Peroxide From Air And Water?

[@connormcneill9024]

Props for posting your failed experiments. Reduce the publication bias! Negative results are just as important as positive ones.

[@user-pp3yi5tv7l]

I really like that you make many experiments with electrochemistry. Making H2O2 is something I wanted to do for a very long time but I've never found a good example. So thanks for your video. I might try these methods on my own.

[@chemistryofquestionablequa6252]

You can do it chemically from alkaline metal peroxides like sodium or potassium peroxide. There's at least one video on KZbin doing that. Edit: Astral Chemistry has a video on it, that's the one I was thinking of.

[@uteschneider3349]

Und wie stellt man Wasserstoffperoxid Puder her, für die Haut? ​@@chemistryofquestionablequa6252

[@uteschneider3349]

​​@@chemistryofquestionablequa6252Und wie stellt man davon Wund- Puder her, was man auf der Haut benutzen kann?

[@benjaminpainter378]

I'm so thankful you're still making videos throughout all of this. Keep up the great work!

[@bryankreinhart]

As per the paper, your 3 chambered experiment required O2 on both electrodes. The porous carbon with O2 diffusion is on both sides. Note, also, that the 3 chamber diagram displays the expected reaction on chamber 1 and chamber 3 of which both show O2, which is supplied via the porous carbon. You omitted this in your experiment. Recheck the paper.

[@leonciopina3618]

No veo la adición del oxígeno en la cámara 1 (anolito), lo que puedo apreciar es la formación de oxígeno molecular debido a la electrolisis del agua en el ánodo (oxidación anódica)

[@philouzlouis2042]

Did you test the stability of H2O2 towards your garden clay pots? I imagine that clay from clay pots contains a big deal of metallic oxydes like Fe2O3 (I say this from the colour). Normally H2O2 or superoxyde anion (HO2(-)) is sensitive to metals like iron. H2O2 is not so sensitive to NaOH as you think. I have worked in a shampoo and hair products factory... we worked with H2O2 (30%) that was dilluted and incorporated into a wax stiffener to make a 10% peroxide cream for professionals... to discolour hairs prior to (re)dye process. Such thick cream was a nightmare if catalytic decomposition of H2O2 ever occured... because the cream would expand like a solid foam... H2O2 30% is 100 volumes so 10% is like 33 volumes... imagine your 10 cubic meter batch that goes 330 cubic meters... not pleasant to see nor to manage. Also sealing caps can't be airthight because of the risk of explosion of the bottles, the use of flipping caps was prohibed because of the risk of splashing to the eyes in the case of an internal overpressure. During the stability testings for long term storage we used various products acids, bases, organics, minerals... and submitted our samples to heat, to UV and determined the volume expension during time. Base was as good as H2SO4 what is often used. One of the best stabilisator was sodium stannate (a product that is quite basic). Maybe the use of Na2CO3 (quite basic) and a bit of Na2SiO4 would help generate sodium percarbonate (2Na2CO3.3H2O2). This paper explains the preparation of percarbonates from carbonates... but they use platinum (maybe MMO electrode will work?) krc.cecri.res.in/ro_2000/111-2000.pdf This one too is about percarbonate via electrolysis. www.researchgate.net/publication/244671808_Simultaneous_Anodic_and_Cathodic_Production_of_Sodium_Percarbonate_in_Aqueous_Solution This one starts from CO2 www.freepatentsonline.com/7094329.pdf Percarbonate is a good source of H2O2...upon acidification it sets H2O2 free (of course one must use an acid that doesn't react with the H2O2 ... HCl, HBr or HI are excluded). PHZ (PHILOU Zrealone)

[@ScrapScience]

I didn't even think about iron in clay pots, that definitely sounds like a likely culprit, amongst other things. Thanks a lot for the info too, I recently got a platinum on titanium anode so I might give percarbonate a go at some stage.

[@vantablack9882]

hey , i have seen your posts on sciencemadness

[@philouzlouis2042]

@@vantablack9882 Yes... that must be one of my many posts there :o) PHZ (PHILOU Zrealone from the Science Madness forum)

[@joshborchardt5050]

Thank you so much for the disclaimer at the start. I very much appreciate your videos, and the fact that you don't want to waste your Watchers time. It's very nice.

[@ziyadamayreh8081]

Although this video is over 3 years, I learned a lot from it, and gain good experience. For me, Some times failure is a good teacher. All your Hard work is Appreciated, Sir.

[@leonciopina3618]

La verdad aprecio el tiempo dedicado a realizar este tipo de experiencia. En realidad el grafito viene a ser un tipo de catalizador pero a la inversa, es decir, favorece la evolución del oxígeno en el cátodo

[@visualinspectator4474]

Can you try this with a solid electrolyte please? Thank you!!

[@loganbrown9553]

Is there such a thing as solid electrolyte?

[@richardnineteenfortyone7542]

With very few exceptions (perpetual motion, antigravity, etc.) the process of awarding a patent is merely a costly legal process that in no way depends on the invention actually working.

[@computerman200]

didn't the paper show 02 not normal air in the cathode? i would be curious to see the results of the same experiment but bubbling oxygen instead.

[@fasted8468]

Thank you very much for that. No time now. check it out later though.

[@nicoenriquelimongecolomer63]

The terracotta pot could decompose the formed peroxide. Try another membrane. If I remember correctly, the terracotta contains also iron (which could decompose the peroxide)

[@ralfvk.4571]

that's right and maybe there can be traces of Manganese dioxide in there too, what destroys all H2O2 immediately.

[@omsingharjit]

30:12 i think he used teflon ptfe as one type of ionic sepretor .. And may be nickel as catalysts

[@CatboyChemicalSociety]

I notice it says at 27:20 current density of 394A/m^2 which is equal to 39.4 ma/cm^2 which means so if your electrode was 1cm^2 then 40ma is ok however it looks like more.

[@ScrapScience]

To be honest, I was struggling to push the correct current through the cell without the voltage raising too high (I still need to get around to making some proper membranes it seems...), so the current I ended up using was substantially less than optimal.

[@CatboyChemicalSociety]

@@ScrapScience I also recommend additives to stabalize the peroxide produced. kzbin.info/www/bejne/gpPJqZtpn66NkLc This is a video of that exact setup.

[@Rivodtadin]

I like your videos and your explanations, i hope that you make a video about making Sulfuric Acid from Sulfur the easy way like you do always. Thank you

[@whatelseison8970]

Did you get your carbon rods from carbon zinc cells? If so, it could be that small amounts of MnO2 remained on them, catalyzing the decomposition of any peroxide as it was produced. BTW, how did you make your gas diffusion electrode? How far did you manage to drill into it? Was it by hand or on a lathe or some other way? Also, do you burn the wax out of your C-Zn cell derived rods before using them for electrochem or just use them straight away? I just found your channel and I'm liking it a lot - subbed right away. It's cool to see someone with similar resources to me having tried so many projects I find interesting. Saves me some bumbling around lol.

[@ScrapScience]

The carbon rods I use are actually 'welding carbons' I found online (much cheaper to obtain than from lantern batteries, I think I got 100 for like $20), so they didn't contain any manganese oxides or waxes. I actually have another video about making the gas diffusion electrode here: kzbin.info/www/bejne/fmXSZaykgbehjqs Glad you enjoy my channel!

[@alllove1754]

I think if you put water under extremely high pressure, freeze it, I mean like ice 7 pressures so the ice doesn't expand, THEN you can do this. Should be water behaves as a polymer at some pressure, and that corresponds to h2o2's physical appearance at 100%, a really thin polymer

[@icebluscorpion]

Can diaphragm short out when they touch? I mean corrent goes where the least resistance is so your pots might have shorted out by putting them on top on another

[@ScrapScience]

I've found that in cases like this, the pots have a much higher resistance than the solution surrounding them, and I wouldn't really expect the small surfaces where the pots are is direct physical contact to account for much. It certainly may have been a contributing factor to inefficiency, but I wouldn't expect all of the ion flow to be shorted out like this.

[@mertlerendustri2173]

I'm so thankful Can you get ammonium per sulfate by electrolysis?

[@ScrapScience]

Yep, you can! I'll make a video on it one day, but likely not for a long while.

[@Prchemist06]

According to my instincts ,dilute and cold solution of 30% H2SO4 would do the job ..I am also trying to immaculately produce Hydrogen peroxide with my earlier mentioned method or so to say .However ,my method would dispair in fashion of using anode and cathode according to a paper I stumbled upon

[@tahanlaoboy]

they might mixed the Hydrogen liquid and Oxygen liquid together then add some bonding agent to it

[@Timestamp_Guy]

What if the reaction is fed with Ozone instead of oxygen? Would that change the need for a catalyst to reduce it? Ozone machines for deodorizing and disinfecting rooms are commercially available online no problem.

[@ScrapScience]

I'm honestly not sure. Ozone is definitely easier to reduce, but the reduction products might not align with the required hydroperoxide ions. Either way, the output of ozone generators is generally very low, so assuming it works, the process would likely take days (or weeks) to make reasonable quantities of peroxide. Might still be worth a try though.

[@ralfvk.4571]

@@ScrapScience Look above, I tried it out again. That doesn't work so easily because of the back reaction of H2O2 with O3. Anyway, there are indeed Generators available that can produce 10g O3 and more per hour, but they normally don't come inside a case, so you have to build them inside a bottle, tube or something and pump air through it. O3 is a very useful stuff, also for making H2SO4 from SO2 and Water (H2SO3) as it oxidizes it very quickly and directly, also SO2 to SO3

[@fieroboom]

For the diffusion method, do you think it would help to create an HHO type cell with separated gas outputs, & pump the pure oxygen through the diffusion electrode instead of just air? 🤔

[@ScrapScience]

Feeding the cathode with pure oxygen would definitely help the rate of the process (by up to a factor of 3 possibly), but I still think the simple graphite electrode just doesn't have the catalytic activity needed for oxygen reduction. Honestly, there are so many factors in this experiment, that it's very difficult to tell what could be changed to make it work (other than copying the original paper perfectly).

[@danieljohanides2625]

Ceramic contain mno2 that decomposes hydrogen peroxide

[@林泽肥]

A very good attempt.

[@ferminenriquezamorapineda2832]

Could it be possible to use ozone instead of oxygen from air?

[@ScrapScience]

It could be, but I've got no idea what the reduction products of ozone would be on the cathode. Might be worth a try...

[@ralfvk.4571]

@@ScrapScience I tried out O3 bubbling into water, years ago, but the Problem is, O3 also is reacting the H2O2 back to H2O and O2, so it has to be separated somehow directly after formation, but I don't know how. However, thank you very much for the inspiration, I was always looking for an alternative method to DIY-H2O2, even with low efficiency, as long as it works. I think about trying out the first method from your pdf-link. the alternating Voltage shouldn't be the big problem if you use some relais for it, that switch the polarity, by every impulse (flip flops). The electrodes are more complicated, cause they need to be out of carbon and different metals according to the pdf. But still should be possible. Would be nice to have an useful result in the end, but I am sure, it can be done. Just don't give up. Thanks again for the inspiration, your ideas and videos are cool and different. :-)

[@topduk]

You might be interested in Palladium-tin catalysts for the direct synthesis of H2O2 with high selectivity - Simon J. Freakley et al. Science 351 , 965 (2016)

[@richardamullens]

Why don't you get yourself a copy of Modern Inorganic Chemistry by J. W. Mellor ? My edition is 1927 and has 1108 pages.

[@SciDOCMBC]

A clay pot as a diaphragm is completely unsuitable here. Rough surfaces lead to rapid decomposition of H2O2. Produced H2O2 decomposes immediately after it is formed.

[@ScrapScience]

Yeah, to be honest, this video is not one of my best. It's riddled with oversights and misinterpretations of the core principles presented in the paper I followed. If I were to do this again, I'd make some pretty big changes, starting with the clay pot diaphragms (as you've mentioned), and the electrodes too.

[@omsingharjit]

I have another idea of producing Hydrogen peroxide using Uv light and Ozone by High voltage plasma i think it will work

[@Preyhawk81]

ozon and uv light destabilize h2o2. only if you added an stabilizer or and diaphragma that remove all h2o2 will work.

[@guigra11]

Nice video. The reason why your experiment failed is clay pots are too thick-wallet to use as diaphrams.The thinner and porose the diaphragm , the better the ion migration.If you want to carry out such an experiment, the vessels should first be cleaned with aqua regia.You approach was correct but the decrayrate was higher than the production rate.If the smallest traces of metals present in the reaction vessel, the decomposition of hydrogenperoxid immediately.

[@ArktourosUltorMaximus7600]

Hey bro continue with the Deuterium Water series

[@ScrapScience]

I promise I'll return to it one day. I've had a couple of issues with the electrolysis cells leaking lately, so it's slow going at this stage.

[@ArktourosUltorMaximus7600]

@@ScrapScience Ok thanks 😎👊

[@sajidhussain2932]

i will try and share

[@austinball4343]

The nickel probably does act as a catalyst

[@jamesdavison6654]

Ac current would switch back and forth by its nature

[@TheRojo387]

This setup is a triolyte.

[@stephenphilp1380]

I love your videos. Love your recycling of things, paper, shoe boxes, computer power supplies and so on. Awesome, I thought I was the only one who did this. Keep up the good work.

[@anti-fz9be]

I have suggested this about a year ago, but can you try making permanganates (sodium/potassium) by electrolysing a solution of (Na/K)(OH) with a manganese metal anode, and the 2 chambers separated by a clay pot? I heard it works very well, and, if you succed, you will be settling a 13-year old topic on sciencemadness. It is a very slow process. But it is stable. I have heard rumors of people having crystals in the anode chamber after a day. I can't do it myself because i could not find metal. It would be very cool! I had a very old paper talking about this, they did hundreds of attempts, and found the best concentrations, placements,etc.

[@ScrapScience]

Awesome! I've always wanted to make permanganates, but got disheartened every time I looked at that sciencemadness topic page. I'll have a serious look into it, if there's any chance of making any reasonable quantity of permanganate, I'll definitely give it a go. Do you still have the paper about it? If not, I'm sure I could find it with a bit of searching around.

[@anti-fz9be]

@@ScrapScience i will try to extract it from my dead HDD.

[@anti-fz9be]

@@ScrapScience I have found the original SMDB post in my backup-ed bookmarks. The drive is certainly dead, so i don't have the full paper, just the important bit. The guy distilled the content from the paper, tried it, posted pictures, he obtained .37 grams of PURE yield, *AND EVERYONE IGNORED HIM* . This is his post : www.sciencemadness.org/talk/viewthread.php?tid=8480&page=16#pid459691

[@ScrapScience]

Cool, thanks. I've managed to find a couple of old papers on the topic (including the one which the sciencemadness user refers to) and they're quite impressive. Pretty crazy that that guy made pure stuff and nothing came of it, but oh well, maybe we'll get it to work too.

[@فريدالقباطي-و1غ]

ممكن ترسل لي بالورقه القديمة سوف اكون ممنونه لك

[@theastroslav]

I like that you post your experiments even if they are not a success. I am excited to see what the next experiment will be!

[@林泽肥]

I guess you may make sure the oxygen reduction reaction on your cathode is working well firstly before performing experiments in your system. Do you have H cell with commercially available membrane to test this half reaction?

[@dmitrygrey]

Ahah, it's yellow. Remember yellow in chemistry = crap xD

[@omsingharjit]

26:48 try 1% real peroxide with same amount of H2so4 and naoh mixture to test if it also gives same yellow colour or not !!

[@NishchayG]

I still remember when you had 500 subs

[@Telectronics]

Well at least you tried it and that is what counts right ? Thank you for taking your time to test it. You are great :)

[@guytech7310]

I suspect you would need to use a platinum or perhaps Palladium to serve as a catalyst for peroxide production. Temperature may also be a factor.

[@whatelseison8970]

Both of those metals catalyze the decomposition of H2O2 as does silver. I'd imagine most of the platinum group would behave similarly.

[@ralfvk.4571]

@@whatelseison8970 that's right, so if you will read the pdf properly, there is told which Elements have to be present that may work as catalyst on page 9. Very interesting, never heard of it before. patentimages.storage.googleapis.com/13/4d/99/dfbb875f401486/WO2010134717A2.pdf

[@Jagdtyger2A]

Peroxide is a very important item for post SHTF medical purposes. So this video should be shared with every prepper you know. Survival in a SHTF world is not all about guns. After all, the only weapon that truly exists sets between the ears. Unfortunately, most people fail to load it

[@sajidhussain2932]

nice video, its theoretically possible but to some extant, but these research articles seems to me exaggerated what they have done.

[@CatboyChemicalSociety]

the issue is that hydrogen peroxide is unstable and will just nucleate at the porous pot walls. you are better off making a 3 compartment cell casting gelatin membrane walls for it impregnated with sodium sulfate mixed into the gelatin. dont use gel bridges as the area and thickness of the membrane is what affects the rate of flow of ions through it. usage of other polymers might be nice like did you try silly putty PVAglue + borax with a scaffold as a membrane preferably some type of plastic mesh. doesnt work for sulfuric acid but might work for peroxide.

[@ScrapScience]

I’ve been planning on testing PVA+borax membranes for a while (not specifically for this process, just in general). Have you done any experiments with them? If so, how well do they work for ion transport? And do you have any data/experience regarding the chemical compatibility (obviously you’ve mentioned sulfuric acid but do sodium hydroxide/chlorine/etc. have the same effect)? If they work well I’d love to add them to my ‘arsenal’ of possible electrolytic membranes. I’ve got so many ideas for electrolysis that would be so much easier with a reliable membrane like this.

[@CatboyChemicalSociety]

@@ScrapScience ive made the ones out of gelatine used them to make copper 2 perchlorate from KClO4 have some posts of it on sciencemadness including pictures. I then converted Cu(ClO4)2 into TACP using ammonia gas on the chilled solution. you have to make the gelatine membranes flat for greater surface area and less resistance.

[@CatboyChemicalSociety]

for sulfuric acid I found its best to use a copper anode to make copper sulfate first then to freeze the solution to remove any sodium sulfate left over. Then finally use lead or graphite anode to plate out the copper and you will be left with sulfuric acid. btw PVA membranes work pretty well for that purpose too though agar is also really good if constructed right.

[@Ma_X64]

Electrochemistry is my most lovable part of the science. I thing it's because you turn pure energy into something you can touch and weight.

[@amaressa1924]

Why didn’t you just test the liquid in the other chambers ? Maybe the hp wasn’t going through the ceramic

[@patriciagoodrich7800]

I'm gratefully for your experiments because I'm wanting to make my own hydrogen peroxide. It is an essential means for survival.

[@f800gt76]

I think, in industry peroxide is made through sulfuric acid electrolysis with following peroxodisulfuric acid hydrolysis

[@ScrapScience]

Sulfuric acid electrolysis was used at some point, but nowadays this has been completely superceded by the anthraquinone process.

[@gert_kruger]

I doubt that oxygen gets adsorbed onto the carbon aerator via bubbling. The alternating polarity method probably has a deadtime in order for hydrogen peroxide to move away from the electrode before switching the alternate polarity.

[@JakobVirgil]

Unlike nearly every other electrolytic process Could AC work for this?

[@bpark10001]

Doesn't nickel & other metals catalyze the decomposition of H2O2?

[@gordonfamilyforge134]

how about uow to make nitric acid from def fluid or uria?

[@semihtolgahaydaroglu7618]

Hi hydrogen peroxide occurs naturally in ice form. when ice breaks, oxygen is released to the environment. there may be a deficiency.thank you for sharing. i can be inspired

[@MoncœrCoyoteSmith]

Missing pure O2 in a gaseous state to oxidate the H2O. H2O + O2 (electricity) -> H2O2

[@Ma_X64]

In industry, the electrolysis of concentrated sulfuric acid is used to produce hydrogen peroxide, and the processes going at the electrodes are quite complex. And the huge problem of home-achieving peroxide is that any heavy metal or protein contamination will destroy the peroxide back into water and oxygen. You should also know that not the current itself you need to control but current density! I.e. current divided by electrode surface area. And this is true for any alectrochemical process. I can try (if you need) to find one old soviet book describing production electrochemistry technologhies of several substances.

[@chemicalaffair.]

I would also be very interested in the book you mentioned. it would be great if you were able to get more informations about this book (i would really appreciate it)

[@allenhonaker4107]

Maybe something in the glaze of the pots reacted with the acids and bases

[@YouMockMe]

Good go! ...experimentation right. Cheers

[@elad4242]

Use AC voltage

[@jamesg1367]

Ozone?

[@chemistryofquestionablequa6252]

I would expect that one serious problem would be that either the electrodes(depending on what you use) or any corrosion from your wiring can both decompose hydrogen peroxide almost as soon as it's made. There's also the problem that a significant percentage of chemistry patents just don't work.

[@simple_fred]

I have noticed that you frequently use clay membranes. Have you tried making clay from dirt and simply pit firing them?

[@ScrapScience]

I was going to attempt that at one stage. I went to the effort of digging up some clay, purifying it, and then letting it reach the right consistency by evaporation. I was going to fire it too, but at some point I lost the sample I'd made and haven't found it since. I'll do it again some day, but it was a lot of effort the first time and I haven't quite got the determination to start all over again just yet.

[@simple_fred]

@@ScrapScience cool, after I watching your video, I looked up other attempts to create H2O2 and found a research group that used a solid state electrolyte, which got me thinking. Anyways, great video.

[@ezequieladrianminniti6252]

anybody can file a patent, even if the invention doesnt work

[@omsingharjit]

Will separator from li ion battery work as Cation membrain ? I think it will work better

[@ScrapScience]

Possibly, but it will depend on the type of li-ion battery, and I don't think the membranes will stand up to strongly acidic conditions like this either. It also doesn't solve the problem of the required anion exchange membrane, which is the most important component for the reaction.

[@terryadams2652]

Dear Scrap Science, *I think you'd love to know that (it appears) Rice University has generated H2O2 from electrolysis.* RU has posted it on their youtube channel, the title of the video is "H2O2 from air, water and electricity" I would just give the URL, but it appears youtube doesn't allow the posting of URLs anymore. Enjoy, please let me know what you think.

[@ScrapScience]

As a matter of fact, that was kind of the inspiration for this experiment. I came across that video when it came out, and thought it might be cool to try, but was disheartened when I discovered that it required solid electrolyte structures and fancy electrocatalysts. In further research, I found the paper I used in this video. Sadly it wasn't meant to be, but maybe one day I'll find a synthesis of H2O2 that's doable.

[@terryadams2652]

@@ScrapScience Mr. Scrap Science, I picked up the excellent reference book, "Industrial Chemicals", 4th edition (1975). The chapter on Hydrogen Peroxide mentions three ways of making H2O2. Two of those ways involves a precious-metals catalyst, BUT, the third way does NOT require a catalyst! It's called the Shell Process. *In this process, 02 oxygen & 2-Propanol are placed inside of a reaction vessel, and the O2, strips the Hydrogen from the 2-propanol, yielding Acetone & H2O2!! I'm in love. Yield is 87% based on conversion of the Alcohol! NO catalyst needed!!* The only catch is the vessel has to be made of Aluminum (or glass, or enamel, or any other material that won't react with H2O2). I think Aluminum would be a great choice. The only other thing is moderate pressures & temp. Temp of 100C to 140C is not a big deal, since Aluminum pressure cookers obviously deal with higher-than-boiling temps. Pressures are only ~16 Atmospheres (which isn't high at all compared to Urea, requiring 2500 to 3000 PSI). If you decide to build a reaction vessel, I think you can just put the Aluminum "tank" inside of a larger "steel" vessel, in which the space between the Aluminum vessel and the steel vessel is filled with a solid concrete-like thermal insulator. I think it's very doable. A pressure vessel is something you build only once in your life, then you've got H2O2 for all eternity, and NO catalyst needed! *Please Let me know if you want me to video record that page of my book for you.* ... Btw, you may also want to look at Ullmann's encyclopedia of industrial chemistry, they have an entire chapter on H2O2, including the Shell Process (I've got it in PDF, it lacks details as it points heavily to other references, including old patents).

[@whatelseison8970]

According to Wiki, simply burning sodium metal in excess oxygen yields primarily sodium peroxide, which can then be dissolved in water to give hydrogen peroxide and sodium hydroxide. A better idea might be to dissolve it in something like phosphoric acid, ultimately shooting for a reasonably stable, neutral, and buffered product which should be possible to distill if desired. Burning potassium in oxygen is supposed to generate the superoxide, which also yields peroxide upon hydrolysis while evolving O2 gas. I wonder if it might be possible to get H2O2 by burning H2 in ozone or if anyone has tried that.. I'm not sure if that even makes sense; it just popped into my head while writing this... I've always found it kind of strange that a chemical that's in some sense "made of" air and water should a) need so many other reagents to prepare, and b) be so harmful to human health given how great air and water are for staying alive. If only it were possible to chug a pint of the stuff and then spend the next hour or so having fun under the sea.

[@mohilkumar7826]

Amazing video and very knowledgeble despite failed experiments 👏👏

[@leerifle2975]

It looks to me that this reaction was carried out under pressure, because the drawing is showing a black line all the way round the cell structure. meaning this was a sealed unit, similar to a car battery. The oxygen and hydrogen may have even been forced through the membrane walls into the middle cell,

[@icebluscorpion]

How do you get rid of the sulfuric acid after having a 10% peroxide solution?

[@ScrapScience]

You could precipitate it out using calcium hydroxide/carbonate. Or you could neutralise the solution and remove the ions with some ion exchange resin. There might be some other methods too, I'm not sure.

[@ralfvk.4571]

@@ScrapScience I would try vaccuum destillation at low temps. Should work.

[@jozefnovak7750]

Super! Beatiful! Thank your very much!

[@thecommentator3594]

Can you try to make chromates from stainless steel by electrolysis? By using a stainless steel electrode in a cloride solution you should break it up faster and cheaper than with hydrochloric acid like extractions & ire did.

[@ScrapScience]

That's a great idea. Using salt and electricity would certainly be cheaper than hydrochloric acid, and dichromates/chromates are pretty useful. It might be a while before I get to it (I've always tried to avoid chromium chemistry due to toxicity issues), but I'll add it to my list of future projects!

[@anti-fz9be]

@@ScrapScience i have tried that. I don't recommend it because the yield really i got was minimal. I also found a method identical to the one for the permanganates, but using chromium metal, in a book.

[@ScrapScience]

Would that book happen to be 'The Manufacture of Chemicals by Electrolysis'? I think I remember it briefly mentioned both permanganates and dichromates.

[@anti-fz9be]

@@ScrapScience precisely!

[@CatboyChemicalSociety]

ive done that it works but not in that way. what I did was just convert chromium into chromium 3 oxide by electrolysis then that resulting green mess is then mixed with NaOH and NaClO3 to make sodium chromate or potassium salts to make potassium chromate.

[@quantumlab9130]

I think you should try building a PEM fuel cell.

[@hrajabi7261]

Light decomposes hydrogen peroxide

[@mamax7169]

can you make a video about h2s2o8 peroxydisulforic acid and its salts? it is a very interesting compound and easy to get :)

[@jeremiezinsalo9083]

Hi Please, where do I can buy h2s2o8 and what's it name in marker

[@geniusdude8975]

Hello harry In my country 1L of h2o2 only cost 6 dollar. It was 30% 100 volume

[@geniusdude8975]

No joke

[@aa18812]

I found a paper on the electrolytic synthesis of hydrogen peroxide using sulfuric acid, potassium bisulphate or ammonium busulphate. It does require vacuum distillation in order to hydrolize the electrolytically obtained persulphates and separate the hydrogen peroxide though. Maybe this is a more viable, or at least more reliable, way of electrolytically making hydrogen peroxide that could be fun to try. This is the paper: journals.co.za/doi/abs/10.10520/AJA03794350_582

[@ScrapScience]

That's definitely a cool process that I've been meaning to try for a long while. There are a couple of things preventing me from doing it at this stage (I don't currently have a solid platinum anode, and vacuum distillation of an oxidiser that can violently decompose scares me quite a bit), but it's currently on my list of future video ideas.

[@Jkauppa]

non-janky method would be through sodium peroxide, Na2O2, soaked in water, and you get sodium hydroxide for free, Na2O2 + 2 H2O -> 2 NaOH + H2O2

[@Jkauppa]

through sodium metal, either from electrolysis of molten NaOH, which you get back, or I assume from electrolysis of molten NaCl

[@Jkauppa]

use Sodium as the one of the main reducers for metal oxides or any compounds, to release the metals

[@Jkauppa]

how about a secondary porous (cloth/paper/diaphragm) separator around the carbon electrodes

[@Jkauppa]

prevent pre-mature decomposition