If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water ($\mathrm{\Delta}T_{f}$), when 0.01 mole of sodium sulphate is dissolved in 1 kg of water, is ($k_{f} = 1.86\ Kkg\ mol^{- 1})\ \$

Question

Dr. Abubacker · Accepted Answer

(b)
$Na_{2}SO_{4} ightarrow 2Na^{+} + SO_{4}^{2 -}$
van’t Hoff factor for$\ Na_{2}SO_{4}$ =3
$\mathrm{\Delta}T_{f} = i 	imes k_{f} 	imes m$
=3$	imes 1.86 	imes 0.01$
$\left\lbrack \because\ \ \ m = \frac{0.01}{1} = 0.01 ightbrack$
=0.0558 K

Q. If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water ($\mathrm{\Delta}T_{f}$), when 0.01 mole of sodium sulphate is dissolved in 1 kg of water, is ($k_{f} = 1.86\ Kkg\ mol^{- 1})\ \$

Explanation

Reviewed by Dr. Abubacker

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