Hello everyone! Harry here, welcome to Scrap Science.
My channel is mainly focused on chemistry experiments (electrochemistry in particular) with relatively basic equipment, though some of my videos will often branch out into other areas of experimental science. The main focus of my videos is to simply document and explain the experiments I do at home, and maybe we'll all learn something along the way.
If you need to contact me, my email is scrapscience0@gmail.com . I can't guarantee I'll reply to everything, but I'll do my best to respond to genuine enquiries.
@@ScrapScienceThanks, I will have to try it out to look at the results, if I can make HClO4 from it I can neutralise it with NaOH or Na2CO3 to make NaClO4 it will be easier than making it via electrolysis as making Sodium or Potassium Perchlorate is a bit tricky by electrolysis.
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When anhydrous, magnesium sulfate will decompose before melting. Even if it didn't, the anode reaction would be rather complex when working with molten sulfates. I don't know exactly what would happen, but I doubt it would be well-behaved...
Of course. Graphite is almost always a more reasonable electrode to use. This electrode is specifically for performing reactions that graphite can't do though. I list some of them at the end of the video.
hi harry I am making a new chlorate cell in November/ December but I need some stuff for it so I've managed to find the 10v dc converter but I need a power supply that you used in your A SODIUM CHLORATE CELL video ,by that I mean a power supply that can supply at least 5 amps and that can handle a electrolysis for multiple days < so could you comment the name I should search in google to get the result in your privallige I will @ your channel in my video (I'm subscribed)
Glad to hear - a chlorate cell is a great project! Nowadays, I just use a lab bench power supply with adjustable voltage and current. But back when I made my chlorate cells, I was using a current controlled buck converter hooked up to an ATX power supply from an old computer. Hopefully you'll be able to find a similar product.
I get it that HCl in water has an azeotrope of 20.2%... Therefore, the LIQUID output from your condensor will be at that strength. However... If you were to use 33% in your boiling flask, and you allowed your condensor output to bubble through the content of your azeotropic receiving flask *thereby re-absorbing HCl gas into the azeotrope), wouldn't you end up with something fairly close to your 33% source acid? (Industrially, 33% HCl acid is produced by absorbing HCl gas into water until it's near saturation. There's many industrial processes that release HCl gas as a 'waste' product and this waste is used to make 33% HCl)
Correct. I just didn't really want to deal with trying to dissolve HCl gas in water in this case. If things went wrong or the gas were improperly absorbed, it would present a pretty big issue.
Only with very pure chlorate, the correct electrodes (MMO anodes will not work), and an additive to prevent back-reduction. I'll eventually make a video about this.
I was Just picking AI's brain. It seems you can also use electrolysis with Sodium Bisulfate (Dry Acid,, PH down from pool stores, NaHS04). Supposedly it's a bit purer. I don't have as much experience. Any comments would be appreciated.
Nice work I’m wondering if you can let it run more time to break down more water hence concentrating the acid a bit more. I realize this is proof of concept but I feel like this would even with 5 times the concentration of copper sulfate. Or, since your acid is very dilute, add more copper sulfate and repeat until the acid or 2 or 3 Molar. Oh I’d like to mention sulfuric acid reduces copper sulfate solubility it water through common ion effect (sulfate). So if you go the route of adding more copper sulfate repeating and repeating you will find a point when it’s no longer feasible to try to add copper sulfate for another run and then you have less water to boil off.
I remember doing this over 40 years ago and used carbon rods from batteries, or maybe stainless steel rods, but I've forgotten my chemistry by now. I boiled the acid next to increase concentration. To what extent can this be done to improve concentration, because from what I remember, acids absorb water and that's the reason they are so harmful to organic matter? (I presume the stainless steel I used wasn't a good idea because of the chrome salts I made.
i bought undercounter battery magnetic lights for 2 bucks each and then parrelleled my still working batteries with the small original batteries of each one so i only have to charge them a couple times per year.
Bravo.......screw magnesium.......it makes hydrogen .......when u put in water........measurements how much yield......also reactor with gas shield.....cheers
Throughout the video, my biggest fear was that you could have blinded yourself with that liquid NAOH. Please be careful! I was adjacent to a sodium-involved accident in the 1970s and thank God, the boy involved recovered fully.
Don't be concerned - I'm always wearing safety goggles AND a full face shield while I'm doing molten electrolysis experiments. This stuff is definitely no joke!
@@ScrapScience Amen! I would love to see what molten NAOH does to animal tissue. It must make very short work of it! My grandfather worked for Western Electric where they made synthetic quartz crystals and -- believe it or not -- those reactors contained chemicals at temperatures and pressures which made molten NAOH seem like a mild base in comparison.
MAybe just put the anode on top and cathode on bottom. After carbon dioxide is gone, you should be left with hydrogen peroxide and sodium hydroxide solution. Maybe you could seprarte them by crystallization.
Did you ever get this to work mate? I'm trying to plate some aluminum with manganese sulfate... However I'm also struggling with the process... Weirdly my manganese sulfate is more of a green color... I made it from mnO2 (with sulfuric acid and oxalic acid) and then made another batch with sulfuric acid, iron and oxalic acid as the reducing agent... However they both turned out green after filtering 🤔
I'm afraid I haven't looked at this since making the video - all the information and experimentation I've gathered/done is here. In general though, plating aluminium is very difficult. For what reason do you need manganese-plated aluminium?
It might be possible, but I’ve never been able to get the pieces to bond properly just by squishing them together. I assume surface oxidation prevents it from working nicely. Even doing it under oil doesn’t seem to allow it.
Try temporarily reversing the current flow right at the start. This might help activate the surface of the Titanium, removing the oxide layer. and kick start the plating.
@@ScrapScience but if use graphite as an anode, it will dissolve with chlorine and pollute the electrolyte. Does titanium has corrosive resistance from chlorine?
Yep! Carbon electrodes will work here, though you’ll need to filter the resulting carbon dust before crystallising your final product. I’m not sure what you’re asking about regarding the current. The current can rise for many reasons.
I've been wondering about why does carbon get destroyed when used as a anode in most conditions its used there isnt anthying that can react with it yet it falls apart, i search for it but the only result i found says that its because carbon is porous but then the Cathode would fall apart too but it doesnt.
The porosity does come into it, but it's not the main reason behind the degradation. When used as an anode, a very small amount of carbon is able to be oxidised to form CO or CO2. Since these electrodes have a porous structure, this oxidation can happen inside the electrode instead of just on the surface, causing them to disintegrate. Without any oxidation, no disintegration occurs. Likewise, making the electrodes less porous (i.e. HOPG electrodes) leads to much less electrode damage (but not zero).
@@ScrapScience Thanks for the reply, that does make a lot of sense. This means that carbon will fall apart faster when making Oxygen like when used in a NaOH solution then when its making cl2?
Correct. When making chlorine from aqueous solution, carbon will fall apart slower (but it will still eventually disintegrate, since there's still water present that could lead to the formation of oxides).
As the lithium comes out of the special percentages LiCl-KCl mix, more of the KCl would remain. This would necessitate the mix temperature to be higher wouldn't it, making the operation a little more difficult to succeed with?
I agree. Removing lithium from the melt increases the melting point of the eutectic. In this particular experiment, removing less than a gram of lithium really wouldn't have changed much, but it is certainly something to consider for longer runs.
