Molar conductivity is a measure of how well ions in a solution conduct electricity when one mole of a substance is dissolved in a specific volume of water. It tells us how efficiently the charged particles (ions) move and carry electricity.
Molar conductivity (Λm) is calculated using this formula:
Λm = κ / C
As you dilute the solution (add more water), the ions move more freely because they have more space. This increases molar conductivity.
Molar conductivity is the conductance property of a solution containing one mole of electrolyte, and it is a function of the solution's ionic strength or salt concentration.
Specific conductance is obtained by multiplying the molarity of the solution by the molar conductance of the solution.
The amount of ions responsible for transporting current reduces when the solution is diluted per unit volume. As a result, as dilution increases, conductivity diminishes. Molar conductivity, on the other hand, rises with dilution.
K/M = molar conductance
K stands for specific conductance.
M is the electrolyte concentration.