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- Electrolysis
- Introduction - Chemistry
- Atomic Structure: Electron, Proton, Neutron etc.
- Periodic Classification of Elements
- Chemical Bonding
- Oxidation & Reduction
- Acids, Bases & Salts
- Behaviour of Gases
- Carbon and its Compounds
- Fuels
- Metallurgy
- Important Facts about Some Metals
- Non Metal
- Some Important & Common Facts in Chemistry
- Man made substances
Electrolysis
1. Electrolytes:
These are the substances which allow the electricity to pass through them in their molten states or in the form of their aqueous solution and undergo chemical decomposition, Examples – acids, bases & salts.
2. Strong electrolytes:
The electrolytes which are almost completely dissociated into ions in solution are called strong electrolytes, Example – NaCl, KCl, HCl, NaOH etc.
3. Weak electrolytes:
The electrolytes which do not ionize completely in solution are called weak electrolytes, Example – CH3COOH, H2CO3, HCN, ZnCl2 NH4OH etc.
4. Electrolysis:
The process of chemical decomposition of an electrolyte by passage of electric current through its molten state or its solution is called electrolysis.
5. Electrodes:
In order to pass the current through an electrolytes in molten state or in aqueous solution, two roads or plates are needed to connect with the terminal of a battery. These roads or plates are called electrodes.
Anode:
The electrode which is attached to positive terminal of battery is called anode. Oxidation occurs at anode.
Cathode:
The electrode which is attached to negative terminal of batteries is called, Reduction occurs at cathode.
Examples – Electrolysis of molten NaCl
At anode: Cl– – e → Cl
Cl + Cl → Cl2
At cathode: Na+ + e → Na
So, Cl2 gas occurs at anode which Na at cathode.
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