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Home  >>  CBSE XII  >>  Chemistry  >>  Solutions
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Calculate the freezing point depression expected for 0.0711m aqueous solution of $Na_2SO_4$.If this solution actually freezes at $-320^{\large\circ}C$,what would be the value of van't Hoff factor? ($K_f$ for water is $1.86^{\large\circ}Cmol^{-1}$)

$\begin{array}{1 1}2.4\\3.4\\4.4\\6.4\end{array} $

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Here $m=0.0711m$
$\Delta T_f=0.320^{\large\circ}$C
$K_f=1.86^{\large\circ}Cmol^{-1}$
$\Delta T_f=iK_fm$
$i=\large\frac{\Delta T_f}{K_f\times m}$
$\;\;=\large\frac{0.320}{1.86\times 0.0711}$
$\;\;=\large\frac{0.320}{0.132}$
$\;\;\;=2.4$
answered Aug 8, 2014 by sreemathi.v
 
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