If a $0.4 \text{ molal}$ solution of a nonvolatile solute in an organic solvent decreases its freezing point by $2.4 \text{ K}$, then the molal depression constant $(K_f)$ of the solvent will be:
- A$3.0 \text{ K kg mol}^{-1}$
- B$4.0 \text{ K kg mol}^{-1}$
- C$5.0 \text{ K kg mol}^{-1}$
- D$6.0 \text{ K kg mol}^{-1}$
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What is the cryoscopic constant of water if $5 \ g$ of glucose in $100 \ g$ of water causes a depression in freezing point of $2.15 \ K$? (Molar mass of glucose $= 180 \ g \ mol^{-1}$)
The freezing point depression of a solution containing $0.6 \ g$ of urea (molar mass $= 60 \ g \ mol^{-1}$) in $100 \ mL$ of benzene (in $K$) is ($K_f$ of benzene $= 4.0 \ K \ kg \ mol^{-1}$).
Identify $(i)$,$(ii)$ and $(iii)$ in the following diagram representing the depression in freezing point:
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View SolutionCalculate the molar mass of the solute when $1.5 \ g$ of a non-volatile solute is dissolved in $100 \ mL$ of a solvent having a density of $0.8 \ g \ mL^{-1}$,which lowers its freezing point by $0.75 \ K$. (Freezing point depression constant for the solvent is $5 \ K \ kg \ mol^{-1}$).
At the freezing point of a solution containing a nonvolatile solute,which of the following are in equilibrium?
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