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
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 :)
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"!!!!!
@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?
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
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 :)
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
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. czcams.com/play/PLikL-gQhJ0DmknULDIeGei3l2Q__dEfI7.html
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.
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!)
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 :)
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.
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.
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.
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.
@@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
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.
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
probably one of the only educational youtube videos i’ve ever found helpful!
in love with your channel!! Thank you so much for your videos
That was really helpful!!! Thank you so much!🙏🙏🙏
The video was Good and really explained clearly and properly! Thank u so much!
OMG I had this one confused for almost months and you made it clear within 5 minutes
TYSM :)
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 :)
whatever you do, if u actually do this electrolysis stuff watch out for poison gas emission!!!
Loved the mehandi on your hand and the lecture too, Thanks a ton.
omg explained SO WELLL
The Explanation was very clear, thank youuuu
Amazing explanation from Henry and Esther
Thank you
perfect explain it is so complete .it make me totally understand.thanks
Demn she has got mehendi on
Lmaooo
What I focus on instead of trying to understand chem... 🥲
you have saved my life thank you
Very clear, super stuff! Mr J
Glad it was helpful!
i legit love you thank u
What a video, honestly teach me chemistry I'd pay anything to study from you
GOAT video love u
Thank you so much
Really helpful
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"!!!!!
Good work... Coincidentally I have done the demonstration experiment for this on my channel.... I see we are in tune... Thank you madam
Thank you so much ✨✨
Thank You So Much !
Thank you very much!
thanks so much
Thanks alot!
Good work
This help me thanks ( from a prepa french student )
thankyou so much for this ❤❤❤❤❤❤
Well done
THANK YOU
thank you so much
@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?
Great video!
Thanks!
Thanks for this vid
Please make videos on the whole chemistry part of 11th and 12th.
1:22 Can you explain why sulfide never gets discharged? is it because it has a higher reduction potential?
What was the amperes that was used ?
And what amp/volts are necessary?
Good job
Thanks :)
Good
Thankyou sm
You’re welcome 😊
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
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 :)
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
Plz mam I am also confused
what happens to the SO42- ions and H+ ions?
They stay in solution :) So you're left with sulphuric acid in the solution
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. czcams.com/play/PLikL-gQhJ0DmknULDIeGei3l2Q__dEfI7.html
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.
How about carbon electrodes? Do they get involved?
Nope :) Graphite is a form of carbon - these electrodes are inert in this scenario
Graphite (Carbon) Electrodes only get involved at high temperatures with Oxygen and some other Elements...
Some people write anode reaction like this
2H2O ->O2+ 4H+ + 4e
What is the difference
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!)
Please explain why in the instance electrolysis of aqueous cuso4 using copper electrodes the anode reaction becomes copper oxidation process 😭
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 :)
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.
What gases are produced in this reaction ?
You get different products depending on which electrodes you use
Supper gal....only the dull wouldn't understand yr crystal klear explanation
mehandi laga ke rakhna doli sajane ke rakhna
Too fast. Had to watch the video many times
why coppaaa! why not copper?
lol she fitttt
Pls speak in English next time ;)
pls slow down with ur explanation, didnt pick up anything from the video. Im sorry. I didnt find this useful.
Really informative....
Good work....
Well explanation
Thankyou very much madam
Thank you!
You're welcome :) hope it helped!
can copper sulfate be used as a replacement for mercury in a Faraday motor 🤔🤷♂️
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.
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.
@@ChemJungle why did copper lose electons just to gain it back
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?
smart
This helped a lot
Why you choose the lower reactivity?
^^??
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.
OK, why was the solution copper sulfate present in refining of copper if we are not separating anything from the electrolyte?
isnt it copper coming out?
@@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
You actually are separating Copper +2 ions from the Electrolyte which then gets reduced at the cathode to form Copper Atoms
What is the observation? When u used copper electrode in copper(||) sulfate
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.
Hi mam i need your help please reply me
what you want