I think it would be good to mention what will be left in the solution. When all copper is reduced. It seems that what will be left is H2SO4, i.e. sulphuric acid. Is that correct? Or does the whole thing become more complicated than that?
You can deduce that the ph is also changing. Since you are losing hydroxide ions, the solution becomes more acidic as you go, right? If it is more acidic than before, it should be because of small amounts of formed H2SO4
Do not compare metals with hydrogen in electrolysis. Compare metals themselves k Na , ca are reactive metals pb , Sn Cu Ag are less reactive metals than K Na etc. In electrolysis lead metal is more reactive than H and goes to the cathode hydrogen which is less reactive than pb remains in solution
^Agree. The comparison should be between the reduction potentials of the metal ion and *water* not hydrogen. Aqueous salts of metals between hydrogen and water will plate out on the cathode during electrolysis, such as nickel or zinc.
![R3.2.15 Predict and explain the products of electrolysis of aqueous solutions [HL IB Chemistry]](http://i.ytimg.com/vi/R__dBvuTCp0/mqdefault.jpg)
Best explanation and animation and experiment
Very informative ....Thank you
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Simply incredible explanation
Chemistry is so cool, I love it!!
OILRIG. Nice way to remember that. Very clever.
So helpful!
Good explanation thankyou
Excellent video, thank you!
very good video! Thank you!
I think it would be good to mention what will be left in the solution. When all copper is reduced. It seems that what will be left is H2SO4, i.e. sulphuric acid. Is that correct? Or does the whole thing become more complicated than that?
You can deduce that the ph is also changing. Since you are losing hydroxide ions, the solution becomes more acidic as you go, right? If it is more acidic than before, it should be because of small amounts of formed H2SO4
Thanks!v much
Do not compare metals with hydrogen in electrolysis. Compare metals themselves k Na , ca are reactive metals pb , Sn Cu Ag are less reactive metals than K Na etc. In electrolysis lead metal is more reactive than H and goes to the cathode hydrogen which is less reactive than pb remains in solution
^Agree. The comparison should be between the reduction potentials of the metal ion and *water* not hydrogen. Aqueous salts of metals between hydrogen and water will plate out on the cathode during electrolysis, such as nickel or zinc.
Good explanation, but you should try to blink sometimes😁
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