$AgNO_3$ (aq.) was added to an aqueous $KCl$ solution gradually and the conductivity of the solution was measured. The plot of conductance ( $\Lambda$ ) versus the volume of $AgNO_3$ is

The conductivity of a strong electrolyte:

What will be the concentration of a solution of an electrolyte if its molar conductivity and conductivity are respectively $230 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and $0.0115 \ \Omega^{-1} \ cm^{-1}$ at $298 \ K$ (in $M$)?

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration $0.1 \, M$ is $100 \, \Omega .$ The conductivity of this solution is $1.29 \, S \, m^{-1}.$ Resistance of the same cell when filled with $0.2 \, M$ of the same solution is $520 \, \Omega .$ The molar conductivity of $0.2 \, M$ solution of electrolyte will be..........$\times 10^{-4} \, S \, m^2 \, mol^{-1}$

Resistance of $0.05 \ M$ electrolytic solution at $298 \ K$ temperature is $30.0 \ \Omega$. The cross-sectional area of the conductivity cell having $Pt$ electrodes is $3.8 \ cm^{2}$ and the distance between the two electrodes is $1.5 \ cm$. What is the molar conductivity of the electrolytic solution?

The resistance of a $0.2 \ M$ solution of an electrolyte is $30 \ \Omega$ and conductivity is $1.2 \ S \ m^{-1}$. What is the value of the cell constant (in $cm^{-1}$)?