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Author: Subject: Permanganates
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[*] posted on 15-2-2018 at 22:25
Permanganate from otc and an alkaline d cell w hypoCl


Quote: Originally posted by urenthesage  
Quote: Originally posted by MadHatter  
Given the recent CPSC(assholes) victory against FireFox, I'm sure that any convenient
method will be appreciated. KMnO4 sales by pyro suppliers are now limited to 1 LB a
year. There's still some OTC sources for now but we don't know how long that'll last.


So dont go to a pyro supplier. I got mine at a water depot, 5 lbs for about 45$. Farmers use it to take iron out of well water for cattle. They didnt even give me a second glance when I bought it.


I got a five pound bag from ace hardware. They don't have it in the store, at least in the state (USA, sorry everybody else not able to buy in ur country) of maryland. They put an order in for me and called about five days to a week later, it cost 39 us$ and needed my ID.
As for the calcium or sodium hypochlorite bleach I used with an old, likely dead d cell battery I had found. I didn't follow strict chemistry, but behaved like a cook, not measuring the hypochlorite bc I don't recall an exact measurement read. What ended up happening makes me concur with whoever said using hypochlorite is messy and difficult. I used about a half cup of standard bleach liquid (generic chlorox) and the crushed dark solid from the battery along with, again (and I DO know better, laziness was the lesson and why to avoid it) along with about a tablespoon of lye, which I found out may have been my problem. I boiled in measuring cup on hot plate, which took forever. Finally once it started it began to foam, bad. I took it off heat immediately and stirred like as if to make whipped cream or soufflé, and somehow succeeded in not spilling any. Thanks to whoever said that the majority of battery electrolyte is carbon bc my filter proved this. I used the top of a plastic water bottle, cut in half, as a funnel and a cotton ball stuffed in the mouth as a preliminary filter. No way was I using anything remotely dear to me for this project. What came thru was a pine green and aquatic blue homegenous transparent fluid, recognized as the manganate it was. However.... Pouring this same solution, this pretty green stuff which I meant to acidify promptly had turned into a dilute champagne/urine liquid, again transparent. Guessing it was mncl. I'll let u guys know how it goes using kno3, the battery innards but DRY, using the method employed by nurdrage, placing this mix in a container to be lit from underneath by torch. lowering ph with bicarbonate of potassium as sodium apparently eats the product before extraction. In hindsight I never have heard of sodium permanganate. Hmm.. I'll utfse. Thanks for your time and wisdom. I learn everyday from everyone on here.
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[*] posted on 4-3-2018 at 07:04


Quote: Originally posted by DerAlte  
Forget K peroxydisulphate unless you have it on the shelf. Even then, it's marginal due to H2O2 formation.

DerAlte


I know this thread is pretty old, but could somebody tell me if they have tried the S2O8 2- oxidation? I can't seem to find its potential in alkaline solution. I would really like to know as Na2S2O8 is really cheap in my country, and so are 6% SO2 solution (to reduce MnO2 to soluble MnSO4) and KOH.

[Edited on 4-3-2018 by CobaltChloride]
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[*] posted on 9-1-2019 at 13:00


Quote: Originally posted by Romain  
Update: The crystals that formed from the evaporated anolyte are highly impure as evidenced by the presence of white crystals and brown crud among the needles of KMnO4. The crystals were dissolved in a small amount of water and the solution was heated up to boiling. It was filtered while hot on a preheated filter funnel (to remove MnO2, again). The filtrate yielded 0.37 g of small (and pure) needles of KMnO4 upon cooling.

(More KMnO4 could be extracted from the anolyte, but this run was just to prove that the method works and I didn't try to be particularly efficient in the extraction.)

The product was tested by adding a few drops of conc. H2SO4 to a crystal to form Mn2O7 and the reaction with ethanol was as expected: it ignited!

After everyone argued about it for ten years, Romain walked up, casually solved the problem on the first try, posted a picture, and nobody even noticed.

I have to say, I find the use of KCl as the potassium source to be perplexing. Chloride is obviously susceptible to oxidation by permanganate. There are a couple of other possibilities, but the most obvious IMHO is potassium acetate.




[Edited on 04-20-1969 by clearly_not_atara]
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[*] posted on 20-2-2019 at 02:49
Properties of pure permanganic acid


It can be and has been made. Stable and easily isolated.
Published in Jacs, in 1969. Sadly, only first page is visible. Has anyone reached the next pages?
https://pubs.acs.org/doi/abs/10.1021/ja01050a058
To summarize the procedure:
  1. Produced pure dilute permanganic acid from stoichiometric amounts of dilute Ba(MnO4)2 and dilute H2SO4, and centrifugating the BaSO4 precipitate - about 0,3 M (3,6 %) permanganic acid
  2. Froze the acid. Did it by putting it into -75 Celsius acetone/dry ice bath and rotating, about 240 ml acid in 500 ml glass flask
  3. Vacuum evaporation. Their vacuum pump was capable of 0,001 Torr, and they sent the vapours through two traps of -75 Celsius acetone/dry ice and -193 Celsius liquid nitrogen. At first, pure ice was sublimed
  4. At some point, pink appeared in the trap - then the -75 Celsius trap was changed to collect separate fraction
  5. Finally, volatile fractions had left. The residue was found to be quite hygroscopic, solid, soluble - and pure HMnO4

    So, what is on the next page/s?
    Did they find out what happens when frozen solid HMnO4 is warmed above +1 Celsius? At what temperature does it melt? Congruently or incongruently?
    Has anyone repeated their synthesis?
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[*] posted on 27-3-2020 at 01:03
ref






[Edited on 27-3-2020 by HeYBrO]

[Edited on 27-3-2020 by HeYBrO]

Attachment: pg2forguy.pdf (279kB)
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[*] posted on 14-12-2020 at 21:13


I found on youtube this really interesting reaction - chemiluminecense from reaction between KMnO4 and Na[BH4]:

https://www.youtube.com/watch?v=gSP_953YMF8&t=187s




If you are interested in aqueous inorganic chemistry look at https://colourchem.wordpress.com/main-page/

I can offer GC analysis of samples. Just U2U to me for more info.

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[*] posted on 7-6-2021 at 11:05


Quick question (that I didn't think was deserving of its own thread, since I found this).

I purchased some Pot Perm Plus some time ago as a technical grade potassium permanganate source, and for just playing around with basic reactions/demonstrations, it's pure enough for that. The MSDS says its 60-100% KMnO4, but you can tell by the photos that there's clearly something else:


I figured maybe I could dissolve the KMnO4 in a solvent, filter it to get any insoluble crap out, then crystalize it. But from what I've gathered, KMnO4 isn't too soluble in acetone[src]. So perhaps just water? Though I know that heating it will cause it to decompose into MnO2.

So I suppose just distilled water and let it evaporate slowly at room temperature? Is that the best way?

P.S. I did look in the latest Purification of Laboratory Chemicals book for for potassium permanganate, but wasn't able to find anything on it.

[Edited on 7-6-2021 by SuperOxide]




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[*] posted on 7-6-2021 at 12:39


Quote: Originally posted by SuperOxide  
Quick question (that I didn't think was deserving of its own thread, since I found this).

I purchased some Pot Perm Plus some time ago as a technical grade potassium permanganate source, and for just playing around with basic reactions/demonstrations, it's pure enough for that. The MSDS says its 60-100% KMnO4, but you can tell by the photos that there's clearly something else:


I figured maybe I could dissolve the KMnO4 in a solvent, filter it to get any insoluble crap out, then crystalize it. But from what I've gathered, KMnO4 isn't too soluble in acetone[src]. So perhaps just water? Though I know that heating it will cause it to decompose into MnO2.

So I suppose just distilled water and let it evaporate slowly at room temperature? Is that the best way?

P.S. I did look in the latest Purification of Laboratory Chemicals book for for potassium permanganate, but wasn't able to find anything on it.

[Edited on 7-6-2021 by SuperOxide]


Isn't it maddening for a simple product to proclaim it could be 60-100% KMnO4 if you were trying to calibrate some repurposed use. Imagine if food was sold that way. Well I guess with potato chips it is as they sometimes list 3 different oils, possibly combined, "and/or" fried in.

[Edited on 7-6-2021 by Morgan]
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[*] posted on 7-6-2021 at 12:56


Quote: Originally posted by Morgan  
Isn't it maddening for a simple product to proclaim it could be 60-100% KMNO4 if you were trying to calibrate some repurposed use. Imagine if food was sold that way. Well I guess with potato chips it is as they sometimes list 3 different oils, possibly combined, "and/or" fried in.

For sure. I think they maybe do it because that gives them some room to vary the amounts of components in the product based on where they're sold/made at. If a certain chemical is cheaper in one city than another, then they may or may not use it for that area. But that's just a theory.




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[*] posted on 7-6-2021 at 16:39


Stop trying to dry permanganate. KMnO4 has a very low solubility at 0 C. The amount that remains in solution is almost always going to be less than what you would lose to decomposition on drying. If you really want to get more out, add excess potassium.



[Edited on 04-20-1969 by clearly_not_atara]
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