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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 300 mL solution is prepared using 2.4 g solute. Its osmotic pressure at 300 K is 0.492 atm. If the solute forms dimers and i = 0.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA 1.0 L solution is prepared by dissolving 2.2 g of a substance. Its osmotic pressure at 300 K is 0.451 atm. If R = 0.082 L atm K⁻¹ mol⁻¹, what is the approximate molar mass of the substance?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryA solution contains 0.6 g of a solute in 0.2 L of solution. If its osmotic pressure at 300 K is 0.369 atm, what is the molar mass? Use R = 0.082 L atm K⁻¹ mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryA 0.2 M electrolyte has an osmotic pressure of 7.38 atm at 300 K. If R = 0.082 L atm K⁻¹ mol⁻¹, what is i, and what type of dissociation does it indicate?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryA 0.05 M solution has an osmotic pressure of 2.46 atm at 300 K. Taking R = 0.082 L atm K⁻¹ mol⁻¹, what are the van’t Hoff factor and the effective number of solute particles?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryIf a 0.2 M nonelectrolyte solution has an osmotic pressure of 4.92 atm at 300 K, what will be the osmotic pressure of a 0.1 M solute with i = 3 at the same temperature?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Medium ChemistryA polymer solution contains 0.2 g polymer in 200 mL solution. At 300 K, its osmotic pressure is 0.0205 atm. If R = 0.082 L atm K⁻¹ mol⁻¹, what is the molar mass of the polymer?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryA 250 mL solution is prepared using 0.25 g of a polymer. Its osmotic pressure at 300 K is 0.041 atm. If R = 0.082 L atm K−1 mol−1, what is the molar mass of the polymer?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryA 500 mL solution is prepared using 0.75 g of an unknown solute. Its osmotic pressure at 300 K is 0.123 atm. If R = 0.082 L atm K⁻¹ mol⁻¹, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryWhy is the osmotic-pressure method considered more reliable for determining the molar mass of large molecules?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf the osmotic-pressure method gives a molarity of 0.015 mol L⁻¹ and 400 mL of the solution contains 1.2 g of solute, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA \(250\,mL\) solution is prepared using \(2.5\,g\) of solute. At \(300\,K\), its osmotic pressure is \(\pi=1.23\,atm\). If \(i=2\), 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 100 mL solution is prepared from 1.0 g of a solute. At 300 K, its osmotic pressure is 0.615 atm and i = 1.25. What is the true molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA 200 mL solution is prepared using 1.2 g of a solute. At 300 K, its osmotic pressure is 0.246 atm. If the solute forms dimers and its van’t Hoff factor is i = 0.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA \(1\,\mathrm{L}\) solution is prepared from \(6\,\mathrm{g}\) of solute. Its osmotic pressure at \(300\,\mathrm{K}\) is \(1.23\,\mathrm{atm}\). The solute is non-dissociating. What is its molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA solution of volume \(500\,\mathrm{mL}\) is prepared using \(1.5\,\mathrm{g}\) of solute. Its osmotic pressure at \(300\,\mathrm{K}\) is \(0.615\,\mathrm{atm}\). If \(R=0.082\,\mathrm{L\,atm\,mol^{-1}\,K^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA \(0.001\,\mathrm{M}\) solution is prepared to determine the molar mass of a protein. Which measurement is most useful for such a very dilute solution?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf \(2.0\,\mathrm{g}\) of solute in \(1.0\,\mathrm{L}\) of solution gives an osmotic pressure of \(0.492\,\mathrm{atm}\) at \(300\,\mathrm{K}\), what is the molar mass? Use \(R=0.082\,\mathrm{L\,atm\,K^{-1}\,mol^{-1}}\).Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryA solution has osmotic pressure \(1.23\,\mathrm{atm}\) at \(300\,\mathrm{K}\). If the concentration of the same solution is halved while the temperature remains \(300\,\mathrm{K}\), what will be the new osmotic pressure?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 17Easy ChemistryWhich colligative property is most suitable for determining the molar mass of macromolecules such as proteins, which have very high molar masses?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium