Sciencemadness Discussion Board
Not logged in [Login ]
Go To Bottom

Printable Version  
Author: Subject: Selectivity in ester transformation
Magelia
Harmless
*




Posts: 28
Registered: 26-10-2011
Member Is Offline

Mood: No Mood

[*] posted on 11-11-2011 at 11:08
Selectivity in ester transformation


Hi Colleagues,

I have this reaction (shown below) I need to perform, but I honestly have NO idea where to start.

The ester at the bottom left is converted into an OH group while the ester at the top right is kept intact.

I honestly have NO clue where to start. Could someone give me a small hint at where to start please? I don't want an answer, just a push in the right direction... or a direction really at this point :)

Thank you!

Conversion.png - 18kB
View user's profile View All Posts By User
bahamuth
National Hazard
****




Posts: 384
Registered: 3-11-2009
Location: Norway
Member Is Offline

Mood: Under stimulated

[*] posted on 11-11-2011 at 11:27


Easiest would probably be to use stoichiometry to saponify just one of the ester groups, release the saponified molecule with acid and separate them on a good column or on a HPLC.

Just a guess though..




Any sufficiently advanced technology is indistinguishable from magic.
View user's profile View All Posts By User
fledarmus
Hazard to Others
***




Posts: 187
Registered: 23-6-2011
Member Is Offline

Mood: No Mood

[*] posted on 11-11-2011 at 14:52


You might just try using mass effects to get it to work - stir it in methanol with a catalytic amount of sulfuric acid and possibly a drying agent. This would set up a transesterification equilibrium between your esters and any available alcohols. The ester on the bottom left would become methyl acetate and eliminate your sterol alcohol. There is such a large excess of methanol that the chances of your acetic acid forming a new ester with the sterol alcohol would be negligible.

The ester on the top right would also equilibrate, but since it is already the methyl ester, it will just keep reforming methyl ester with all the methanol. Again, the methanol is far in excess of the sterol alcohol, so you should get very little of any dimerization.
View user's profile View All Posts By User
smuv
International Hazard
*****




Posts: 842
Registered: 2-5-2007
Member Is Offline

Mood: Jingoistic

[*] posted on 12-11-2011 at 13:35


I agree with fledarmus. At first I thought it was a very difficult problem, but yes, it is as simple as methanol with catalytic acid. A convenient procedure is to add a catalytic quantity of acetyl chloride to methanol (forms HCl in situ) and then add your ester.





"Titanium tetrachloride…You sly temptress." --Walter Bishop
View user's profile View All Posts By User
Magelia
Harmless
*




Posts: 28
Registered: 26-10-2011
Member Is Offline

Mood: No Mood

[*] posted on 12-11-2011 at 16:42


Thanks a lot guys!

Things really can be very simple sometimes!
View user's profile View All Posts By User
ziqquratu
National Hazard
****




Posts: 385
Registered: 15-11-2002
Member Is Offline

Mood: No Mood

[*] posted on 14-11-2011 at 01:39


It should be pretty easy... I would just stir with K2CO3 in MeOH. The methyl ester that you want to keep intact will remain so, whilst the acetyl group will be transesterified to give the alcohol and methyl acetate.

Using even a weak base, such as K2CO3, should be faster and more efficient than using acid
View user's profile View All Posts By User
Nicodem
Super Moderator
*******




Posts: 4230
Registered: 28-12-2004
Member Is Offline

Mood: No Mood

[*] posted on 14-11-2011 at 13:22


I agree with ziqquratu that a base catalysed transesterification might be more efficient, but I would point out that the acetate ester function is an ester of a secondary alcohol and might thus not be so easy to transesterify with K2CO3/MeOH as an ester of a primary alcohol would be. It might require the use of K3PO4/MeOH or NaOMe/MeOH, which on turn can cause (partial) epimerization at the enolizable chiral carbon. No matter what kind of methanolysis you use, you would better check that no epimerization occurred. I'm sure it can be avoided though.



…there is a human touch of the cultist “believer” in every theorist that he must struggle against as being unworthy of the scientist. Some of the greatest men of science have publicly repudiated a theory which earlier they hotly defended. In this lies their scientific temper, not in the scientific defense of the theory. - Weston La Barre (Ghost Dance, 1972)

Read the The ScienceMadness Guidelines!
View user's profile View All Posts By User
smuv
International Hazard
*****




Posts: 842
Registered: 2-5-2007
Member Is Offline

Mood: Jingoistic

[*] posted on 14-11-2011 at 18:54


I think a literature search is the best bet... This system is pretty common.



"Titanium tetrachloride…You sly temptress." --Walter Bishop
View user's profile View All Posts By User

  Go To Top