Your voice is incredibly relaxing

I love when even a successful chemist like yourself is not afraid to talk about their mistakes (and then pus safety). Great Job!!

your best video ever!!! can´t get enough.:-)

top notch stuff, as always! thanks :]

I have isolated bromine before using the reaction Ca(ClO)2 + 4NaBr + 2HCl --> 2Br2(l) + 4NaCl + Ca(OH)2. The reaction occurred rapidly, and the Bromine produced was in a very concentrated solution that i distilled to yield pure bromine. I was working outside as the fumes were very nasty, I will try to shoot a video of the reaction sometime.

Great video! Thanks for the info. I found it personally helpful.

Wow, good thing they confessed.

I tried the same thing at one point, and i too wound up with a brown liquid. I figured, no problem, just get it up around the Br boiling point (under 60C). I had the darn thing near 100 and it was just barely vaporizing. My plan was to send the gas into a tube immersed in dry ice/acetone (-79C) to get Br crystals. The result was just a fuming mess with no yield. I concluded the Br water doesn't like to separate as much as you would think it would. I'd still love to make some Br sometime.

to make bromine, you can distill a mixture of manganese dioxide, sulfuric acid, and sodium bromide. Nurdrage has a video about how to get manganese dioxide from batteries

This reminds me of a lab my AP Chemistry class did. We were doing a synthesis of Aspirin, and something went very wrong for another one of the lab groups, and they ended up with only 3% yield. I know every chemist has had his or her fair share of error.

@FortNikitaBullion Oh, yes - I was accidentally considering bromide a cation rather than an anion. Thanks for pointing that out!!

When I was a kid, I used to think red food coloring was bromine. They look so similar!

That is interesting. Do the varying outcomes depend on obvious variables such as temperature, purity, proper mixing etc or is it genuinely just chance

Thanks!

@98JMA To go from bromide ion to elemental bromine, you would have to lose an electron. It's oxidation.

@TheHomeScientist Yes, that's one thing to worry about : a water bromine solution. Probably the best method is with high conc HCl or H2SO4 and NaBr.

Just wondering, is the aerial concentration of bromine from this reaction dangerous; chronically or acutely?

@TheHomeScientist you would have to use Hydrofluoric acid also right?

Can you do this for chlorine as well, or is it just bromine and iodine?

@TheHomeScientist what kind of things are you working on?

Heat the bromine water to the boiling point of water and condense the bromine. Now you will have high purity bromine!

What about electrolysis of a NaBr solution. It should form Br droplets at the anode.

Thanks! Do you have any recommendations? Suppliers that have reasonable prices and good value? Thanks again!

Failure is always an option in science! You could use electrolysis to do this with better yield, but that raises a question: I have titanium cathodes (my dad is an engineer), but where would you recommend I find cheap platinum or platinum-plated anodes? Graphite rods from a lantern battery work alright, but the particle contamination can be a real pain. Thanks!

I think the problem is too much water. You dissolved the sodium bromide in water, added hydrochloric acid, which is typically 64% water, and drugstore hydrogen peroxide which is 97% water. Also, bromine is a liquid, not like solid iodine, so the bromine was dissolved in the water.

How about auto-oxidation of hypoclorite to chlorite? no chlorine dioxide needed.....

So since this is bromine water, is this acidic at all?

I think the problem was the peroxide. The bromine probably reacts with it to form bromates, which are also colorless. Have you tried the reaction with bleach instead?

@isaisai9192 the bromine is quite volatile and slowly leaves the soln.

How about solve the bromine out of solution using benzene and isolating the bromine by destillation? Or maybe directly use the benzeneous bromine-solution for brominating the benzene by adding a lewis-acid?

How do i make hydrocloric acid?

@quantumdude it is expensive and why not use chlorate or something. sure, you can order it from like strem chemicals but that is for companies only.

Would you consider showing how to make sodium chlorite from sodium chloride?

is this nurdrage?

I always preferred a reaction surplus

Well.... When heated, sodium (or caclium) hypcolorite decomposes oxidizing another hpyoclorite molecule, to form chlorite. Further decomposition makes it up to chlorate and even perchlorate. This can be done on a water solution safely if admixed with a stronger oxidizer than chlorate, like permanganate or persulphate. peroxide doesnt work. I tried it.

Hope it's not really too late to say this but, bubbling chlorine gas into a saturated or supersaturated solution of NaBr will produce bromine. After much testing I found that a VERY excess amount of chlorine is needed to get good results. With 12g NaBr I made 5ml of bromine and 20ml of strong bromine water. And of course for good chlorine just use HCl and pool chlorinator tablets.

the most best way to make bromine is to bubble chlorine gas into a sodium or potassium bromide solution and than destill the bromine water^^ you would get almost 100% sodium or potassium bromide reacted.

Did you figure what went wrong? I think there was too much water.

Nice video! I imagine this reaction would work with lithium bromide as well? Any ideas why yours didn't turn out as you expected? I'm trying to find a good way to get elemental bromine for my element collection.

@SodiumInteresting

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Electrolysis of sodium bromide and sodium bisulphate. I made a br element sample yesterday

you said you can oxidise the sodium bromide solution with laundry bleach. you mean sodium hypochlorite?

No, as he said the bromine produces a lot of gases. By a lot he means a ton. Elemental bromine will completely evaporate if left out in a few minutes. Heating it will cause it to vaporize faster.

why not distill it?

2Br- --> Br2 + 2e- H2O2 + 2H+ + 2e- --> 2H2O Without a stoichiometric amount of acid, the reaction will not go to completion. It does not appear that you used enough HCl from the video. Others have had near theoretical yields of bromine when using a slight excess of acid.

Humm... Too bad it didnt work. I would like to try to oxidize halogens, like bromine to hypobromite.

I know it should make no practical difference really, but in your preparation I would not use HCl, preferring H2SO4 as then there can be no funny halogen interactions (although it should not matter anyway, as any Cl2 produced should in turn oxidise your bromide to bromine). You mention in one of your replies that next time you would use electrolysis - what electrode would you favour for the production of bromine?

Thanks for the info - I have platinum wire, but even this is not cheap :(

Aren't the bromide ions REDUCED to elemental bromine rather than oxidized?? 'OIL RIG' - Oxidation is Loss, Reduction is Gain.

how about dissolving the NaBr in H2O2 and then adding H2SO4? thats how I made it on a large scale, just keep it cold...

i did this with potassium bromide and potassium permanganate as the oxidizer. The reaction went almost too fast for my taste (it became QUITE warm and lots of bromine evaporated... it was really nasty o0)

exothermic?

He died a couple years ago, apparently. RIP.

Can you bear my children?