In theory, you should be able to do all of these things with strontium instead of barium. Strontium might be easier to get for some people and it is not toxic. Only problem is, strontium sulfate is somewhat more soluble than barium sulfate. (but still not very soluble)
+Astral Chemistry That is same with any preparation method. Strontium instead of Barium is the smarter choice. The only problem with that is; People who have uploaded the video think that they know best, and that their experiment is more efficient. Do the experiment yourself with said Strontium in another video to prove that you use your criticism constructively and you are willing to try new, more efficient methods.
I ve researched the net but every good sience site wrote that Strontium forms only an peroxyd if you press Oxygen or air with 100 Bar pressur and heat it to 700 C. Barium doesnt Need the pressure and ist the only earth Alkalien metal who has this Reaktion. So Strontium is useless.
bevor ww2 they made it with BaO2 and Phosphoric acid because they could make higher concentrations in first step (16%). i think only one H atome from the Phosphoric was used. Because with sulfuric acid not all BaO2 will react the insuloble sulfate will isulate the BaO2 from the acid.
Thanks for an informative video. Did you have to use the computer voice? I hate that thing - gaps and pronunciation that's very difficult to understand in places. I'm wondering, do you do this because you have problems with English yourself? Just asking. I feel the same way about lots of synthesized voices on RUclips and I'm trying to understand why.
Thank you. The only reason why we use the TTS software is so that our voice is not all over the internet. But we're working on posting the text we used for the TTS under each video.
Thanks for the video. This is awesome. I feel it is partially my fault you got a huge mess to clean up afterward. Need some time to digest the video. I take it that making clean hydrogen peroxide from for example barium peroxide is a bit complicated to do? Awesome and thank you again.
Thank you very much! Nice to hear that you like the video, since we tried to show everything in great detail. For the mess, we basically knew what would happen to the watchglass, so it is our fault. Sadly, we got no poor first year student to assign the cleaning to. But the surface cleaned up suprisingly well with a little wiping off. :) It is actually not that complicated and the hydrogen peroxide is fearly clean. This is because the barium sulphate formed is practically insoluble. The excess of sulphuric acid can be removed by treatment with barium carbonate, which is also insoluble and will form insoluble barium sulphate. So in the end, after filtration, you're left with a practically pure solution of hydrogen peroxide. Just remember to use ice cubes made from distilled water.
Thanks again for the explanation. I think this video is very unique and very detailed compared to other videos on youtube. It has really good content. I would do something about the TTS which may scare away some people because they think it is one of those robot promotion videos. If you can't do it the NurdRage style then at least show in the beginning some moving pictures. Automatic marketing videos uses mostly still images so avoid that. There is a very good TTS I use that is called Neospeech Julie. It speaks almost like a real human. Keep making these awesome videos and good luck.
Thanks for the tip! We'll take a look at fixing the voice, as we know that it is not optimal. We might also do a follow up video with hydrogen peroxide from percarbonates, as those are easy to get. Thanks for your kind words!
Could I use a soluble calcium salt to make Ca(OH)2 and then CaO2? I know that calcium sulfate is very slightly soluble in water, but I wouldn't mind a slight contamination. The only barium salt I have is 50% Ba(NO3)2 from a sparkler with unknown impurities. Also, I'd prefer not to work with toxic soluble salts.
I don't think that calcium would work since the peroxide decomposes at very low temperature ( ~ 250 °C). The reaction of the calcium oxide with oxygen would most likely require much higher temperatures. But you can always try it and test for the presence of hydrogen peroxide. But if you want to use the method with the dilute hydrogen peroxide then that shoudl probably work.
Hi Cody! :) It is very difficult to find an ionic peroxide with suitable properties. Heavy metals like barium are also known to decompose the hydrogen peroxide. I guess the barium oxide / oxygen route is a nice experiment to learn something about chemistry. Probably not the best method just for getting a hold of hydrogen peroxide.
In theory yes but even the tiniest trace of transition metal ion or a scratch on the beaker would result in a violent decomposition. We never tried it but I don't think it would work. If you want to try it, you have to cool extremely well.
Very nice video, very interesting topic. While being at the topic of hydrogen peroxide: Is there a way to separate it from sodium percarbonate? I thought maybe it's possible to get rid of the carbonate with hydrochloric acid, but could this produce chlorine? H2O2 + 2HCl --> 2H2O + Cl2 ? I am not sure and don't want to risk producing chlorine...! Maybe acetic acid would work too. Then adjusting the pH to basic and adding barium hydroxide would precipitate BaO2, right? Also, can the last reaction be done with H2CO3 formed by passing CO2 in the solution? BaCO3 is very insoluble in water, just as BaSO4, but it could form soluble barium salts like chlorides much more easily that the sulfate, so the barium is not lost. Sorry for the many questions, but I find this really interesting and thought-provoking. :D Also, are you german? The Chemiker-Kalender is letting me think that. Good work, keep it up! Cheers
Thanks a lot! Sorry for the delay. It is possible to form chlorine gas via oxidation of chloride with hydrogen peroxide. Some chlorate could also form. What really happens is really dependant upon the exact reaction conditions. We already discussed obtaining hydrogen peroxide from percarbonates with the user "P.Fx." in the comments on this video. So it is definitly possible. You might want to check out that conversation. Adjusting the pH is not very important since barium salts will also precipitate hydrogen peroxide from slightly acidic solutions. H2CO3 could be possible. That would be a good idea so that the barium salts are easy to recycle. No problem. Well, I guess. XD Just as a hint: If you really want to get hydrogen peroxide for actually using it and not for exploring its chemistry I'll suggest you to buy a bunch of gow sticks and take the H2O2 from them.
Astral Chemistry Thank you for your helpful advice and suggestions! I'll probably try both, as I can explore the chemistry of barium compounds and of hydrogen peroxide that way. The conversation with P. Fx. was also interesting. So, thank you and have a nice day! Cheers
the rougemillenial Terrifying! 99% you say? Wow, that is some dangerous stuff. I can't believe that that'd be even legal to sell. I mean, here in Germany you get mostly the 3% or even 1% stuff. Well, I guess you can substitute the hydrochloric acid with acetic acid. Should work the same way, I think. (I refer to my plan to make H2O2) Maybe even Calcium would suffice?
Well, for all practical purposed, you can go as high as you want to. Even highly concentrated hydrogen peroxide will not just detonate, as some chemistry textbooks want to tell us. As long as you avoid impurities that will decompose the hydrogen peroxide and you cool well, there is no danger.
Yes, absolutely. In fact, as sodium percarbonate is just an adduct of hydrogen peroxide with sodium carbonate, it is enough to just add the sodium percarbonate to water. This will then form free hydrogen peroxide and sodium carbonate in solution. The sodium carbonate could of course be neutralised but for most purposes it wont interfere. We might actually make another video showing that. Thanks! Heres a good paper on that subject: www.sciencedirect.com/science/article/pii/004040209500304Q
I tried adding a little to some sodium bromide solution but maybe I wasn't patient enough. Otherwise I have been experimenting with soap manufacture for our own domestic purposes and percarbonate is probably the bleaching agent most compatible with our domestic sewage treatment. Looks like a good paper. I'll try to find a way of obtaining a paper version.
I think the solution could have been too alkaline to oxidize the bromide to bromine in that case. We thought about the percarbonate and its pretty simple: Since the percarbonate is just an adduct (as mentioned above), we can free the hydrogen peroxide by simply destroying the carbonate ions. So for all practical purposes, we will trie to prepare a suspension of percarbonate, cool it well and then slowly add in HCl until an slightly acidic pH is reached. In theory, we should be left with a strong solution of hydrogen peroxide, which would contain some NaCl. This sounds very easy in theory and percarbonates are that easy to get (compared to barium salts and sodium) that we will try it tomorrrow. I dont now how we could have forgotten the most obvious way. Thanks for that idea!
Golden Retriever I don’t know who told you that, but that’s a terrible idea. H2O2 is not a fuel, it is an oxidizer. It does not burn, it makes other things burn. Such as your vehicle.
H2O2 can technically be used as a propellant. For concentrations over 90%, the decomposition (Either catalytically or at High temperature) produces enough gas to work as a propellant. The US Mercury space missions used H2O2 as the propellant for the capsule's thrusters. It was replaced with Hydrazine in future missions (which has about twice the specific impulse of H2O2). That said as ecstasy.apostasy said, driving around in a car with a tank full of 90% H2O2 is an absolutely terrible idea. There's plenty of videos on youtube showing what effect Highly concentrated peroxide has (High Test Peroxide) on objects. As well as that at high concentration, the energy produced by the decomposition of the H2O2 is enough to vaporise the H2O2.
I'm so glad I found your alter ego! I'm in need some super peroxide also.. You know, there was this show in the eighties I watched as a kid called "mr wizard" and he put some sodium peroxide on some cereal, shot it with a squirt gun and went on to explain calories as heat. That was a cool show.
Richard_AKL its what they do, so no. Besides their other channel was taken down about two years ago, moving to a different platform so i don't think they are qctive on this one anymore to respond.
From my understanding of the video, you use an excess of the Metal Peroxide. This makes sure that that all the sulphuric acid is consumed and leaves only insoluble Metal Sulphates and Peroxides in the mixture, that can be filtered out.
unfortunately we have a different language. It's clear : - ruclips.net/video/FXQbVf6Oric/видео.html but your not, it's not clear: - what substance is taken how it is not always clear if you post your machine text under the link ("description") below, it will be better. in languages there is a grammatical difference. but if there are formulas and the number(quantity) of substances taken, then immediately everything is clear.
qwerty qwerty Barium nitrate: Ba(NO3)2. You can use as much as you want, but the more you use, the greater the danger. Decomposition with heat will yield barium oxide, BaO. You can start with that if you have it. Reaction with atmospheric oxygen in a low CO2 (carbon dioxide) environment will yield Barium Peroxide, BaO2. Alternatively, you can make Ba(OH)2 by reacting any barium salt with any alkali hydroxide, or you can purchase it. If you react that with hydrogen peroxide (h2o2), you will get barium peroxide. If you have hydrogen peroxide that you would like more pure, that would be the purpose of that method. Nevertheless, if you react a very concentrated acid like sulfuric acid (h2SO4) with barium peroxide, you will get a very concentrated solution of hydrogen peroxide.
do you honestly think that this would be a practical way of producing hydrogen peroxide on a macro economic scale. the answer is no. we are just adding an extra oxygen to water. this is not a good way to make hydrogen peroxide in mass quantities.
Peroxide is produced Industrially using the Anthraquinone process, which CodysLab did a video on. The process involves Hydrogenating a 2-alkyl-anthraquinone to a 2-alkyl-anthrahydroquinone. The 2-alkyl-anthrahydroquinone is then reacted with oxygen to produce Hydrogen peroxide and the original 2-alkyl-anthraquinone. On an industrial scale it's more economic as the starting 2-alkyl-anthraquinone can be reused. In a lab setting it's less practical as it requires a Hydrogenation with palladium catalyst, the Peroxide is extracted using water and so must be distilled under reduced pressure in order to achieve higher concentrations.
Do you know what the purpose of this video is? It says right at the beginning this is “old school”! It’s just to explore the science, not an attempt at making mass quantities of peroxide.
@@zeo_crash7984 An Methode of H2O2 Produktion was after ww2 heating Isopropylalcohol with Little bit H2O2 as catalyst to around 80C and bubbling air throught it.It produces Aceton and H2O2.
Good content but very poor video making. Half an hour is insanely long even for chemistry enthusiasts. You should cut down on the time showing the reaction taking place, maybe 30s max on something that looks the same. You don't have to show the entire process, you can speed up parts. Otherwise good video!
and the sound levels between the almost silent parts where the artificial voice barely covers the sound of the fume extraction and the music that comes blasting at full volume out of nowhere.
Why are all the good chemistry channels not playing?
In theory, you should be able to do all of these things with strontium instead of barium. Strontium might be easier to get for some people and it is not toxic.
Only problem is, strontium sulfate is somewhat more soluble than barium sulfate. (but still not very soluble)
Thats right. The solubility won't be a problem, as long as you don't intend to store the hydrogen peroxide for a long time.
+Astral Chemistry That is same with any preparation method. Strontium instead of Barium is the smarter choice. The only problem with that is; People who have uploaded the video think that they know best, and that their experiment is more efficient. Do the experiment yourself with said Strontium in another video to prove that you use your criticism constructively and you are willing to try new, more efficient methods.
I ve researched the net but every good sience site wrote that Strontium forms only an peroxyd if you press Oxygen or air with 100 Bar pressur and heat it to 700 C. Barium doesnt Need the pressure and ist the only earth Alkalien metal who has this Reaktion. So Strontium is useless.
Great, but what concentration did you manage to make in the end?
bevor ww2 they made it with BaO2 and Phosphoric acid because they could make higher concentrations in first step (16%). i think only one H atome from the Phosphoric was used. Because with sulfuric acid not all BaO2 will react the insuloble sulfate will isulate the BaO2 from the acid.
Thanks for an informative video. Did you have to use the computer voice? I hate that thing - gaps and pronunciation that's very difficult to understand in places. I'm wondering, do you do this because you have problems with English yourself? Just asking. I feel the same way about lots of synthesized voices on RUclips and I'm trying to understand why.
Thank you. The only reason why we use the TTS software is so that our voice is not all over the internet. But we're working on posting the text we used for the TTS under each video.
Thank you. Yes, captions would be very helpful.
Yes please do that. TTs is hard to understand the chemical's that was used and the proper steps.
Awesome video and loved the music!😎
Astral Chemistry I knew there was something odd with that voice... though I simply thought it was your accent. That TTS is quite good...
Thanks for the video. This is awesome. I feel it is partially my fault you got a huge mess to clean up afterward. Need some time to digest the video. I take it that making clean hydrogen peroxide from for example barium peroxide is a bit complicated to do?
Awesome and thank you again.
Thank you very much! Nice to hear that you like the video, since we tried to show everything in great detail.
For the mess, we basically knew what would happen to the watchglass, so it is our fault. Sadly, we got no poor first year student to assign the cleaning to. But the surface cleaned up suprisingly well with a little wiping off. :)
It is actually not that complicated and the hydrogen peroxide is fearly clean. This is because the barium sulphate formed is practically insoluble. The excess of sulphuric acid can be removed by treatment with barium carbonate, which is also insoluble and will form insoluble barium sulphate. So in the end, after filtration, you're left with a practically pure solution of hydrogen peroxide. Just remember to use ice cubes made from distilled water.
Thanks again for the explanation. I think this video is very unique and very detailed compared to other videos on youtube. It has really good content. I would do something about the TTS which may scare away some people because they think it is one of those robot promotion videos. If you can't do it the NurdRage style then at least show in the beginning some moving pictures. Automatic marketing videos uses mostly still images so avoid that.
There is a very good TTS I use that is called Neospeech Julie. It speaks almost like a real human.
Keep making these awesome videos and good luck.
Thanks for the tip! We'll take a look at fixing the voice, as we know that it is not optimal. We might also do a follow up video with hydrogen peroxide from percarbonates, as those are easy to get. Thanks for your kind words!
How to separate sodium hydroxide from the hydrogen peroxide? Please answer
Somehow I figured... The video quality would be crap. Starts with a fancy intro screen. Then goes on to use synthesized voice.
Why bother
Great content! I didn't know your channel till it pops on my channel's related list. there is another chemplayer joined this community
Thanks a lot! Now we just have to get a hold of some ants...
Could I use a soluble calcium salt to make Ca(OH)2 and then CaO2? I know that calcium sulfate is very slightly soluble in water, but I wouldn't mind a slight contamination. The only barium salt I have is 50% Ba(NO3)2 from a sparkler with unknown impurities. Also, I'd prefer not to work with toxic soluble salts.
I don't think that calcium would work since the peroxide decomposes at very low temperature ( ~ 250 °C). The reaction of the calcium oxide with oxygen would most likely require much higher temperatures. But you can always try it and test for the presence of hydrogen peroxide. But if you want to use the method with the dilute hydrogen peroxide then that shoudl probably work.
calcium ions slowly decompose hydrogen peroxide so no that wont work.
Hi Cody! :)
It is very difficult to find an ionic peroxide with suitable properties. Heavy metals like barium are also known to decompose the hydrogen peroxide. I guess the barium oxide / oxygen route is a nice experiment to learn something about chemistry. Probably not the best method just for getting a hold of hydrogen peroxide.
@@astralchemistry8732 so you basically produced sodium peroxide and once you add water the reaction starts?
surely if you use the exact molar ratios of water to sodium peroxide, then the NaOH and H2O2 you produce is anhydrous (100% concentration)?
In theory yes but even the tiniest trace of transition metal ion or a scratch on the beaker would result in a violent decomposition. We never tried it but I don't think it would work. If you want to try it, you have to cool extremely well.
yes i understand both the risks and the decomposition, and to be honest a 35% - 50% solution of hydrogen peroxide is perfectly fine for further use.
1:51 “H2O (aq)”? Isn’t that redundant? 😂
Very nice video, very interesting topic. While being at the topic of hydrogen peroxide: Is there a way to separate it from sodium percarbonate? I thought maybe it's possible to get rid of the carbonate with hydrochloric acid, but could this produce chlorine? H2O2 + 2HCl --> 2H2O + Cl2 ? I am not sure and don't want to risk producing chlorine...! Maybe acetic acid would work too. Then adjusting the pH to basic and adding barium hydroxide would precipitate BaO2, right? Also, can the last reaction be done with H2CO3 formed by passing CO2 in the solution? BaCO3 is very insoluble in water, just as BaSO4, but it could form soluble barium salts like chlorides much more easily that the sulfate, so the barium is not lost.
Sorry for the many questions, but I find this really interesting and thought-provoking. :D
Also, are you german? The Chemiker-Kalender is letting me think that.
Good work, keep it up!
Cheers
Thanks a lot! Sorry for the delay.
It is possible to form chlorine gas via oxidation of chloride with hydrogen peroxide. Some chlorate could also form. What really happens is really dependant upon the exact reaction conditions.
We already discussed obtaining hydrogen peroxide from percarbonates with the user "P.Fx." in the comments on this video. So it is definitly possible. You might want to check out that conversation.
Adjusting the pH is not very important since barium salts will also precipitate hydrogen peroxide from slightly acidic solutions. H2CO3 could be possible. That would be a good idea so that the barium salts are easy to recycle.
No problem. Well, I guess. XD
Just as a hint: If you really want to get hydrogen peroxide for actually using it and not for exploring its chemistry I'll suggest you to buy a bunch of gow sticks and take the H2O2 from them.
Astral Chemistry Thank you for your helpful advice and suggestions! I'll probably try both, as I can explore the chemistry of barium compounds and of hydrogen peroxide that way.
The conversation with P. Fx. was also interesting.
So, thank you and have a nice day!
Cheers
Thanks. Nice to hear that I could help. I'd love to hear about your results!
Have some nice lab work!
the rougemillenial Terrifying! 99% you say? Wow, that is some dangerous stuff.
I can't believe that that'd be even legal to sell. I mean, here in Germany you get mostly the 3% or even 1% stuff.
Well, I guess you can substitute the hydrochloric acid with acetic acid. Should work the same way, I think. (I refer to my plan to make H2O2)
Maybe even Calcium would suffice?
I can understand the attraction of the barium route. Is there a sane limit to final H2O2 concentration for safe demonstration pursposes?
Well, for all practical purposed, you can go as high as you want to. Even highly concentrated hydrogen peroxide will not just detonate, as some chemistry textbooks want to tell us. As long as you avoid impurities that will decompose the hydrogen peroxide and you cool well, there is no danger.
Could this philosophy be extended to percarbonate salts with the obvious evolution of CO2? I enjoyed the video. Thank you :-)
Yes, absolutely. In fact, as sodium percarbonate is just an adduct of hydrogen peroxide with sodium carbonate, it is enough to just add the sodium percarbonate to water. This will then form free hydrogen peroxide and sodium carbonate in solution. The sodium carbonate could of course be neutralised but for most purposes it wont interfere.
We might actually make another video showing that. Thanks!
Heres a good paper on that subject: www.sciencedirect.com/science/article/pii/004040209500304Q
I tried adding a little to some sodium bromide solution but maybe I wasn't patient enough. Otherwise I have been experimenting with soap manufacture for our own domestic purposes and percarbonate is probably the bleaching agent most compatible with our domestic sewage treatment. Looks like a good paper. I'll try to find a way of obtaining a paper version.
I think the solution could have been too alkaline to oxidize the bromide to bromine in that case.
We thought about the percarbonate and its pretty simple: Since the percarbonate is just an adduct (as mentioned above), we can free the hydrogen peroxide by simply destroying the carbonate ions. So for all practical purposes, we will trie to prepare a suspension of percarbonate, cool it well and then slowly add in HCl until an slightly acidic pH is reached. In theory, we should be left with a strong solution of hydrogen peroxide, which would contain some NaCl. This sounds very easy in theory and percarbonates are that easy to get (compared to barium salts and sodium) that we will try it tomorrrow. I dont now how we could have forgotten the most obvious way. Thanks for that idea!
I’ve heard ideas of running a car with hydrogen peroxide
I mean it Is used as a rocket fuel so from what I can tell it’s not a bad idea
Golden Retriever
I don’t know who told you that, but that’s a terrible idea. H2O2 is not a fuel, it is an oxidizer. It does not burn, it makes other things burn. Such as your vehicle.
H2O2 can technically be used as a propellant. For concentrations over 90%, the decomposition (Either catalytically or at High temperature) produces enough gas to work as a propellant. The US Mercury space missions used H2O2 as the propellant for the capsule's thrusters. It was replaced with Hydrazine in future missions (which has about twice the specific impulse of H2O2).
That said as ecstasy.apostasy said, driving around in a car with a tank full of 90% H2O2 is an absolutely terrible idea. There's plenty of videos on youtube showing what effect Highly concentrated peroxide has (High Test Peroxide) on objects. As well as that at high concentration, the energy produced by the decomposition of the H2O2 is enough to vaporise the H2O2.
17:44 top 5 jumpscares of 2022
I'm so glad I found your alter ego! I'm in need some super peroxide also.. You know, there was this show in the eighties I watched as a kid called "mr wizard" and he put some sodium peroxide on some cereal, shot it with a squirt gun and went on to explain calories as heat. That was a cool show.
Is it possible to demonstrate the quinone method, that's how it's done industrialy,isn't it?
I know it’s pretty late to ask, but I was wondering if instead of barium I could use calcium?
a really nice job! im happy to find your channel. got here from a scrapsince user.
What music you take for your experiments?
It sounds nice!
While reducing restrict to later increase percentage
28:00 I wasn't expecting that...
Haha XD
Found ya in yet another comment section @untitled
@@scrp7142 ? leo??
Hi ;)
Yes cornflaks contain iron ! I mean litteraly ;)
Mixed Flaks+ water in a bag+water + magnet
;)
I did not know that you can reach 600 deg with a butane torch?🤔
26:34 ooo sparks in water
Its alchemy XD
Whate about potassium superoxide?
It's a Chemplayer!! *it subscribes*
Thanks a lot!
You're very welcome! It's been ages that I were seeking for a way to generate high concentrations of H202: a 30% bottle here is rated at 40€ DX
Only Chemplayer can use red phosphorus.... Probably only Chemplayer can GET red phosphorus!
Check Alibaba. You can definitely find it there.
What software is used to read and create the voice?
TTSApp.
Can you not just record your voice? The computer voice is sooo frustrating :(
Richard_AKL its what they do, so no. Besides their other channel was taken down about two years ago, moving to a different platform so i don't think they are qctive on this one anymore to respond.
I like the music at 17:44 it spoke to my soul >.
Enjoyed this a lot...thank you!
Isn t contaminate with h2so4 from barium metod and naoh from sodium metal?is not pure h2o2
From my understanding of the video, you use an excess of the Metal Peroxide. This makes sure that that all the sulphuric acid is consumed and leaves only insoluble Metal Sulphates and Peroxides in the mixture, that can be filtered out.
Terrific video!!!!!
I got scared shitless at around 17:50 when the music hit because I had my volume up so I could hear the weird text-to-speech kind of voice talking...
24:40 natriumperoxid sodium peroxide
a trøbbeled way to h2o2 , i gess the simpel way is verboten ?
Chemplayer? Cool!
Are you studying chemistry or is this just your hobby?
Was für ein Zufall! Den Chemiker Kalender habe ich erst heute in der Bibliothek gefunden
the max headroom digital voice narration just sucks completely,
unclear(not understand)
what are you doing.
please specify the formulas on the screen.
What exactly is unclear?
unfortunately we have a different language.
It's clear : - ruclips.net/video/FXQbVf6Oric/видео.html
but your not, it's not clear: -
what substance is taken
how
it is not always clear
if you post your machine text under the link ("description") below, it will be better.
in languages there is a grammatical difference.
but if there are formulas
and the number(quantity) of substances taken,
then immediately everything is clear.
qwerty qwerty
Barium nitrate: Ba(NO3)2. You can use as much as you want, but the more you use, the greater the danger. Decomposition with heat will yield barium oxide, BaO. You can start with that if you have it. Reaction with atmospheric oxygen in a low CO2 (carbon dioxide) environment will yield Barium Peroxide, BaO2.
Alternatively, you can make Ba(OH)2 by reacting any barium salt with any alkali hydroxide, or you can purchase it. If you react that with hydrogen peroxide (h2o2), you will get barium peroxide. If you have hydrogen peroxide that you would like more pure, that would be the purpose of that method.
Nevertheless, if you react a very concentrated acid like sulfuric acid (h2SO4) with barium peroxide, you will get a very concentrated solution of hydrogen peroxide.
Super!
not from scratch, i cannot get any hydrogen peroxide
Are you German?
do you honestly think that this would be a practical way of producing hydrogen peroxide on a macro economic scale. the answer is no. we are just adding an extra oxygen to water. this is not a good way to make hydrogen peroxide in mass quantities.
Do you have a better method?
Peroxide is produced Industrially using the Anthraquinone process, which CodysLab did a video on. The process involves Hydrogenating a 2-alkyl-anthraquinone to a 2-alkyl-anthrahydroquinone. The 2-alkyl-anthrahydroquinone is then reacted with oxygen to produce Hydrogen peroxide and the original 2-alkyl-anthraquinone.
On an industrial scale it's more economic as the starting 2-alkyl-anthraquinone can be reused.
In a lab setting it's less practical as it requires a Hydrogenation with palladium catalyst, the Peroxide is extracted using water and so must be distilled under reduced pressure in order to achieve higher concentrations.
Do you know what the purpose of this video is? It says right at the beginning this is “old school”! It’s just to explore the science, not an attempt at making mass quantities of peroxide.
“just asking an extra oxygen to water” i think this phrase is an extreme underestimation of the task here, why are you so dismissive
@@zeo_crash7984 An Methode of H2O2 Produktion was after ww2 heating Isopropylalcohol with Little bit H2O2 as catalyst to around 80C and bubbling air throught it.It produces Aceton and H2O2.
PerHOCKSside
Interesting but the robot voice is really boring....
Too demanding to listen to with robotic voice, but got the idea......
Was meint das F um 7:00?
Good video , bu fk that song -_-
the voice effect and the music are boring, unbearable !
The robot gets on my nerves!!
it was unwatchable.
the voice is unbearable and makes the video unwatchable
Good content but very poor video making. Half an hour is insanely long even for chemistry enthusiasts. You should cut down on the time showing the reaction taking place, maybe 30s max on something that looks the same. You don't have to show the entire process, you can speed up parts. Otherwise good video!
and the sound levels between the almost silent parts where the artificial voice barely covers the sound of the fume extraction and the music that comes blasting at full volume out of nowhere.
What is wrong with this videoooooooooooo???? AI readers are better now.
Horrible vocals...