Conductance of Electrolytic Solutions - Measurement of the Conductivity of Ionic Solutions

Give reasons:

Conductivity of CH₃COOH decreases on dilution.

When measuring conductivity with a conductivity cell, cell constant denoted by the symbol G* is given by (electrode area of cross-section equal to ‘A’ and separated by distance ‘l’)

The decreasing order of electrical conductivity of the following aqueous solutions is:

1. 0.1 M Formic acid,
2. 0.1 M Acetic acid,
3. 0.1 M Benzoic acid.

The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Ω. What is the cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0.146 × 10⁻³ S cm⁻¹.

The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm⁻¹. Calculate its molar conductivity.

Assertion: Conductivity of all electrolytes decreases on dilution.

Reason: On dilution number of ions per unit volume decreases.

Give reasons:

On the basis of E° values, O₂ gas should be liberated at anode but it is Cl₂ gas which is liberated in the electrolysis of aqueous NaCl.

The conductivity of 0.01 m NaCl solution is 0.00147 ohm^–1cm^–1. What happens to the conductivity if extra 100 ML is added to the above solution:-