An ideal molar solution at `0^(@)C` will have an osmotic pressure of

Options

A. 10 atmosphere
B. 20 atmosphere
C. 22.4 atmosphere
D. 4.3 atmosphere

Explanation

To determine the osmotic pressure of an ideal molar solution at 0°C, we can follow these steps:

### Step-by-Step Solution:

1. **Understand Osmotic Pressure**: Osmotic pressure is the pressure required to prevent the flow of solvent into a solution through a semipermeable membrane. It is directly proportional to the concentration of solute particles in the solution.

2. **Use the Formula for Osmotic Pressure**: The osmotic pressure (π) can be calculated using the formula:
\[ \pi = iCRT \]
where:
- \(i\) = van 't Hoff factor (number of particles the solute dissociates into)
- \(C\) = molar concentration of the solution (in moles per liter)
- \(R\) = universal gas constant (0.0821 L·atm/(K·mol))
- \(T\) = temperature in Kelvin

3. **Convert Temperature to Kelvin**: Since the temperature is given in Celsius, we need to convert it to Kelvin:
\[ T(K) = 0°C + 273.15 = 273.15 K \]

4. **Assume Ideal Conditions**: For an ideal molar solution, we assume that the concentration \(C\) is 1 mol/L and the van 't Hoff factor \(i\) is 1 (for non-electrolytes like sucrose).

5. **Substitute Values into the Formula**:
\[ \pi = (1)(0.0821 \, \text{L·atm/(K·mol)})(273.15 \, \text{K}) \]

6. **Calculate Osmotic Pressure**:
\[ \pi = 0.0821 \times 273.15 \approx 22.4 \, \text{atm} \]

7. **Conclusion**: Therefore, the osmotic pressure of an ideal molar solution at 0°C is approximately 22.4 atm.

### Final Answer:
The osmotic pressure of an ideal molar solution at 0°C is **22.4 atm**.

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