Rf= 0.52).
Cyclisation to the lactone
The crude product obtained in the first step was dissolved in 30mL heptane, giving a very slightly amber limpid solution. An equal weight of Amberlyst
15 cationic resin was added, and the mixture heated to reflux for 1H with strong stirring.
The flask was then cooled, and the colorless limpid supernatant decanted into a 100mL flask. The resin was washed with 3x10mL Et2O, which were added
to the heptane solution.
The solvents were removed, leaving 4.6g (29.45 mmol, 97.74%) of a pale yellow oil, with a strong coconut smell, very "natural" smell.
The lactone was thus obtained in a 73.63% yield from the aldehyde.
The Amberlyst-catlyzed reaction was very clean and effective, I am surprised at the selectivity of this catalyst, considering the extremly simple
workup an dthe fact that it can be recyled numerous times.. Agreed, it is a bit expensive, but worth the effort IMHO... I think I will try it with
other acid-catalyzed condensations and see how it goes!
I think this reaction is generaly applicable for substitued lactones, using various aldehydes.
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
-Alice Parr
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panziandi
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Hexan-1-ol and Octano-1-ol are more widely available than the heptan-1-ol in my experience atleast.
Perhaps chain extension of the acids from butanoic acid or similar would be feasible for people who want to make it for the fun of it and then reduce
to the heptanol and oxidise to heptanal?
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Klute
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Well, 1-halogenohexane could bve made from the alcohol, the grignard reagent prepared and reacted with formaldehyde to the heptanol, which could then
be oxidized...
In anycase, the preparation of the aldheyde is even harder than the reaction tiself, which is a pity... Maybe other (shorter) aldheydes give a
simialr smell? There is another dicyclic butyrolactone wich is said to have a coconut smell:
"Coconut decanone"
This is basicly a cyclized 4-pentylbutyrolactone with a methyl attache don the 3 position of the side chain, so maybe a straight octan chain will
behave similarily? Only experimenting can tell! 
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
-Alice Parr
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panziandi
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Tempting! I have some hexanal kicking about I think but not sure about the malonic acid. Maybe if I have some time I may try it with that.
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Klute
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I think you can substitute malonic aicd for diethyl malonate, although I'm not a 100% certain this might no cause the elimination to happen between
the alpha et beta carbon..
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
-Alice Parr
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Ebao-lu
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Very interesting reaction, because usualy knoevenagel is known to give a,b-unsaturated products.
Also, the gamma-lactones can be prepared from AcOH, Mn(OAc)3 and alkenes - but i've seen it only in a book, without procedure.
As for heptanal, probably it can be made from olein acid(sunflower oil major fat acid) - via epoxidation and oxidation of diol (hypervalent
iodine/DMP)
[Edited on 17-10-2008 by Ebao-lu]
[Edited on 17-10-2008 by Ebao-lu]
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Klute
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Indeed, I was pretty surprised at first, I suppose the dehydratation to the unsaturated acid occurs before the decarboxylation, and that the acidic
methylene H-R (alpha from the carboxylic acids) is too delocalized by the malonic acid synthon to be favored in the formation of the double bond from
the carbocation compared to the gamma H-R. I would have thought that the conjugated a,b-unsaturated acid would be more energetically farvored, but
apparently not so. I also quite surprised there isn't any isomeration during the reflux with the amberlyst resin. I guess it would happen if there was
presence of water (so maybe usual acids like H2SO4 or H3PO4 would not work here?)
Has anybody got a definate explanation for the unusual regioselectivity?
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
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Ebao-lu
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I think, firstly conjugated unsaturated acid is formed indeed(like in usual knoevenagel), but then it is isomerised to the beta-gamma unsaturated,
that is probably more stable for such long-chain carbonic acids because of some reasons.. Thats because the beta-gamma unsaturated product can not
result from eliminaton of H2O, because the gamma-hydrogen is not acidic.
As for regioselectivity of amberlyst, thats probably because it is a "mild" catalyst that does not form a reactive carbocation(that can be further
isomerised), it just activates the double bond a bit. And the gamma lactones are the most stable and easily formed because of steriochemical reasons
also
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Klute
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Thank you for your interpretation, it makes sense. making the aldehdye from oleic acid is indeed a very good idea. I will ahve a look on the diol
oxidation, to see if anything else can be used.
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
-Alice Parr
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Ebao-lu
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Heptanal seems to be avaliable product. Just read that it is produced in industry from castor oil and recinoleic acid methyl ester via decomposion at
500C and reduced pressure. While distillation of castor oil at normal pressure heptanal also forms, but as for yield i dont know. Anyway, technical
heptanal should be avaliable, not more expensive then hexanal etc.
As for diol breakup, i think it is possible to use hypervalent iodine compounds, like phenyl iodosoacetate PhI(OAc)2, which is highly selective to
diol oxidaion. It is prepared from phenyliodide, 30%H2O2 and AcOH(or maybe Ac2O, i forgot). The most interesting thing is to combine epoxidation
step(by AcOH/H2O2) and oxidation of diol in one reaction, or at least one pot reactions, and make phenyliodide a catalyst at small quantities. I
should inquire, weather Ac2O or AcOH is used for PhI(OAc)2 preparation.
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Ebao-lu
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forgot to say, phenyl iodosoacetate reacts with diol to give PhI back
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Klute
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I think it's Ac2O. I have no problem accesing heptanal, but that's because I cna purchase chemicals from suppliers, which isn't the case of lot of
people here. Working on a pretty clean reaction from vegetal oil and recycleable reactant seems like a good idea
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
-Alice Parr
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Ebao-lu
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I've checked, in that procedure indeed Ac2O was used. But fortunately, i found another one, that uses AcOOH/AcOH
http://www.orgsyn.org/orgsyn/prep.asp?prep=cv5p0660
Peracetic acid is easily formed from AcOH and H2O2 in the presence of catalytical H2SO4 (even in procedure they seemed to use an equilibrium mix).
Due to comperatively high yields of PhI(OAc)2 (83-91%) and fast reaction, the formation of PhI(OAc)2 from catalytical PhI should not be an issue also.
Now i'll look for any procedure of glycol oxidation by PhI(OAc)2, if it is carried out in same mild conditions or not..
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Fery
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3-nonenoic acid
In 250 ml 3-neck RBF were mixed:
12,5 g of malonic acid (120 mmol, M = 104,06 g/mol)
13,7 g heptaldehyde (120 mmol, M = 114,19 g/mol, should be 17,0 ml, density 0.80902 at 30 °C)
18,2 g triethylamine (180 mmol, M = 101,193 g/mol, should be 25,1 ml, density 0.7255).
(The flask was on a scale - I prefer weighing reactants instead of measuring volumes).
Liebig reflux condenser was attached, a thermoprobe of heating mantle was inserted and the third neck was stoppered (using 2-neck flask would be
enough, there is no need to drop liquid reactants through the third neck using dropping funnel).
The content was refluxed for 1 hour at temperature above 100 C inside the flask (heating mantle target T was set to 105 C).
At 81 C there was already little of tiny bubbling. Reflux vs. CO2 evolution ? - but the CO2 should not evolve, it should be bound by the triethylamine
into the amine carbonate or hydrogencarbonate.
At 85 C there was already a condensate dripping back into the reaction from the reflux condenser.
At 87 C there were already few drops per second dripping back to the reaction from the condenser. According the b.p. it looks like some azeotrope
because b.p. triethylamine 89 C, heptanal 153 C and also some reaction water may be present too. Or it was just refluxing triethylamine and the T was
few C within the tolerance of the thermoprobe and heating mantle.
At 103 C white fumes observed in the flask and the condenser (below that T there was just pure reflux without fumes). The fumes were in the flask but
also in the top part of the condenser. After half an hour the white fumes observed only in the flask (but in reduced quantity) and not in the
condenser anymore, in the condenser there were just clear droplets of a condensate. Maybe the decarboxyllation finished (or just decomposition of
triethylamine hydrogencarbonate)?
Using smaller flask 100 ml would be better (not much bubbling either CO2 evolution), less air in the apparatus = reduction of the oxidation of the
aldehyde. I used too big flask due to expected massive CO2 evolution which did not occur (or occured at slow rate).
The reaction mixture was transferred into 250 ml separatory funnel, RBF was rinsed with 3 x 20 ml diethylether, ether washings were added into the
separatory funnel.
Now the amine was neutralized with HCl which requires at least 180 mmol of HCl. It is exothermic which could boil out the ether which is undesirable.
Strongly cooled HCl was prepared by mixing 20 g of crushed ice with 13,0 ml of 35 % HCl.
20 g of crushed ice was added into the separatory funnel and then the above chilled diluted HCl dropwise in portions while stirring. Bottom water
phase was discarded, testing with pH paper showed strong acidic reaction (if not add few more drops of diluted HCl), upper organic layer was kept.
The ether layer was washed with 2 x 20 ml of water, bottom water phase discarded and the upper organic layer kept.
Now the 3-nonenoic acid was neutralized into its sodium salt. It requires theoretically 120 mmol of NaOH (4,8 g).
5,2 g NaOH (slight excess) was dissolved in 80 ml of water + 20 g of crushed ice. Chilled solution of NaOH was added dropwise into the separatory
funnel to the ethereal solution of the 3-nonenoic acid dropwise while stirring. It is again exothermic. Do not allow ether to boil out, eventually add
10 g of crushed ice into the separatory funnel.
Bottom water phase containing sodium 3-nonenoate was kept and upper ether layer discarded (ether could contain unreacted heptanal and organic
sideproducts and so on, Klute extracted the upper organic layer twice with water and added it to the water phase of sodium nonenoate to increase
yield, but I didn't and my yield was comparable good).
Water phase was then extracted with 2 x 20 ml of ether (to remove e.g. unreacted heptanal and possible organic sideproducts). The upper ether phases
discarded and bottom water phase was kept.
Water solution of sodium 3-nonenoate was returned into the separatory funnel. Testing with pH paper showed strongly alkaline reaction pH above 12. If
there were no significant loses of the product in the previous extraction step, it should prove that the product is not mainly dicarboxylic acid and
that its decarboxylation occurred.
Now there is necessary convert sodium salt back into free acid which requires 120 mmol of chilled HCl = 8,5 ml of 35% HCl plus some excess to
neutralize the small excess of NaOH.
120 mmol of HCl = 8,5 ml of 35% HCl.
To the separatory funnel was added cold 11 ml 35% HCl dropwise while stirring (slight excess due to previous slight excess of NaOH). Exothermic! 9 ml
35% HCl was not enough - tested with pH paper (just week acidic pH and still not strongly acidic), but after 11 ml HCl the pH paper showed highly
acidic result. There was some ether present (estimated 10-15 ml) - slightly larger volume of the upper organic layer observed than a volume of only
sole 3-nonenoic acid. After cooled down 10 ml more ether was added, shaken and separated. The upper organic phase containing 3-nonenoic acid was kept
and bottom water phase was extracted with 2 x 20 ml ether. The ether extracts were combined together and washed with 50 ml of concentrated NaCl
solution.
Then the organic layer was transferred into 100 ml Erlenmeyer flask and dried with anhydrous Na2SO4.
Diethylether was distilled out.
16,9 g of pale yellow product obtained (108 mmol = 90 %, M = 156.22 g/mol)
COOL !!! This is more than the weight of the reactant heptanal also its scent is
completely different from the scent of the heptanal and very close to the scent of nonanoic acid.
photos:
reagents
reactants mixed in RBF
small bubbling already at 81 C
 
T increases
 
at 103 C white fumes observed in the flask and also at the top of condenser
   
After half an hour the fumes only in the RBF and not in the condenser anymore
 
After 1 hour of reflux around 105 C the reaction was done.
After addition of diethylether and acidification with HCl. Upper organic layer kept. Bottom water phase discarded after checking that its pH is
strongly acidic.
After neutralization with NaOH. Bottom water phase containing sodium 3-nonenoate kept (pH strongly alkaline due to small excess of NaOH) and upper
ether phase discarded (unreacted heptanal + organic sideproducts and so on).
After converting sodium salt to free acid using HCl. Upper ether layer kept and bottom water phase discarded (pH of water phase strongly acidic on
universal indicator paper, using small excess of HCl). Note this photo is soon after vigorous shaking before both phases separated sharply.
Washing ether extract with saturated water solution of NaCl to reduce water present in the ether. Upper ether layer kept and bottom water phase
discarded.
drying with Na2SO4
distilling out ether
3-nonenoic acid, the desired product
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Fery
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gamma nonalactone
Please use method by Klute (strongly acidic resing catalyst + reflux in heptane).
If you don't mind low yield, messy long lasting workup and your goal is preferably at least know the scent of the lactone - continue further reading.
I found some very limited info here:
https://prezi.com/5yxmrydde1-2/synthesis-of-gamma-nonalacton...
| Quote: | Heptanal (6.70mL), malonic acid (5.20g), triethylamine (10.0mL) in a flask, heat
Separate with ethyl ether (30mL) and cold concentrated HCl (8mL/25g ice)
Wash with water, dry
Add 85% H2SO4 (10.0mL), heat for an hour
Pipette into 20g sodium bicarbonate in 90mL water
Separate with ethyl ether, wash with water, dstill
Oily brown liquid
Smelled very strongly of coconut
88% yield
SDBS IR/NMR for CAS: 104-61-0
Panda, H. Perfumes and Flavors Technology Handbook; Asia Pacific Business Press Inc.: Kamla-Nagar, 2010
Wade, L.G. Organic Chemistry, 8th Ed.; Person: Upper Saddle River, 2013 |
84% H2SO4 was prepared this way:
4,0 g H2O + 30,0 g 95% H2SO4 (28,5 g 100% H2SO4) = 28,5/34 = 84%
To a beaker with 4,0 g H2O was dropwise added 30,0 g 95% H2SO4 while stirring and cooling the beaker on ice-water bath (extremely exothermic !!!)
To 16,9 g of 3-nonenoic acid in 100 ml RBF was added dropwise while stirring the above 34 g of cooled 84% H2SO4. The both liquids were completely
miscible (seems H2SO4 immediately adds to the C=C double bond ?). Stir bar added and the reaction was refluxed while magnetically stirring (maybe the
stirring is unnecessary, but I have good experience in preventing bumping using magnetic stirring). I suppose the reflux condensate is an azeotrope of
H2O + 4-pentyl-gamma-butyrolactone as there were a mixture of water with immiscible liquid visible in a form of tiny white droplets in the condenser.
The reaction was refluxed for 1 hour (maybe shorter time or lower temperature are enough and better ???). External infrared thermometer showed T
inside 98-107 C (the accuracy of the thermoprobe is very likely something like +-5 C). Rancid gas evolved (shorter chain organic acids or HCl from
remainders of NaCl ???) so an adapter was inserted into the top of the condenser to which a hose was connected and its open end was led outside of
lab.
30 g 95% H2SO4 (M = 98 g/mol) means (30 * 0,95) / 98 = 0,29 mol H2SO4.
NaHCO3 molar mass 84 g/mol. 0,58 mol NaHCO3 = 48,7 g.
50g NaHCO3 (0,60 mol, slight excess) + 250 ml H2O were mixed in 500 ml Erlenmeyer + glass stirring rod inserted. NaHCO3 is not fully soluble in the
above amount of water but it is going to be reacted with H2SO4. The environment needs to be as close to neutral as possible. More alkaline as well
more acidic environment would hydrolyze the lactone.
To the Erlenmeyer flask was dropwise added in portions while stirring the reaction mixture (cca not more than 0,5 ml evey time). The process is very
slow and messy due to bubbling+foaming and perhaps some soap like sodium salt of organic acid present. At the end also RBF was rinsed with the
contenet from the Erlenmayer flask and the content was returned to the Erlenmeyer flask (but a lot of tar stayed adhering to RBF). More than 3 hours
of workup was required and the process was very messy as the content in the RBF was very thick, contained a lot of tar. Dirtyness and slowness is
comparable with workup of phenol nitration. Use Klute method rather (clean, fast, high yielding).
The content was transferred into 500 ml separatory funnel and the product extracted with 3 x 30 ml of diethyl ether.
Ether extracts were combined and washed with 50 ml of saturated water solution of NaCl.
Organic layer dried with Na2SO4.
Ether distilled out.
A little of very impure product was obtained which was unsuitable for vacuum distillation. Steam distillation was rather tried to test whether the
lactone does not easily hydrolyze. Clevenger apparatus was used. Do not just steam distill without such apparatus. The solubility of lactone in water
is slightly more than 1 g per liter. You need Clevenger apparatus so the water returns back into the distilling flask.
A little of red-brown product obtained.
Its scent was noticeable already during workout. I perceived it like 50% coconut + 50% fruit (closest to peach). It is not pure coconut but also a lot
of fruit (mostly peach). If you would like pure peach, start not from heptanal (intermediate 3-nonenoic acid) but from octanal (intermediate
3-decenoic acid and product gamma decalactone) - read the following post containing messy compilation of various useful data gathered from internet.
Heptanal could be obtained by distilling castor oil with colofony pine resin at elevated temperature while applying water pump vacuum.
photos
mixed 3-nonenoic acid + 84% H2SO4
heating + stirring the reaction mixture already darkened
the reaction much more darkened during time
there were small droplets of immiscible organic compound visible in the condenser (careful eye required, do not confuse with plenty of air bubbles in
cooling liquid)
 
completely dark black and tarry mixture obtained
long lasting and messy neutralization with NaHCO3
ether extraction, the layers almost impossible to distinguish, a small hand lamp helped, this is the first extraction, the second extraction is
slightly better visible and the third extraction already well visible, here only the first extraction before and after draining out some bottom water
phase
 
ether extractions combined and dried with Na2SO4
ether distilled out
crude product
purification by steam distillation and Clevenger apparatus
[Edited on 28-8-2024 by Fery]
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Fery
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compilation of various info gathered from internet
https://www.chemspider.com/Chemical-Structure.96738.html
Non-3-enoic acid
Density 0.9±0.1 g/cm³
Boiling point 261.4±9.0 °C at 760 mmHg
https://pubchem.ncbi.nlm.nih.gov/compound/Gamma-nonalactone
Gamma-nonalactone
BP: 134 °C at 12 mm Hg
Haynes, W.M. (ed.). CRC Handbook of Chemistry and Physics. 95th Edition. CRC Press LLC, Boca Raton: FL 2014-2015, p. 3-186
Hazardous Substances Data Bank (HSDB)
The boiling point at 1.7 kPa is 136 °C.
Fahlbusch et al; Flavors and Fragrances. Ullmann's Encyclopedia of Industrial Chemistry. 7th ed. (1999-2015). New York, NY: John Wiley & Sons.
Online Posting Date: January 15, 2003.
http://www.thegoodscentscompany.com/data/rw1000531.html
gamma-nonalactone (aldehyde C-18 (so-called))
nonano-1,4-lactone
5-pentyloxolan-2-one
Specific Gravity: 0.95800 to 0.96500 @ 25.00 °C.
Specific Gravity: 0.96000 to 0.97000 @ 20.00 °C.
Refractive Index: 1.44600 to 1.44900 @ 20.00 °C.
Boiling Point: 243.00 °C. @ 760.00 mm Hg
Boiling Point: 121.00 to 122.00 °C. @ 6.00 mm Hg
Soluble in water, 1201 mg/L @ 25 °C (est)
Odor Type: coconut creamy waxy sweet buttery oily
https://www.scentree.co/en/Gamma-Nonalactone.html
Stability: Lactones tend to polymerize through time, making them more viscous and leading to a phase shift in alcohol.
https://www2.chem.wisc.edu/areas/clc/uw-only/organic/345/FC/...
Acid Catalyzed Hydrolysis of Lactones
This reaction is the reverse of the Fisher esterification. It is under thermodynamic control but the use of a large excess of water pushes the
equilibrium toward the hydrolysis product. The reaction is slower with five and sixmembered ring lactones, smaller ring lactones hydrolyze faster.
https://en.wikipedia.org/wiki/Lactone
Heating a lactone with a base (sodium hydroxide) will hydrolyse the lactone to its parent compound, the straight chained bifunctional compound. Like
straight-chained esters, the hydrolysis-condensation reaction of lactones is a reversible reaction, with an equilibrium. However, the equilibrium
constant of the hydrolysis reaction of the lactone is lower than that of the straight-chained ester i.e. the products (hydroxyacids) are less favored
in the case of the lactones. This is because although the enthalpies of the hydrolysis of esters and lactones are about the same, the entropy of the
hydrolysis of lactones is less than the entropy of straight-chained esters. Straight-chained esters give two products upon hydrolysis, making the
entropy change more favorable than in the case of lactones which gives only a single product.
Some examples are γ-decalactone (4-decanolide), which has a characteristic peach flavor;[18] δ-decalactone (5-decanolide), which has a creamy
coconut/peach flavour; γ-dodecalactone (4-dodecanolide), which also has a coconut/fruity flavor,[18] a description which also fits γ-octalactone
(4-octanolide),[19] although it also has a herbaceous character;[18] γ-nonalactone, which has an intense coconut flavor of this series, despite not
occurring in coconut,[20] and γ-undecalactone.
https://en.wikipedia.org/wiki/%CE%93-decalactone
γ-Decalactone
It has an intense peach flavour
https://www.sciencemadness.org/whisper/viewthread.php?tid=11...
https://www.tesble.com/10.1080/00304948.2013.743759
https://www.tesble.com/10.1016/j.apcata.2007.09.013
https://sci-hub.53yu.com/10.1002/adsc.200303234
http://www.thegoodscentscompany.com/data/rw1000531.html
Specific Gravity: 0.95800 to 0.96500 @ 25.00 °C.
Boiling Point: 243.00 °C. @ 760.00 mm Hg
Boiling Point: 121.00 to 122.00 °C. @ 6.00 mm Hg
https://prezi.com/5yxmrydde1-2/synthesis-of-gamma-nonalacton...
Heptanal (6.70mL), malonic acid (5.20g), triethylamine (10.0mL) in a flask, heat
Separate with ethyl ether (30mL) and cold concentrated HCl (8mL/25g ice)
Wash with water, dry
Add 85% H2SO4 (10.0mL), heat for an hour
Pipette into 20g sodium bicarbonate in 90mL water
Separate with ethyl ether, wash with water, dstill
Oily brown liquid
Smelled very strongly of coconut
88% yield
SDBS IR/NMR for CAS: 104-61-0
Panda, H. Perfumes and Flavors Technology Handbook; Asia Pacific Business Press Inc.: Kamla-Nagar, 2010
Wade, L.G. Organic Chemistry, 8th Ed.; Person: Upper Saddle River, 2013
synthesis from hexanol and methyl metacrylate:
Attachment: 00304948.2013.743759.pdf (108kB)
This file has been downloaded 65 times
synthesis via Baeyer-Villiger oxidation on tin catalyst (Sn-beta + H2O2)
Attachment: adsc.200303234.pdf (90kB)
This file has been downloaded 58 times
synthesis via strongly acidic resign catalysts (method used by Klute in the initial post)
Attachment: j.apcata.2007.09.013.pdf (295kB)
This file has been downloaded 61 times
[Edited on 28-8-2024 by Fery]
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