If the specific conductivity of $0.1 \, N$ nitric acid is $6.2 \times 10^{-2} \, \Omega^{-1} \, cm^{-1}$,what will be the molar conductivity of the solution in $\Omega^{-1} \, cm^{2} \, mol^{-1}$?

At $298 \ K$,the equivalent conductance of $0.1 \ M$ acetic acid is $5.20 \ S \ cm^{2} \ eq.^{-1}$. Calculate the degree of dissociation of acetic acid at this concentration in $\%$. Given: $\lambda^{\infty} (H^{+}) = 349.8 \ S \ cm^{2} \ mol^{-1}$ and $\lambda^{\infty} (CH_{3}COO^{-}) = 40.9 \ S \ cm^{2} \ mol^{-1}$.

The resistance of a conductivity cell of $0.1 \ M$ $KCl$ solution is $120 \ \Omega$ and conductivity is $1.64 \times 10^{-4} \ S \ cm^{-1}$. What is the value of cell constant (in $cm^{-1}$)?

Which of the following statements is incorrect?

Resistance of a decimolar solution between two electrodes $0.02 \ m$ apart and $0.0004 \ m^2$ in area was found to be $50 \ \Omega.$ Specific conductance $(\kappa)$ is .......... $S \ m^{-1}$

What is a conductivity cell constant? Provide a note on the conductivity cell constant $(G^*)$.