Solution and colligative properties in physical chemistry.
Solution and colligative properties in physical chemistry.
Solution:
- A solution is a homogeneous mixture of two or more substances, where one substance (the solute) disperses uniformly throughout another substance (the solvent). The solute particles are molecularly or ionically dispersed within the solvent, forming a single-phase system.
Ideal Solution:
- An ideal solution is a theoretical concept in which the interactions between solute-solute, solvent-solvent, and solute-solvent particles are identical. In other words, the molecules of the solute and solvent exhibit no significant attractive or repulsive forces between them.
Non-Ideal Solution:
- A non-ideal solution is a real-world solution where the interactions between solute and solvent particles are not identical. The attractive or repulsive forces between the solute-solvent and solvent-solvent particles differ from those between solute-solute particles.
Raoult's Law:
- Raoult's Law describes the vapor pressure of an ideal solution. According to this law the vapour pressure of any volatile component of a solution is equal to the vapour pressure of pure component multiplied by the mole fraction of that component in solution.Mathematically, for a binary ideal solution, the vapor pressure of component A (PA) and its mole fraction (XA) are related as: PA = XA * P^0A, where P^0A is the vapor pressure of pure component A.
Colligative Properties:
- Colligative properties is the property in which solution depend on the concentration of solute not on the nature of solute. These properties are primarily influenced by the number of solute particles, not their identity.
Types of Colligative Properties:
Vapor Pressure Lowering: On adding non volatile solute in a solvent the vapour pressure of solvent is lowered. This phenomenon is explained by Raoult's Law.
Boiling Point Elevation: Adding a solute to a solvent raises the boiling point of the solvent. This occurs because the presence of solute particles hinders the escape of solvent molecules into the vapor phase.
Freezing Point Depression: On adding a solute into a solvent the freezing point of the solvent decreases.The presence of solute particles disrupts the formation of the solvent's crystal lattice during freezing.
Osmotic Pressure: Osmotic pressure is the pressure required to prevent the flow of solvent molecules into a more concentrated solution through a semipermeable membrane. It is directly proportional to the concentration of solute particles.
Colligative properties find applications in various fields, such as determining molar masses, osmotic processes, and controlling the freezing and boiling points of solutions.