Synthesizing a copper complex salt. The tetraamminecopper (II) sulfate monohydrate ⚛️👨‍🔬⚛️

[@pushpendrapatel4321]

Those instruments are really good!

[@ClownWhisper]

about five years ago I was doing this synthesis and I did it a little different just out of playing around instead of usinginstead of using ammonia I used an ammonia generator and pumped ammonia gas into the solution and it instantly crystallize into Tetra aiming crystals and I realized about a hundred percent yield it was amazing. I no longer have my notes on this reaction I got very sick and almost died from a neurological condition completely unrelated to chemistry I will add.if you could take her around and reproduce this by using ammonia gas you'd be very satisfied with the results

[@Glattuh]

Oh happy to read you commenting so! Thank for the idea! I may revisit this video in the future.

[@hichembenameur6679]

i love the backgroud sound effect

[@Glattuh]

I made it myself hehe :D Thanks!

[@sciencek]

I'm so glad to see you again with your chemistry videos !

[@Glattuh]

Yess I am back! Nice to see you here!

[@YourWealthCome]

Beautiful job! Beautiful Color and welcome back!

[@Glattuh]

Thank you¡ Glad to come again after a long time :D

[@arunkumarkr1822]

Great video presentation with a sophisticated instruments and apparatus helps a lot thank you so much

[@TheFireGoose]

Very nice

[@Ruphrush08]

Glad to see you again, missed your videos man!!

[@Glattuh]

Thanks¡¡ I am back again :D

[@Ruphrush08]

@@Glattuh and what reactions or projects do you have in mind for next videos?

[@Glattuh]

Thats a nice question. To tell you, I have more than 70 projects for individual videos. they may be splitted in more videos and I came up with new ideas most of the time, if I have paper to take notes of them haha. So yes, I have a lot of work to do. From organic to inorganic and even analytical chemistry will be uploaded here :D

[@Ruphrush08]

@@Glattuh awesome can't wait to see more content, keep up the quality man!!

[@huzaifakhalid7003]

was very help thank you !!

[@AntsMierenAvonturen]

Looks very interesting!:)

[@Andrew-my1cp]

I love the color of this complex! I made a small amount of the explosive nitrate complex and it was the prettiest explosive I have made. Great video!

[@Glattuh]

Hi!! Thanks for watching and comenting!! Actually, im interested. Since YT dont like those kind of videos anymore (xplsvs) :D I can not make anything more about that topic. In fact I had one video making potassium chlorate and it was banned... Anyways, did the colour of the nitrate complex salt differ from this one? Also what about its purification? I found that precipitating it with ethanol is a good and efficient idea, but not very large crystals are formed.

[@Andrew-my1cp]

@@Glattuh Hi! Yea KZbin really hates explosives and chemistry. I can see why on the explosives but the chemistry is just crap. KClO3 has potential to be misused but I just don't think it's worth removing the video over it. Check out BitChute and sciencemadness if you want to post/learn about some explosives. It's a fun hobby but is very very dangerous and you have to be very careful with laws. Anyway, I made tetraamine copper nitrate by placing thin copper wire into household grade ammonia and ammonium nitrate and letting it sit and blow oxygen into the bottle every now and then. I was too lazy to use my glassware so just used a plastic bottle. A more efficient, faster,and cleaner way is to make copper nitrate with copper metal or copper oxide with nitric acid. You either need to be very precise in your nitric acid addition to prevent getting the solition too acidic or else you'll have ammonium nitrate impurities. A better way is to crystallize the copper nitrate and dissolved in minimal water. Then add 25% lab grade ammonia until all of the copper nitrate complexed. After I did my ghetto method I added the same volume of methanol as there was solution and chilled to -15°C in the freezer. My method was probably low yielding but I really wasn't going for high yield at all. The color was the same as your complex. The sensitivity was relatively low and required multiple strong strikes from a hammer to detonate. I didn't recrystallize but you can using ammonia water. Also when in solution it was a dark to medium dark blue and when acetone was added to the solution and left to sit the solution turned a beautiful dark purple.

[@fernandodiazmarin250]

Have you tried you tried to use it for synthetisize Guyard's Violet (Cupric potassium ferrocyanide). That's supposed to be Copper pigment prepared by heating the precipitate of copper ammonium sulfate and potassium ferrocyanide at 170° C

[@ELBlDu]

cool! Great to see your back in action. RU taking requests? More distillation projects please. Different set ups? Less spendy glass maybe? Tossing out ideas

[@Glattuh]

Thanks!! It is also great to have you giving feedback! I will for sure make more distillations yes! Steam, fractionall, vacuum normal... But I am beeing sponsored so I dont gurantee the less expensive glassware... Anyway thanks for commenting!

[@ELBlDu]

@@Glattuh Yay, yes all processes, even with spendy glass would be great to see. Im glad your being sponsored, able to get proper equipment, and do it RIGHT! (versus lavender oil in my kitchen with a modified pressure cooker) Cant wait to see more to come. thanks for the response. really looking fwd to more. Do you use any solvents in some projects? IDk if you can get your hands on CO2 method or Ether, (both fractional I believe) but would really love to see some extracts made and the filtering process after distillation. Your videos are so well done, I hope you are very successful with upcoming projects. Very excited to see .

[@Glattuh]

Thanks for the comment! That seems to be more serious request. If you want you can write an email. You can find the address in my vhannel information page ;)

[@ELBlDu]

@@Glattuh thats about as specific as I can get due to limited knowledge and experience. I was trying to make lavender oil, but not sure what I did wrong, came out very cloudy, thought it needed filteration, prob characoal apparatus of sorts.. It was just my ideas running away from a failed experiment on this end. Thanks again .

[@corneliuswp4491]

Hello, great experiment hands off!! Btw im having problems in the same experiment to synthesis copper complex so I have some question if you dont mind, firstly how many mol ratio did you use in this experiment? Secondly, what you think about using reflux method for this? And lastly did you conduct UV-vis measurement for the yielded complex? Thanks in advance

[@drstoler]

Should be (NH4)2SO4, not NH4SO4 at 2:35. But great video nonetheless)

[@Glattuh]

Nice catch!!! Totally acurate, thanks for commenting that!

[@ivanbombana7282]

@@Glattuh I did this synthesis in this video some years ago, but when I put NH3 I obtaibed a gas ... I think the gas was NH4Cl.. why did I forme NH4Cl in your opinion?

[@anhhoanganh181]

Why should we let ethanol fall dropweise to the produkt? Why can't we mix it immediately? Can somebody explain?

[@Glattuh]

Hi! That is done to favor forming larger crystals. If a rapid mixing is done then the crustalls will really small and youll get more like a powder

[@anhhoanganh181]

@@Glattuh thank u very much

[@mariapap8558]

Great job! Cool video! I am little confused I google searched Cu(NH3)4H2OSO4 and in many websites showed that the H2O molecule wasn’t directly connected with Cu 2+ because it wasnt ligand. Which is the right? Is H2O ligand in the final product?

[@Glattuh]

Hi and thanks! Sometimes water is included in the crystall structure to make it more stable. In this case, I can guarantee that water acts as ligand, although is bond length tells us that the bond is not too strong. In chemistry there are no whites and blacks, but all is grey. What I mean is that, from my point of view, it is 85% ligand and 15% water of crystallisation. In the paper I found there is some crystallographic data. I use that to build the unit cell and I can say that water electrons ar paired with the copper atoms, not only because their position above/below the square of tetramminecopper but also because copper is out of the square plane. That fact is key, showing that copper is being pulled by the action of the water ;D The paper: journals.iucr.org/q/issues/1955/03/00/a01372/a01372.pdf If you are interested I will upload some photos of what I did on my IG (@nationofourhobbies), tell me yours if you want to be featured ;D Bests, NOOH

[@joanna4004]

Good i had this question too!

[@abrilnav]

Disculpa es una reacción exotérmica o endotermica?

[@Glattuh]

Exotérmica. Mira el minuto 3:30. No puedo darte el valor de la entalpia porque no lo encontré. No estoy seguro de que se haya medido.

[@titaniadragon3806]

You introduce pentahydrate compound but in your chemical reaction you have hexaaquo complex ? I don't understand, can you explain me please ? (Vous introduisez un composé pentahydraté mais dans le réaction c'est un complexe hexahydraté ? Pouvez-vous m'expliquer, s'il vous plait ?)

[@Glattuh]

Hi! Yeah I used the pentahydrate form of copper sulfate which is the most stable in normal conditions. Once you dissolve it in water, some water molecules enter the coordination sphere of every copper. It is common to find hexaligand complexes in chemistry, this is no exception. Six water molecules act as ligans via the oxygen electron pairs forming a octaedric complex with two positive charges, as the copper remains in an oxidation state of +2 and water is a neutral molecules. The nomenclature for the complex is the next -> [Cu(OH2)6]2+ The sulfate anion balances the charge so the mixture remains neutral in terms of charge. In adittion the rest of water molecules solvates both the complex and the sulfate so that they remain in solution, dissolved. In solid state the sphere of coordination is different. Each copper atom is bonded with six oxigen atoms, four of which comes from water and the rest two comes from the sulfate ion. The geometry of the crystall structure makes the global stoichiometry to be a pentahydrate. You can check it in the link I share with you: materialsproject.org/materials/mp-1196039/ If that is not clear enough, kist think that copper is the limitant reagent in all the reactions as it can be in different forms. You only have to take the stoichometry in mind when something needs to be weigh. In my case I weighed a certain amount of the pentahydrate sulfate so that I know how many moles of copper i have in my flask. Then I did some calculations to know how much ammonia needs to be added according to literature. Normally this is an excess. You also need to understand that the water molecules that are not in the final compound remain in solution. Thanks for your question! If you need something more just tell me :D Btw I do not really speak french hehe but I appreciate the "just in case" ;D

[@titaniadragon3806]

@@Glattuh Nation Of Our Hobbies Nation Of Our Hobbies I have any doubt about your skill in french x) but my english is very bad and... I really need to understand your manipulation... I had hope you able to use a translator if that was... Disaster... In fact, your video participe for my final work in my study in chemistry. So, i thank you a lot for your time to help me x) (i hope you can inderstand what i say...) So, if i understand your explain. The copper is able to form a bound with water molecule (oxygen atom) because of copper degrea of oxydation or ? What type of bound is ? And when you dissolved the pentahydrate... You enrich the compound with water ? And you obtain the hexaaqua ? More over... How you process in your calculation ? You said the water molecule is absent in final compound but... It still one finally ? I really hope you can understand me... Is pretty difficult for me... And you are able to help me haha, in writing... Is really hard... Nevertheless, i thank you a lot for your explication and help ♥️ thanks for to be here and help everyone

[@jjahhan8468]

can you list the ppe and precaution? do you wear mask while handling [cu(h2o)6]so4? and didnt u have to measure ammonia in fume hood?

[@sofiasim.5785]

Hii ..its so nice video!! Could you explain me why in solid state complex loses a molecule of water?Im confused and i searched this on many sites but i didnt found any info. Is it either based on a specific phenomenon or its because the bond is weak and during the rinsing breaks?thanks in advance!!

[@Glattuh]

Thanks for commenting! It seems like this video is gaining interest in the past few days hehe. The copper tetraammine complex exists in water as an ochtahedral geometry because two main factors: the ammonia is stronger as ligand that water and then, there are a lot of water molecules so the rest of the coordination sphere is filled with those molecules. However, solid state is another story. In solid state, bond lengths are shorter and the whole system evolves to the more stable state, thermodynamicly speaking. I am sure we can study it in therms of enthalpy of solution and bonds that are formed and broken in both states but there is no point in that. Here we touch one of the most beautiful thing I found in this, from my point of view, and its just a word: nature. Somehow it prefers to lose a water molecule because it is not needed to make it stable in solid state. I asume it has to be something about hydrogen bonds and so, maybe with just one water the crystall structure has enouch hydrogen bonds to be stable enough. If you want, you can check my latest post on my IG @nationofourhobbies to see something related to this ;) Bests

[@farisarman6525]

Hey there I have a question.. What is the device that is used to stir named? And what is the white thing does it has names or part of the device?

[@Glattuh]

It is a magnetic stirrer. You can refer it by magnetic hotplate too. The white thing is a magnet coverd in PTFE :). It allows us to stir magnetically. Behind the hotplate is a magnet attached to a motor that can be controlled by the device. Simple machine, revolution in chemistry :D

[@MG-og4zp]

maybe a darker text...it blends in with the white background.a but hard to read at times...great video..love the colour!!

[@Glattuh]

Yeah I am working on it. Since I have return to the channel it is getting some hard work until all things are good! Thanks for commenting and wqtchming me!

[@yondaaducative4980]

CUALITY VIDEO THANKS

[@Glattuh]

Thanks!!

[@chirallabs226]

Why is adding the reagent off of the balance good practice? To avoid dropping it on the balance?

[@Glattuh]

Hi! Exacly. You may be asking that after seeing my very cheap (but trusty) balance here but in labs in general, much more acurate balances are used and those can cost thousands so trying to avoid to dropp reagents on the balance plate is always a good idea yes. Thanks for commenting!

[@ΑγγελικήΣτρατή-ρ9λ]

Shall I heat during the dissolution of CuSO4 *5H2O ?

[@Glattuh]

If you want to speed things up, apply only low heat. At higher temps divalent copper evolves producing Copper (II) oxide, which is a dark insoluble compound. If copper sulfate is used then CuO and H2SO4 are produced

[@tayyabajabeen8489]

this is complexed copper? what is the percentage of copper in this powder?

[@Glattuh]

You could say so yes! It is a solid compound in which the copper atom is coordinated to 4 ammonia molecules, and two water molecules, one considerably more strongly than the other. Based on a 30secs calc i did the copper percentage in the compound is abot 25,9%.

[@n1n0_]

Hi, nice video ! I tried the experiment and it works really well 👍🏻 I just have a question though, do you know what solvent I could use for a recrist ? I didn't find much useful documentation on internet. Keep up with the great content !

[@Glattuh]

Hi! I have just filmed a video, yet to be edited in the upcoming months, about that. Best solvent I found is a hot mixture of water, cc ammonia solution an ethanol :D

[@n1n0_]

@@Glattuh Can't wait to see it !

[@Glattuh]

@@n1n0_ Just checking the comment here after editing the new video, expect it to be uploaded on friday 12:00 GMT :D

[@joanna4004]

Hello great and extremely interesting video! Could you explain me more about why [ Cu(H2O)2(NH3)4 ]SO4 isnt the real molecule? And how the water leaves and we take CuH2O(NH3)4SO4? I mean is it happenig a chemical reaction ? Can someone explain?

[@Glattuh]

Yes. The diaquotetraaminecopper (II) cation exists only in solution. Upon crystallization, one molecule of water escape from the sphere of coordination of copper, leaving a square pyramidal species. That water molecule is then part of the solvent mixture. The later product is not very stable, in fact, water in the ambient can coordinate with it, producing ammonia gas and returning the copper (II) sulfate pentahydrate from the begining. That kind of reactions belong to what is consider a field by itself within chemistry, and it is called chemistry of coordination complexes. Talking more scientifically deep, it studies the interaction between metals and their unocupated outer orbitals with the electrons of ligands such as water, ammonia, cyanide, all halides and a quite large list. If the ligand is organic then we enter the organometallic chemistry. I am sure you have heard of tetraethyllead, which was used to increase fuel octane number and it was banned due to health issues. Just fun fact to add, and to make it clear this is not so easy chemistry as it looks, copper sulfate pentahydrate (a quite common reagent in chemistry that everybody knows because of its crystall colour and ease of recrystallization) formula can lead you to think that copper is surrounded or coordinated by five water molecules, and then the sulfate arranges around that to compensate charge. In reality, at solid state, copper s surrounded by 4 water molecules and 2 oxygen atoms coming from one sulfate each respectively in an octahedral arrange. The remaining water is what is called water of crystallization and does not take place in the complex chemistry, it is just needed to form the crystalls. The result are blue crystals because water can alterate the electronic behaviour of copper. If you heat it, water is removed and youll find that the compound you get is pure white, because sulfate by itself is not "strong" enough as a ligand to alterate that electronic behaviour ;D Hope that helps hehe. If you want to learn more just search on google chemistry of coordination complexes. Bests, NOOH

[@joanna4004]

​@@Glattuh Thank you soo much for answering me so soon!! Indeed , it was very helpful! I am a chemist student but i couldnt understand that part. May it sound silly and i am really sorry for insisting . So the Cu(H2O)2(NH4)4 SO4 isnt solid? Thank you soo much again !!

[@Glattuh]

Nope, it is the form that the copper adopts in solution only!

[@joanna4004]

@@Glattuh Oh ok thank you again!

[@isabelvasquez3294]

Hi, could somebody explain to me how the weighed was taken? Because the container and sulfate weigh 20 g but I think the container weight is included in it. And why the reaction yield is higher than 100%?

[@Glattuh]

Hi! The container weigh is included on that by an option all balance must include and it is called the tare. You first weigh the container, empty, then tared it so the balance displays a zero. Then you add your powder or whatever you want to weigh and mesaure it. The yield is higher because it still contained alcohol.

[@adrianprinsloo5930]

How is copper peptide made?

[@HyunAYuchi]

Maybe try dissolve cotton then precipitate it as a demo

[@Glattuh]

I thought about that but I better find an application for that first, then I will for sure put it in my future projects list ;)

[@Glattuh]

Hi Sphene. The video you saw before was put on public by error. I had to do this for a university task hehe. Nevertheless, the program I used is Avogadro and it is free to download ;D

[@HyunAYuchi]

@@Glattuh Okay, thanks. Will wait for your next video then :)

[@mania6986]

can we use copper 2 nitrate? why?

[@Glattuh]

Yes you can, its a nother simple salt of Cu(II). The only thing is that its more expensive and overall if you have copper sulfate, its better to use it instead of the nitrate.

[@mania6986]

@@Glattuh Thank you.And why should we use concentrated ammonia?

[@Glattuh]

No problem! The copper is in solution coordinated with water. If diluted ammonia is used we risk that not all the copper is coordinated with 4 molecules of ammonia. So it is better to use both excess and conecntrated ammonia

[@mania6986]

@@Glattuh Thank you very much for your help🙏🏻

[@raghoudahellany7876]

what was the role of the ethanol

[@Glattuh]

Hi! The product we are synthetising here is not very soluble in ethanol, but very solble in water. By adding ethanol to the mixture we force the salt to precipitate. If in addition this is done by adding the ethanol dropwise, then the crystalls that form have the chance to be larger. Still you get a powder but at microscopic level the crystals are larger and that makes the filtration step way easier, as the paper is not clogged. Hope that helps!

[@GigaJinjo]

Give us more give us more!! something applied to cooking?

[@AlyGuez]

Hola! Y eso para que se usa? :)

[@Glattuh]

Hola!! Pues tiene algunos usos interesantes. He encontrado que se puede utilizar para preparar nanoparticulas de cobre y tambien, un reactivo similar, es usado para disolver celulosa y preparar fibras de rayon. En realidad es un compuesto intermedio de dichas reacciones aunque es aislable en este caso ;) Gracias por comentar!

[@AlyGuez]

Nation Of Our Hobbies que interesante...la verdad que no sé nada de química (soy graduada en Filosofía) pero me gusta ver cómo se hace 🙂

[@raghoudahellany7876]

can somebody explain plz

[@Glattuh]

Explain what? I asume the video is pretty clear enough but feel free to ask if you have questions :D