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Dissociation

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

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 ChemistryAn AB₂ solute has a true molar mass of 120 g mol⁻¹ and is 80% dissociated. What will be its observed molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryThe true molar mass of a solute is 150 g mol⁻¹, but its molar mass determined by a colligative-property method is 100 g mol⁻¹. What is the van’t Hoff factor, and what is the probable behaviour of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf the observed molar mass of a solute is 0.625 times its true molar mass, what are the van’t Hoff factor (i) and the type of behaviour shown by the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryAn AB-type solute is 75% dissociated. If its observed molar mass is 80 g mol⁻¹, what is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryThe observed molar mass of an AB3-type solute is 4/7 of the true value. What is the degree of dissociation?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 16Hard ChemistryThe true molar mass of AlCl3 is 133.5 g mol−1. If the observed molar mass from a colligative method is 44.5 g mol−1, what is the degree of dissociation?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16Hard ChemistryWhen 1.6 g of a substance is dissolved in 200 g of water, the freezing-point depression is 0.744 K. If the normal molar mass is 80 g mol⁻¹ and Kf = 1.86 K kg mol⁻¹, what is the van’t Hoff factor i?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryA salt of type AB₃ undergoes 50% dissociation. If its normal molar mass is 200 g mol⁻¹, what will be its observed molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryFor a solution, the observed freezing-point depression is 0.558 K. For the same amount assuming normal behaviour, the expected depression is 0.372 K. What is the van’t Hoff factor?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Medium ChemistryA salt of the type AB₂ is 75% dissociated. If its normal molar mass is 120 g mol⁻¹, what will be its observed molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryThe normal molar mass of a solute is 90 g mol⁻¹. If its observed molar mass obtained from a colligative-property measurement is 60 g mol⁻¹, what is the van’t Hoff factor?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Medium ChemistryA solute has an observed molar mass of \(72\,g\,mol^{-1}\). If its van’t Hoff factor is \(i=1.5\), what is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryAn \(AB\)-type solute is 25% dissociated. If its observed molar mass is \(80\,g\,mol^{-1}\), what is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryAn \(AB_2\) solute has a true molar mass of \(150\,g\,mol^{-1}\). If it is dissociated to the extent of 50%, what is its observed molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryIn a solution, the true molar mass of the solute is 100 g mol⁻¹, but the vapour-pressure method gives an observed molar mass of 50 g mol⁻¹. Which conclusion is correct?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 16Medium ChemistryIf the observed molar mass of a solute is 0.8 times its true molar mass, what is the van’t Hoff factor, i?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 16Medium ChemistryThe molar mass of a solute determined by the freezing-point depression method is much lower than its true molar mass. Which reason is most probable?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16Medium ChemistryThe true molar mass of a solute is \(180\,\mathrm{g\,mol^{-1}}\), but a colligative-property measurement gives an apparent molar mass of \(90\,\mathrm{g\,mol^{-1}}\). What is the value of the van’t Hoff factor \(i\)?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Medium ChemistryA sample has a normal molar mass of \(98\,\mathrm{g\,mol^{-1}}\), but its experimentally determined molar mass is \(49\,\mathrm{g\,mol^{-1}}\). Which statement best explains this result?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Medium