Ionic Conductance in Electrochemistry
Ionic conductance is a fundamental concept in electrochemistry that quantifies how well ions can move through a solution when an electric field is applied. It is crucial for understanding the behavior of electrolytes in various chemical processes.

Definition and Formula
The ionic conductance (\( \Lambda \)) is defined as the conductivity of an electrolyte solution per unit concentration of ions. It can be expressed mathematically as:
\[ \Lambda = \kappa / c \]
Where:
- \( \Lambda \) = Ionic conductance (S·cm²/mol)
- \( \kappa \) = Conductivity of the solution (S/cm)
- \( c \) = Concentration of ions (mol/L)

Factors Affecting Ionic Conductance
Several factors influence ionic conductance in a solution:
- Ionic Mobility: The ability of ions to move through the solvent affects conductance.
- Temperature: Higher temperatures generally increase ionic mobility, enhancing conductance.
- Ion Valence: Monovalent ions have higher conductance than divalent ions due to their charge-to-mass ratio.

Applications of Ionic Conductance
Ionic conductance plays a critical role in various fields:
- Electrochemical Cells: It helps in determining the efficiency of batteries and fuel cells.
- Water Quality Testing: Conductance measurements are used to assess the purity of water.
- Biological Systems: Understanding ionic conductance is vital for physiological processes in living organisms.
In summary, ionic conductance is an essential parameter in electrochemistry, aiding in the analysis and application of electrolytes in a wide range of scientific domains.