Concept: Conductance of Electrolytic Solutions - Variation of Conductivity and Molar Conductivity with Concentration

Calculate the degree of dissociation (α) of acetic acid if its molar conductivity (Λ_m) is 39.05 S cm² mol⁻¹.

Given λ^°(H⁺) = 349.6 S cm² mol⁻¹ and λ^°(CH₃COO⁻) = 40.9 S cm² mol⁻¹

Why does the conductivity of a solution decrease with dilution ?

Why conductivity of an electrolyte solution decreases with the decrease in concentration ?

State Kohlrausch law of independent migration of ions. 

The conductivity of sodium chloride at 298 K has been determined at different concentrations and the results are given below:

Calculate `Lambda_m` for all concentrations and draw a plot between `Lambda_m` and `c^(1/2)` Find the value of `Lambda_m^0`

The conductivity of 0.20 mol L⁻¹ solution of KCl is 2.48 × 10⁻² S cm⁻¹. Calculate its molar conductivity and degree of dissociation (α). Given λ⁰ (K⁺) = 73.5 S cm² mol⁻¹ and λ⁰ (C1⁻) = 76.5 S cm² mol⁻¹.

State Kohlrausch Law

The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm⁻¹. Calculate its molar conductivity.

State Kohlrausch’s law of independent migration of ions.

Define the following terms: Molar conductivity (⋀_m)

Define "Molar conductivity".

Conductivity of 0.00241 M acetic acid is 7.896 × 10⁻⁵ S cm⁻¹. Calculate its molar conductivity and if `Lambda_m^0` for acetic acid is 390.5 S cm² mol⁻¹, what is its dissociation constant?

Define limiting molar conductivity.

The conductivity of 0.001 mol L-1 solution of CH₃COOH is 3.905× 10-5 S cm-1. Calculate its molar conductivity and degree of dissociation (α) Given λ°(H⁺)= 349.6 S cm² mol-1 and λ°(CH₃COO)= 40.9S cm²mol^-1.