Electrolysis of copper sulfate CuSO4 (aq) using graphite and copper electrodes - GCSE Chemistry

[@kat1070]

i don't normally comment on videos especially as this was made years ago but i have to say that this is the most helpful video on electrolysis i have seen so far and trust me i have been watch ALOT ahaha

[@dog360]

probably one of the only educational youtube videos i’ve ever found helpful!

[@debra6968]

Wow, superb explanation. Nicely penetrating and sinking into the system. Thanks so much for this video. Full of passion and commitment. Seems you have done your HW, so well planned and precise. Loads of love from Sri Lanka. God bless you :)

[@magnuswootton6181]

whatever you do, if u actually do this electrolysis stuff watch out for poison gas emission!!!

[@omkarpawar1594]

Loved the mehandi on your hand and the lecture too, Thanks a ton.

[@yashkhandelwal641]

The video was Good and really explained clearly and properly! Thank u so much!

[@golammorshed7260]

OMG I had this one confused for almost months and you made it clear within 5 minutes TYSM :)

[@sahilagarwal6601]

Demn she has got mehendi on

[@yashkhandelwal641]

Lmaooo

[@Rarafb2761]

What I focus on instead of trying to understand chem... 🥲

[@samsononi7164]

Amazing explanation from Henry and Esther Thank you

[@SalsaKingoftheApes]

Very clear, super stuff! Mr J

[@ChemJungle]

Glad it was helpful!

[@MuhammadHassan-jq8jp]

What a video, honestly teach me chemistry I'd pay anything to study from you

[@omarmoustafa6672]

That was really helpful!!! Thank you so much!🙏🙏🙏

[@drsirmechemistrymaster]

Good work... Coincidentally I have done the demonstration experiment for this on my channel.... I see we are in tune... Thank you madam

[@jitendraempire5627]

Well explanation

[@SethuChandra]

omg explained SO WELLL

[@SarahNakalembe-r2k]

Hi

[@angel-nr3vg]

perfect explain it is so complete .it make me totally understand.thanks

[@ruba588]

in love with your channel!! Thank you so much for your videos

[@galaxy_tv104]

1:22 Can you explain why sulfide never gets discharged? is it because it has a higher reduction potential?

[@345surf_excel_washingpowder]

Yes it lies at a higher position in the electrochemical series therefore it has a property to undergo reduction better than others

[@boliusabol822]

there is no sulfide, it's sulfate. Sulfate has a very low oxidation potential. . You can look up anion discharge series, you'd see sulhate and nitrate low. And Chlorine Bromine and Iodine high. There's OH- in the series too but it's a funny one 'cos while it has a high oxidation potential, it has poor kinetics so its tendency to discharge is not so high. Also when you have a copper anode, the anode itself oxidises, no anion oxides at it.

[@readoryx373]

Could this apply to rocks high in Iron, by placing the iron ore in an electrolyte of iron sulphate, an iron cathode?

[@ivygracelane]

you have saved my life thank you

[@energyforever720]

@chemjungle i heard you say the sulfate never comes out, but when i did electrolysis of copper sulfate a strange yellow thing appeared. I was using a 5 volt power supply and graphite electrodes, which made it very clear to see the yellow thing on the dark black graphite electrode. Idk what it was but my guess was elemental sulfer. Any ideas why that happened?

[@DaveFer]

Hey now. Thanks for this educational video. I've been doing chem experiments with my kids while we're quarantined and I have question perhaps you are uniquely qualified to answer: I have several grams of Cu that we precipitated and dried from a reaction of CuSO4 + Al. It's a tiny amount and probably contaminated. I'd like to use electrolysis to purify it and I have copper thread that I can use as an cathode (anode?). I can weigh the precipitate and the copper thread prior to start. And I'd like to show my kids how all the copper in the precipitate is purified and deposited on the copper thread ... both visually and by weight. My question is, which electrolyte should I use, CuSO4 solution? Acetic acid? NaCL solution? Which electrolyte WILL NOT donate Cu or any other atom to the cathode? Will the CuSO4 donate to the cathode? I'll probably do this in a large test tube. I'll try using a graphite rod (pencil "lead"?) on one side and copper thread on the other. (I'll think the pencil graphite will conduct ... I'll test it.) Here's our playlist. You're input would be highly valuable. kzbin.info/aero/PLikL-gQhJ0DmknULDIeGei3l2Q__dEfI7

[@ChemJungle]

Hey! I think you've probably got an amount of impure copper from your reaction. In order to make this work you need to use your impure copper as the anode and your pure copper as the cathode. If your product isn't suitable to be used as an electrode then you might struggle to purify in this way. At home, I wouldn't use any of these electrolytes though - CuSO4 will deposit Copper from the solution, acetic acid doesn't conduct well, NaCl will produce Chlorine as a byproduct which is super toxic.

[@truth3137]

Great video!

[@ChemJungle]

Thanks!

[@antonisaristidoukokkinou9948]

how does the copper ion go to the anode when the anode attracts negative ions and why in the half equation for the anode it doesn't have a positive charge but is simply its element? are you saying that it first got purified from the cathode and this whole time nothing was happening at the anode so it went to the anode to oxidise??? I'm a confused 16 year old help.

[@ChemJungle]

Eeeek I'm sorry this has confused you! The copper ions go to the cathode and get reduced to copper in both scenarios. At the anode, oxidation happens. There are a few things in the solution that could lose electrons: OH- SO4(2-) or the Cu in the electrode , but actually the Cu in the electrode is the most easily oxidised of the 3 options so it goes to Cu2+ in the solution.

[@samina9131]

@@ChemJungle why did copper lose electons just to gain it back

[@Alex-xq5qz]

This help me thanks ( from a prepa french student )

[@varpilajain5895]

hey sis...am in luv with ur channel completely...my doubts are cleared explicitly. i had doubts abt explanation on preferrential discharge but by seeing ur video..i am delighted...keep doing well| "GOOD DAY"!!!!!

[@wilsonbashaija2293]

after the copper from anode goes to cathode and the sand sinks, what is that small thing that is left after copper refining, that is being compared to the recent big pure copper

[@ChemJungle]

If you let the electrolysis run forever then it would stop as soon as the anode stopped conducting electricity because your circuit would be broken. There might still be very small amounts of metal left but it's mostly going to be the rock it started as remaining :)

[@mochimoy8865]

The Explanation was very clear, thank youuuu

[@mariaaxp0]

i legit love you thank u

[@arty6287]

GOAT video love u

[@varpilajain5895]

i also had a doubt...anode attracts negative ions..but in this case the copper atom turns into ions and gets discharged....and on what basis does copper gets oxidised in preference with sulphate and hydroxide ion....could u pls clear my doubt

[@rosemarychacko3690]

Plz mam I am also confused

[@boliusabol822]

Electrons are pulled from the copper anode and that oxidises the copper anode itself. That's the oxidation that occurs there. It's of the anode itself. If it were a graphite anode then it'd attract anions. One has to know whether the electrode itself is reacting, or ions at it are reacting. A metal cathode will not react, but a metal anode will oxidise. Graphite would be inert whether it is the anode or the cathode.

[@tashspond]

And what amp/volts are necessary?

[@turboslayer9473]

Thank you so much Really helpful

[@CLR-mx4bu]

I don’t understand why the copper2+ becomes copper but the SO2- doesn’t become SO4? Why doesn’t the least reactive one always get discharged?

[@krivansemlani7984]

smart

[@boliusabol822]

Something at A level or AP, rather than GCSE, would show that The SO4^2- has a very low oxidation potential. (this can be seen looking at a table of reduction potentials). So SO4^2- will stay in solution. The metals below hydrogen in the reactivity series (low in reactivity series), don't tend to stay reacted in their ionic compound, they tend to reduce and become neutral. A table of reduction potentials show that Cu^2+ has a high reduction potential. Very unreactive ones in the reactivity series are strong candidates to get discharged. We don't see reactive metals like potassium getting discharged, but do with a metal much less reactive, like Copper.

[@gikscollections6280]

Good work

[@manishkumartiwari6762]

Please make videos on the whole chemistry part of 11th and 12th.

[@abigalebailey182]

What was the amperes that was used ?

[@sengkathirparri9311]

Thank You So Much !

[@lahiruperera3805]

Some people write anode reaction like this 2H2O ->O2+ 4H+ + 4e What is the difference

[@ChemJungle]

Both processes happen, and both make the same products so in most syllabuses you can write either answer and score the points... The water one you have here is a little more "correct" as the water would be in higher conc than the OH- so would be more likely to oxidise (the last gcse syllabus I taught wanted the OH- one though hence why it's in this video!)

[@aashishgottumukkale3043]

How about carbon electrodes? Do they get involved?

[@ChemJungle]

Nope :) Graphite is a form of carbon - these electrodes are inert in this scenario

[@covid-21delta99]

Graphite (Carbon) Electrodes only get involved at high temperatures with Oxygen and some other Elements...

[@magnuswootton6181]

watch out using electrolysis with sulphates, cause u might get mustard gas. it is actually magnesium sulphate that does it, copper sulphate doesnt, cause of extra complications, its not a simple model.

[@nellvincervantes3223]

Why you choose the lower reactivity?

[@shreyabhatia5507]

^^??

[@daemonk756890]

If it's lower reactivity it is more able to receive an electron and therefore get reduced. It's like the opposite of how you explain the group 1 metals getting more reactive as you go down the group. The outer shell electron is further away from the nucleus so therefore it is more easily lost and the metals get more reactive.

[@waseemahmed5682]

Really informative.... Good work....

[@DonaldSleightholme]

can copper sulfate be used as a replacement for mercury in a Faraday motor 🤔🤷‍♂️

[@jailnet]

OK, why was the solution copper sulfate present in refining of copper if we are not separating anything from the electrolyte?

[@magnuswootton6181]

isnt it copper coming out?

[@jailnet]

@@magnuswootton6181 concentration of copper ions remains constant in case of using pure copper as cathode and impure copper as anode. Explaination copper ions are both being removed and replaced at the same rate because formation (oxidation) of copper ions at anode happen at same rate of removal (reduction) of copper ions at form atoms at cathode. I hope this made sense

[@covid-21delta99]

You actually are separating Copper +2 ions from the Electrolyte which then gets reduced at the cathode to form Copper Atoms

[@leslieedirisingha5333]

Please explain why in the instance electrolysis of aqueous cuso4 using copper electrodes the anode reaction becomes copper oxidation process 😭

[@ChemJungle]

Because copper is more easily oxidised than the hydroxide ion or the water that's present. It's always the thing that's most easily oxidised that will lose electrons :)

[@alcurist]

THANK YOU

[@hixe7399]

what happens to the SO42- ions and H+ ions?

[@ChemJungle]

They stay in solution :) So you're left with sulphuric acid in the solution

[@kurulusxdestan]

thankyou so much for this ❤❤❤❤❤❤

[@mingiiyaa5673]

Thank you so much ✨✨

[@Oli-vj4pi]

thanks so much

[@minkhant1683]

Thanks alot!

[@mechackkaba8578]

Well done

[@nelsonandong263]

Good job

[@ChemJungle]

Thanks :)

[@TheCerberusInferno]

What gases are produced in this reaction ?

[@ChemJungle]

You get different products depending on which electrodes you use

[@manalkhan5048]

Thank you!

[@ChemJungle]

You're welcome :) hope it helped!

[@dribrahimel-nahhal2477]

Thanks for this vid

[@chamodrashmitha7454]

Thankyou very much madam

[@devanshimishra9969]

What is the observation? When u used copper electrode in copper(||) sulfate

[@ChemJungle]

You would see the cathode getting bigger (still orange with the copper) and the anode getting smaller. The blue solution would stay the same colour as every Cu2+ that gets used up, another one gets released into the solution (if you have graphite electrodes it gets paler and eventually colourless). No change to H+/OH- concentration so no change to pH.

[@abhilash5565]

Good

[@chandakatongo5992]

Thankyou sm

[@ChemJungle]

You’re welcome 😊

[@williamtamale9469]

Supper gal....only the dull wouldn't understand yr crystal klear explanation

[@ubinin7923]

This helped a lot

[@aguyfromaimagination9983]

Maccha pls teach me as my teacher pls

[@kcaptured6459]

Unne mehndi layi hui aye

[@husnainali3123]

Hi mam i need your help please reply me

[@dennismihailov136]

what you want

[@krivansemlani7984]

mehandi laga ke rakhna doli sajane ke rakhna

[@inkosiivumilethapelo3000]

Too fast. Had to watch the video many times

[@krivansemlani7984]

why coppaaa! why not copper?

[@johhnylhandes134]

lol she fitttt

[@ssathiabalan]

pls slow down with ur explanation, didnt pick up anything from the video. Im sorry. I didnt find this useful.

[@dylanjones9499]

Pls speak in English next time ;)

[@tanushbedi2667]

thank you so much

[@cryfan6828]

Thank you very much!