*This battery reconditioning program exceeded my presumptions. It worked on any drill battery, several AA and AAA batteries, **batery.repair** and any camera battery. The steps are simple and the act itself is exciting to do. No matter what type of battery you`ve got, it is sure to function again!*
because it's wrong XD, those ions must be already in the solution, either leaving copper oxidize in sulfuric acid on it's own or charging the battery or pouring copper sulfate in the solution which is already oxidized, otherwise copper will not oxidize easily if connected with the more basic(zinc sulfate) solution so copper atoms are not going to abandon the metal surface easily they will rather make zinc oxidize faster. For the discharging reaction to occur you must have zinc metal oxidizing in an acid and copper ions reducing to go back copper metal
Well, it's a little bit tricky because I explained it the "soft" way. In fact, the salt bridge also transfers ions from one pot to the other. So, there is an exchange between: a) salt bridge AND left pot, b) salt bridge AND right pot, and left pot AND right pot.
Best explanation I found after spending soo much time looking. Other videos don't explain the role of the salt bridge. They also make it sound like copper won't release ions in aqueous solutions. Like there's some fundamental difference between copper and zink in that regard.
well what makes you think that the creator of this video is correct? Maybe copper actually doesn't release ions in aqueous solution for example. This guy looks like he mostly does graphic design and translation but is he a chemist?
The anode is the negative TERMINAL, meaning the electrons flow from the anode (zinc) to the cathode(copper). The Anode is negative because the electrons stay in the zinc strip and later flow to the cathode, while the zinc atoms from where the electrons are released from jump INTO the solution and become ions. So basically, only the electrons and the normal atoms of zinc remain in the anode while the atoms that become positive LEAVE the anode.
2:10 I'm confused by Oxidation. If both rods are initially uncharged and the zinc/copper in the solution are positively charged, then why wouldn't the electrons flow into the solution? Why do the atoms move into the solution as positive ions (positive into positive) and leave electrons on the rod? 2:45 If both rods are gaining electrons, then why does the zinc become positively charged and the copper negatively charged? Shouldn't both gain a negative charge, but the zinc would gain it faster? I'm still confused by this process
+maxpowers3732 I think this is the reason, as you doubted Cu too can lose electrons. But in this case Zn loses electrons easily than Cu. So released electrons from Zn travel to Cu plate(electrode. Then Cu plate becomes negatively charged. As you know negatively charged Cu plate attract positive ions. Look at the electron configuration of Cu and Zn. For Zn it is easy to lose 2 electrons but in Cu to become Cu2+ ion i have to 1 d-electron from inner shell. Cu:[Ar] 3d10 4s1 Zn: [Ar] 3d10 4s2 or other way, Zn can achieves more stability than Cu due to fully filled d-orbital by losing 2 valence electrons. Cu:[Ar] 3d9 4s2 Zn: [Ar] 3d10 4s2
6 ปีที่แล้ว +1
GOOGLE THERMITE! GOOGLE HOW THAT WORKS! GOOGLE DISPLACEMENT REACTIONS! That's ALL you need.
You messed up. You show the Positive copper ions leaving their electrons in the electrode and becoming part of the copper sulfate solution. the electrons are pulled from the electrode by the sulfate creating negative ions in the electroe not the electrolyte. this creates a potential energy as the electrons left in the zinc electrode create a current that fills the positively charged copper ions in the copper electrode. The electrons expelled from the copper electrode (in a battery) pass through the membrane to neutralize the zinc negative ions
why can't electron pass thru the salt bridge? why can't you form a battery with copper and zinc touching each other? why doesn't zinc atom donate the electron to the H+ and form H2, why does it flow thru the circuit? Why doesn't zinc atom donate e to the H+ and form H2 WITHOUT any closed circuit? why do you need a salt bridge at all? why can't you just have 2 solutions mixed together? if it is indeed the magic of the salt bridge, what about a lead acid battery? Why doesn't any TH-cam video comes close to explain those questions? have any video maker thought thru the entire process at all?
your video explained how's, you seldom explained why's, and you never explained any why not's. Please, if possible, answer the other half of my questions that weren't in the video
If both electrodes are becoming negatively charged, it seems misleading that both start at 50, and the zinc climbs to 80, and the copper lowers to 20. Would it not be more appropriate to raise the zinc from 50 and raise the zinc to a higher number?
I dont understand how positive ions can go to the B side (cathode), when the electrons from A side go there, but they can't just return to A side. You would probably say because of the oxidation. But this oxidation happens on both sides. Does anyone has idea?
I don't understand why zinc can lose its electrons even if it is in ZINC sulphate solution? I mean the zinc atoms in the anode and the zinc ions in the solution are both zinc!
Because here to metallic pressure is greater than osmotic pressure so to balance we increase osmotic pressure by increasing concentration in solutions. To increase concentration of solution add ions.
If the solution in the salt bridge is used for balancing the two reservoirs, why is the bridged connection required at all? Why not just have two disconnected tubes? Please help. I've been trying to wrap my head around the salt bridge for days now. No one I've talked to has any answers...
Hai,Thanks for the video.It was helpful. I have a doubt regarding this by the way.I understand that salt bridge is Na2SO4 salt.When Oxidation happens, Zinc atom loses its 2 electron which goes to the external circuit and zn2+ ion will be in the zinc sulphate solution.Zinc ion reacts with SO4 2- ions from the salt bridge and the electrolyte would be neutral.Now in the cathode part Copper from copper sulphate solution combines with the 2 electrons from the anode and copper metal deposites on the cathode leaving soa 2- ions.This makes the electrolyte at cathode negative in charge. 1.What happens to SO4 2- ions,does it combine with Na2+ ions in the salt bridge turning the solution a mixture of Na2SO4 and Cu2SO4 solution? 2.Untill what condition does the redox reaction prolong,Is it untill zinc totally gets consumed or at a condition where there is no more Na2+ or SO4 2- ions in Salt bridge to balance the electolytes?
1-YOU HAVE TAKEN SO4 ALL WHERE THATS WHY IT IS KIND OF CONFUSING OF WHICH SO4 YOU ARE TALKING ABOUT SO LET ME TAKE NANO3 AS SALT BRIDGE SALT .WHEN Zn metal loses electrons it get converted to Zn ion WHICH IS POSITIVE SO AS IT CONTINUES TO LOSE ELECTRONS THERE IS ACCUMULATION OF +ive CHARGE AND IN COPPER HALF CELL THERE IS VERY LESS Cu+2 AS COMPARED TO SO4-2 AS MOST OF Cu+2 IS CONVERTED TO CU METAL BY GAINING THOSE 2 ELECTRON LOST BY ZINC METAL SO -ive CHARGES ARE BUILD THIS WILL STOP FLOW OF ELECTRONS SO NOW SALT BRIDGE COMES IN IN MY CASE To balance +ive zinc NO3 FROM SALT BRIDGE WILL COME IN ZINC HALF CELL ,AND TO BALANCE -ive so4 Na +from salt bridge will come in copper half cell. 2-in both conditions i.e when salt bridge is removed and when complete zinc metal will be used the flow of electrons will be stopped.
Thanks for the explanation, but can anyone please explain to me how the flow of charges is maintained after the Cu ions are pulled to the Cu electrode and the electrode hence becomes neutral?
your voice confused me. but other than that it was good, i would like to request a video on electrolysis(mainly history, electroplating, and how its done using different voltage).
2:14 Okey, zinc is reactive, but I still can't understand what causes zinc to lose electrons if the solution is uncharged. Will the mere presence of sulfate ions around the metallic zinc induce the ionization?
At 2:38 - 2:43, can anyone explain when CU metal lose electrons at a much slower rate than Zn, why Zn still lose electrons to CU? I thought electrons usually flow to areas when it has fewer electrons?
*This battery reconditioning program exceeded my presumptions. It worked on any drill battery, several AA and AAA batteries, **batery.repair** and any camera battery. The steps are simple and the act itself is exciting to do. No matter what type of battery you`ve got, it is sure to function again!*
2:32 - Many textbooks fail to mention this point.
You are right
because it's wrong XD, those ions must be already in the solution, either leaving copper oxidize in sulfuric acid on it's own or charging the battery or pouring copper sulfate in the solution which is already oxidized, otherwise copper will not oxidize easily if connected with the more basic(zinc sulfate) solution so copper atoms are not going to abandon the metal surface easily they will rather make zinc oxidize faster. For the discharging reaction to occur you must have zinc metal oxidizing in an acid and copper ions reducing to go back copper metal
True
I didn't grasp everything because I'm kinda STOOPID but I appreciate that you've made this well done explanation. It makes a bit more sense
It doesn't matter if you're stoopid if you're sexy.
The best thing about this video is the soundtrack.
A very helpful explanation. Thank you
There will be a day, when I will do exactly this! Thank you for your input.
That's what it's supposed to do. Thank you for your comment :)
Thank you! You may just have saved my chemistry grade!
Thanks for your comment. I'll keep it up :)
The real science explanation ,👍👍👍👍not just a fancy blackboard imagination 😂
Thank you🙏🙏🙏🙏
love the way the electron red-ox are presented in the animation. Makes it easier to understand.
And thank you for your comment :)
A salt bridge can be any solution that is able to harmonize the two solutions. KNO3 is just an example.
Wonderful!!! Thank you for your comment! :)
wow this was very good. im an visual learner so to look at how this REALLY works really helped
Well, it's a little bit tricky because I explained it the "soft" way. In fact, the salt bridge also transfers ions from one pot to the other. So, there is an exchange between: a) salt bridge AND left pot, b) salt bridge AND right pot, and left pot AND right pot.
Thank you very much :)
Best explanation I found after spending soo much time looking.
Other videos don't explain the role of the salt bridge. They also make it sound like copper won't release ions in aqueous solutions. Like there's some fundamental difference between copper and zink in that regard.
well what makes you think that the creator of this video is correct? Maybe copper actually doesn't release ions in aqueous solution for example. This guy looks like he mostly does graphic design and translation but is he a chemist?
@@aymi6393 yeah i have the same doubt...
Because ions must travel from one pot to another. If not, there will be an imbalance. It's clear if you watch the animation closely.
no problem, id been having trouble with this and redox reactions in general and text books can be confusing. This video helps a lot.
Perhaps in the future, yes.
Thank you. finally got a better understanding 👍
DangerouslyFunny is this man!
Thank YOU, for your comment :)
Well explaination
The anode is the negative TERMINAL, meaning the electrons flow from the anode (zinc) to the cathode(copper). The Anode is negative because the electrons stay in the zinc strip and later flow to the cathode, while the zinc atoms from where the electrons are released from jump INTO the solution and become ions. So basically, only the electrons and the normal atoms of zinc remain in the anode while the atoms that become positive LEAVE the anode.
Wow great explation...Thank you....i am a high school student and i am struggling a much in this concept of electrochemistry...
2:10
I'm confused by Oxidation. If both rods are initially uncharged and the zinc/copper in the solution are positively charged, then why wouldn't the electrons flow into the solution? Why do the atoms move into the solution as positive ions (positive into positive) and leave electrons on the rod?
2:45
If both rods are gaining electrons, then why does the zinc become positively charged and the copper negatively charged? Shouldn't both gain a negative charge, but the zinc would gain it faster?
I'm still confused by this process
+maxpowers3732
I think this is the reason,
as you doubted Cu too can lose electrons.
But in this case Zn loses electrons easily than Cu.
So released electrons from Zn travel to Cu plate(electrode. Then Cu plate becomes negatively charged. As you know negatively charged Cu plate attract positive ions.
Look at the electron configuration of Cu and Zn. For Zn it is easy to lose 2 electrons but in Cu to become Cu2+ ion i have to 1 d-electron from inner shell.
Cu:[Ar] 3d10 4s1
Zn: [Ar] 3d10 4s2
or other way,
Zn can achieves more stability than Cu due to fully filled d-orbital by losing 2 valence electrons.
Cu:[Ar] 3d9 4s2
Zn: [Ar] 3d10 4s2
GOOGLE THERMITE!
GOOGLE HOW THAT WORKS!
GOOGLE DISPLACEMENT REACTIONS!
That's ALL you need.
@ shut up
Thank YOU for your wonderful comment :)
Nice video , looking forward for more of such videos
Thank you!
Can I get your Instagram ID
Very nice explanation, cheers!
Thank you! This is so clear.....
I still didn't get it
Thank you
@ well this is not the answer which he was searching for!!!!
Physical chemistry uni exam tomorrow, thank u so much!
OMG YOU SAVED MY LIFE
Very nice
Thank you :)
very well explained
its vry use full for study......
Love your videos!!!! Please keep up the good work! Best regards!
Man thank you so much 😊😊😊😊😊😊
Really helpful, finally, I got it, thanks for sharing.
why did both zinc and copper became ions when placed in the solution and left their electrons on the electrodes?
Watch again!
You messed up. You show the Positive copper ions leaving their electrons in the electrode and becoming part of the copper sulfate solution. the electrons are pulled from the electrode by the sulfate creating negative ions in the electroe not the electrolyte. this creates a potential energy as the electrons left in the zinc electrode create a current that fills the positively charged copper ions in the copper electrode. The electrons expelled from the copper electrode (in a battery) pass through the membrane to neutralize the zinc negative ions
why can't electron pass thru the salt bridge?
why can't you form a battery with copper and zinc touching each other?
why doesn't zinc atom donate the electron to the H+ and form H2, why does it flow thru the circuit? Why doesn't zinc atom donate e to the H+ and form H2 WITHOUT any closed circuit?
why do you need a salt bridge at all? why can't you just have 2 solutions mixed together? if it is indeed the magic of the salt bridge, what about a lead acid battery?
Why doesn't any TH-cam video comes close to explain those questions? have any video maker thought thru the entire process at all?
Just watch again. Half of your questions can be easily explained when watching the animation carefully :)
your video explained how's, you seldom explained why's, and you never explained any why not's. Please, if possible, answer the other half of my questions that weren't in the video
Thomas Schwenke
yeah but still, it's only half
does the creator of this video even know chemistry? What if he wasn't correct in that copper and zinc both release ions to their solution?
YL Storage
Thnx brother... god bless u
Helpful
Thanks
Every other person understood the video... Perhaps you should check Wikipedia or another website.
Cleared my doubt!
:)
keep making these vids man !
Thx. I'll try to do so!
Awesome
Thank you
well explained
very nice
Salt bridge also complete the circuit and maintains neutrality
great explanation. but when this redox reaction will stop and why?
You're welcome :)
Thanks!!!!!!! Super video!!!
best electrochem vid I have seen so far, thank you!
Thank you for your comment :)
Great :)
Thanks man :D really helpfull
So the difference in potential is due to the different number of electrons in both electrodes ?
If both electrodes are becoming negatively charged, it seems misleading that both start at 50, and the zinc climbs to 80, and the copper lowers to 20. Would it not be more appropriate to raise the zinc from 50 and raise the zinc to a higher number?
I dont understand how positive ions can go to the B side (cathode), when the electrons from A side go there, but they can't just return to A side. You would probably say because of the oxidation. But this oxidation happens on both sides. Does anyone has idea?
Really helpful 👍
Thanku so much
Thanks
I don't understand why zinc can lose its electrons even if it is in ZINC sulphate solution?
I mean the zinc atoms in the anode and the zinc ions in the solution are both zinc!
Because here to metallic pressure is greater than osmotic pressure so to balance we increase osmotic pressure by increasing concentration in solutions. To increase concentration of solution add ions.
Sir, you cleared doubt
verry nice
can i ask? how do concentration of the solutions affect the voltage? hope u will reply to this
Electric potential is an intensive property, so the concentration does not affect it.
If the solution in the salt bridge is used for balancing the two reservoirs, why is the bridged connection required at all? Why not just have two disconnected tubes? Please help. I've been trying to wrap my head around the salt bridge for days now. No one I've talked to has any answers...
I could not understand why the anode is negative when its give out electrons to the other electrode ?
Unbelievable ;)
Watch again! You'll understand sooner or later.
Nice helped me a lot...😄
thanks Thomas
Hai,Thanks for the video.It was helpful.
I have a doubt regarding this by the way.I understand that salt bridge is Na2SO4 salt.When Oxidation happens, Zinc atom loses its 2 electron which goes to the external circuit and zn2+ ion will be in the zinc sulphate solution.Zinc ion reacts with SO4 2- ions from the salt bridge and the electrolyte would be neutral.Now in the cathode part Copper from copper sulphate solution combines with the 2 electrons from the anode and copper metal deposites on the cathode leaving soa 2- ions.This makes the electrolyte at cathode negative in charge.
1.What happens to SO4 2- ions,does it combine with Na2+ ions in the salt bridge turning the solution a mixture of Na2SO4 and Cu2SO4 solution?
2.Untill what condition does the redox reaction prolong,Is it untill zinc totally gets consumed or at a condition where there is no more Na2+ or SO4 2- ions in Salt bridge to balance the electolytes?
1-YOU HAVE TAKEN SO4 ALL WHERE THATS WHY IT IS KIND OF CONFUSING OF WHICH SO4 YOU ARE TALKING ABOUT SO LET ME TAKE NANO3 AS SALT BRIDGE SALT .WHEN Zn metal loses electrons it get converted to Zn ion WHICH IS POSITIVE SO AS IT CONTINUES TO LOSE ELECTRONS THERE IS ACCUMULATION OF +ive CHARGE AND IN COPPER HALF CELL THERE IS VERY LESS Cu+2 AS COMPARED TO SO4-2 AS MOST OF Cu+2 IS CONVERTED TO CU METAL BY GAINING THOSE 2 ELECTRON LOST BY ZINC METAL SO -ive CHARGES ARE BUILD THIS WILL STOP FLOW OF ELECTRONS SO NOW SALT BRIDGE COMES IN IN MY CASE To balance +ive zinc NO3 FROM SALT BRIDGE WILL COME IN ZINC HALF CELL ,AND TO BALANCE -ive so4 Na +from salt bridge will come in copper half cell.
2-in both conditions i.e when salt bridge is removed and when complete zinc metal will be used the flow of electrons will be stopped.
@@shaikhzoya2002 nicely explained....thanx yrr
Nice intro music 😂✌️
Thanks for the explanation, but can anyone please explain to me how the flow of charges is maintained after the Cu ions are pulled to the Cu electrode and the electrode hence becomes neutral?
a salt bridge is used
Why do we need a Salt Bridge if Electrons can travel through a copper wire?
Thank you!! Now I understand :)
Great 👍👍👍
can this be recharchable?
see this is what happens when science is put in plain English, people get it !!
your voice confused me. but other than that it was good, i would like to request a video on electrolysis(mainly history, electroplating, and how its done using different voltage).
what an explanation sir!y the hell i wont understand by reading books?
can you explain the salt bridge working and significance a little more elaborate ..if possible?
2:14 Okey, zinc is reactive, but I still can't understand what causes zinc to lose electrons if the solution is uncharged. Will the mere presence of sulfate ions around the metallic zinc induce the ionization?
At 2:38 - 2:43, can anyone explain when CU metal lose electrons at a much slower rate than Zn, why Zn still lose electrons to CU? I thought electrons usually flow to areas when it has fewer electrons?
Hats off
What if the solutions I will use are different? For example hydroxhloric acid
Help pls asap
now get it✌
tnxx
Thank you!!!
Which one is the indicator electrode??
BRAVO
2:46 at this copper 2+ ion gets deposited on cathode but what are you showing in not true.
ty
awesome
This reaction will go on until the salt bridge looses its free ions.
All my childhood, I was told anode is positively charged electrode 😭😭, please help.
MeM fisto Anode is positively charged, thus it attracts negative charged ions.
Anode is positively charged in electrolytic cell but negatively charged in galvanic cell.
@@jhanvihemlani8248 Poor explation
@@AyushSingh-eg4jq yes correct
@@khusburawat9305 No, it wasn't a poor explanation. I literally said a correct statement.
Remove the background nuisance
Plz
Can you please do something on Electrolysis.
Electrolysis is much easier than this
Galvanic cell is much harder than this