Match List-I with List-II

Choose the correct answer from the options given below:

(A)-(III), (B)-(I), (C)-(II), (D)-(IV)

The correct answer is (2) (A)-(III), (B)-(I), (C)-(II), (D)-(IV).

Molarity:

The molarity of a solution is defined as the number of moles of the solute dissolved per litre of the solution.It is represented as ′M′. Mathematically,

\[Molarity = \frac{\text{Moles of solute}}{\text{Volume of solution in liters}}\]

Molality:

The molality of a solution is defined as the number of moles of the solute dissolved per 1000 g (or 1 kg) of the solvent. It is denoted by m. Mathematically,

\[Molality = \frac{\text{Moles of solute}}{\text{Mass of solvent in kilograms}}\]

Colligative properties:

Osmotic pressure is a colligative property. Colligative properties are properties of solutions that depend on the number of solute particles in solution, but not on the identity of the solute particles. Osmotic pressure is the pressure that must be applied to a solution to prevent the flow of pure solvent across a semipermeable membrane. It is caused by the difference in concentration of solute particles between the solution and the pure solvent.

Osmotic pressure is an important property in many biological systems. For example, it is responsible for the movement of water between cells and their environment. It also plays a role in kidney function and blood pressure regulation.

Here are some other examples of colligative properties:

• Vapor pressure lowering
• Freezing point depression
• Boiling point elevation

Colligative properties can be used to measure the concentration of solutions and to determine the molecular weight of solutes.

Non-ideal solution:

Non-ideal solution means deviation from Raoult's law.  Raoult's law is a law that describes the behavior of ideal solutions. In an ideal solution, the solute particles do not interact with each other or with the solvent particles. This means that the vapor pressure of a component in an ideal solution is proportional to its mole fraction in the solution.

Non-ideal solutions are solutions in which the solute particles interact with each other or with the solvent particles in a way that causes the solution to deviate from ideal behavior. This can cause the vapor pressure of a component in a non-ideal solution to be higher or lower than expected from Raoult's law.

There are two types of non-ideal solutions:

• Positive deviation from Raoult's law: This occurs when the vapor pressure of a component in a solution is higher than expected from Raoult's law. This is typically caused by weak interactions between the solute and solvent particles.
• Negative deviation from Raoult's law: This occurs when the vapor pressure of a component in a solution is lower than expected from Raoult's law. This is typically caused by strong interactions between the solute and solvent particles.

Non-ideal solutions are very common. Most real solutions are non-ideal to some extent. However, some solutions are more non-ideal than others. For example, solutions of electrolytes, such as sodium chloride in water, are typically very non-ideal.

Non-ideal solutions are important in many different areas of chemistry, including chemical engineering, biochemistry, and environmental chemistry. For example, non-ideal solutions are used in distillation processes and in the development of new materials.