Electrolysis of Aqueous Solutions

Practical work based on electrolysis offers opportunities for learners to investigate chemical reactions and apply their knowledge of the reactivity series.

Investigate electrolysis of aqueous solutions with this simple experiment using copper(II) sulfate as the example. The supporting resources introduce electrolysis of other aqueous solutions, including sodium chloride and hydrochloric acid.

Animations show movement of ions and electrons to help learners visualise what is happening at a particle level and help them link theory to their practical work.

Chapter titles
00:09 Introduction
00:56 Experiment set up
02:54 The negative electrode
03:48 The positive electrode
04:44 Oxidation and reduction

[preethalal]

Best explanation and animation and experiment

[BigParadox]

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?

[robertoalbertini]

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

[Berghiker]

OILRIG. Nice way to remember that. Very clever.

[ismailabdi-kf]

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

[Mystic-km]

Good explanation, but you should try to blink sometimes😁

[mondayinedu]

This Lady looks like my Capricorn girl.she look smart and serious . She's very beautiful