For a strong electrolyte,the molar conductivity is given by $\wedge _m = \wedge _m^o - 10 \sqrt{C}$. Calculate $\wedge _m$ at $0.01 \ M$ if its value at $0.16 \ M$ is $200 \ S \ cm^2 \ mol^{-1}$.

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

For an $HCl$ solution at $25^o C$,the equivalent conductance at infinite dilution is $425 \ \Omega^{-1} \ cm^2 \ eq^{-1}$. The electrical conductivity of the $HCl$ solution is $3.825 \ \Omega^{-1} \ cm^{-1}$. If the degree of dissociation is $90\%$,what is the normality of the solution in $N$?

Identify the factor from the following that does not affect electrolytic conductance of a solution.

Calculate the molar conductivity of $CH_2ClCOOH$ at zero concentration if molar conductivities of $HCl$,$KCl$,and $CH_2ClCOOK$ at zero concentration are $4.2$,$1.4$,and $1.1 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ respectively.

The molar conductivity of $0.007 \ M$ acetic acid is $20 \ S \ cm^{2} \ mol^{-1}$. What is the dissociation constant of acetic acid? (In $\times 10^{-5} \ mol \ L^{-1}$)
$[\Lambda_{H^{+}}^{\circ}=350 \ S \ cm^{2} \ mol^{-1}, \Lambda_{CH_{3}COO^{-}}^{\circ}=50 \ S \ cm^{2} \ mol^{-1}]$