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Osmotic Pressure

Class 12 Chemistry के इस tag से जुड़े questions। हर question के साथ chapter, topic, level और difficulty दी गई है।

ChemistryA solution has higher osmotic pressure than another solution at the same temperature. If both contain the same mass of solute, what is the most suitable conclusion about the first solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryIf 0.5 g of a solute in 250 mL solution gives an osmotic pressure of 0.82 atm at 27 °C, find its molar mass. Use R = 0.082 L atm K⁻¹ mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryIn the osmotic-pressure method, using M = wRT/(πV), what does V represent?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Easy ChemistryWhy is the osmotic-pressure method considered especially useful for determining the molar mass of biomolecules?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryThe molar mass of a solute determined by osmotic pressure is lower than its normal value. What is the most suitable reason?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryA 1 L solution is prepared from 3.6 g of a solute. At 300 K, its osmotic pressure is 0.369 atm. If the solute undergoes 25% dimerization, what is its approximate true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryIf 0.3 g of a solute in 150 mL of solution gives an osmotic pressure of 0.123 atm at 300 K, and i = 1, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA solute of concentration 0.02 M has an osmotic pressure of 0.984 atm at 300 K. If R = 0.082 L atm mol⁻¹ K⁻¹, what is the van’t Hoff factor (i), and what does it indicate about the solute’s behaviour?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA 300 mL solution is prepared using 1.8 g of solute. At 300 K, its osmotic pressure is 0.492 atm. If i = 1.2, what is the true molar mass? Use R = 0.082 L atm K⁻¹ mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA solution contains 2.4 g of solute in 400 mL of solution. Its osmotic pressure at 300 K is 0.492 atm. If i = 0.8, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA 500 mL solution is prepared using 2 g of solute. At 300 K, its osmotic pressure is 0.615 atm. If i = 1.25, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryA 0.04 M solution has an osmotic pressure of 1.476 atm at 300 K. If the true molar mass is 150 g mol⁻¹, what will be the observed molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA 250 mL solution is prepared from 3.0 g of a solute. At 300 K, its osmotic pressure is 0.738 atm. If the solute has i = 0.75, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA 1 L solution is prepared from 2.0 g of a solute. At 300 K, its osmotic pressure is 0.164 atm. If the solute forms dimers to the extent of 50%, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryIf 0.2 g solute in 100 mL solution gives an osmotic pressure of 0.123 atm at 300 K and i = 1, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA 0.01 M solute has an osmotic pressure of 0.369 atm at 300 K. If R = 0.082 L atm mol⁻¹ K⁻¹, what are i and the likely behaviour of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA 500 mL solution is prepared from 4.5 g of solute. At 300 K, its osmotic pressure is 0.738 atm. If the van’t Hoff factor is 1.2, what is the true molar mass? Use R = 0.082 L atm K⁻¹ mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA solution contains 3.0 g of solute in 600 mL of solution. Its osmotic pressure at 300 K is 0.615 atm. If the van’t Hoff factor is i = 0.75, what is the true molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA 250 mL solution is prepared from 3 g of solute. At 300 K, its osmotic pressure is 1.845 atm. If i = 1.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA 0.05 M solution has osmotic pressure 1.845 atm at 300 K. If the true molar mass of the solute is 120 g mol−1, what observed molar mass will be obtained from the colligative method?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16Hard