The resistance of a conductivity cell with cell constant $1.14 \, cm^{-1}$,containing $0.001 \, M \, KCl$ at $298 \, K$ is $1500 \, \Omega$. The molar conductivity of $0.001 \, M \, KCl$ solution at $298 \, K$ in $S \, cm^{2} \, mol^{-1}$ is ...... . (Integer answer)

The conductance of a $0.0015 \ M$ aqueous solution of a weak monobasic acid was determined by using a conductivity cell consisting of platinized $Pt$ electrodes. The distance between the electrodes is $120 \ cm$ with an area of cross section of $1 \ cm^2$. The conductance of this solution was found to be $5 \times 10^{-7} \ S$. The $pH$ of the solution is $4$. The value of limiting molar conductivity $\left(\Lambda_{m}^0\right)$ of this weak monobasic acid in aqueous solution is $Z \times 10^2 \ S \ cm^{2} \ mol^{-1}$. The value of $Z$ is

What benefit do we get by forming a thin layer of $Pt$ particles on the electrodes of a conductivity cell?

The electrical conductance of unit volume $(1 \ cm^3)$ of solution is called as

The specific conductivity of a $0.01 \ M$ salt solution is $1.061 \times 10^{-4} \ S \ cm^{-1}$. The molar conductivity of this solution is:

$A$ graph was plotted between molar conductivity of various electrolytes ($NaCl$,$HCl$ and $NH_4OH$) and $\sqrt{C}$ (in $mol \ L^{-1}$). Identify the correct assignment for the curves $I$,$II$,and $III$.