A) \[1.85\times {{10}^{-5}}\]
B) \[32.76\times {{10}^{-5}}\]
C) \[1.85\times {{10}^{-7}}\]
D) \[32.76\times {{10}^{-7}}\]
Correct Answer: A
Solution :
\[\wedge _{m}^{C}=\frac{\kappa \times 1000}{\text{molarity}}\] \[=\frac{7.896\times {{10}^{-5}}S\,c{{m}^{-1}}\times 1000\,c{{m}^{3}}{{L}^{-1}}}{0.00241\,\,mol\,{{L}^{-1}}}\] \[=32.76\,Sc{{m}^{2}}\,mo{{l}^{-1}}\] \[\alpha =\frac{32.76}{390.5}=0.084\] \[K=\frac{c{{\alpha }^{2}}}{1-\alpha }\] \[=\frac{0.00241\times {{(0.084)}^{2}}}{1-0.084}=1.85\times {{10}^{-5}}\]
You need to login to perform this action.
You will be redirected in
3 sec
