The molar conductivities $(\lambda_{m}^0)$ at infinite dilution of $KBr$,$HBr$,and $KNH_2$ are $120.5$,$420.6$,and $90.48 \ S \ cm^2 \ mol^{-1}$ respectively. Find the value of $\lambda_{m}^0$ for $NH_3$.

The dissociation constant of acetic acid is $1.75 \times 10^{-5}$ and $\Lambda _{CH_3COOH}^o = 370.6 \times 10^{-4} \, S \, m^2 \, mol^{-1}$. The specific conductance of $0.01 \, M$ acetic acid solution will be:

The resistance of a conductivity cell containing $0.001 \ M$ $KCl$ solution at $300 \ K$ is $150 \ \Omega$. What is the cell constant if conductivity of $KCl$ solution is $1.5 \times 10^{-4} \ \Omega^{-1} \ cm^{-1}$ (in $cm^{-1}$)?

Among the following,the plot that correctly represents the conductometric titration of $0.05 \ M \ H_2SO_4$ with $0.1 \ M \ NH_4OH$ is

An electrolyte of a polymer-salt complex of poly(ethylene oxide)-LiCF$_{3}$SO$_{3}$ is shaped into a free standing circular film of $20 \ mm$ diameter and a thickness of $20 \ \mu m$. When it is sandwiched between $2$ stainless steel circular electrodes of the same diameter, this cell exhibits a conductance of $\frac{314}{5} \ S$. What is the specific conductivity of the electrolyte?

Solutions of two electrolytes $A$ and $B$ are diluted. The $\Lambda_m$ of $B$ increases $1.5$ times while that of $A$ increases $25$ times. Which of the two is a strong electrolyte? Justify your answer.