(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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Molal depression constant for a solvent is $4.0 \, K \, kg \, mol^{-1}$. The depression in the freezing point of the solvent for $0.03 \, mol \, kg^{-1}$ solution of $K_2SO_4$ is .............. $K$ (Assume complete dissociation of the electrolyte).

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In an aqueous solution of potassium ferrocyanide,the degree of dissociation of the salt is $80\%$. The value of the van't Hoff factor is:

Medium

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Carnallite in solution in $H_2O$,shows the properties of

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$80$ mole percent of $MgCl_2$ is dissociated in aqueous solution. The vapour pressure of $1.0$ molal aqueous solution of $MgCl_2$ at $38^{\circ} C$ is $.........$ $mm$ $Hg$. (Nearest integer)
Given : Vapour pressure of water at $38^{\circ} C$ is $50$ $mm$ $Hg$.

MediumJEE MAIN 2023

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The Van't Hoff factor will be highest for

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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

Molal depression constant for a solvent is $4.0 \, K \, kg \, mol^{-1}$. The depression in the freezing point of the solvent for $0.03 \, mol \, kg^{-1}$ solution of $K_2SO_4$ is .............. $K$ (Assume complete dissociation of the electrolyte).

In an aqueous solution of potassium ferrocyanide,the degree of dissociation of the salt is $80\%$. The value of the van't Hoff factor is:

Carnallite in solution in $H_2O$,shows the properties of

$80$ mole percent of $MgCl_2$ is dissociated in aqueous solution. The vapour pressure of $1.0$ molal aqueous solution of $MgCl_2$ at $38^{\circ} C$ is $.........$ $mm$ $Hg$. (Nearest integer)Given : Vapour pressure of water at $38^{\circ} C$ is $50$ $mm$ $Hg$.

The Van't Hoff factor will be highest for

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$80$ mole percent of $MgCl_2$ is dissociated in aqueous solution. The vapour pressure of $1.0$ molal aqueous solution of $MgCl_2$ at $38^{\circ} C$ is $.........$ $mm$ $Hg$. (Nearest integer)
Given : Vapour pressure of water at $38^{\circ} C$ is $50$ $mm$ $Hg$.