At $291 \mathrm{K}$, saturated solution of ${\mathrm{BaSO}}_4$ was found to have a specific conductivity of $3.648\times {10}^{-6}{\mathrm{ohm}}^{-1}{ \mathrm{cm}}^{-1}$ and that of water being used is $1.25\times {10}^{-6}{\mathrm{ohm}}^{-1}{ \mathrm{cm}}^{-1}$. If the ionic conductance's of ${\mathrm{Ba}}^{2+}$ and ${\mathrm{SO}}_4^{2-}$ are $110$ and $136.6{\mathrm{ohm}}^{-1}{ \mathrm{cm}}^2{ \mathrm{mol}}^{-1}$ respectively, the solubility of ${\mathrm{BaSO}}_4$ at $291 \mathrm{K}$ will be [Atomic masses of$\left.\mathrm{Ba}-137,S-32,0-16\right]$

• A

  $1.435\times {10}^{-3}{\mathrm{gL}}^{-1}$
• Correct answer
  B

  $2.266\times {10}^{-3}{\mathrm{gL}}^{-1}$
• C

  $2.843\times {10}^{-3}{\mathrm{gL}}^{-1}$
• D

  $1.768\times {10}^{-3}{\mathrm{gL}}^{-1}$

Hence, the correct answer is option: 'B'.