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Van't Hoff Factor

An aqueous so...

Question

An aqueous solution containing 12.48g of barium chloride ( $B a C l_{2}$ ) in 1000g of water, boils at ${100.0832}^{o}$ C. Calculate the degree of dissociation of barium chloride. ( $K_{b}$ for water = $0.52 K k g m o l^{- 1}$ , at. wt. Ba = 137, Cl = 35.5)

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Solution

$w_{B a C l_{2}}$ =12.48 g; $w_{H_{2} O}$ = 1000 g; $Δ T_{b}$ = 0.0832 K; $K_{b}$ =0.52 Kkg/mol
$Δ T_{b} = i K_{b} m m = \frac{w_{B a C l_{2}}}{M_{B a C l_{2}}} \times \frac{1000}{w_{H_{2} O}} m = \frac{12.48}{208} \times \frac{1000}{1000} = 0.06 i = \frac{0.0832}{0.52 \times 0.06} = 2.7 A l s o, i = N u m b e r o f m o l e s a t e q u i l l i b r i u m B a {C l}_{2} 1 - x ⇌ {B a}^{2 +} x + 2 {C l}^{-} 2 x i = 1 - x + x + 2 x = 1 + 2 x = 2.7 x = 0.85$
Therefore degree of dissociation is 85 %.

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