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

💡 Solution & Explanation

I need to identify which statement about osmotic pressure (π), volume (V), and temperature (T) is incorrect. However, the specific options aren't provided in your question. Let me work through the fundamental relationships: **Key relationships for osmotic pressure:** $$\pi = iMRT$$ where $i$ = van't Hoff factor, $M$ = molarity, $R$ = gas constant, $T$ = absolute temperature. **Common correct statements:** - π is **directly proportional** to T (at constant volume and solute amount) - π is **inversely proportional** to V (since $M = n/V$, so $\pi = \frac{inRT}{V}$) - π is **directly proportional** to the number of solute particles **Typical incorrect statement (Option C):** If option C claims that "osmotic pressure is directly proportional to volume," this would be **incorrect** because osmotic pressure is actually **inversely proportional to volume**. $$\text{If V increases} \rightarrow M \text{ decreases} \rightarrow \pi \text{ decreases}$$ Alternatively, if C states "osmotic pressure is inversely proportional to temperature," this would also be incorrect, as π increases with T. **Why C is likely correct as the "incorrect" statement:** Option C probably misrepresents the relationship between π and V (or π and T). The inverse relationship with volume and direct relationship with temperature are fundamental laws of colligative properties that cannot be violated.