Which one of the following statement is false?

Options

A. Raoult’s law states that the vapour pressure of a component over a binary solution of volatile liquids is directly proportional to its mole fraction
B. Two sucrose solutions of the same molality prepared in different solvents will have the same depression in freezing point
C. The correct order of osmotic pressures of 0.01 M solution of each compound is `BaCl_(2) gt KCl gt CH_(3)COOH gt` "glucose"`
D. In the equation osmotic pressure `pi` = MRT, M is the molarity of the equation

Answer

To determine which statement is false, we will analyze each statement one by one based on the principles of chemistry, particularly focusing on Raoult's law, colligative properties, and osmotic pressure.

### Step-by-Step Solution:

1. **Understanding Raoult's Law**:
- Raoult's law states that the vapor pressure of a component in a solution is directly proportional to its mole fraction in the solution.
- This applies to ideal solutions where both components are volatile.

**Hint**: Recall that Raoult's law is applicable for ideal solutions and relates vapor pressure to mole fraction.

2. **Analyzing the First Statement**:
- The first statement claims that Raoult's law states the vapor pressure of a component over a binary solution of volatile liquid is directly proportional to its mole fraction.
- This is true as it aligns with the definition of Raoult's law.

**Hint**: Check if the statement accurately reflects the definition of Raoult's law.

3. **Analyzing the Second Statement**:
- The second statement discusses two sucrose solutions with the same molality but in different solvents, claiming they will have the same depression in freezing point.
- This statement is false because the depression in freezing point depends on the nature of the solvent. Different solvents will have different freezing point depressions even if the molality of the solute is the same.

**Hint**: Consider how colligative properties like freezing point depression depend on the solvent's properties.

4. **Analyzing the Third Statement**:
- The third statement refers to osmotic pressure and compares solutions with different solutes based on their Van't Hoff factors.
- It correctly states that osmotic pressure is dependent on the number of particles in solution, which is influenced by the degree of ionization of the solute.

**Hint**: Remember that osmotic pressure is related to the number of solute particles in solution.

5. **Analyzing the Fourth Statement**:
- The fourth statement mentions the formula for osmotic pressure as \( \Pi = ICRT \) and discusses the use of molarity.
- This statement is also true as it correctly describes the relationship between osmotic pressure, the Van't Hoff factor, concentration, and temperature.

**Hint**: Verify the formula for osmotic pressure and the significance of each variable.

### Conclusion:
After analyzing all statements, the false statement is the **second statement**, which incorrectly claims that two sucrose solutions with the same molality in different solvents will have the same depression in freezing point.

### Final Answer:
The false statement is the **second statement** regarding the freezing point depression of sucrose solutions in different solvents.

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