(B) Sodium sulphate $(Na_2SO_4)$ dissociates in aqueous solution as follows:$Na_2SO_4(aq) \rightarrow 2Na^+(aq) + SO_4^{2-}(aq)$Since it dissociates i

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(B) Sodium sulphate $(Na_2SO_4)$ dissociates in aqueous solution as follows:$Na_2SO_4(aq) \rightarrow 2Na^+(aq) + SO_4^{2-}(aq)$Since it dissociates into $3$ ions,the van't Hoff factor $(i)$ is $3$.Given:Molality $(m) = \frac{0.01 \ mol}{1 \ kg} = 0.01 \ mol \ kg^{-1}$$K_f = 1.86 \ K \ kg \ mol^{-1}$The depression in freezing point is given by the formula:$\Delta T_f = i \times K_f \times m$$\Delta T_f = 3 \times 1.86 \times 0.01 = 0.0558 \ K$

Class 12 Chemistry Solutions Colligative properties of electrolyte

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

AIEEE 2010 All AIEEE

A
$0.372$
B
$0.0558$
C
$0.0744$
D
$0.0186$

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

Similar Questions

Write the value of the van't Hoff factor $(i)$ for $K_{2}SO_{4}$ and $K_{4}[Fe(CN)_{6}]$.

The freezing point of a $2\%$ aqueous solution of $[Ag(CH_3NH_2)_2]Cl$ is:

If $13.44 \ g$ of $CuCl_2$ is dissolved in $1 \ kg$ of water,calculate the elevation in boiling point of the solution. $[K_b = 0.5 \ K \ kg \ mol^{-1}$,molar mass of $CuCl_2 = 134.1 \ g \ mol^{-1}]$

For very dilute solutions of $BaCl_2$ $(t_1)$ and $KCl$ $(t_2)$ having the same molarity,what is the correct relationship between their boiling points?

For a dilute aqueous solution of glucose,the van't Hoff factor $(i)$ is:

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