Question

State and explain kohlrausch law of independent migration of ions with an example. explain how the hydration of ion effect conductance.

Answer 1

The law states that limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and cation of the electrolyte.
Kohlrausch`s law can be expressed asΛ0 = Σ λ0+ + Σ λ0–
For example, for ion, one should write . These studies of Kohlrausch in 1876 led him to generalize the results in the form of a law, called Kohlrausch's law of independent migration of ions after his name.
 Kohlrausch's law of independent migration , which states that in the limit of infinite dilution, Each ionic species makes a contribution to the conductivity of the solution that depends only on the nature of that particular ion, and is independent of the other ions present.

Small ions have small areas. There is less resistance as they move through the solution.

For example, in molten salts, the conductivity of Li+ is greater than that of Cs+.

Small ions have high charge density.

In aqueous solutions, this gives them a large hydration shell that moves with them.

For example, hydrated Li+ ions are larger than hydrated Cs+ ions.

Answer 2

The law states that limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and cation of the electrolyte.Kohlrausch`s law can be expressed asΛ0 = Σ λ0+ + Σ λ0– For example, for ion, one should write . These studies of Kohlrausch in 1876 led him to generalize the results in the form of a law, called Kohlrausch's law of independent migration of ions after his name. Kohlrausch's law of independent migration , which states that in the limit of infinite dilution, Each ionic species makes a contribution to the conductivity of the solution that depends only on the nature of that particular ion, and is independent of the other ions present.Small ions have small areas. There is less resistance as they move through the solution.
For example, in molten salts, the conductivity of Li+ is greater than that of Cs+.
Small ions have high charge density.
In aqueous solutions, this gives them a large hydration shell that moves with them.
For example, hydrated Li+ ions are larger than hydrated Cs+ ions.