Lab Notes - Failure in Making Sodium Nitrite
Vložit
- čas přidán 20. 10. 2023
- In this video i synthesize nitrosylsulfuric acid and isopropyl nitrite, and i tried to make sodium nitrite but i failed.
My original goal was to make sodium nitrite. Sodium nitrite sets itself apart from the more common sodium nitrate by having one less oxygen atom, which makes it quite unstable under various conditions. This particular challenge intrigued me, and I thought I'd give it a try, even though I knew it's notoriously tricky for amateur chemists like me to produce.
I wanted to develop a low-temperature method, which involved several chemical reactions. I began by crafting nitrosylsulfuric acid from fuming nitric acid and sulfur dioxide.
Having successfully created nitrosylsulfuric acid, I moved on to the next stage: generating isopropyl nitrite. The idea was to eventually use this compound to produce sodium nitrite. The formation of isopropyl nitrite was quite intricate and required careful temperature control to keep the reagents and products stable.
I attempted to break down isopropyl nitrite into sodium nitrite using sodium hydroxide and methanol but this failed. I ended up with the decomposition of isopropyl nitrite instead.
But at least i found a way to make isopropyl nitrite without starting with nitrites.
Donate to NurdRage!
Through Patreon (preferred): / nurdrage
Through CZcams Memberships: / @nurdrage
Twitter: / nurdrage
Reddit: / nurdrage
Instagram: / nurdrageyoutube
Do you guys want me to make a proper isopropyl nitrite video from this?
Usually, its best to operate on principal to see something the whole way through. You started, so you'll finish. Knowing you, you won't be happy with failure, so the only reason you asked this is because you must be busting to get at some other project your excited about. Otherwise, if youre gonna do something, do it right..
Evan faillure can teach U how to NOT DO That ;)
Yes
Yes
There is very little content on CZcams covering successful nitrite synthesis, so I guess we would all be interested in more videos about this topic. Maybe the alkyl nitrate can be converted to sodium nitrite in less harsh conditions, would appreciate if you invested in another attempt
While I don't think there's much if any use for isopropyl nitrite offhand, I really appreciate this failure video, because failure is the mother of learning, and it's always interesting as a layperson with an interest in science to see things like these and whether or not they pan out or not.
It's mostly used for rec-reational purposes
I commented a few years ago but wanted to give an update: I started watching your videos back in 2009/2010 when I was in 5th grade, Im currently in my second year of getting my PhD in physical chemistry and definitely wouldnt have done it without your content.
wow that's amazing! I'm also sorry for ruining your life ;)
@@NurdRage my life has only gotten better the more ive learned. But you sitll share that blame ;)
Glad you are posting these sorts of videos to show that research isn’t all success and the pathway to discovering things isn’t always linear!
"Research is what I'm doing when I don't know what I'm doing" - Dr. Werner von Braun. You're in excellent company. Keep it up.
Would really love a series from an actual tinkerer like Nurdrage who tries things out on a solid procedure for making sodium nitrite. Ever since that kid unalived himself and parents flipped out at lawmakers, it’s been impossible to get for anyone in the US.
More failure videos please. Everyone puts out successes and makes it look so easy, but it isn't. It is the dozens of failures which actually impart knowledge.
i’m excited to watch this :) so happy you’re still posting videos!
Great video as always! Love the lab notes videos! Even when it doesn't go as planned there is still a lot of lessons to be learned.
👍
Well I did not expect to see the synthesis of such a party chemical on your channel XD
I remember using similar nitrites for making diazonium salts in anhydrous conditions, it was a very special use case, but still worth to be known about.
As for the idea, it may be not as farfetched as you think, but you overshoot it probably XD I found that one of the papers mentioned the stability of nitrite during organic nitrite hydrolysis, and it seems buffer is needed, and a bit of acidic pH with halide nucleophile. But maybe I read the papers wrong.
References:
Nitrosation by alkyl nitrites. Part 5. Kinetics and mechanism of reactions in acetonitrile; Michael J. Crookes and D. Lyn H. Williams
Kinetics of the aminolysis and hydrolysis of alkyl nitrites: Evidence for an orbital controlled mechanism; P. García-Santos, E. Calle, S. González-Mancebo & J. Casado
Evidence for concerted acid hydrolysis of alkyl nitrites; Emilia Iglesias, Luis García-Río, J. Ramón Leis, M. Elena Peña and D. Lyn H. Williams
Kinetics and mechanism of the nitrosation of alcohols, carbohydrates, and a thiol; S. Elaine Aldred, D. Lyn H. Williams and Michael Garley
Hydrolysis, nitrosyl exchange, and synthesis of alkyl nitrites; Michael P. Doyle, Jan W. Terpstra, Ruth A. Pickering, and Diane M. LePoire
Thank you for bringing us along on the success and the failures. I had/have a bit of a learning disability so chemistry was not an option in public school but you Cody's lab poor man's chemist and AvE have enriched my life so much thank you and I love you
Glad you're still active, been watching since I was 10!
🤯
I think the nitrosylsulfuric acid production is quite interesting just by itself. It is unfortunate that it needs RFNA, but the product can do some of what you would use the nitrite, like making organic nitrites, diazoniums, etc.
Great stuff! Failures are in some ways more useful than success.
Hope to see you follow through and succeed in the synthesis!
The easiest way I found to make nitrites happened by accident and early on. I was a pyrotechnics nerd back in the day and I tried to eyeball firecrackers flashpowder, recognizing a gray powder. It never dawned on me that aluminum would find use in fireworks at that age, so I assumed the ratios I'd been told for "flash" black powder (6-1-1) were by volume, not by weight, so I did that, ending up with a gray powder--one that didn't burn that well and oddly seemed to leave these little puddles that would solidify as a cement that looked like dried toothpaste (white toothpaste) albeit with weird color patches in it. This turned out to be slightly decomposed KNO3 or NaNO3 (I was using fertilizer grade so it was likely NaNO3) and was a combination of assumed nitrate salt and nitrite salts. A simple test is to break a piece and drop it into HCl, noting the NO2. I found the most efficient way to get nitrites is 1/1 up to 2/1 nitrate to sulfur by volume. Mix to homogeneity, burn, collect cement that forms. It's effective for amateurs.
A formal procedure for isopropyl nitrite as well as isopropyl nitrate, along with an explanation on why the methods differ so much despite ending up with so (relatively) similar compounds would be interesting.
the lab notes do offer invaluable insight from the perspective of a professional, and reminds me as a chem undergrad to never neglect my own lab notes in the first place. undergrad lab sessions do suck and i know it'll get better once i start my master's year because there's always room for errors at that point, unlike undergrad where you have everything breathing down your neck everywhere! i wonder how benchtop nmrs would sound (if it is within your budget) to look for binary indicators of product in the first place. as always, thank you! you are i believe the first to inspire me to undertake the path i'm on now and that was many years ago now...
Both Nitrosylsulfuric acid as well as isopropyl (or many other alkyl) nitrites are absolutely useful chemicals that can be used for further synthesis. Alkyl nitrites are frequently used as mild nitrosating agents, e.g to make Nitrosoresorcinol, nitrosophenol etc from which you can make interesting dyes. So yes, please go ahead! :)
Bubbling nitrogen oxides from dissolving copper in HNO3 through a NaCO3 solution works quite well and you can recover the HNO3 by decomposition of the copper nitrate.
really cool process to see.
Interesting video as always! Failures are also knowledge, thanks for posting it. Nice intro xD
I don't think a proper video and procedure on how to make isopropyl nitrite is necessary, I don't really see a use for it and if someone really wanted to make it, this labnotes video is more than enough. The nitrosyl sulfuric acid part is very useful! I never needed it, but that's definitely a good thing to know.
Thanks for sharing
Hey! I suppose that you needed to use a tertiary alcohol, not a secondary one to make the nitrite.
Tertiary carbocations are more stable and have a higher rate of success with nucleophilic substitution, if you can stabilize the leaving group properly. A basic pH and the size of the NO2- leaving group should be enough for it. This could work better than the Sn2 mechanism you were trying to go for.
Also the Sn1 reaction, that the tertiary carbocation nucleophilic substitution follows requires polar protic solvents, so you don't need to worry about anhydrous conditions. So for example you could start from t-butil-alcohol, make it into t-butil-nitrite and put it in a solution of NaOH or KOH. Just be aware of the flame danger.
Very cool !
Very interesting! It's unfortunate the hydrolysis of isopropyl nitrite results in tar, otherwise it would be a useful route for purifying nitrite via thermolysis too. That's great way synthesising nitrosylsulfuric acid though!
@NurdRage I´ve seen good wields of sodium nitrite when it comes to reaction which involves heating a mixture of sodium hydroxide and sodium nitrate while slowly and carefully add bits of sulfur from time to time.
Potassium nitrite is much easier to make yust by heating a mixture of potassium nitrate and calcium formate until it starts to.react. After letting it cool down the mixture is suspended and the suspension filtrated: the nitrite is in the filtrate then and has to be boiled down until all impurities cristallize out. The decanted supernatent contents our desired pure nitrite and can be evaporated hot to dryness.
I made a video about this precudere on my channel.
So you did. Nice video and nice channel.
Interesting, I'll take a look
@@rodneyvinen1594Thanks.
@@NurdRageThanks.
the OG of the youtube science community
Fantastic work!!! Your videos never disappoint in any way but educate with great details.
Also do primary and tert alcohols work too with this method ?
Yep! It's a broadly applicable method
Great
The problem may be hidden in the proton near OH. Isopropanol has always seemed to me as somewhat more reactive alcohol. Once I added a bit of 68% HNO3 to an isopropanol in a test tube and it went nuts a mad 30 seconds later. I would try distillation of the ester and hydrolysis in an aqueous solution to prevent a too basic environment from appearing. It's more painful to purify than just suction but maybe (I'm not about to guarantee it) will work.
Love this channel.
He's like the grizzled adult version of NileRed.
Have you tried the sodium nitrate/calcium sulfite method? You said you didn't want to use a high temperature method, but it only requires 300C.
I think that sodium azide can be made by using isopropyl nitrite in reaction with hydrazine. Sodium azide is interesting and very useful chemical, so making a video about that will be nice.
Nice one NurdRage. The old book I read said that if you melt sodium or potassium nitrate in an open crucible, then drop in charcoal powder a bit at a time, which goes up in flames. You keep adding the charcoal till it no longer combusts. Then you wash out the remaining salt, filter and crystalise to purify. But actually, I'm not 100% sure the resulting salt is a Nitrite, as the book is old and different terms are used. It was an assumption on my part. Does anyone with experience know if this would result in a Nitrite? If not, what else might it be?
I would suggest to modify the experiment. Adding water to the NO(HSO4) will decompose the intermediate and generate dinitrogen trioxide (N2O3). This gas can directly be used to form sodium nitrite or isopropyl nitrite. There is no need to isolate the intermediate.
now this is a subject dear to my heart; one of the very first projects I tried was making inorganic nitrites, with very mixed success
the big drawback with high-temperature methods is the poor purity of the end product, not least because it's readily oxidised to nitrate in air at the temperatures the reaction is carried out at - an inert atmosphere is essential
for a while I've actually had half a mind to prepare inorganic nitrites this way, and I'm delighted to see it done in practise
here's an idea: would it be worth diluting it in conc. sulphuric acid before adding it (dropwise) to a cold sodium hydroxide solution?
I immediately knew the problem, when he got methanol and sodium hydroxide...I literally just said "idiot" over and over again 😂
out of curiosity, what are some of the sites you got to (besides ebay) when looking to get labware (new or used) on a budget?
Great video as always
Nothing special I'm afraid, most eBay, Amazon and AliExpress
So far the most convenient nitrite production I found is roasting metal or metal oxide with nitrate e.g. Cr2O3 with sodium nitrate (the side product is sodium chromate - also useful chemical).
Another option is heating nitrate in a metal pipe over fire with somewhat controlled temperature - then nitrate and nitrite are separated by means of solubility. More precise separation of nitrate and nitrite is possible but takes more steps - this is often not necessary (some nitrite will inevitably oxidize to nitrate anyway).
Vogel also mentions nitrate reduction with zinc in alkaline environment but I haven't tried yet.
"separated by means of solubility" could you expand on that? From what I saw is that nitrate and nitrite solubility are almost the same in various solvents
@@user-py9cy1sy9u "separated by means of solubility" means you shall regret the whole procedure you're trying to do
@@user-py9cy1sy9u Sorry I wasn't concrete enough. Both salts are generally soluble but potassium nitrate is considerably less soluble than nitrite and might be removed by fractional crystallization (it should precipitate preferentially - but I haven't tried). The solubility can be decreased by common ion effect. Barium nitrate is even less soluble compared to corresponding nitrite but it can be removed more completely by just heating the solution (it will decompose). If lead was used for nitrate reduction, then residual lead nitrate can be decomposed by boiling in anhydrous methanol. Both barium and lead are toxic but can be removed by bubbling carbon dioxide through solution (in case of lead, dissolve it first in alkali as plumbate, then add CO2). If you already have a mixture of sodium salts, I think one possible separation is with calcium hydroxide - this will precipitate double salt of calcium nitrite-calcium hydroxide that will redissolve in more water. Conversion to sodium nitrite can then be done by double displacement and removal of insoluble calcium salt by filtration. Some separations are possible in form of other double salts and mixed crystals, but there are various eutectic mixtures. See e.g. "Ullmann's Encyclopedia of Industrial Chemistry - Nitrates and Nitrites"
intresting
Cool
Gonna show this one to my organic chem wife later, she'll *love* it :D
Thank you
I am NOT laughing at your results as your efforts and work were GENUINE. What I would suggest is to reduce sodium nitrate in various ways. Sodium nitrate melts at about 306C and sodium nitrite starts to decompose at 320C. There IS a narrow window available! I would guess you know what a temperature controller is[with a relay]. If you have a Nichrome or Kanthal wire firebrick oven, why not set the lower temp at 306C and the upper limit at 320C?! The hot black wire[inside the oven power cord] is cut and insulation stripped to connect one wire to relay screw and the othe wire connects to other relay screw.I would try heating 0.5 mole or 1 mole NaNO3 for 1 hour. A second idea is to reduce the NaNO3 with tin metal shot to possibly improve the yield. NaNO2 has been made with lead with 72.5% yield. Lead does not melt until 327C which is actually in the decomposition area of NaNO2. Tin melts about 232C and has lower atomic weight than lead. Tin is less toxic than lead and is more costly than lead. If all goes well you should get NaNO2 and stannous oxide.Please make video on these ideas! I was VERY IMPRESSSED with your synthesis of nitrosyl-sulfuric acid!
wow this is amazing video one question though! how water should I add with sodium hydroxide to dissolve the flesh of an farm animal that is exactly 152pounds? 🤔🤔🤔
this is easy: Potassium Nitrate + Sulfur + Sodium Hydroxide ignite the mixture (outside). Presto: Potassium Nitrite.
If you want a very expensive way to get purify sodium nitrite, here's one way I did it.
No matter how you can the impure nitrite, you add calcium or magnesium nitrate to precipitate insoluble carbonates and hydroxides. Filter. Then add silver nitrate to the solution and it will selectively precipitate silver nitrite. Filter the silver nitrite. Add sodium chloride to the supernatent to precipitate silver chloride.
Dissolve the pure silver nitrite in water and add sodium chloride and boil it for a while. It will precipitate silver chloride and leave behind pure sodium nitrite solution. Evaporate the supernaturnt under vacuum for best purity sodium nitrite.
Recover all the silver chloride and decomposite it under heat to pure silver. If you're very efficient, I think you can recover almost all the silver and reuse many times. One ounce of silver will probably get you 15 grams of nitrite so it's extremely inefficient. The biggest loss is having to remake silver nitrate again.
thats a pretty good idea! i'll keep it mind for purification.
Would this work with copper nitrate?
@@LFTRnowI'm not sure how stable copper nitrite is. If you mean to use copper nitrite to displace carbonates and hydroxides, then yes it would work.
Could the isopropyl nitrite be decomposed with a strong, non-nucleophilic base like NaH or NaNH3? Elimination reaction to give propene and NaNO2, plus either H2 or NH3
I have always wondered how well the method of bubbling nitrous oxides through an hydroxide solution works. How easy is it to separate the nitrite from the nitrate? According to the literature is just about solubility, but what is the yield? And couldn't feeding the nitrate back into the reaction lead to a somewhat quantitative yield, step by step?
Have you tried the NO2 + NO gas into NaOH method for sodium nitrite yet? It seems to be a promising route.
Isopropyl nitrite is useful in making Sodium Azide with Sodium Hydroxide, ethanolic Hydrazine and catalytic amounts of the nitrite. So, it's useful, for sure. From memory.
Nice! Wouldn't sodium nitrate thermally decompose into nitrite? I remember from Wikipedia that it happens with potassium nitrate and quick google search suggests that it should work with sodium nitrate too.
you should recreate the nitrosylsulfuric acid and then use it to prepare a few azo dyes!
I’m working with NHO3 and Hg, are laytex gloves alright because it’s what I have been using….I’d rather avoid a horrible death from Mercury poisoning…
you just heat up NaNO3 and Cu metal powder, then you melt the nitrate for maybe 20 minutes and you get quite pure nitrite
either electrolytic copper sponge, or more effortless: CuCl2 + Al = Cu + AlCl3
for CuCl2 you wanna wash the formed Cu with NaOH otherwise it gives an strange smell
Cu2O also works, the CuO formed can be turned into Cu2O with glucose + NaOH, boiled for an amount of hours, otherwise CuO + HCl might be used rather
original recipe was posted as Cu from CuAc decomposition, thermal + KNO3 but i have frustrating results using KNO3 for some reason, NaNO3 seems more willing.
also removing oxygen helps with nitrite yields, butane may be helpful for this.
Can someone please help explain why the reaction didn't work?
I am just an amateur but my guess is in the reaction the the methanol competed for the NaOH and form sodium methoxide and other side products.
@NurdRage So I am new to the home chem realm and am accumulating the labware needed.. How many cheap amazon vacuum pumps should i expect to go through in the first year or so? I imagine things like nitric acid or very basic solutions will be hard on the pump and tubing.. figure ill just buy 2 or 3 so im not out of one when i need it, but i didnt know what to expect and that you might have some words of wisdom lol
oh my, you shouldn't be destroying vacuum pumps! The "Rotary vane" or "reciprocating" vacuum pumps you see on amazon SHOULD NOT be used for hard chemistry! They'll get destroyed. Something better for chemistry is the "water circulating vacuum pump". You need to fill them with water first, but they are much more resistant to chemicals. You still have to maintain them and change the water often, especially after a heavy experiment. But they are great and robust compared to rotary vane pumps.
Never suck actual liquid into a vacuum pump no matter what type it is. Vacuum pumps are for gas, liquid pumps are for liquids.
The vane pumps on amazon are good for refrigerator repair and degassing, they're designed for safe gases like air. But anything even slightly corrosive destroys them.
Daaaamn. Thats a ton of poppers rage us gonna be huffin that for a while lol
Would electrolysis of sodium nitrate with silver electrodes or platinum work in driving off some oxygen from the nitrate ?
i'd probably like to see some uses of isopropyl nitrite first
Isopropyl nitrite I made with homemade sodium nitrite (molten NaNO3 + NaOH, then sulfur added) decomposed into a similar orange sludge upon sitting around a few days. IPN made with boughten sodium nitrite lasted months. Perhaps your problem is due to impurities in your IPN, not the method of converting it to sodium nitrite.
Why not try membrane electrolysis? There is a patent out there that uses electrolysis to produce high purity nitrite from nitrate salts.
It would be very cool to see someone exploring this approach!!
Some patents, that describes this are e.g. EP0713928B1 and EP0713928A1.
The interesting part is, that a special cathode is used from silver with high surface area or metal-doped carbon.
Yet, it seems not to be too complicated and although there is no explicit example efficiency seems to be high with no nitrate left in the end. So workup would be simple.
isopropyl nitrite huh? One whiff and I bet you could take a Erlenmeyer flask.
Exactly what I thought when I first saw isopropyl nitrite lmaoo
I re-read "take a Erlenmeyer flask," two or three times before I connected the dots 💀
HAHAHA@@tnebt
Maybe try bubbling NO2 into a sodium carbonate solution?
You could wash out unreacted sodium carbonate with methanol.
6:56 So, what exactly is the sludge? Interesting that such small molecules could yield tar(?) in such reaction conditions.
Thumbnail looks like this candle with candy trash I got off in and left between my bed/nightstand partially covered for like a good month.
Swear I heard it talking one night.
I think the reason it failed is because your sodium hydroxide actually has small amounts of water in it that caused the reaction to fail. Another source of failure is that sodium hydroxide actually reacts with isopropanol to produce small amounts of sodium isopropoxide and water. The water then quickly decomposes any nitrosylsulfuric acid to regular sulfuric acid and nitrogen oxides. Feel free to correct me if I'm wrong though!
question, why not add the nitrosyl sulfuric acid to sodium methoxide in methanol instead of sodium hydroxide in water?
Dear, can you make ammonium perchlorate in a possible way?
I'm not a chemist, so how do you clean up after creating these experiments?
Please show a method of making sodium nitrite. It has become hard to get!
Only thing I know about Sodium Nitrite is it's used in those pink preserving/curing salts used in meat products to kill off unwanted nasties and make stuff like canned meats and ham & bacon a thing, though reading up on it, the stuff you buy is mostly made up of regular salt (sodium chloride) with a sprinkling of the sodium nitrite, so, probably would be a PITA to extract it I guess... :\
Pro-cure sells pure sodium nitrite as bait curing salt.
It's always a good day when you post! I noticed something in your disclaimer.
It reads "outside or in a fume hood." But it should be "outside, or in a fume hood".
Technically, everywhere is outside or in a fume hood. 😂
Sir please make full process of potassium nitrite
You could try reducing nitrate to nitrite with hydrogen gas.
It doesn't work but I like that you're thinking
reduction is possible but not with hydrogen - either alkaline zinc or reacting nitrogen dioxide over sulfite (if I remember an old patent application correctly)...
What if you mixed the isopropyl nitrite with another sodium salt like chloride? Could that preform the ion swap and let the sodium nitrite precipitate out? Im also an amature chemist trying to figure this out haha
Could be worth trying to make sodium nitrite by heating a mix of sodium nitrate with calcium sulfite (which, in turn, can be made of sodium sulfite and any calcium salt, like chloride). Same way it could be possible to make a mix of sodium nitrite and sulfate (which wouldn't interfere most reactions) by heating sodium nitrate and sulfite (or maybe metabisulfite with addition of lye).
That much RFNA going to waste could make a grown man cry
you could just react nitrogen dioxide with potassium hydroxide to make a mixture of potassium nitrite and nitrate. Then separate them using freezing cold water as the nitrite is way more soluable than the nitrate.
Potassium nitrite is very similar to sodium nitrite and you (probably) should not have any issues using it
Even a failure results in more knowledge: "don't do this next time".
When can you update on Bilibili? Friends in China are very worried about you and hope to see your videos again
Hey could you or someone please tell me how/if you can separate petroleum and methylene chloride, there’s a local paint striper here that contains methylene chloride but also petrol and I see they have similar boiling points
Is there a solution that one or the other is soluble in but not the other
I would like to see some videos about making chemicals That would be very handy during a nuclear apocalypse When you don't have the chance to go out and buy from a shop And just have things laying around
Is it possible to use electrochemistry to reduce nitrate ions? Of course if the nitrite is easier to reduce, the whole idea is dead, as it will get further reduced.
Possible and its slow
@@user-py9cy1sy9u Slow as in days or as in months? If the cell does not require attention speed is not a problem, just leave it running in a corner for a week.
@@TheBackyardChemistsearch for "Making Nitroethane With Electrolysis"
That video is fake. Notice how he conveniently fails to show any video footage of the final product work-up or product characterisation? Instead he just cuts to waving a bottle around and claiming success. Also notice in the comments how he conveniently ignores ALL questions regarding product characterisation? @@user-py9cy1sy9u
@@user-py9cy1sy9u What tells you, that it is slow? There are patents and other studies out there, that let it seem pretty feasible.
The trick is probably to use a special cathode material with a high surface area (silver sponge or cu/ag-doped carbon) and also other conditions (e.g. to prevent reoxidation at the anode) to keep the efficiency high.
Could you use this method to produce nitromethane?
not nitromethane, if you tried reacting nitrosylsulfuric acid with methanol you get methyl nitrite instead. Nitromethane requires a very different process. But it's not too hard to get as a solvent so it might be more straightforward to obtain it that way.
Thank you so much for our answer. I found on wikipedia that when producing methyl nitrite from iodomethane and sodium nitrite reaction yields mostly nitromethane because nitrogen is more nucleophilyc so MeONO converts to MeNO2. In the same article it says that MeONO can be prepared by reacting iodomethane with NO2 gas. Maybe one could substitute iodomethane with sodium iodide and produce sodium nitrite that way?
Is it really so hard to buy NaNO2? It is a food additive, among other things.
Yeah I can't buy it anymore where I am.
The main contributor to scarcity, at least in the US, was a highly publicized teen suicide and the ensuing outrage, which caused it to be banned from public sale.
When people started to kill themselves with it then it became hard to get. At some point amazon's algorithm bundled all things necessary for this task...
I know you can make potassium nitrite from the electrolysis of potassium nitrate with inert electrodes I bet the same thing might work with sodium nitrate
ok but... what actually is the case at 6:39 ?
Isoamyl nitrite???
Poppers?
is this salt used for curing bacon 🥓 or is that the nitrate salt ?
Both nitrates and nitrites can be used , and the more organic methods use celery juice powder which contains a high amount of both salts , for those who implicitly believe there is somehow a difference between 2 identical molecules .
The answer is in nature.
At least it’s not yellow
My fish tank produces a ton of Nitrite, can't I just dump some Sodium in and BAM, Sodium Nitrite?
The amount a tank produces is extremely tiny, it's just super killer to fish which is why it must be monitored.
@@NurdRage Not to mention the small problem of the exploding fishtank
@@Ms.Pronounced_Name neither situation is possible. Nitrite in fish tanks is measured in parts per million.
Safety note, isopropyl nitrite is very toxic to human retinas. Exposure can affect eyesight over time.
To much yellow
The sign of failure was there from the start :)
Any amount of *yellow* is too much *yellow*
Hello, Chemist! I am your fan from bilibili! Why don't you post chemistry videos on bilibili anymore
The company that did the localization work stopped contacting me.
Don't fix what ain't broke
يرجى اضافة اللغة العربية
I love your contents, you are a very good CZcamsr, can I get comment heart?
When o when will all this knowledge be just a calculator program you can just punch in result or input chemicals and get an answer :D