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The physical changes that occur when a solute is added to a solvent are known as collitive characteristics. Colligative Properties are affected by the number of solute particles present as well as the amount of solvent present, but not by the kind of solute particles, albeit they are affected by the type of solvent.
A solution can have the following colligative properties which are give below-:
- Increase of the boiling point
- Depression at the freezing point
- Vapour pressure is being reduced in a relative sense.
- Osmotic pressure osmotic pressure osmotic.
Different Types of Solution Colligative Properties
A solution’s colligative qualities come in a variety of forms. Vapour pressure is reduced, boiling point is raised, freezing point is lowered, and osmotic pressure is reduced.
Reduced Vapour Pressure
A solvent’s vapour pressure in a solution is always lower than the pure solvent’s vapour pressure. The reduction in vapour pressure is proportional to the mole fraction of the solute. This is known as Raoult’s Law.
Psolution =Xsolvent P°solvent
where P°solventis the pure solvent’s vapour pressure and Xsolvent is the solvent’s mole fraction. Due to the fact that this is a two-component system (solvent and solute),
Xsolvent + Xsolute=1
where Xsolute is the mole fraction of the solvent or solute. The difference in vapour pressure (∆P) can be calculated.
∆P=(Xsolvent-1)P°solvent=Xsolute P°solvrnt
Boiling Point Elevation
Solution boiling points are always higher than the boiling point of the pure solvent. The difference in boiling points between the pure solvent and the solution is proportional to the solute particle concentration:
∆Tb=Tb(solution)-Tb(solvent)=Kbm
where Tb denotes the boiling point elevation, Kb denotes the boiling point elevation constant, and m denotes the solute’s molality (mol/kg solvent).
Freezing Point Depression
The introduction of solute molecules to a solvent causes freezing point depression, which is a colligative feature observed in solutions. The freezing point of a solution is always lower than the freezing point of a pure solvent, and it is proportional to the molality of the solute.
∆Tf=Tf(solvent)-Tf(solution)=Kfm
where Tf is the freezing point depression, Tf (solution) is the solution’s freezing point, Tf (solvent) is the solvent’s freezing point, Kfis the freezing point depression constant, and m is the molality
Osmotic Pressure
Diffusion of a fluid through a semipermeable membrane is referred to as osmosis. Only solvent molecules can flow through a semipermeable membrane (animal bladders, fruit and vegetable skins) that separates a solution from a solvent. The pressure difference required to inhibit solvent flow over a semipermeable membrane is known as the osmotic pressure of a solution. The molar concentration of the solute particles in solution determines a solution’s osmotic pressure.
Π=i(n/V)RT=iMRT where
R is the ideal gas constant (0.0821 L atm / mol K),
T is the temperature in Kelvin,
i is the van’t Hoff Factor
n is the number of moles of solute present,
V is the volume of the solution,
and M is the molar concentration of the new solute
Different Types of Solution
Isotonic solution: An isotonic solution is a pair of solutions that have the same osmotic pressure at the same temperature. There is no osmosis when such liquids are separated by a semipermeable membrane.
Hypotonic solution: A hypotonic solution has a lower osmotic pressure than the surrounding environment, implying that the concentration of solute particles is lower. When a semipermeable barrier separates the hypotonic solution from the water, water moves out of the hypotonic solution.
Hypertonic solution: A hypertonic solution has a higher 2.osmotic pressure than the surrounding environment, indicating that the concentration of solute particles is higher. Water moves inside the hypertonic solution if the hypertonic solution is separated by a semipermeable membrane.
Conclusion
The physical changes that occur when a solute is added to a solvent are known as collitive characteristics. Colligative Properties are affected by the number of solute particles present as well as the amount of solvent present, but not by the kind of solute particles, albeit they are affected by the type of solvent.
