WHY EQUIVALENT CONDUCTANCE INCREASES WITH DILUTION

What is Equivalent Conductance?

The equivalent conductance of a solution, represented by the symbol Ʌ, is a measure of the ability of ions in a solution to conduct electricity. It is defined as the conductance of a solution containing one equivalent weight of a substance dissolved in a volume of solution that is sufficiently large to ensure complete ionization.

Conductivity vs. Conductance

Conductivity and conductance are often used interchangeably, but they are technically different concepts. Conductivity (κ) is a measure of the ease with which a material allows the flow of electric current. It is an intrinsic property of the material and does not depend on the amount of material present. Conductance (G), on the other hand, is a measure of the ability of a specific sample of material to conduct electricity. It depends on both the conductivity of the material and the geometry of the sample.

The Relationship Between Equivalent Conductance and Dilution

The equivalent conductance of a solution typically increases as the solution is diluted. This is because dilution results in an increase in the number of ions per unit volume, which leads to a decrease in the resistance of the solution and an increase in its ability to conduct electricity.

Factors Affecting Equivalent Conductance

The equivalent conductance of a solution is affected by several factors, including:

Concentration: As mentioned above, the equivalent conductance of a solution increases as the concentration decreases. This is because dilution results in an increase in the number of ions per unit volume, which leads to a decrease in the resistance of the solution and an increase in its ability to conduct electricity.

Temperature: The equivalent conductance of a solution also increases with increasing temperature. This is because higher temperatures increase the kinetic energy of the ions, which allows them to move more freely and conduct electricity more effectively.

Nature of the Ions: The equivalent conductance of a solution also depends on the nature of the ions present. For example, ions with smaller radii and higher charge densities tend to have higher equivalent conductances than ions with larger radii and lower charge densities.

Applications of Equivalent Conductance

Equivalent conductance is a useful tool for studying the properties of electrolytes and for determining the concentration of solutions. It is also used in various analytical techniques, such as conductometry and potentiometry.

Conclusion

The equivalent conductance of a solution is a valuable tool for understanding the behavior of electrolytes and for performing various analytical techniques. It increases with dilution due to an increase in the number of ions per unit volume, which leads to a decrease in the resistance of the solution and an increase in its ability to conduct electricity.

Frequently Asked Questions

1. What is the difference between equivalent conductance and conductivity?

Equivalent conductance is a measure of the ability of ions in a solution to conduct electricity, while conductivity is a measure of the ease with which a material allows the flow of electric current.

2. Why does equivalent conductance increase with dilution?

Dilution results in an increase in the number of ions per unit volume, which leads to a decrease in the resistance of the solution and an increase in its ability to conduct electricity.

3. What factors affect the equivalent conductance of a solution?

The equivalent conductance of a solution is affected by concentration, temperature, and the nature of the ions present.

4. What are some applications of equivalent conductance?

Equivalent conductance is used for studying the properties of electrolytes, determining the concentration of solutions, and performing various analytical techniques.

5. How can I measure the equivalent conductance of a solution?

The equivalent conductance of a solution can be measured using a conductivity meter.