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Van't Hoff Factor

A 1.00 mola...

Question

A $1.00$ molal aqueous solution of trichloroacetic acid $(C C l_{3} C O O H)$ is heated to its boiling point. The solution has the boiling point of ${100.18}^{o} C$ . Determine the van't Hoff factor for trichloroacetic acid. ( $K_{b}$ for water = 0.512 K kg mol $^{- 1}$ )

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Solution

$C C C l_{3} C O O H \to C C l_{3} C O O^{-} + H^{+}$
$Δ T_{b} = (100.18 + 273) - (100 - 273) = 0.18 K$
Molality is 1.
Hence, $Δ T_{b} = i K_{b} m = i K_{b} \times 1$
$i = \frac{0.18}{0.512}$
$i = 0.351$

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