myst32YT - 2010-11-10
In this video we will be making Ethyl Bromide (Bromoethane) for use in the future. Halocarbons in general are potentially dangerous alkylating agents. Bromides are better alkylating agents than chlorides, thus exposure to EtBr should be minimized. EtBr is classified by the State of California as carcinogenic and a reproductive toxin.
new mic? great vid btw
Awesome video! Your new setup is great!
Hi Nice video Thanks Id prefer to see the reaction taking place because I can see your setup and it would make it easier for me to do it as well. I don't have much experience so seeing it done would be nice Thanks
Hi Can you let the synthesis of bromoacetone in Channel?
Great video, what do you have planned for the ethyl bromide? I have everything I need to make it so I might depending on what the use is.
@myst32YT What was the yield?
did the synthesis myself, first yield was around 70%, i worked sloppy and didnt use exact measurements, expected yield for this reaction is close to 90%
I love the new video setup it is very comprehensive and i like your use of editing to show the distillation setup being assembled also i like the little person giving tips! aslo i would like to know, who did the artwork for the intro also who are they supposed to be ?
Thank you for publishing these videos!
Can this be achieved without sulfuric acid? Perhaps through some roundabout procedure or substitution?
In Europe sulphuric acid is HEAVILY regulated, but most other acids are easily available. The only way to get sulphuric acid is to buy car batteries and take it from there, which is rather expensive. The reason is mostly environmental, the ground water is an important issue here, but also that they want to prevent shake-and-bake labs which require H2SO4.
Heaan Lasai go to a junk yard for old batteries. Keep in mind an old discharged lead acid battery may be highly contaminated with various sufides and sulfites of lead and zinc.
he fast forwarded the shaking of the separatory funnel, I wonder if anyone has shaken it vigorously like that splattering the hell out of themselves
It is sometimes used, yes, to prepare the Gringard reagent ethylmagnesium bromide.
potassium bromide instead of NaBr?
@lexichronicle2 I did ethyl iodide by that same method (The Reaction between Aluminium, Iodine, Ethyl alcohol, and Water. By A. O. Jones and G. Melling Green doi:10.1039/JR9262902760). In the end i came up with iodoethane/ethanol-water boiling at 78-79°C in the Vigreaux (i tried it two times). For purification i used sodium and distilled it as mentioned in Purification of Laboratory Chemicals 4th ed, p. 216 Good Luck!
لو كان بالعربية لكان احسن
MȁȟẞǿŁ Ṕằȑɨš صح
MȁȟẞǿŁ Ṕằȑɨš ماهي المادة التي تتقطر بعد برومواثيل؟؟
No you may not blow up childrens hospital
is the ethylsulfate easier to protonate with hbr than ethanol? would you need sulphuric acid if you used very concentrated HBr?
Hi. Do you know a good method for making chloroethane?
By "for use in the future" do you mean to make ethyl magnesium bromide for use as a Grignard reagent?
What is your wash bottle??
I tried yodoacetate with elemental iodine just dropped by in glacial acetic acid.
Can phosphoric acid be used instead of sulfuric?
Nope. Don’t waste that H3PO4. Use drain cleaner which you can find some near 98% sulfuric acid via the msds
acid is only needed in catalytic amounts i think
The only question is: why sulfuric acid? Sulfuric acid, even if diluted partially oxidates bromide in bromine. May be phosphorous acid will be better.
Don't you think is dangerous to use your condeser without a clamp?
of course, its just methylbromide is a gas so capturing it is a little different... boiling point is 3C which isn't too low... so if you had an ice bath that could maintain 0 degrees or lower you could liquify it. dry ice would do the trick. best bet, have ether or some sort of organic solvent in the receiving flask so that it dissolves the gas. even still the yields won't be phenomenal.
If it is your intention to make ethyl hydrogen-sulfate, why use so much sulfuric acid? Is it because you are making the HBr in situ?
yes it can but, why not using concentrated HCl? it would be more pure and easier, any way it would be difficult to storage since it is a gas at room temperature
Chloroethane has a boiling point of 54 degrees Fahrenheit, which is interesting as this is only slightly below room temperature. Is there a similar method for making it?
@john black
Thanks.
@john black
I've always liked this kind of stuff, just wish I had more of the equipment to do cool science experiments.
@john black
It's not just that, the place where my family lives is not great on space and its a rental. But thanks for offering to help.
could I benzyl alochol insted of ethanol?
Do you know what the ethyl in the ethyl bromide stands for?
I think they are prety much different.... this is an ester of Hbr and ethanol and tribromoethane is more like a halogen-C compound. So it would need a whole different process.
He is doing legitimate amateur chemistry, nothing illegal here.
Purification of Ethyl Bromide The main impurities are usually EtOH and water, with both of which it forms azeotropes. Ethanol and unsaturated compounds can be removed by washing with conc H2SO4 until no further coloration is produced. The Ethyl bromide (CAS NO. 74-96-4) is then washed with water, aq Na2CO3, and water again, then dried with CaCl2, MgSO4 or CaH2, and distd. from P2O5.
multiple ways to do it. 1. dissolve a base in ethylacetate, it'll give you acetic acid mixed with ethanol. 2. mix diethyl ether with concentrated sulfuric acid, every 1 mole of ether will yield 2 moles of ethanol. or 3. a really cheap way of getting ethanol that always stands out... just fermentation and then distillation. but diethyl ether in sulfuric acid would be most efficient. mix the 2 and lead right into where this video starts out. in situ is always convenient...
in my state Gujarat (a western part of india) it is illegal to buy or get ethanol anyhow... i have diethyl ether, ethyl acetate, H2SO4 ~99% and potassium bromide... any way to make C2H5Br ? plz answer if possible nice video, though :)
Hydrolisis of ethyl acetate to get ethanol and acetic acid
It seems the theoretical yield should be 113gNaBr*(molNaBr/102.9gNaBr)(molBr/molNaBr)(molEtBr/molBr)(109gEtBr/molEtBr)(mlEtBr/1.46gEtBr) = 101.6mL, yet the final product volume looks to be quite more than that.. leads me to think there is quite a bit of ether contamination. What was the final volume?
@free8704 err sorry 140g is what I meant not 113g
@free8704 Any thoughts on purification?
For everybody asking if you can make ethyl chloride this way, probably not. Chloride isn't a good enough nucleophile and primary alcohols already react slowly with HBr and HI. Notice the excess H2SO4 which is used to force the reaction even with HBr, which is a stronger nucleophile. You might be able to use a mixture of zinc chloride and conc HCl (called Lucas reagent), however the high temp required would vaporize any EtCl formed and it would be hard to condense. So in short, no.
3:48 Should be "high vapor pressure" but that's not all that critical. For anyone repeating this, it would be wise to wash the organic phase with concentrated sulfuric acid (perhaps after the NaHCO3 wash to avoid bromine formation, and followed by another NaHCO3 wash) to remove any diethyl ether byproduct as diethyloxonium bisulfate. Also, it is very effective at removing residual ethanol, though in this procedure, the multiple water washes should remove it quite well.
Anita Gomez - 2011-07-27
3:49 High vapour pressure : )