To calculate the osmotic pressure $\Pi$ of the solution, we'll use the formula:

$\Pi = \frac{n}{V} \cdot R \cdot T$

Where:

• $\Pi$ is the osmotic pressure.
• $n$ is the number of moles of solute.
• $V$ is the volume of the solution in liters.
• $R$ is the ideal gas constant ($R = 0.0821 \, \text{L} \cdot \text{atm} \cdot \text{K}^{-1} \cdot \text{mol}^{-1}$).
• $T$ is the temperature in Kelvin.

Given:

• Number of moles of naphthalene ($n$) = 0.156 mol/L
• Volume ($V$) = 1 L (since the concentration is given per liter)
• Temperature ($T$) = 14°C = 287.15 K (converted from Celsius to Kelvin by adding 273.15)

Now we can plug these values into the osmotic pressure formula:

$\Pi = \left(\frac{0.156 \, \text{mol}}{1 \, \text{L}}\right) \cdot 0.0821 \, \text{L} \cdot \text{atm} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} \cdot 287.15 \, \text{K}$

Now, calculate:

$\Pi = 0.156 \cdot 0.0821 \cdot 287.15$

$\Pi \approx 3.67 \, \text{atm}$

Final Answer:

The osmotic pressure $\Pi$ of the solution at 14°C is approximately 3.67 atm.

Would you like more details, or do you have any questions about this calculation?

Here are five related questions:

1. How does the osmotic pressure change with temperature?
2. What effect does increasing the concentration of naphthalene have on osmotic pressure?
3. How would you calculate osmotic pressure for a solution with multiple solutes?
4. What assumptions are made in the ideal gas law when calculating osmotic pressure?
5. How does osmotic pressure relate to colligative properties?

Tip: Always ensure the temperature is in Kelvin when applying the osmotic pressure formula to avoid errors.