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

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 cell constant is the product of resistance and ______

The conductivity of 0.20 M solution of \[\ce{KCl}\] at 298 K is 0.0248 S cm⁻¹. Calculate its molar conductivity.

In an aqueous solution how does specific conductivity of electrolytes change with addition of water?

Conductivity_K, is equal to:

(i) `1/R l/A`

(ii) `G^∗/R`

(iii) Λ_m

(iv) `l/A`

Assertion: For measuring resistance of an ionic solution an AC source is used.

Reason: Concentration of ionic solution will change if DC source is used.

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

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:-