Making Permanganate 

I think cycles of evaporation to a super saturation state, followed by cooling would have resulted in better crystals. Heat destroys permanganate crystals.

I read on wiki that pyrolysis of zinc acetate can give acetic anhydride, maybe you should try it?

Neat article on making potassium permanganate by electrolysis that is cool.

I haven't come across anyone that can make a permanganate with great success.

Love your channel!

Super! Beatiful! Thank your very much!

Great process it seems like evaporating in a large wide glass dish would help. I'm wondering if using Bismuth and manganese as an anode would help. This chemical is so tricky it even reacts with filter paper which using glass wool is the only way

I was really rooting for you that you'd be able to separate the permanganate, sorry it didn't work out. I did a synthesis of this once but it was one of the high temperature variants. I had basically the same result. Lots of dark purple reactive solutions but no solid. I tried slow evaporation as well and that didn't work either. I just got a sludge of manganese dioxide and potassium hydroxide. If I revisit this and figure anything out you can be sure that I'll let you know.

this channel is so underrated

During the electrolysis process, crystals should form in the mother liquor. (which must be collected in a special recess in the sloping bottom of the electrolyzer) If this does not happen, then the correct electrolyte composition is needed. Sorry for the Google translation

As far as crystallization goes temp changes are a problem. You gotta dry it. I leave it open to the air in a dry place for weeks and it will grow crystals. Crystals don’t like to grow fast

I'd expect your bisulfite titration values to be affected by other alkali impurities, and color+turbidity to actually be more accurate for permaganate content with a less eyeball-based measurement (cell phone camera light level sensors come to mind for a hack maybe). Recycling the electrolyte got the cell running, but topping off with potassium carbonate solution might have kept the product cleaner. Fantastic work regardless, it's amazing what can be accomplished with humble but pure materials, a little electricity, and a lot of persistence.

Missed ya :3

Gday mate! New follower to your channel, love your work. I've been messing with home chem for a couple years now (mostly simple synthesis for crystal growing) and have had no luck whatsoever getting permanganate crystals to grow nicely, even through recrystallisation from pure crystals. Its an absolute nightmare of a chemical to crystallise from my (albeit small) attempts. That aside, its awesome to see a cool synthesis method! I've been meaning to get more creative with electrolysis and you're giving me mad inspiration. Keep up the awesome work!!

Without seeing the date of the paper, I got a pretty good ballpark when you held up a page and I read a reference to Bakelite.

Being that you got some small crystals and a salt structure and being the potassium permangante is of a crystalline structure maybe you just didn’t either yield enough or the concentration you were using to boil and cool werent high enough.. but I think in fact you 100% got KMnO4 though!

I really enjoy your videos. As a suggestion, could you please find some better illumination for your experiments? LED lights are so bright and cheap I'm disappointed that at times we can't really adequately SEE the results of your considerable work. Keep it up!

Should have used the titration station that you made in that old video I reckon

you can test it by adding glychirine on your yild when in catch fire it potassium permanganate... just charing idea...bro

Can you make HCl from NaCl (without acids) in next video?

Very cool! Too bad about the crystallization. I can't remember what solvents and technique I used to extract and recrystallize KMnO4 from these packets that you put in the refrigerator produce bin to extend the shelf life, but I was able to do it. I want to say I ended up extracting an aqueous solution multiple times with DCM, hexane or something like that. Trying to crystallize from water resulted in mostly MnO2 I think.

In an old chemistry book ive read only on an short note that an electrolysis of an manganese salt in an alkalien solution between iron or better nickl electrodes yield to permangante. Has someone tried this?

Can potassium permanganate expire?

Hi. I love your videos. I do have an idea for making a possibly better membrane for your experiments. I haven't tried it yet but it should work. 1. Grind some salt (table salt, rock salt, etc) into as fine a powder as possible. The finer the better. (Best to use a ball mill for the finest particles). 2. Take some HDPE plastic from either a milk jug or a shopping bag and melt it in a small pan over a hot plate. Make sure that you use enough plastic to make a thin sheet and that you put the hot plate on a low heat, just enough to melt it. 3. When melted add the salt powder into the plastic and stir it with a spoon or stick until both components are mixed thoroughly. 4. Make sure that you spread out the plastic/salt mixture as thinly as possible. Turn off the hot plate and take the pan off and let the mix cool. 5. Take off the plastic/salt film and then soak it in hot water to dissolve the salt away. Repeat this step several times to ensure that all the salt has been dissolved out of the plastic. This will make a porous film that will hopefully be better than using a clay pot as a diaphragm since this is thinner, allowing for both more electrical current and ions to flow through. You can probably make it even better if you add a small amount of graphite powder to make it more electrically conductive. I hope this idea helps you with your experiments. Cheers.

@19:25 Should have shown before and after weights of the Mn metal chunks. By knowing how much mass was dissolved off the samples, you should be able to determine how much product you've made with stoichiometry.

Is the permanganate in a high enough concentration to react with glycerin? Would give you a good idea of how well you did 💡😁👍

Could you try to make Ferrates? I think the electrolytic process is pretty similar to the one shown in the video. Instead of manganese iron would be used as the anode.

Based on colour, I had a prototype instrument that could measure 10 PPM , it is very intense.

Hi there. As someone who's attempted permangenates before I know how tricky the actual extraction is. My suggestion is to pay attention to PH when boiling down your solution. Permangenates break down at a Ph of around 10 back into mangenate, so keeping the ph neutral is quite important as it will rise with the removal of water. Also, permanganic acid is pretty unstable and will break down during the boiling of the soloution.

I was excited to see how easily the purple color developed but unfortunately I think you need to run this far far longer or with more amperage so long as the temperature does not get above 30 Celsius. The issue I see is your taking manganese from 0 oxidation state up to 7 and a lot of electrons must be pumped into the anolyte. This would take more than even making sodium chlorate from rock salt. It took me a month to make like 750 grams of sodium chlorate back 2007 with a 1 liter cell and roughly 6 amps current! Might I suggest melting MnO2 and KOH with KNO3 to make the green manganate and use a similar divided cell to oxidize that with a monel metal anode and a nickel plated copper cathode?

Give this man a doctor title

now all i need is manganese metal, the easiest way i can do is thermite reaction hope thisll work

KMnO4 dec at boiling point

What if you used a welder with carbon rods to melt your homemade manganese into a smol chunk And make it 100% homemade permangante

What is the cathaode in?

If you freeze the solution you could pull a vacuum on it to sublime the water?

very doable by just melting NaOH with MnO2 seems about 50g batches is the sweet spot for a camping propane burner this forms manganate first up when can then be precipitated with barium salt and then be acidified (with HAc, not HCl- forms Cl2) to yield watersoluble barium permanganate, this can then be reacted with potassium sulfate to give barium sulfate and potassium permanganate biggest issue in this is getting rid of the MnO2, because it clogs up filters and you cant see what is MnO2 and what isnt, its like being blindfolded as a bonus the manganate has a blue-green color to it, and if you simply put that into water, once it comes plenty close to neutral pH it turns pink, for water purification just this will do fine

Hey, at least it worked!! I suck at recrystallizing things too. Nilered does it so well. I think maybe try purifying before recrystallizing. Find something that KMnO4 is soluble in but the other things like KCO3 and KOH are insoluble in. ...actually, KMnO4 oxidizes everything but water, so the only solute you can use is water, so nevermind. Well, even in water, the solubility of KCO3 and KMnO4 are very different. solubility of KMnO4 = 76.5g/L @ 25 C, solubility of KOH = 970g/L @ 0C, KCO3 = 1103 g/L @ 20C. (numbers from wikipedia, tried to use something around 0C bc you will need cool the solution to lower solubility and speed up crystallization) So you can boil the water to drive it off and make the KMnO4 supersaturated but all the KOH and KCO3 unsaturated. But the high temperature might decompose the KOH. So let the water boil/evaporate at room temperature in a vacuum chamber. Oh wait, but you also used NaHCO3, which has a much lower solubility of 69g/L @ 0C. (That's really close to 76.5g/L, so those purple things most likely were KMnO4 and NaHCO3). You could put it in the oven to make Na2CO3 (2NaHCO3 -> Na2CO3 + H2O + CO2), which has a slightly better solubility of 70g/L @ 0C. You could use NaOH, which has solubility 418g/L @ 0C. I'm getting a sense that potassium just has higher solubility and you should use only potassium compounds as the anolyte. Is it not fair of me to compare solubility in g/L? Should I compare the molarity at saturation instead? K is 22.989769u while Na is 22.989769u, so maybe K's bigger molar mass is why KOH has more g/moles. Well let's see: KOH has saturation molarity 970g/L / 56.1056g/mol = 17.3mol/L and NaOH has saturation molarity 418g/L / 39.997g/mol = 10.5mol/L. Either by molarity or g/L, KOH seems better. Anyways, I'm wondering if here's anything easy to make and is more soluble than KCO3. Maybe Cl2 + KOH makes KClO. Solubility 25% (temperature not given), so 25g KCLO/ 100g H2O = 25g / 100mL = 250g / 1L Cl2 + NaOH makes NaClO. Solubility 293g/L @ 0C. Nah, I think it's easier to just take some ashes and mix it with water, wait for the sludge to settle, pour the clear-ish liquid on the top through some coffee filters, and use that as anolyte. Or if you're concerned about purity then just buy KCO3. Or get KHCO3 (100.115g/mol) and stick it in the oven to turn it into KCO3(138.205g/mol) by (2KHCO3 -> K2CO3 + H2O + CO2). Because you should end with half the moles KCO3 as the moles of KHCO3 you started with, you should have 138.205(.5) / (100.115) = 69.0231% of the mass at the end. Anyway, after that try the boiling in a vacuum chamber and putting it in the freezer for a couple hours. And then vacuum filtering out the aqueous KOH. Then pour some water and wash out any leftover KOH/KCO3 until u think it's pure. And then if you're still paranoid like Nigel, then do a melting point test and see if the melting point you get is 240 C +/- 10 degrees. Keep recrystallizing by adding water and boiling in vacuum chamber. until you get it right. You lose yield with each recrystallization bc some of the KMnO4 dissolves in the water each time, but purity increases. Hope you get some pure KMnO4 if you do this again! :)

Long time no see

Can you make a video about the synthesis of 1,2-Dichloroethane

What do you use or suggest as a plug for the hole in a terracotta pot?

can th Mn be forged to get a flater electrode? or it would just breake apart

I worked on the Mississippi River here in US and we had barges upon barges of Mg metal. Most of the battery companies buy all the stuff up. Maybe the initial carbon anode was driving the formation of MnO4. Batteries are after all MnO rxn w/ carbon. I’m gonna look I used to have a ton of the Mn in the raw from the side of the barges.

How well does a clay pot work as a separator, compared to other methods, lambskin condoms, gelatin etc?

What's the power supply you're using? If it's DIY, could you share some links?

マンガン電池とさらし粉を煮るで結論出てる

is that a new boost converter?

Can you try the Synthesis of Formalin by electrolysis?

Can I use maganese plated on aluminium ,as an anode ??? Can I use KOH or NaOH instead of carbonates of potassium & sodium??

Anode chamber??? I think you mean the "ANOLYITE". Also get rid of the clay pot and use same porous Viton shipping bags.

Can’t permanganate be sublimated?

Why don't you let it stand in a dry room for 6 weeks and see what you get? 2 months might be better.

Huh, I thought there would be much more MnO2 junk in there.

just dry it you don't have to predict the concetration

Why can I not view your replies?

Really you can't by this ether!😔