(D) When a solution containing a non-volatile solute freezes,the solid phase that separates out is pure solid solvent. Therefore,the equilibrium is es

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solid solvent $\rightleftharpoons$ solvent in solution

(D) When a solution containing a non-volatile solute freezes,the solid phase that separates out is pure solid solvent. Therefore,the equilibrium is established between the pure solid solvent and the solvent present in the liquid solution. The equilibrium can be represented as: $\text{solid solvent} \rightleftharpoons \text{solvent in solution}$.

Class 12 Chemistry Solutions Depression of freezing point of the solvent

Easy

When a solution containing a non-volatile solute freezes,which equilibrium exists?

A
solid solvent $\rightleftharpoons$ liquid solvent
B
solid solute $\rightleftharpoons$ liquid solution
C
solid solute $\rightleftharpoons$ liquid solvent
D
solid solvent $\rightleftharpoons$ solvent in solution

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Depression of freezing point of the solvent

$A$ solvent freezes at $17^{\circ} C$ and it has a latent heat of fusion of $180 \ J \ g^{-1}$. The molal depression constant $(K_{f})$ of the solvent is (in $K \ kg \ mol^{-1}$):

MediumTS EAMCET 2022

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Ethylene glycol is used as an anti-freezing agent. Calculate the amount of ethylene glycol to be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^{\circ}C$. ($K_f$ for water $= 1.85 \ K \ kg \ mol^{-1}$) (molar mass of $(CH_2OH)_2 = 62 \ g \ mol^{-1}$) .......... $g$.

Medium

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When an aqueous solution of glucose is frozen,which crystals will separate out first?

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The freezing point of a solution containing $4.8 \ g$ of a compound in $60 \ g$ of benzene is $4.48 ^\circ C$. What is the molar mass of the compound $(K_f = 5.1 \ K \ kg \ mol^{-1})$,(freezing point of benzene $= 5.5 ^\circ C$)?

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Calculate the molality of the solution of a nonvolatile solute if it freezes at $-0.36 \ ^{\circ}C$. [Given: $K_{f}$ for solvent $= 1.86 \ K \ kg \ mol^{-1}$]

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When a solution containing a non-volatile solute freezes,which equilibrium exists?

Similar Questions

$A$ solvent freezes at $17^{\circ} C$ and it has a latent heat of fusion of $180 \ J \ g^{-1}$. The molal depression constant $(K_{f})$ of the solvent is (in $K \ kg \ mol^{-1}$):

Ethylene glycol is used as an anti-freezing agent. Calculate the amount of ethylene glycol to be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^{\circ}C$. ($K_f$ for water $= 1.85 \ K \ kg \ mol^{-1}$) (molar mass of $(CH_2OH)_2 = 62 \ g \ mol^{-1}$) .......... $g$.

When an aqueous solution of glucose is frozen,which crystals will separate out first?

The freezing point of a solution containing $4.8 \ g$ of a compound in $60 \ g$ of benzene is $4.48 ^\circ C$. What is the molar mass of the compound $(K_f = 5.1 \ K \ kg \ mol^{-1})$,(freezing point of benzene $= 5.5 ^\circ C$)?

Calculate the molality of the solution of a nonvolatile solute if it freezes at $-0.36 \ ^{\circ}C$. [Given: $K_{f}$ for solvent $= 1.86 \ K \ kg \ mol^{-1}$]

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