Question

Molar conductivity of $0.15$ M solution of KCl at $298$ K, if its conductivity is $0.0152$ S $c{m}^{-1}$ will be:

• A. $124{\Omega }^{-1}$ $c{m}^2$ $mo{l}^{-1}$
• B. $204{\Omega }^{-1}$ $c{m}^2$ $mo{l}^{-1}$
• C. $101{\Omega }^{-1}$ $c{m}^2$ $mo{l}^{-1}$
• D. $300{\Omega }^{-1}$ $c{m}^2$ $mo{l}^{-1}$

Answer 1

The correct option is C $101{\Omega }^{-1}$ $c{m}^2$ $mo{l}^{-1}$

Molar conductivity is defined as the conductivity of an electrolyte solution divided by the molar concentration of electrolyte.

Given,

$M=0.15M,\kappa =0.0152Sc{m}^{-1}$

We know the relation,

${\Lambda }_m=\frac{\kappa \times 1000}{M}$

$⟹{\Lambda }_m=\frac{1.52\times {10}^{-2}\times 1000}{0.15}=101{\Omega }^{-1}c{m}^{2}mo{l}^{-1}$