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Freezing point lowering expression is ...

Freezing point lowering expression is
`DeltaT_(f)=K_(f)m` (molality)
Which of the following assumptions are considered for the validity of above equation ?

A

The solution is dilute

B

The `DeltaH_(f)` (latent heat of fusion of solvent) is independent of temperature between the actual and normal freezing point.

C

The solid-phase consists of pure solvent when solution is allowed to cool

D

`DeltaT_(f)` is not equal to `3K_(f)` for `3 "mol" :^(-1)` solution

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To solve the question regarding the assumptions for the validity of the freezing point lowering expression \(\Delta T_f = K_f \cdot m\), we can break it down into a step-by-step explanation. ### Step-by-Step Solution: 1. **Understanding the Equation**: The equation \(\Delta T_f = K_f \cdot m\) relates the change in freezing point (\(\Delta T_f\)) to the molality (m) of the solution and the freezing point depression constant (\(K_f\)) of the solvent. 2. **Assumption of Dilute Solutions**: ...
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A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. Dissolution of a non-volatile solute into a liquid leads to

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