Question

Explain with Diagramatic representation the elevation of Freezing point in terms of Vapour Pressure Lowering.​

Answer 1

Answer:

The freezing point depression can be calculated using the pure solvent freezing point and the molality of the solution.

At the freezing point, the vapor pressure of both the solid and liquid form of a compound must be equal.

The freezing point of a substance is the temperature at which the solid and liquid forms are in equilibrium.

To reattain equilibrium, the freezing point of the solute and solvent mixture is lowered relative to the original pure solvent.

Terms

freezing point depressionAdding a solute to a solvent decreases the temperature at which the liquid solvent becomes a solid.

vapor pressureThe pressure that a vapor exerts, or the partial pressure if it is mixed with other gases.

van ‘t Hoff factorA measure of the effect of a solute on colligative properties.

freezing pointThe temperature at which a liquid freezes, and the solid and liquid phases are in equilibrium; normally the same as the melting point.

Freezing point depression is the phenomena that describes why adding a solute to a solvent results in the lowering of the freezing point of the solvent. When a substance starts to freeze, the molecules slow down due to the decreases in temperature, and the intermolecular forces start to take over. The molecules will then arrange themselves in a pattern, and thus turn into a solid. For example, as water is cooled to the freezing point, its molecules become slower and hydrogen bonds begin to “stick” more, eventually creating a solid. If salt is added to the water, the Na+ and Cl–ions attract to the water molecules and interfere with the formation of the large network solid known as ice. In order to achieve a solid, the solution must be cooled to an even lower temperature.

The freezing point depression can also be explained in terms of vapor pressure. Adding solute to a solvent will essentially dilute the solvent molecules, and according to Raoult’s law, this leads to a decrease in vapor pressure. Considering the fact that the vapor pressure of the solid and liquid forms must be the same at freezing point, because otherwise the system would not be at equilibrium, the lowering of the vapor pressure leads to the lowering of the temperature at which the vapor pressures of the liquid and frozen forms of the solution will be equal.