Ionic Conductance: Full Explanation
1. Introduction to Ionic Conductance
Ionic conductance refers to the ability of ions to carry electric current in a solution. It depends on the
number of ions, their charge, and mobility. This concept is crucial in electrochemistry and industrial
applications.
2. Factors Affecting Ionic Conductance
- Nature of Ions: Smaller ions and highly charged ions conduct better.
- Solvent Properties: Solvent polarity and dielectric constant affect ion mobility.
- Temperature: Higher temperature increases ion movement and conductance.
- Viscosity: More viscous solutions slow down ion movement, reducing conductance.
3. Types of Ionic Conductance
- Molar Conductance: Conductance of a solution containing one mole of solute.
- Equivalent Conductance: Conductance per equivalent of solute.
- Specific Conductance: Conductance of a solution per unit length and cross-sectional area.
4. Laws and Theories of Ionic Conductance
- Kohlrausch's Law: The limiting molar conductance of an electrolyte is the sum of the conductance
of individual ions.
- Debye-Hückel Theory: Explains ionic interactions affecting conductance.
- Ostwald's Dilution Law: Relates conductance of weak electrolytes to their dissociation.
5. Measurement of Ionic Conductance
- Conductivity Cells: Special cells with electrodes measure conductance.
- Electrodes: Platinum electrodes are commonly used.
- Experimental Procedure: The solution is placed in a conductivity cell, and a conductivity meter
measures the conductance.
6. Applications of Ionic Conductance
- Electrochemistry: Helps in understanding ion transport in batteries and fuel cells.
- Water Quality Testing: Used to determine purity of drinking and industrial water.
- Industrial Applications: Used in chemical industries for monitoring reactions.
7. Conclusion
Ionic conductance plays a vital role in scientific and industrial applications. Understanding its
1. Introduction to Ionic Conductance
Ionic conductance refers to the ability of ions to carry electric current in a solution. It depends on the
number of ions, their charge, and mobility. This concept is crucial in electrochemistry and industrial
applications.
2. Factors Affecting Ionic Conductance
- Nature of Ions: Smaller ions and highly charged ions conduct better.
- Solvent Properties: Solvent polarity and dielectric constant affect ion mobility.
- Temperature: Higher temperature increases ion movement and conductance.
- Viscosity: More viscous solutions slow down ion movement, reducing conductance.
3. Types of Ionic Conductance
- Molar Conductance: Conductance of a solution containing one mole of solute.
- Equivalent Conductance: Conductance per equivalent of solute.
- Specific Conductance: Conductance of a solution per unit length and cross-sectional area.
4. Laws and Theories of Ionic Conductance
- Kohlrausch's Law: The limiting molar conductance of an electrolyte is the sum of the conductance
of individual ions.
- Debye-Hückel Theory: Explains ionic interactions affecting conductance.
- Ostwald's Dilution Law: Relates conductance of weak electrolytes to their dissociation.
5. Measurement of Ionic Conductance
- Conductivity Cells: Special cells with electrodes measure conductance.
- Electrodes: Platinum electrodes are commonly used.
- Experimental Procedure: The solution is placed in a conductivity cell, and a conductivity meter
measures the conductance.
6. Applications of Ionic Conductance
- Electrochemistry: Helps in understanding ion transport in batteries and fuel cells.
- Water Quality Testing: Used to determine purity of drinking and industrial water.
- Industrial Applications: Used in chemical industries for monitoring reactions.
7. Conclusion
Ionic conductance plays a vital role in scientific and industrial applications. Understanding its
