Electrochemistry deals with the study of production of electricity from energy released during spontaneous chemical reactions and the use of electrical energy to bring about non-spontaneous chemical transformations.
Electrolytes : Substances which allow the passage of electricity through their fused state or aqueous solution and undergo chemical decomposition are called electrolytes.
e.g. aqueous solution of acids, bases and salts.
Electrolytes are of two types :
Strong Electrolytes : The electrolytes that completely dissociate or ionise into ions are called strong electrolytes.
e.g. HCI, NaOH, K2SO, etc.
Weak electrolytes : The electrolytes that dissociate partially are called weak electrolytes.
e.g. CH3COOH, H2CO3 NH4OH, H2S etc.
Non-electrolytes : A non-electrolyte is a compound that does not conduct an electric current in either aqueous solution or in the molten state.
e.g. glucose, urea, benzene, chloroform, ether etc.
Electrolytic Cell : The cell through which the process of electrolysis is carried out in a container is called electrolytic cell.
An electrolytic cell consists of two metallic rods called electrodes.
The electrode which is attached with positive terminal of the battery is called cathode.
The electrode which is attached with negative terminal of the battery is called anode.
The conduction of electricity through the electrolyte solution is due to the movement of ions of electrolyte.
Electrochemical series it is a list that describes the arrangement of elements in order of their increasing electro potential value.
