0Electrolytes- Substances which get dissociated into ions on dissolving in polar solvents like water are called electrolytes due to free ions their solutions conduct electricity.
Examples-HCl , NaOH, NaCl, CH3COOH, NH4OH etc.
By the degree of dissociation (ionisation) in the water, these are classified in 3 categories.
Here let me explain you the degree of dissociation.
The degree of dissociation =mole dissociated at any time/Total mole taken initially
1.Strong Electrolytes
2.Weak Electrolytes
3.Non-Electrolytes
Strong Electrolytes- Substances which ionise when dissolved in water are called strong Electrolytes. Strong acids like HCl, H2SO4 and strong bases like NaOH, KOH are strong electrolytes.Generally, all salts are strong electrolytes except some insoluble salts.
Weak electrolytes- Substances which ionise partially or in very less extent on dissolving in water are called weak electrolytes. Weak acids like CH3COOH and other organic acids and weak bases like NH4OH and Mg(OH)2 are weak electrolytes.
Non-electrolytes - Substances which do not get dissociated in ions on dissolving in water are called non-electrolytes. Organic compounds like urea, glucose etc. do not ionise on dissolving in water. Hence they are non-electrolytes, and they don't conduct electricity in their aqueous solution.
Aqueous Solution- A solution in which water is solvent is called aqueous solution.means when a solute is dissolved in water then solution obtained is called aqueous Solution.
