The correct answer is Option (3) → (A), (B), (C) and (D)
The conductivity of an electrolytic solution is a measure of its ability to carry electric current, which occurs through the movement of ions. This movement is influenced by several physical and chemical factors.
Factors Influencing Conductivity
- (A) Nature of Electrolyte: Strong electrolytes (like $NaCl$ or $HCl$) dissociate completely into ions, providing a higher concentration of charge carriers and thus higher conductivity. Weak electrolytes (like $CH_3COOH$) dissociate only partially, leading to lower conductivity.
- (B) Nature of Solvent: Solvents with higher polarity and dielectric constants (like water) promote better ionization of the electrolyte. Additionally, the viscosity of the solvent plays a role; a more viscous solvent offers more resistance to the movement of ions, decreasing conductivity.
- (C) Temperature: As temperature increases, the kinetic energy of the ions increases and the viscosity of the solvent typically decreases. Both factors lead to an increase in ionic mobility, which directly increases conductivity.
- (D) Size of Ions Produced: Smaller ions move more easily through the solvent than larger, bulkier ions. However, it is important to consider solvation (hydration); sometimes a small ion (like $Li^+$) becomes heavily hydrated by solvent molecules, making its "effective size" larger and reducing its mobility compared to a less hydrated, larger ion (like $Cs^+$).
|
