Conductance in Electrolytic Solutions

The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S  $c{m}^2$  $mo{l}^{-1}.$  Calculate the conductivity of the solution.

The molar conductivity of a $1.5 \mathrm{M}$ solution of an electrolyte is found to be$138.9 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$. Calculate the conductivity of the solution?

The resistance of a conductivity cell containing 0.001 M KCI solution at 298 K is 1500  $\Omega .$  The cell constant would be (if the conductivity of 0.001 M KCI solution at 298 K is  $0.146\times {10}^{-3}\text{S}{\text{cm}}^{-1}$  ):  

The conductivity of centimolar solution of $\mathrm{KCl}$ at $25°\mathrm{C}$ is $0.0210 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$ and the resistance of the cell containing the solution at $25°\mathrm{C}$ is $60 \mathrm{ohm}$. The value of cell constant is

What is meant by ionic mobility?

What are the factors that affect the conductivity of an ionic (electrolytic) solution?

What is the effect of polarity and viscosity of the solvent on electrolytic conductance?

The nature of solvent can affect electrolytic conductivity.

How the nature of solvent affect electrolytic conductivity.

Electrolytic conductivity is affected by the nature of solute.

Which of the following factors affect electrolytic conductivity?

Explain how nature of electrolyte affect conductivity.

How nature of solute affect electrolytic conductivity?

If ${\text{K}}_{\mathrm{a}}$ is the ionization constant of a weak acid and ${\mathrm{K}}_{\mathrm{b}}$ is that of the conjugate base, then $\mathrm{p}{\text{K}}_{\mathrm{a}}+\mathrm{p}{\text{K}}_{\mathrm{b}}=$_____ .

If ${\text{K}}_{\mathrm{a}}$ is the dissociation constant of a weak acid and ${\mathrm{K}}_{\mathrm{b}}$ is dissociation constant of its conjugate base, then $\mathrm{p}{\text{K}}_{\mathrm{a}}+\mathrm{p}{\text{K}}_{\mathrm{b}}= {\mathrm{pK}}_{\mathrm{w}}$