Introduction
The equivalent conductance of a substance is defined as the conductance of a solution containing one equivalent of the solute. As a solution is diluted, the equivalent conductance typically increases due to a rise in the degree of ionization.

Ionization and Dilution
- When a strong electrolyte is dissolved in water, it dissociates into ions. The degree of ionization refers to the fraction of the solute that ionizes in solution.
- In a concentrated solution, the ions are closely packed, leading to increased inter-ionic interactions which can hinder further ionization.
- However, as the solution is diluted, the distance between ions increases, reducing these interactions and promoting further ionization.

Factors Influencing Conductance
- **Increased Ion Concentration**: Dilution reduces the number of ions in a given volume, but as the degree of ionization rises, the overall number of ions in the solution can still increase.
- **Mobility of Ions**: Dilution improves the mobility of ions due to reduced inter-ionic attraction, allowing ions to move freely and conduct electricity more effectively.

Conclusion
In summary, the increase in equivalent conductance upon dilution is primarily due to:
- The increase in the degree of ionization, which allows more solute to dissociate into ions.
- Enhanced mobility of ions in a less concentrated solution, leading to improved electrical conductivity.
This relationship is a key concept in understanding electrolyte behavior in solutions, particularly relevant in NEET examinations.