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The property of the conductor (metallic or electrolytic), which allows it to pass electricity through it, is known as conductance. The conductance of a solution of definite dilution enclosed in a cell having two electrodes of unit area separated by one centimetre apart is known as specific conductance. The conductance of all the ions produced by one gram equivalent of an electrolyte in a given solution is equivalent conductance. The conduction of all the ions produced by ionisation of 1g mole of an electrolyte when present in V ml of solution.
What is Electrolytic conductance?
The electrolytic conductance of electrolytic solutions refers to their capacity to allow the electric current to flow through them. This ability is due to the ions present in the solution due to the separation of the electrolytes. Electrolytes can only conduct electricity when molten or liquid, not when they are solid. The mathematical formula for electrolytic conductance is given by:-
G= 1/V = 1/R
Where, V denotes potential difference
R denotes resistance
Common examples are KCl, KNO3, NaCl, and other electrolytes that conduct electricity in the liquid or the molten state. The conductivity of electrolytes is affected by several factors, including ion concentration and electrolyte type.
The conductivity of electrolytic solution depends on the following factors:
Nature of the electrolytes
Size or dimension of the ions produced
Viscosity and nature of the solvent
Electrolyte’s Concentration
Temperature (conductivity rises with rising in the temperature)
Electrolytic and Metallic Conductors
All objects do not allow electrical current to pass through them. Conductors are the materials that allow the electric current to pass through them. The best conductor metal is silver, tin, copper, etc. On the other hand, the objects that do not allow electricity to pass through them are called insulators or non-conductors. Some basic examples of insulators are wax, wood, rubber, glass, etc.
Some of the differences between electrolytic and metallic conductors:
Metallic conduction | Electrolytic conduction |
This happens due to the flow of the electron through the object. | This happens due to the flow of the ions through the object. |
In this process, only physical change occurs. | In this process, the decomposition process occurs. |
Here, the process does not transfer any material. | Here, ions transfer the form of the material. |
Conductivity decreases with the rise in temperature. | Conductivity rises with the rising temperature and degree of hydration due to the decline in viscosity of the medium. |
Factors affecting Electrolytic Conductance
The Interionic attractions: These are the attractive interactions between the ions of the electrolyte solution. The greater the interionic attraction, the less the freedom of movement, and the smaller the electrical conductivity will be.
The solvation of ions: This is the attractive interaction between the electrolyte ions and the solvent molecule. The larger the solute-solvent interactions greater is the extent of solvation, and the lower will be the electrical conductivity of the solution.
The viscosity of solvent: This factor depends upon the attractive interaction between the solvent and the molecule. The larger the solvent-molecule interactions, the larger the viscosity, and the lower the electrical conductivity.
Temperature: As the temperature of the electrolyte increases, the kinetic energy of the ions increases. This increases the electrical conductance of electrolytic solutions.
Conclusion
In this chapter, we got study material notes on electrolytic conductance, properties of electrolytic conductance, factors affecting electrolytic conductance, and the difference between metallic conduction and electrolytic conduction. We have gone through the definition that the electrolytic conductance of electrolytic solutions refers to their capacity to allow the electric current to flow through them. This ability is due to the ions present in the solution due to the separation of the electrolytes. So, if you want to qualify for your exam with good marks, do not skip this chapter during your preparation.
