What is depression of freezing point? Explain.
(N/A) The freezing point of a substance is defined as the temperature at which the vapour pressure of the substance in its liquid phase is equal to its vapour pressure in the solid phase.
When a non-volatile solute is added to a solvent,the vapour pressure of the solution decreases.
Consequently,the solution freezes at a lower temperature than the pure solvent.
This difference in freezing point is known as the depression of freezing point,denoted by $\Delta T_f$.
When a non-volatile solute is added to a solvent,the vapour pressure of the solution decreases.
Consequently,the solution freezes at a lower temperature than the pure solvent.
This difference in freezing point is known as the depression of freezing point,denoted by $\Delta T_f$.
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What is the value of $K_{f}$ if $30 \ g$ urea (molar mass $60$) dissolved in $0.5 \ dm^{3}$ of water decreases the freezing point by $0.15^{\circ}C$?
The normal freezing point $(f.p.)$ of nitrobenzene is $278.82 \ K$. If a non-volatile solute is dissolved in it and a solution of $0.25 \ molality$ is prepared,the observed freezing point of the solution is $276.82 \ K$. Evaluate the cryoscopic constant $(K_f)$ of nitrobenzene in $K \ kg \ mol^{-1}$.
Medium
View SolutionWhich of the following has the lowest freezing point?
DifficultJEE MAIN 2019
View SolutionCalculate the molality of the solution of a nonvolatile solute if it freezes at $-0.36 \ ^{\circ}C$. [Given: $K_{f}$ for solvent $= 1.86 \ K \ kg \ mol^{-1}$]
Calculate the molality of a solution having freezing point depression $3.6 \ K$ and freezing point depression constant $4.8 \ K \ kg \ mol^{-1}$.
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