Question

Discuss the factors which affect electrolytic dissociation.

Answer 1

1. Nature of electrolyte (Interionic attraction): Strong electrolytes dissociate completely due to low interionic attraction, whereas weak electrolytes exhibit significant solute-solute interaction, leading to lesser dissociation.
2. Solvation of ions (Solute-solvent interaction): Highly solvated ions experience restricted movement, reducing the extent of dissociation and conduction. For instance, Li⁺ is more solvated than Na⁺, thus reducing conduction in LiCl solution compared to NaCl.
3. Viscosity of solvent (Solvent-solvent interaction): Higher viscosity due to strong solvent-solvent interactions limits ion mobility, thereby decreasing dissociation and conduction.
4. Nature of solvent and concentration of solution: Polar solvents like water promote greater dissociation. Higher concentration leads to less dissociation due to the common ion effect and crowding of ions.
5. Temperature: Increasing temperature reduces interionic and solute-solvent interactions, promoting dissociation and improving conduction.