Question

The specific conductance of a saturated solution of AgCl at ${25}^o$C is $1.821\times {10}^{-5}$ mho $c{m}^{-1}$. What is the solubility of AgCl in water (in g$L^{-1}$), if limiting molar conductivity of AgCl is $130.26$ mho $c{m}^2$ $mo{l}^{-1}$?

• A. $1.89\times {10}^{-3}$g$L^{-1}$
• B. $2.78\times {10}^{-2}$g$L^{-1}$
• C. $2.004\times {10}^{-2}$g$L^{-1}$
• D. $1.43\times {10}^{-3}$g$L^{-1}$

Answer 1

Answer: (C)

$2.004\times {10}^{-2}$g$L^{-1}$

The specific conductance of an electrolyte solution is a measure of its ability to conduct electricity. The SI unit of conductivity is siemens per meter.

Given,

${\Lambda }_m^0=130.26$ $mho$ $c{m}^{2}mo{l}^{-1}$

$\kappa =1.821\times {10}^{-5}mho$ $c{m}^{-1}$

Also,

Molar mass of $AgCl=108+35.5=143.5$

We know,

$Solubility=\frac{\kappa \times 1000}{{\Lambda }_m^0}$

$=\frac{1.821\times {10}^{-5}\times 100}{130.26}=13.97\times {10}^{-5}mol$ $L^{-1}$

$⟹13.97\times {10}^{-5}\times 143.5=2.004\times {10}^{-2}g{L}^{-1}$