Part 2 of the Boron video. See Part 1 here: • Elemental Extractions ... And here is a link to my blog post on the research I've done regarding this reaction: thehomescientis...
Holy smokes man, I remember watching your videos year's ago, awesome to see you back, you probably had a helping hand in my decision to pursue a career in a chem related field. I probably watched your nitric acid synth video 20 or 30 times and eventually recreated it on my own. Keep up the awesome work!
Considering the "green color" disappeared when you added more water, I'd take a guess it was copper chloride. The HCl and copper probably reacted with O2 from the air as a catalyst as it sat out over those couple of days. Normally the copper wouldn't dissolve in HCl, but after that amount of time enough oxygen could have diffused in.
For carbon just do the classic carbon pillar experiment, smash the product and wash it with a base and water, dry it and grind it, you can run it thru few acids but this isn't really needed, I did it some time ago (but I didn't film it) and it was quite pure actually
I think the green colored solution came from the iron in the stainless steel crucible that was your reaction vessel. At high temperatures iron will bond with oxygen to form a black iron II oxide, and this will react with hydrochloric acid to produce a green solution of Iron II chloride. The solution remains green when it has a relatively high concentration, but the color will disappear when it becomes very dilute.
I’m not sure what you mean at 8:35. If you got less than your expected, that just means there were some side products that reacted away, it would be at most 80% pure if your actual yield was greater than the theoretical.
Hm. Dang, you're right. I'm not sure what I can say about purity now since it's lower than theoretical. Thanks for pointing that out. CZcams got rid of annotations so I can't change it in the video, so I guess my mistakes last forever now!
Use sodium borate and boric acid eact with magnesium and aluminum. The reaction is not as violent. You do get more boride but lots more boron. You want the reducing agent in slight excess. The reaction yeilds boron sodium metal vapor sodium oxide, hydrogen, sodium metal vapor magnesium oxide borides of both aluminum and magnesium and aluminum oxide.. to purify mix with dilute HCl adding more until it stays acidic. Rinse twice then react with NaOH and let marinate for a few days. You will be left with technical grade boron. ❤
It wouldn't surprise me if in the elevated temperatures of the reaction of the Boric Oxide and Magnesium on air, you formed some Boron Nitride, that's likely what frosted up your glass.
so ive collected 1,2g of expected 1,16g ..but loads got lost in the filtration processes. do u know any analysis reactions for boron? (edit, 1,2g of wet boron powder, in the end it problaby weighs under 0,9g) sec. edit now i have 0,87g
I want to prepare primarily a boride salt. Would you say that my approach should be to keep the magnesium in excess during the reaction? Magnesium borides are somewhat unstable, though, so even when the formed Boron reacts with the Magnesium to form boride, that boride will disassociate into the elements.
Excess would ensure you react all your boric oxide, just don't go too far or you'll make a lot of the boride instead. The magnesium boride should all be consumed in the acid step so you'll still get pure B.
@@mrhomescientist I want the magnesium boride as a source of boranes, so I do want to go there. The idea is that excess magnesium would ensure any boron that is formed is converted back into a boride. The part to be careful seems to be the proclivity of magnesium boride to decompose into boron, so if you heat too strongly, the yield of the boride will suffer. Thoughts on this approach. I want to repeat this again--my intention is to recover the magnesium boride, not boron.
Start with borax which is sodium salt of boric acid mixed 70:30 with boric acid. Mix in aluminum and magnesium powder in significant excess. Then you will get magnesium and aluminum borides as your main product. Reacting this with HCl in the absence of oxygen will give borane
@christopherleubner6633 Interesting. What reactions are taking place to get from borate to boride? There look to be a couple redox reactions taking place between the HCl, metals, and borax.
@@devvrath123 Unlikely on both counts. Acetic acid might not be strong enough to dissolve the borides, and even if it did it would probably way longer than the already-slow HCl. Magnesium ribbon bits won't be small enough to react efficiently either. Surface area is very important in these sorts of reactions.
If you are into Boron chemistry right now good sir, I have an experiment I have been cooking up for a while. I lack anyway to try the experiment as of now, would you be willing to try it?
Holy smokes man, I remember watching your videos year's ago, awesome to see you back, you probably had a helping hand in my decision to pursue a career in a chem related field. I probably watched your nitric acid synth video 20 or 30 times and eventually recreated it on my own. Keep up the awesome work!
Considering the "green color" disappeared when you added more water, I'd take a guess it was copper chloride. The HCl and copper probably reacted with O2 from the air as a catalyst as it sat out over those couple of days. Normally the copper wouldn't dissolve in HCl, but after that amount of time enough oxygen could have diffused in.
For carbon just do the classic carbon pillar experiment, smash the product and wash it with a base and water, dry it and grind it, you can run it thru few acids but this isn't really needed, I did it some time ago (but I didn't film it) and it was quite pure actually
I think the green colored solution came from the iron in the stainless steel crucible that was your reaction vessel. At high temperatures iron will bond with oxygen to form a black iron II oxide, and this will react with hydrochloric acid to produce a green solution of Iron II chloride. The solution remains green when it has a relatively high concentration, but the color will disappear when it becomes very dilute.
Sounds plausible!
I’m not sure what you mean at 8:35. If you got less than your expected, that just means there were some side products that reacted away, it would be at most 80% pure if your actual yield was greater than the theoretical.
Hm. Dang, you're right. I'm not sure what I can say about purity now since it's lower than theoretical. Thanks for pointing that out. CZcams got rid of annotations so I can't change it in the video, so I guess my mistakes last forever now!
Use sodium borate and boric acid eact with magnesium and aluminum. The reaction is not as violent. You do get more boride but lots more boron. You want the reducing agent in slight excess. The reaction yeilds boron sodium metal vapor sodium oxide, hydrogen, sodium metal vapor magnesium oxide borides of both aluminum and magnesium and aluminum oxide.. to purify mix with dilute HCl adding more until it stays acidic. Rinse twice then react with NaOH and let marinate for a few days. You will be left with technical grade boron. ❤
It wouldn't surprise me if in the elevated temperatures of the reaction of the Boric Oxide and Magnesium on air, you formed some Boron Nitride, that's likely what frosted up your glass.
Some brazing fluxes contain borax, borates, fluoroborates, if you want to explore other sources.
Might it not help to filter after a first addition of distilled water?
Now how do you make gluconic acid? To make boron gluconate the supplement? This supply would last you a lifetime. For achy joints.
I guess the green color was due to chlorine or copper chloride (II).
Nope! The green flame is characteristic of boron.
why didnt u heat the mixture, would increase the dissolving much..
True, but it also increases the rate of the elemental boron dissolving, according to my research.
well, ive done same reaction on 0,107 molar scale. now im trying to dissolve inpurities in my magnetic stirrer on 80degrees celsius... we will see :D
ReaktionChamber Good luck! Let me know how it works out.
so ive collected 1,2g of expected 1,16g ..but loads got lost in the filtration processes. do u know any analysis reactions for boron? (edit, 1,2g of wet boron powder, in the end it problaby weighs under 0,9g) sec. edit now i have 0,87g
I want to prepare primarily a boride salt. Would you say that my approach should be to keep the magnesium in excess during the reaction? Magnesium borides are somewhat unstable, though, so even when the formed Boron reacts with the Magnesium to form boride, that boride will disassociate into the elements.
Excess would ensure you react all your boric oxide, just don't go too far or you'll make a lot of the boride instead. The magnesium boride should all be consumed in the acid step so you'll still get pure B.
@@mrhomescientist I want the magnesium boride as a source of boranes, so I do want to go there. The idea is that excess magnesium would ensure any boron that is formed is converted back into a boride. The part to be careful seems to be the proclivity of magnesium boride to decompose into boron, so if you heat too strongly, the yield of the boride will suffer. Thoughts on this approach. I want to repeat this again--my intention is to recover the magnesium boride, not boron.
Start with borax which is sodium salt of boric acid mixed 70:30 with boric acid. Mix in aluminum and magnesium powder in significant excess. Then you will get magnesium and aluminum borides as your main product. Reacting this with HCl in the absence of oxygen will give borane
@christopherleubner6633 Interesting. What reactions are taking place to get from borate to boride? There look to be a couple redox reactions taking place between the HCl, metals, and borax.
Is it alright to use strong industrial-grade acetic acid instead of Hydrochloric acid or Sulphuric acid at 5:37?
And also would it be fine to use magnesium ribbon cut up into small pieces or turnings?
@@devvrath123 Unlikely on both counts. Acetic acid might not be strong enough to dissolve the borides, and even if it did it would probably way longer than the already-slow HCl. Magnesium ribbon bits won't be small enough to react efficiently either. Surface area is very important in these sorts of reactions.
@@mrhomescientist Oh. Thanks for the info!
Awesome back to making extractions!
yeah great come back !
Heyyyy Sulfur would be a good one to do, could you extract S from something?
If you are into Boron chemistry right now good sir, I have an experiment I have been cooking up for a while. I lack anyway to try the experiment as of now, would you be willing to try it?
Pyro213 Depends on what it is and if I have the materials!
Dude, welcome back! Love the work, is it cool if I throw you in my Sub box?
College Chemistry Of course! Thanks for the support. Keep an eye out for the carbon video this weekend!
Ooooooorrrrrrrrrrr Indium Oxide from phone screens? lol