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

💡 Solution & Explanation

I need to analyze statements about osmotic pressure (π), volume (V), and temperature (T), but the question options aren't provided in your prompt. However, based on standard colligative property relationships, here's the framework for identifying incorrect statements: **Key relationship for osmotic pressure:** $$\pi = iMRT = \frac{i n RT}{V}$$ where $i$ = van't Hoff factor, $M$ = molarity, $R$ = gas constant, $T$ = absolute temperature, $n$ = moles of solute, $V$ = volume of solution. **Correct relationships:** - π is **directly proportional** to $T$ (at constant V and composition) - π is **inversely proportional** to $V$ (at constant T and composition) - π is **independent** of the nature of solute (depends only on solute concentration) **Common incorrect statements (likely option C):** - "π is inversely proportional to T" ✗ (should be directly proportional) - "π is directly proportional to V" ✗ (should be inversely proportional) - "Osmotic pressure depends on the molar mass of solute" ✗ (it depends only on number of particles, not their mass) - "Doubling V at constant T decreases π" ✓ (This would be correct) **To identify C as incorrect:** If option C states that π is **inversely related to T** or **directly related to V**, it contradicts the van't Hoff equation. The osmotic pressure must increase with temperature and decrease with dilution (increased volume). Please share the complete options so I can provide the specific explanation for why C is incorrect.