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 [email protected] . I can't guarantee I'll reply to everything, but I'll do my best to respond to genuine enquiries.
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Excelente...""""!!!!😇🤩🤗
But how do I install that into my vacuum cleaner?
what about Carbon glass electrode? is it better?
Glassy carbon? Yes, they're much better as an electrode in most cases. Still not impervious though.
Sorry to bother you, my friend, but this is the last question about sodium chlorate! When I finish the electrolysis process, I heat the solution and filter it well. I evaporate it completely through a metal bowl until not a drop of water remains in the bowl and only the salt remains. When I mix this salt with sugar, it ignites well, but the remaining chloride in the chlorate makes the ignition a little weak. Is there a way to separate it from Chlorate
Yes. Recrystallisation is the only means of doing this.
So this will probably be the last 5 questions i will ask about this video , 1 being : i have got a glass jar witch will be suitable for my cell but i need a lid that can resist chlorine gas , my lid has got a white coating at the inner part and its metal But i want to know if it will not dissolve or corrode . Question : What material or lid did you use? Question 2 : will any ATX power supply do and does it need to have a specific amperage and what section of the power supply did you use (i think you used the input to the motherboard but just to be sure) . Question 3 : i need to know how much salt i need to add around the course of 20 days Question 4: i have some fiber glass sheet laying around, but with filtering out the hypochlorates, must it be fiber or can i use a small sheet in the funnel. Question 5 : How did you crystalise / dry the crystals because you did not film this in your video 🤔. I hope you will react to this comment.
No worries! Answers are as follows: 1) If it's the type of jar I'm thinking of, the white coating is not enough to stop the lid from being attacked by the chlorine and oxidising solution. You need a jar with a plastic lid if you want to avoid corrosion. The jars I use in my own chlorate cell videos have a thick (~5mm) plastic disc underneath the metal that is capable of protecting it. I found them in a garage sale and I've actually been unable to find anything else like them... 2) Most ATX power supplies will provide appropriate current for any moderately sized chlorate cell. I've never seen one that would be inadequate for the task. For my own cells, I used the 12 volt output hooked up to a buck converter to give me controllable voltage and current. The exact current you need will depend on the surface area of your electrodes, the size of your cell, and your personal preference. 3) That will depend on the size of your cell and how much chlorate you want. This isn't really something that can be explained in a KZread comment alone, so you'll need an understanding of stoichiometry to do these calculations. As a starting point, this website gives an overview of runtime for a certain quantity of starting chloride material: www.chlorates.exrockets.com/runtime.html 4) Is the fibreglass sheet fibrous or solid? As long as liquid can flow through it, it should work. You just want to use it as a filtering medium. 5) I talk about the crystallising and drying stages from 14:03 to 17:50. In particular, I show my method of drying the crystals at 17:01. Hope that helps!
Thank you so much , i will not bother you again about this matter and i will mention you in the description & video 😊@@ScrapScience
My friend, what is the correct way to separate sodium chloride from chlorate? Is it useful to pour ice cold water on it or must it be recrystallized? Please reply and thank you.
It depends on the purity you need. Generally it will require a recrystallisation or two.
My dear friend, thank you for your effort, but please, I have a question that concerns me very much, and I hope you can answer it. My cell operates with an appropriate current, and even the amount of gases generated by the electrodes is normal, but with the passage of two days of not adding more chloride to the cell, the amount of gases increases in large quantities. Is this a result of the decrease in chloride in the cell, or what?
Are you constantly measuring current? Has the current increased or is this extra gas generation occurring at the same current as before?
@@ScrapScience No, the current and voltage themselves did not increase anything, and as for the electrodes, I use carbon electrodes, and as another note? When I want to extract sodium chlorate from the solution, I do not evaporate half the amount of water because the crystallization process does not work for me, meaning the chlorate does not crystallize at the bottom. No matter how much I evaporate half the amount of water and leave it to cool, I do not find any chlorate crystallization. Instead, I evaporate all of the water until only salt remains. Is this the case? It is true, and even if it is true, how do I separate chloride from chlorate after the total evaporation process?
An increase in gas formation still sounds most likely to be from the cell drawing more current as it increases in temperature (this is common for cells that are supplied with a fixed voltage). However, if you're directly measuring current and confirming that it is not changing, it's a possibility that you've begun generating more oxygen as the choride level drops, though this is still a very strange situation. If you're unable to crystallise chlorate out of the cell upon volume reduction, you probably just haven't made enough. Do diagnose this properly, I'm going to need to know a lot more about your cell: How big is your cell (in mL)? How much current has it been drawing? How long did you run the cell for? How much chloride did you add? And in what intervals? Did you include other additives? What are the surface areas of your electrodes? To answer your final question, simply boiling down the cell solution to dryness will give you your chlorate. However, it will definitely be contaminated with significant chloride impurity (as you've suspected), and will need a recrystallisation if you want a pure product. What do you actually need the chlorate for? It's possible a potassium chlorate cell would be more appropriate for your needs...
6:57 "and we will put this other 250ml in..." (without rinsing the apparatus) Grandpa called that: "sloppin' back!"
4:43 can i use PbO2 anode?
That really depends on how the lead dioxide electrode was made. Platinum, MMO, and graphite are almost always better choices.
@@ScrapScience thanks
If i put KClO3 to Cathode and Distilled water at Anode with the same setup would it prouduce Chloric Acid or Perchloric Acid?
I'm honestly not sure. Possibly both.
@@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.
Hello sir I am from India I talk to you sir so you please give me your WhatsApp number?
yeah showing the reaction in youtube. great. lol
The Philippines is one of the luckiest country in the World . Why ? All kinds of minerals could we found in the Philippines like this one at the picture the Deuterium , which means heavy water . not only that can be found in the Philippines , we have also the biggest deposit of oil and Nat. Gas in Liguasan marsh , which according to Sciencetist it holds Billions tons of oil . WPS is coming second , like Malampaya , Spratly ,Benham Rise ,Sulu sea ,Cebu , this was not the end but more to be discovered . time will come the Philippines will be the richest country in the world .
What about epson salt?, ir si cheaper, can i extract nagnessium from there ando sepárate ir from the sulphurim that😀 can be useful as well?
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...
goes into hi-fi territory of equipment pride, use graphite almost always instead
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.
@@ScrapScience okay thank you i will try to find that power supply , thank you for replying and i enjoy watching your videos
What haopens if u use more voltsge... Say 19v or 20v
The reaction will run faster, but at a lower energy efficiency. Additionally, you'll generate more heat in the cell.
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.
Potassium chloride can be taken from lo salt contains 66.6%, sodium chloride 33.3% and magnesium carbonate 1%
2NaHSO4=H2SO4+Na2SO4
Q: can I continue with same process to oxidize NaClO3 to NaClO4 ??
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.
@@ScrapScience Thank you, I hope you make that video
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.
Any sulfate salt will work for this process to some degree when you use this method. I can't say if sodium bisulfate would be any better though.
Realisticly, how much could you make with a 24 volt supply in say 24 hours. I think you mentioned that you made a liter with this method.
That really depends on how big you can build your cell, your electrode surface area, and the current you can draw from the supply.
You should also analyze the product on cathode side, acetate maybe reduced to aldehyde
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.
good talent
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.
whats in the anode pot?
A graphite electrode, if I'm understanding your question correctly.
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.
Are you using a glazed or unglazed pot?
Unglazed. Glaze will block the movement of ions.
@@ScrapScience Thanks, it was kind of hard to tell from the vid.
Best exclusive explanation
Best exclusive explanation
how to Ion move to Clay Pot . when clay pot is Isolator .. ?
The clay pot is porous. Ions can move through the water that's soaked into the structure.
"Yo!... Mr. White.. This is Glass!" ;-)
Bravo.......screw magnesium.......it makes hydrogen .......when u put in water........measurements how much yield......also reactor with gas shield.....cheers
Why didn’t you just test the liquid in the other chambers ? Maybe the hp wasn’t going through the ceramic
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?
I'd like to send you a sample of pytolitic graphite for a future video I'm sure you are smart enough to make a awesome video using it. 😊
Diamond's are forever untill you heat them up and submerge it in pure o2 😂
Does the carbon rod will be eated and degraded by the electricity??? Or it will remain the same after that??? If yes, what cai use instead of them???
Yes, the carbon degrades when used for this process. The only common electrode material that doesn't degrade in this process is platinum.
Is the water level actually running over into The large container or is the clay pot absorbing the water ?
If it is a very soft metal, why would you try to melt it into one piece? You could just hammer a bunch of them together into one ingot.
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.
Why didn't you boil it
I don’t need it to be concentrated. I also don’t like to deal with boiling hot sulfuric acid in any capacity.
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.
It takes much less time if you neutralize extra acid.
can i use titanium for anode and graphite for cathode?
No, but you can do the exact opposite.
@@ScrapScience but if use graphite as an anode, it will dissolve with chlorine and pollute the electrolyte. Does titanium has corrosive resistance from chlorine?
Hello. I have a question. Can I use carbon electrodes for both cathode and anode? And the current at the few first days can rise???
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.
Okay I will try it, thanks for response. Your film is very good, I learned a lot of things. 👍🏻