The osmotic pressure of a solution containing 0.1 mol of solute per litre at 300 K is

Answer

To calculate the osmotic pressure (π) of a solution, we can use the formula:

\[ \pi = \frac{n}{V} \cdot R \cdot T \]

Where:
- \( n \) = number of moles of solute
- \( V \) = volume of the solution in liters
- \( R \) = universal gas constant = 0.0821 atm·L/(K·mol)
- \( T \) = temperature in Kelvin

### Step-by-Step Solution:

1. **Identify the given values**:
- Number of moles of solute (\( n \)) = 0.1 mol
- Volume of the solution (\( V \)) = 1 L (since it is given per liter)
- Temperature (\( T \)) = 300 K

2. **Substitute the values into the formula**:
\[ \pi = \frac{0.1 \, \text{mol}}{1 \, \text{L}} \cdot 0.0821 \, \text{atm·L/(K·mol)} \cdot 300 \, \text{K} \]

3. **Calculate the concentration**:
\[ \frac{0.1 \, \text{mol}}{1 \, \text{L}} = 0.1 \, \text{mol/L} \]

4. **Calculate the osmotic pressure**:
\[ \pi = 0.1 \cdot 0.0821 \cdot 300 \]

5. **Perform the multiplication**:
\[ \pi = 0.1 \cdot 24.63 = 2.463 \, \text{atm} \]

6. **Final Result**:
The osmotic pressure of the solution is approximately \( 2.463 \, \text{atm} \).