Thank you for this video! My mind tends to hit a brick wall at such confusing equations but the way you explained it really helped me understand. Again thank you!
iron + copper sulphate ------> copper + iron sulphate A displacement reaction occurs since carbon is more reactive than iron, you can check in the Reactivity Series. Symbol equation: Fe + CuSO4 ------> FeSO4 + Cu
Can you please explain to me more about the electroplating iron with copper in the laborarory using the copper sulphate solution. Copper as a anode and iron as a cathode
I believe in that case there must be additional reducing agent that provides 2e or otherwise the Iron would just be eaten away. In the case of PCBs, manufacturers used to use Formadahyde and hydrogen oxide to get the extra electrons. Copper bags are submerged in Formadahyde solutions and electric fields blasts these towards the PCB anode.
One of the three test that passivate technicians would do is the "copper sulfate test" if said part has had removal og ferrous contaminants like free iron from their surface then when dipped into copper sulfate, the part shouldn't turn pink.
this is a rather old video. however, say you let the entire nail dissolve in an oversaturated copper sulfate solution. when seperated and dried; often i find 2 but sometimes 3 distinctly colored "powder", one black one white and the familiar "rose color"; am i right to assume the black and white are in fact the 2 copper oxides? as a side note/mention i find distilled water produced more "typical" rose colored particles. if you add a little bit of silicone oil to the copper sulfate solution and either , remove or let what ever catalyst fully dissolve; then seal and shake the container the copper particles will cling to the silicone oil and form spherical balls of varying size, it looks like you have airsoft bbs floating in the solution. and it becomes nearly impossible to dissipate the spheres, they are far more likely to combine with eachother to form a bigger ball. the key here is the silicone oil, however i dont know exactly why or how, bht assume it has something to do with surface tension as the spheres are only just a shell. and to be clear, there is no definate "core" or center, and i dont believe its just sticking to the silicone oil like dust to chewing gum, because the balls can drift up and down while the silicone oil leaves an almost clear seperation like oil and vinegar. oh ya almost forgot, if you poke them with a stick or rod etc, they will break apart and the particulates will eventually drift down to the bottom as you would expect.
+Princess Pineapple Exactly as it appears in the video. Until I bring in the second beaker, this is filmed in real time. There is no speeding up. The solution does not bubble, The iron nail simply becomes coated with pink copper. The solution changes from blue to green over the course of about an hour.
When Iron nail is added to Blue solution copper sulphate , it gives Green Solution i.e Ferrous Sulphate and a pink lustrous metal Copper .... This is the observation what I usually write .
It is in aqueous solution at the end of the reaction. Iron II Sulphate is quite a pale green crystal in solid form but creates a slightly darker green solution. In my video, the colour could also be possibly be a little darker due to minute copper particles which have detached and have yet to settle (partial suspension)
If you were to do this with a steel nail, what would happen to the carbon in the steel? Would it simply crumble out of the iron and form a black layer over the copper?
+Connor Steppie The percentage of Carbon in normal mild steel is only up to about 0.25% so you would not see a layer. In order to get the whole nail to react, it is best to dislodge (by stirring or scraping off) the copper to reveal the unreacted iron below. The Carbon would simply be mixed in with the copper sludge that is produced.
is anyone not watching this for homework? some people actually do this at home. im using zinc instead of iron to make zinc sulfate for electroplating motorcycle parts. and see how it compares to a vinegar + Epsom salt solution. it still gives off copper in the process.
+Mr.chang cooler Indeed! In fact, I often use a drop or two of Copper Sulphate solution to get aluminium/acid reactions going as they are impeded by the aluminium oxide layer. Unfortunately, although this does get the reaction going, bits of copper appearing in the reaction can be a level of complexity too much for students.
Moonlight - This is absolutely a chemical reaction as new products are formed and, as Iron is the more reactive metal, copper will never be able to displace it to reverse the reaction.
Yes - But evaporate gently (without Bunsen if you have time). The pale green crystals can easily lose their water of crystallisation to become brown anhydrous Iron II Sulphate and if heated further this may release Sulphur Trioxide (white acidic fumes - very dangerous by inhalation) and reddish brown Iron III Sulphate
I did not use a pre-made solution. A couple of spatulas full in 100ml water gave a nicely coloured solution. Estimating the mass to be about 5g this equates to a 0.2M solution.
Only sorry I can't get to the lab to do more videos during these difficult times. My very best wishes to everyone. Stay safe & stay well.
Thank you for this video! My mind tends to hit a brick wall at such confusing equations but the way you explained it really helped me understand. Again thank you!
@Kabeer Sharma I by mistake wrote to you but i wanted to ask it to Martin Godber
This is poop
@@samyakjagtap3763 ???
OP hai bhai
"Small amount in the beaker" *uses half bottle of Cuso4*
It's a small bottle.... and a small beaker!! :-)
2 shots of vodka
Anyone here after getting the link from an online class....?
Me
hello my friend
Me
Me lmfao
Me
Hi Martin!! Lovely to hear your voice! I am showing this clip to my students tomorrow during our 'live lesson'. Hope you are well.
Thanks you really helped me with my homework!!!!!!!!!!!!!!!!!
Lol same!
OMG! me too!...CHEM HW
pls reply
@@pathexe13 I got u
Every one of us has The same homework?
iron + copper sulphate ------> copper + iron sulphate
A displacement reaction occurs since carbon is more reactive than iron, you can check in the Reactivity Series.
Symbol equation:
Fe + CuSO4 ------> FeSO4 + Cu
It's because Iron is more reactive than Copper. There's no Carbon involved.
@@martingodber3907 He means to say in the reactivity series Copper (Cu)is more reactive than Iron (Fe)but still it displace copper, why?
@@sakshiankur4607 no. Iron is more reactive than copper.
@@martingodber3907 Yes you are absolutely right, I just told you what this men wants to say. That's it
finally someone that can explain science on youtube thank you
This is a brilliant and simple video that helped me a lot with my common entrance practise, thank you! 😄👍🏻
That was extremely concise and quick to the point! I enjoyed every second. You earned a subscriber.
Thank you sir My daughter doing this project to her she helped this activity
I left st pauls 2 years ago but your still helping me with chemistry now. Cheers Mr Godber thanks for the help
Glad I could help!
This helped me so much for my practical thank you :)
Thanks for this, it honestly couldn't have been more simply helpful
Oh man thank you very much man...its because of you that i was able to do my homework thank you.☺😊😀
Short but very brief! Thanks
thank you!!!!!!!!!!
you made my exam good for me!!!!!!
best man !!!!!!!
so interesting, we learn new things everyday
THANKYOU SOOO MUCH!!! IT REALLY HELPED - IT HELPED A LOT. THANKS KEEP IT UP!!!
so Fe + CuSO4 ====> FeSO4 + Cu
yeah basically
@@tenzonium Nothing happens in FeSO4 + Cu
Copper is less reactive, so the aqueous solution won't work.
@@anasnasarullah5055 thank you
@@tenzonium Welcome
anyone here after they have homework on this or their online teacher sent it
yah
i missed the demonstration she did on zoom so im using this video lol
This video is really super duper cool. One day I hope i can preform a medical procedure such as this
wow ur so cool
no you
Your video was really helpful for me
WAIT WUT??? i initially thought that it was rust!! THANK YOU FOR MAKING THIS VID!!
its not even the same color as rust...
@@darkshadowsx5949 still can be easy to mistake though.
Thanks so much!! Science made easy 😁
Who is here 4 homework?
Copper recovery lab 😑
people still have homework? its 2019
It's me
Me
Hiya
Thanks a lot for the explanation
I need this explanation for the test
It’s old Tommy in it
Martin great work
Sir you tell v.v good. This is the best video for this reaction
Interesting and helpful
Nice explanation sir,kindly upload more videos to elaborate chemical reaction
Can you please explain to me more about the electroplating iron with copper in the laborarory using the copper sulphate solution. Copper as a anode and iron as a cathode
I believe in that case there must be additional reducing agent that provides 2e or otherwise the Iron would just be eaten away. In the case of PCBs, manufacturers used to use Formadahyde and hydrogen oxide to get the extra electrons. Copper bags are submerged in Formadahyde solutions and electric fields blasts these towards the PCB anode.
Very nice video
Thanks! Really helpful vid.
Thank you :-)
Your video was really helpful for me ❤
Emejing
One of the three test that passivate technicians would do is the "copper sulfate test" if said part has had removal og ferrous contaminants like free iron from their surface then when dipped into copper sulfate, the part shouldn't turn pink.
as i could not hear the video i searched it on youtube and i am here
How do you get such a shiny copper layer? When I perform this test I get a lustreless brown collor :(
nice video
thank you for your help for my examinition
The explanation was perfect.plzz make other videos plzz.
Glad it made sense. Hope to be back in my lab in September!
Wonderful. Thanks 😊
Great
Thank you sir...
thnx
this is a rather old video. however, say you let the entire nail dissolve in an oversaturated copper sulfate solution. when seperated and dried; often i find 2 but sometimes 3 distinctly colored "powder", one black one white and the familiar "rose color"; am i right to assume the black and white are in fact the 2 copper oxides?
as a side note/mention
i find distilled water produced more "typical" rose colored particles. if you add a little bit of silicone oil to the copper sulfate solution and either , remove or let what ever catalyst fully dissolve; then seal and shake the container the copper particles will cling to the silicone oil and form spherical balls of varying size, it looks like you have airsoft bbs floating in the solution. and it becomes nearly impossible to dissipate the spheres, they are far more likely to combine with eachother to form a bigger ball. the key here is the silicone oil, however i dont know exactly why or how, bht assume it has something to do with surface tension as the spheres are only just a shell. and to be clear, there is no definate "core" or center, and i dont believe its just sticking to the silicone oil like dust to chewing gum, because the balls can drift up and down while the silicone oil leaves an almost clear seperation like oil and vinegar. oh ya almost forgot, if you poke them with a stick or rod etc, they will break apart and the particulates will eventually drift down to the bottom as you would expect.
makasih abang video nya sangat membantu semoga abang dijemput ajal dalam keadaan sehat
thanks alot
helped with my exam
So iron is more reactive when it comes to acid than copper right?
Absolutely. Iron is more reactive than Copper generally. Acids, Oxygen etc.
Thank you sooo much sir!😮😮😮
Thanks a lot!❤️
cheers mate really helped
VERY COOL
THANK FOR THE COOL NAIL :[]
this explanation is best....u saved the day...
Glad you liked it!
Thanks for my exhibition
+Martin Godber What is an observation you will see during the reaction?
+Princess Pineapple Exactly as it appears in the video. Until I bring in the second beaker, this is filmed in real time. There is no speeding up. The solution does not bubble, The iron nail simply becomes coated with pink copper. The solution changes from blue to green over the course of about an hour.
When Iron nail is added to Blue solution copper sulphate , it gives Green Solution i.e Ferrous Sulphate and a pink lustrous metal Copper .... This is the observation what I usually write .
wowwww it was amazing!!!
Please make more videos of chemistry's experiments
Who else are watching this when their teacher shown them in class
where has feso4 gone?
It is in aqueous solution at the end of the reaction. Iron II Sulphate is quite a pale green crystal in solid form but creates a slightly darker green solution. In my video, the colour could also be possibly be a little darker due to minute copper particles which have detached and have yet to settle (partial suspension)
so clear. thanq so much sir.....:)
Hello Mr! I'm doing a copper sulfate aluminium copper battery! Do you have any recommendations on how I should handle a copper sulfate solution?
Thanks sir.
Can u tell me the texture of copper displaced?
Like, does it form a rough and granular surface or is it flaky?
That kind of looks like cool-aid. Anyways thanks for the help on the homework
Thanks sir 👍👍
thanks realy helpful
love your accent
thank you
mm that blue rasperry sprite look tasty
If you were to do this with a steel nail, what would happen to the carbon in the steel? Would it simply crumble out of the iron and form a black layer over the copper?
+Connor Steppie The percentage of Carbon in normal mild steel is only up to about 0.25% so you would not see a layer. In order to get the whole nail to react, it is best to dislodge (by stirring or scraping off) the copper to reveal the unreacted iron below. The Carbon would simply be mixed in with the copper sludge that is produced.
Long answer :
Short answer : congratulations you got a molten iron and copper sulphate reincarnat as a iron sulphate and becomes green
very cool
Glad you like it. It's a great bit of chemistry!
Very interesting
Thanks Sir
does the total mass of iron in the nail change after the solution ? does the iron break away from the nail and form feSO4?
Yes, That's correct.
@@martingodber3907ok thanks
Is the product (iron sulfate) ferrous sulfate or ferric sulfate? (I'm guessing it's ferrous sulfate, no?)
It's Iron (II) Sulphate (Ferrous) - Hence the distinctive green colour.
is anyone not watching this for homework? some people actually do this at home.
im using zinc instead of iron to make zinc sulfate for electroplating motorcycle parts. and see how it compares to a vinegar + Epsom salt solution.
it still gives off copper in the process.
what would be the effect on heating the ferrous sulfate then? Thanks in advance
M in class 7, so helpful
😀 understood in only 1 min
Glad it helped!
Thank s
I am a poolman. Copper sulphate is a great algaecide. Can you tell me how to suspend copper sulphate in water. namely swimming pool water?
Hi! I was wondering if this is a chemical change or a physical change.
Definitely a chemical change - New substances are formed - Rearrangement/re-bonding of constituent atoms
0:16 pardon me sir but , you didn't added few drops of dilute sulphuric acid
There is no need to acidulate the solution to obtain a reaction.
👍👍👍👍👍
So, if you placed aluminium in a copper sulfate solution, would the aluminium displace the copper as well?
+Mr.chang cooler Yes it would.
Martin Godber Even with its oxide layer?
+Mr.chang cooler Indeed! In fact, I often use a drop or two of Copper Sulphate solution to get aluminium/acid reactions going as they are impeded by the aluminium oxide layer. Unfortunately, although this does get the reaction going, bits of copper appearing in the reaction can be a level of complexity too much for students.
Martin Godber Amazing! Thank you for your response.
Nice vid
Nice, Thanks
What is the colour of the copper after displacement reaction?
Pink initially but brown (almost black) as a large deposit builds up.
I know it is copper.
Is it a chemical change or a physical change though?
Moonlight - This is absolutely a chemical reaction as new products are formed and, as Iron is the more reactive metal, copper will never be able to displace it to reverse the reaction.
Martin Godber Okay tyvm!!
its Chemical
Obviously a new substance is formed
Can we crystalize this few04 solution to form ferrous sulphate crystals
Yes - But evaporate gently (without Bunsen if you have time). The pale green crystals can easily lose their water of crystallisation to become brown anhydrous Iron II Sulphate and if heated further this may release Sulphur Trioxide (white acidic fumes - very dangerous by inhalation) and reddish brown Iron III Sulphate
can stainless stick also work at this reaction ?
Anymore vids?
well in
Sir brown layer is cu or Fe??????
Copper. The Copper is displaced from the Copper Sulphate by the (more reactive) Iron.
What molarity should someone use when making the solution?
I did not use a pre-made solution. A couple of spatulas full in 100ml water gave a nicely coloured solution. Estimating the mass to be about 5g this equates to a 0.2M solution.
The 100 dislikes: students