Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
Separation of Xylenes using Formic Acid Azeotrope
Xylenes commonly are found in the hardware store sold as Xylol. It comes as a mixture of the o, m, and p isomers. Sometimes it is necessary to
separate these isomers which can be hard.
By adding formic acid to the mixture an azeotrope forms between it and the m-xylene that boils at ~97C. M-xylene is not used for much so it can be
kept in with the formic acid. The rest of the mixture then boils off at ~140C as a combination of o-xylene and p-xylene. The boiling points of these
are similar but their freezing points aren't. P-xylene freezes at 13C and can be extracted. O-xylene freezes at much lower temperatures and will
remain a liquid. From there you have separated isomers.
I have not actually validated this procedure. Please tell me if there is something wrong with this. If nothing is wrong then I recommend going through
the procedure a few times especially the crystallization of p-xylene to obtain a purer product.
[Edit] Clarified title
[Edited on 9-28-2016 by zts16]
|
|
|
Sulaiman
International Hazard
Posts: 3721
Registered: 8-2-2015
Location: 3rd rock from the sun
Member Is Offline
|
|
just a noob thinking ....
could the m-xylene be separated from o-xylene and/or p=xylene by freezing ?
if so the overall setup would be simpler.
Doing the formic acid separation after separation by freezing would give at least one isomer free of formic acid contamination.
CAUTION : Hobby Chemist, not Professional or even Amateur
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
Quote: Originally posted by Sulaiman  | just a noob thinking ....
could the m-xylene be separated from o-xylene and/or p=xylene by freezing ?
if so the overall setup would be simpler.
Doing the formic acid separation after separation by freezing would give at least one isomer free of formic acid contamination.
|
Technically it could as the freezing point of m-xylene is -25C while o-xylene is -45C but the mixture of all the Xylenes has a freezing point of ~-44C
so I think by removing the m-xylene first the temperature difference between the FP of o and p xylene is enough to have the p-xylene freeze separately
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
| Quote: Originally posted by Sulaiman | just a noob thinking ....
could the m-xylene be separated from o-xylene and/or p=xylene by freezing ?
if so the overall setup would be simpler.
Doing the formic acid separation after separation by freezing would give at least one isomer free of formic acid contamination.
|
Technically it could as the freezing point of m-xylene is -25C while o-xylene is -45C but the mixture of all the Xylenes has a freezing point of ~-44C
so I think by removing the m-xylene first the temperature difference between the FP of o and p xylene is enough to have the p-xylene freeze separately
|
|
|
Texium
Administrator
Posts: 4618
Registered: 11-1-2014
Location: Salt Lake City
Member Is Offline
Mood: PhD candidate!
|
|
To me the procedure seems plausible, and I would be interested in trying it sometime but I have a lot on my plate right now so it would have to go to
the back burner along with many other procedures of interest. Why don't you try it out, Meltonium? Keep in mind too that commercial xylene may contain
up to 20% ethylbenzene, which may complicate things. It's worth a try though.
Formic acid could easily be removed from any xylene isomer by extracting with a dilute sodium hydroxide solution and then drying/redistilling the
xylene.
By the way, I changed the title of the thread because separation of xylenes has been discussed many times here before, but not by this specific method
as far as I can tell.
[Edited on 9-28-2016 by zts16]
|
|
|
Texium
|
Thread Moved
28-9-2016 at 08:43 |
Maroboduus
Hazard to Others
Posts: 257
Registered: 14-9-2016
Location: 26 Ancho Street
Member Is Offline
Mood: vacant
|
|
Water forms a 94.5C boiling azeotrope with Meta Xylene as well, but that doesn't mean it is useful for separation. Still it would be cheaper to try
than formic acid.
I suspect that there's just more azeotrope info for the meta than for the other isomers, and that it'll be a big mess when you actually try distilling
the isomers with all sorts of azeotropes of the three isomers coming over.
I sure hope not, this would be really handy. I am skeptical however.
Same with the freezing thing. Freezing out to separate similar substances can be tricky because of eutectics and all that jazz.
And bear in mind that the freezing point is for the pure compound without solvents involved. Sucrose freezes at 186C, but you can't freeze the sucrose
out of an aqueous solution by cooling it below 186C.
In my admittedly limited experience of purification by freezing, I have found that mixtures of similar components have a tendency to just sort of gel
and slowly solidify. Sometimes you get better results if there's some solvent in there of a dis-similar character to the components you're trying to
separate.
[Edited on 28-9-2016 by Maroboduus]
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
M-xylene also forms an azeotrope with acetic acid at around 117C and afterward it can be removed by water washings because Xylenes are practically
insoluble in water. As for the azeotrope meta has with water, I didn't find that. Although my source is the azeotrope tables from Wikipedia. If there
is ethylbenzene contamination, it could be removed through water washings because it is very slightly soluble.
|
|
|
Texium
Administrator
Posts: 4618
Registered: 11-1-2014
Location: Salt Lake City
Member Is Offline
Mood: PhD candidate!
|
|
| Quote: Originally posted by Maroboduus | | In my admittedly limited experience of purification by freezing, I have found that mixtures of similar components have a tendency to just sort of gel
and slowly solidify. Sometimes you get better results if there's some solvent in there of a dis-similar character to the components you're trying to
separate. |
While that is often true, sometimes it is not. For instance, p-nitrotoluene and o-nitrotoluene are
separable by freezing out the p-nitrotoluene. I don't know if it would work in this situation, but removing the m-xylene, which is supposed to be
about 40% of commercial xylene, should increase the likelihood that it will.
|
|
|
Boffis
International Hazard
Posts: 1879
Registered: 1-5-2011
Member Is Offline
Mood: No Mood
|
|
Hi Meltonium, do you have a reference for this procedure? It sounds potentially very interesting but I wonder if the azeotrope with m-xylene only
forms a simple system in the absence of the o and p-isomers so that with a mixture of the 3 isomers you get a "common" azoetrope. It would be very
useful if it worked from the mixed isomer commercial xylol though  .
Also what strength is your formic acid; 99% or the standard 85% industrial grade?
Interestingly I have been experimenting recently with the azeotropic distillation of 85% formic in an attempt to upgrade it to >97% so I can use it
directly to product formate esters. What is interesting is that instead of the water distilling over with the solvent the formic acid distils over in
a slightly enriched form; 85 up to 93% in one distillation with petroleum ether (80-100 C boiling range). I found that the higher strength formic acid
was not misible with the petroleum and so could be separated in a separating funnel. So if the m isomer distils off with the formic acid it should be
easily separated.
Like you say the o and p isomers should be fairly readily separated by the freezing method. I have a reference to this somewhere amongst my papers.
Another method of removing the m isomer is by treating with sulphuric acid. This works on the principle that only the m-isomer reacts with sulphuric
acid of <85% and since water is generated by the sulphonation of xylene the liberated water soon limits sulphonation to solely the m-isomer, the o
and p enriched residue can then be fractionated or frozen to separate thje remaining isomers. There are several refs to this procedure, I seem to
remember that the original lead was from Ullmans encyclopedia.
|
|
|
Maroboduus
Hazard to Others
Posts: 257
Registered: 14-9-2016
Location: 26 Ancho Street
Member Is Offline
Mood: vacant
|
|
| Quote: Originally posted by zts16 | | Quote: Originally posted by Maroboduus | | In my admittedly limited experience of purification by freezing, I have found that mixtures of similar components have a tendency to just sort of gel
and slowly solidify. Sometimes you get better results if there's some solvent in there of a dis-similar character to the components you're trying to
separate. |
While that is often true, sometimes it is not. For instance, p-nitrotoluene and o-nitrotoluene are
separable by freezing out the p-nitrotoluene. I don't know if it would work in this situation, but removing the m-xylene, which is supposed to be
about 40% of commercial xylene, should increase the likelihood that it will. |
The polarity of a nitro group may make this more possible. My experiences are largely with essential oils which have less dramatic polarity, and more
complex structures (lots of alkyl and phenol ether side chains).
I can see where, given the different resonance structures contributing to the character of the para isomer, it would be quite different from the other
xylene isomers in charge distribution(not just it's symmetry, but more charge on the methyls), but I'd still bet against getting a good separation by
cooling. But I do think it's worth trying.
EDIT: turns out there are plenty of patents that involve crystalizing out the Para isomer at -30C to -60C. These are often patents for detailed
processes to separate the isomers which involve fractionating and freezing.
[Edited on 28-9-2016 by Maroboduus]
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
| Quote: Originally posted by Boffis | Hi Meltonium, do you have a reference for this procedure? It sounds potentially very interesting but I wonder if the azeotrope with m-xylene only
forms a simple system in the absence of the o and p-isomers so that with a mixture of the 3 isomers you get a "common" azoetrope. It would be very
useful if it worked from the mixed isomer commercial xylol though .
Also what strength is your formic acid; 99% or the standard 85% industrial grade?
|
I have no reference other than myself and Wikipedia azeotrope tables. XD
As for the formic acid, I have none at the moment but I'd imagine that it would need to be near pure because the azeotrope it forms with water has a
lower BP than the azeotrope formed with the m-xylene.
When I get around to doing this (hopefully this weekend if time allows) I will probably use glacial acetic acid instead of formic acid and let yall
know how it goes.
|
|
|
Texium
Administrator
Posts: 4618
Registered: 11-1-2014
Location: Salt Lake City
Member Is Offline
Mood: PhD candidate!
|
|
I have 95% formic acid, so I can try it out some time and make a video of the procedure, but currently I have a few other projects that I'm working on
that I'd like to complete first. If this thread ends up getting buried without anyone trying it, I will make sure to revisit it and post my results.
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
I've preformed the separation using acetic acid and below is my written work:
Separation of Xylenes
Objective: To separate xylene isomers using an acetic acid azeotrope
Materials:
- 200mL Xylenes
- 100mL Glacial Acetic Acid
- Distilled Water
Procedure:
1) Add the Acetic Acid and Xylenes to a 500mL RBF
2) Mix for ~10 minutes
3) Fractionally distill over at 117C
4) Wash distillate with water to obtain Acetic Acid and dry over a drying agent
~
5) Take remaining fractions that distill over 120C
6) Place fractions in a freezer for ~1-2hours
7) Decant solution and collect crystals in separate container
8) Repeat for purer product
Observations/Analysis:
- Upon addition of the Acetic Acid, the solution became cloudy. This is likely from a suspension of undissolved acetic acid or from water present in
the acid.
- Upon heating, the solution underwent significant thermal expansion bringing it close to overfilling the RBF
- The first fraction started coming over at ~95C; the distillate separated into two layers, one cloudy and one clear. They both seemed to be growing
at the same rate. As more distillate collects, the top layer seems to be clearing up and the bottom layer becoming more cloudy.
- A new fraction was collected when the temperature reached 111C. This fraction is clear and smells of xylene. The temperature stabilized at 115C for
most of this fraction.
- A third fraction was collected when the temperature rose to 120C
- To prevent possible photo-degradation of the separated xylenes (as claimed in another post under phthalic anhydride from o-xylene) the lights were
dimmed.
- A fourth fraction was collected when the temperature rose to 132C. This fraction stabilized at 140C into the fifth fraction.
- Distillation was stopped at the start of the fifth fraction; most of the liquid in the RBF had been distilled.
- Left in the RBF is a dirty, champagne colored liquid.
- Fractions 3-5 were transferred to a 250mL beaker, covered with Saran wrap, and placed in the freezer (-14C). Thin flaky crystals formed in the
bottom of the beaker after ~1 hour.
Because the azeotrope of acetic acid and meta-xylene boils at 117C, it is reasonable to assume that fraction two is almost all acetic acid
and m-xylene. Fractions 3-5 are most definitely a mixture of xylenes, ortho being most prominent after the p-xylene crystals are removed. Due to the
lack of abundance of p-xylene crystals, it seems like the ortho and meta isomers are most prevalent in the unpurified xylene. There is likely ethyl
benzene mixed with this o-xylene because the MSDS for the commercial Xylol used suggested 0-30% ethyl benzene. The ethyl benzene could be removed
through many, many water washings as it is more soluble than o-xylene. As for the first fraction, I suspect that the cloudyness is from a suspension
of water droplets that may have been present in the RBF, collection beaker, or the acetic acid.
About 5-10mL of p-xylene was collected after the crystals were remelted.
[Edited on 2-10-2016 by Meltonium]
|
|
|
Metacelsus
International Hazard
Posts: 2539
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
Those are definitely some interesting results. What kind of distillation column were you using?
Also, is there any good way to check the proportions of xylenes in your fractions? (GC would be obviously the best, but that's probably not
available.) Could you do something with the density or refractive index?
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
| Quote: Originally posted by Metacelsus | Those are definitely some interesting results. What kind of distillation column were you using?
Also, is there any good way to check the proportions of xylenes in your fractions? (GC would be obviously the best, but that's probably not
available.) Could you do something with the density or refractive index? |
I used a 400mm Vigreux column connected to a 400mm Leibig condenser although a 300 leibig would've done just fine.
I was thinking about how to check the proportions, but I don't think density is the best way for me. I don't have a scale or a graduated cylinder with
enough decimal places to differentiate between the isomers since they have pretty similar densities. I didn't think to look at the refractive index,
but that's a good thought and I'm open to any more suggestions.
- -
Turns out the refractive indexes are pretty much the same too. 
[Edited on 2-10-2016 by Meltonium]
|
|
|
Metacelsus
International Hazard
Posts: 2539
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
Maybe you could oxidize a sample of them to the dicarboxylic acids, and analyze those by TLC? They'll probably be visible as separate spots.
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
| Quote: Originally posted by Metacelsus | | Maybe you could oxidize a sample of them to the dicarboxylic acids, and analyze those by TLC? They'll probably be visible as separate spots.
|
Good idea! I'll try that just as soon as I get this crud out of my 100mL RBF
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
I'm a little confused about the oxidation of these isomers and the contaminants. Organic chemistry is not my fortay, but I know the xylene isomers
will be oxidized to their phthalic acids, but my fraction that I think contains mostly ortho-xylene is likely to have ethyl benzene as well. I do not
know what ethyl benzene will oxidize to. Can yall help me?
P.S. I plan to use potassium permanganate to oxidize my samples if that helps any
|
|
|
Metacelsus
International Hazard
Posts: 2539
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
Ethylbenzene would be oxidized to benzoic acid by permanganate.
|
|
|
Maroboduus
Hazard to Others
Posts: 257
Registered: 14-9-2016
Location: 26 Ancho Street
Member Is Offline
Mood: vacant
|
|
So any idea what that first fraction was?
EDIT: And what were the volumes of the fractions?
[Edited on 12-10-2016 by Maroboduus]
|
|
|
byko3y
National Hazard
Posts: 721
Registered: 16-3-2015
Member Is Offline
Mood: dooM
|
|
You need approx 70 theoretical plates to efficiently separate o-xylene and m-xylene (vs 100 for pure xylenes). I have no idea what heppens to other
isomers. Formic acid is one of the best azeotropic entrainer for xylene isomer separation, yet the difference is not as large as you might wish.
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
Today I attempted to oxidize my ortho fraction and convert it to phthalic anhydride and use that to indicate the % of ortho really in the fraction. ~3
hours into the oxidation through KMnO4 I mistakenly grabbed a beaker labeled for HCl instead of distilled water and added that to the reaction.
Needless to say, I scrapped what was left and won't be attempting it again any time soon. (It is very messy) So I'll probably send my fraction to a
lab for analysis. When the results come, I'll scan the document and post it here.
On another note, I am very certain that the first fraction I collected was un-azeotroped acetic acid along with low-boiling organically with suspended
water droplets.
|
|
|
Meltonium
Hazard to Self
Posts: 97
Registered: 23-9-2016
Location: Home in pajamas
Member Is Offline
Mood: Fluorinated
|
|
Previously, it was unknown to me that there was an azeotrope between ethyl benzene and water, as well as an azeotrope between m-xylene and water; both
boil at 92C according to my source. The first fraction likely then was water azeotroped with the ethyl benzene or some m-xylene and when it condensed
and cooled the liquids separated out.
Knowing this, I can now separate the ethyl benzene from my o-xylene fraction using the water azeotrope. Ethyl benzene is assumed to be the major
contaminant of the o-xylene fraction.
On another note, both the m-xylene and the ethyl benzene can be separated from the original mixture using this water azeotrope. The BP is lower than
that of the acetic acid azeotrope I used, therefore; the fractional distillation is likely to yield a purer product.
I will try the water separation method and post the results below.
Results
I used ~500mL of Xylol and from that ~350mL came over at 92C with the water added.
The still head then climbed to 100C briefly and progressed until 135C where it stabilized and slowly climbed.
It may be that all of the xylene isomers have an azeotrope with water and the azeotrope tables I use do not list it..
[Edited on 21-11-2016 by Meltonium]
[Edited on 21-11-2016 by Meltonium]
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
