Introduction:

The molar conductivity of an electrolyte is a measure of its ability to conduct electricity. It is influenced by various factors such as concentration, temperature, and the nature of the electrolyte. In general, strong electrolytes have higher molar conductivity compared to weak electrolytes at the same concentration. However, under certain circumstances, the molar conductivity of a weak electrolyte can be greater than that of a strong electrolyte at a particular concentration.

Factors influencing molar conductivity:
1. Concentration: The molar conductivity of an electrolyte increases with increasing concentration due to the increased number of ions available for conduction.
2. Nature of the electrolyte: Strong electrolytes dissociate completely into ions in a solution, whereas weak electrolytes only partially dissociate. The degree of dissociation affects the molar conductivity.
3. Temperature: Molar conductivity generally increases with increasing temperature as it enhances the mobility of ions.

Reasons for the molar conductivity of weak electrolyte being greater than strong electrolyte:
1. Degree of dissociation: Weak electrolytes have a lower degree of dissociation compared to strong electrolytes. However, at a particular concentration, the weak electrolyte may have a higher degree of dissociation, resulting in a higher molar conductivity. This can occur when the strong electrolyte is highly concentrated, leading to ion-ion interactions and reduced mobility of ions.
2. Ion size and charge: The size and charge of ions also affect molar conductivity. In some cases, the weak electrolyte may have smaller or more highly charged ions, which can contribute to higher molar conductivity compared to the strong electrolyte.

Example:
Consider the weak electrolyte acetic acid (CH3COOH) and the strong electrolyte sodium chloride (NaCl) at a particular concentration. At low concentrations, acetic acid may have a higher degree of dissociation compared to sodium chloride. This is because acetic acid is a weak acid that only partially dissociates into acetate ions (CH3COO-) and hydrogen ions (H+), while sodium chloride readily dissociates into sodium ions (Na+) and chloride ions (Cl-). Due to the higher degree of dissociation, the molar conductivity of acetic acid can be greater than that of sodium chloride at the same concentration.

Conclusion:
In conclusion, while strong electrolytes generally have higher molar conductivity compared to weak electrolytes, there are instances where the molar conductivity of a weak electrolyte can be greater than that of a strong electrolyte at a particular concentration. Factors such as the degree of dissociation, ion size, and charge play crucial roles in determining the molar conductivity of electrolytes.

No. Bcuz, the molar conductivity of both weak and strong electrolytes increases with dilution. i. e. . decrease in the concentration.
The molar conductivity is the conductance of all the ions produced by one mole of electrolyte. .for the strong electrolyte, the molar conductivity increases sharply with increase in concentration .