What is the conductivity of $0.02 \ M \ KCl$ solution if the cell constant is $1.29 \ cm^{-1}$ and the resistance is $645 \ \Omega$?

Resistance of $0.2 \, M$ solution of an electrolyte is $50 \, \Omega$. The specific conductance of the solution is $1.4 \, S \, m^{-1}$. The resistance of $0.5 \, M$ solution of the same electrolyte is $280 \, \Omega$. The molar conductivity of $0.5 \, M$ solution of the electrolyte in $S \, m^2 \, mol^{-1}$ is:

The specific conductance of $0.0025 \ M$ acetic acid is $5 \times 10^{-5} \ S \ cm^{-1}$ at a certain temperature. The dissociation constant of acetic acid is $...... \times 10^{-7}$. (Nearest integer) Consider limiting molar conductivity of $CH_3COOH$ as $400 \ S \ cm^2 \ mol^{-1}$.

The resistance of a $0.1 \, N$ solution of a salt is $2.5 \times 10^{3} \, \Omega$. If the cell constant is $1.15 \, cm^{-1}$,what will be the equivalent conductance of the solution in $\Omega^{-1} \, cm^{2} \, eq^{-1}$ (in $.6$)?

What is the conductivity of $0.02 \text{ M}$ $AgNO_3$ solution having cell constant $1.2 \text{ cm}^{-1}$ and resistance $95.0 \text{ } \Omega$?

Explain the effect of change in concentration on the conductivity of a solution.