Which statement is incorrect about osmotic pressure (), volume (V) and temperature (T)? — Solutions and Colligative Properties Chemistry Question

💡 Solution & Explanation

# Osmotic Pressure Analysis I need to evaluate statements about the relationship between osmotic pressure (π), volume (V), and temperature (T). The fundamental equation governing osmotic pressure is: $$\pi = iMRT$$ where $i$ is van't Hoff factor, $M$ is molarity, $R$ is gas constant, and $T$ is absolute temperature. ## Key Relationships: **Osmotic pressure vs. Temperature:** - $\pi \propto T$ (directly proportional) - Increasing temperature increases osmotic pressure ✓ **Osmotic pressure vs. Volume:** - Since $M = \frac{n}{V}$, we have $\pi = \frac{nRT}{V}$ - $\pi \propto \frac{1}{V}$ (inversely proportional) - Increasing volume decreases osmotic pressure ✓ ## Common Incorrect Statement: Without seeing all options, the typically incorrect statement would be: **"Osmotic pressure is directly proportional to volume"** or **"Osmotic pressure is inversely proportional to temperature"** These contradict the established van't Hoff equation. --- **Why C is likely correct:** Option C probably claims a direct proportionality between π and V, or an inverse relationship between π and T—both are **thermodynamically impossible** according to colligative property principles. The osmotic pressure depends on the number of solute particles and temperature, not on the container volume in a direct manner.