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Does this mean ebonizing wood with iron (II) sulfate also produces small amounts of sulfuric acid in the wood after the iron tannate complex forms? I know you say it doesn't work with other acids but if they weren't reacting there wouldn't be tons of black complex crashing out and dyeing the wood.

I wonder if you can boil it and then boil the secondary solution and repeat the process a few times. If ammonia leaves before H20

There really is no excuse for a bad manual anymore. That one looks like a 40 year old Xerox of an 80 year old book.

59:53

Following this channel since 1999. Great stuff as always.

How do you trap the gas in a container?

Does using electric to tarnish Platinum Palladium and rhodium differ from the tarnish of silver? I guess what I'm asking is do they produce their own colors differently than silver?

Amazing stuff man I'm just imagining like what woman does not want some pretty blue purple rainbow silver coin in her purse when we switch back over to the hard currency it's going to be an emotional thing to both give and receive for whatever the work is it makes more valuable the moment of your life.

Gotta love me some good reducing agents ;)

it was really usefull,thanks a lot.but i have a question. is this possible to connect the negative end of the battery to the aluminium foil?

Awesome! Where do you get the radioluminescence tritium ligths?

Hi NR, I have a few ideas for you to try: You can use the cheap coil hotplate if you use an appropriate heat spreader. Try using a heavy bottom stainless steel frying pan of the type used with induction hot plates. It will survive acid spills at the working temperature of this process. It will also help if you use a heat transfer fluid between the pan and the bottom of your flask. I would suggest a molten salt eutectic of 60:40 mixture of sodium nitrate and potassium nitrate, which is a liquid between 260-550 °C (500-1,022 °F). You won't need much. This is easy to make and pretty safe since you have no organic material nearby, and will survive acid spills with only a little release of HNO3 vapor at operating temp. Just don't let the salt freeze around your flask during cooling. Raise the flask or lower the pan. Your process is at the upper limit of silicone heat transfer fluids, so they are not very stable and may smoke or gel. There are previous suggestions of a sand bath, and while this could work, thermal conductivity and thus temperature controllability is poor. Use a fluidized bed system instead if you want to use this approach. In any case, use a stainless steel sheathed type K thermocouple in the molten salt or sand near the bottom of the reaction flask with an electronic PID controller like a REX-C100PID to closely regulate your temperature, the same as you could use with a Glas-Col mantle. The PID controller allows you to tune and compensate for the thermal mass of the heating system and is much better than the older SCR type heater controls. For your safety catch pan, use a kitty litter tray or steel tray half filled with dry clay type kitty litter. It will safely absorb a hot acid spill. I looked up the prep: Preparation of Sulfur Trioxide and Oleum, by GARAGE CHEMIST on ScienceMadness.org: He has some useful ideas. His use of Sodium Peroxydisulfate (Persulfate) is interesting. The advantage over Sodium Pyrosulfate is that it is non-hygroscopic, so it can be dried completely at low temperature. It decomposes at 180 °C to O2 and dry Pyrosulfate, so there is no water to distill off prior to SO3 production. If this release of O2 happens in solid phase, (I think this is the case) it would be a handling advantage. GC used a *small* amount of concentrated H2SO4 as a decomposition catalyst to lower the reaction temperature, much less Sulfuric than you are using, and this should improve yield. Distilled concentrated Sulfuric still has about 2% water due to high temp decomposition of vapor. This decomposes some pyrosulfate before SO3 is formed. This is why your use of 2x sulfuric acid gave lower yield. It looks like the Persulfate plus small amount of Sulfuric in the GC setup is a slightly damp powder, and remains so, which would eliminate any need for a stir bar. Your Erlenmeyer flask is a better idea than his RB flask for purpose of even heat transfer. Persulfate is commercially made from Bisulfate by electrolysis. I wonder if it could also be made by adding an appropriate amount of 30% H2O2 (or even 3%?) to the Bisulfate and gently heating to dryness? If so, this would be an easier route to Pyrosulfate even for regeneration of residual Na2SO4 for later batches. You might have to break up caked Persulfate. If it works out right, there will be no initial distillation of water before SO3 production, and no molten salt to deal with, so yield will improve. At worst, you might get some Piranha. There is no need to collect the water in a pre-distillation. You can just let your blanketed reaction flask vent to the air until it starts to fume, then you can install your short-path condenser. This keeps your glassware dry. Another observation is that it looks like there would be an advantage to adding some Sodium Bisulfate to a batch of Sulfuric acid when distilling the acid to obtain 98% concentrate. This might prevent bumping and eliminate need for stirring. How much? IDK, try empirical. Maybe a little, or maybe a lot. Erlenmeyer flask looks better than RB in this case too. Less trouble even if it does bump. I don't have an appropriate safe setup for this ATM or I would try it all myself. Regards... D

Centrifuge.

The over-unity wackos might see this video and say HHO! HHO! Free infinite energy! Just hook the electrodes together with a light bulb! I sell plans online!

I have been watching your videos for so long it's ridiculous; I just have a quick comment on a possibility for an improvement in this one. Would there be any possibility of improvement in the copper method using a very fine Celite? Or rather more specifically, would you be able to separate an extra fine celite powder from the distillate and then be able to use the resulting solution? Unfortunately instead of my original college degree being chemistry (like 7 years ago), I decided to go with Finance, so I truly don't know if there's any major issues with this thought, but if you or anyone else cares to respond, I would be thrilled to gain any knowledge y'all have about this process!! =)

Please tell me where I can buy this elemen. Or what name of this element?

Naw that little baby round bottom boiling flask!

this looks like it should be agonizingly painful...

I feel like if you could continuously filter the precipitate out the magnesium yield would go up. Like use a cheap aquarium pump to cycle it through a filter. Might take longer but bulk processing "hands off" is still pretty good.

Excellent! after googling I found that iron sulphate heptahydrate is = ferrous sulphate, te one easy to get that I use on the garden. Oxalic acid is also easy to get as wood bleacher.

F****** orbeez

Nitric acid seems really expensive. Is it worth the time and inputs to make it in my own lab instead of buying it?

So like...... IS THIS LEGAL, PUT IT IN A CONTAINER AND YOU MADE A BOMB.

What the hel for ?

6:00 As a reducing agent you can use regular iron wool. It reduces Fe3+ to Fe2+ while going in solution as Fe2+, gives a purer product and can be easily filtered off.

❤ interesting 😎

It's crazy to think how much my life has changed since first finding this channel. I have got married, had a kid, bought a house, paid it off, and had my 12th anniversary in the meantime. The videos have stayed at the same high quality. No annoying sponsorships, no over the top clickbait, just good repeatable information. Here's to another 15 years or so, Mr. Rage.

Do you have a project you're working towards? I'm trying to see if the last few videos are forshadowing anything.

Oh it's SUN light. I was wondering what the devil sulphur uranium nitride is?

Excellent. Thank you

That odd moment when Barkeeper's Friend is for more than just cleaning up brightwork.

How does the yield compare to dry-distilling the Iron Sulphate directly, like back in the days of alchemy? Suppose I bought a 50lb sack of the stuff because it's not particularly expensive, and making an iron retort isn't a problem.

I hate it when the reaction is making weak ass ids.

From a molecular bio approach, I think centrifugation is probably the best way to seperate the milk of coppernisia you made, though this requires a centrifuge. If you have one already this might be worth exploring

I do enjoy the clarification of parallel methods that may (or may not) work. It's fascinating how transition metals with supposedly equivalent behaviors end up being entirely different when you go to try the method. Should the metal oxylate form? Sure thing. Does it? Probably. Can you separate it? Not at all, yes, and maybe.

Sweet. Great to see more accessible syntheses.

Do you think aluminium sulfate could be used instead of ferrous sulfate. It is also insoluble in water, so it should be nearly the same reaction, or is there something more to ir

Será que não dá pra fazer ácido sulfúrico com ácido sulfamico + ácido nítrico??

Pretty sure you are some kind of genius

that clip of Astarion yelling about sun was so unexpected i nearly choked on my tea.

Please make sure the video is not blocked off by 2-minute unskippable ads of lame games. Could not watch the video to the end, and I'm not staying around for 2 minutes of a game ad.

Don't they usually use some polyaluminates to flocculate more effectively? great vid tho. I really thought the magnesium would work; ion radii are similar so you'd think it would just electrostatically sort of work out... clearly more going on of course :)

Ahh...the forbidden Blue Milk.

Is the yield of the se reactions Better than electrolysis of copper sulfate?

so to get artound the dirty filtrate i put one filter a top another and put it on a stand and yeah worked great 2 filtering steps and its clear as anything this was the calcium nitrate method is viable for me at least its very pure NaNO3 from this process of dissolving it the calcium form and then adding sodium carbonate which produces the same chalk like white paste of just calcium carbonate (i think) im not a chemist by any means just an amateur with a hobby and a love for the science!

I bet you are unaware of the impressive number of people that became chemists fom your inspiration just by simply helping me pave my way to it since I made sure to perpetrate the passion for it and I'm pretty confident I'm not the only one.

All through this video, I was thinking about the big bag of copper sulphate out in the shed... so thanks for answering my inevitable question without me even having to ask it. :)

Up next sulphuric to pure sulphur ?

Would alum help the copper oxalate settle?