{"id":163035,"date":"2026-05-03T04:36:56","date_gmt":"2026-05-03T04:36:56","guid":{"rendered":"https:\/\/news.gyankatta.org\/?p=163035"},"modified":"2026-05-03T05:27:56","modified_gmt":"2026-05-03T05:27:56","slug":"class-12-chemistry-solutions-advanced-challenge-asset-pro-max","status":"publish","type":"post","link":"https:\/\/news.gyankatta.org\/?p=163035","title":{"rendered":"Class 12 Chemistry: Solutions – Advanced Challenge (ASSET Pro Max)"},"content":{"rendered":"\n
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Class 12 Chemistry: Solutions – Advanced Challenge (ASSET Pro Max)<\/h2>\n    
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Q1.<\/strong> A student observes that a mixture of Chloroform and Acetone becomes noticeably warm during the mixing process. Which of the following best explains the molecular behavior and the resulting vapor pressure of this solution?<\/p>\n        
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  • (A) The mixture shows a positive deviation from Raoult\u2019s Law because the new interactions are weaker than the pure component interactions.<\/li>\n            
  • (B) The mixture shows a negative deviation from Raoult\u2019s Law because hydrogen bonding occurs between the different molecules, lowering the total vapor pressure.<\/li>\n            
  • (C) The vapor pressure increases linearly with the mole fraction because the enthalpy of mixing is zero in this specific case.<\/li>\n            
  • (D) The boiling point of the mixture will be lower than that of both pure components due to the exothermic nature of the process.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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    Q2.<\/strong> Why is the molarity of a solution considered an unreliable unit for experiments conducted across a wide range of temperatures, whereas molality remains consistent?<\/p>\n        
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    • (A) Molarity depends on the mass of the solvent, which can fluctuate due to evaporation at higher temperatures.<\/li>\n            
    • (B) Molarity is defined by the volume of the solution, which expands or contracts with temperature changes, altering the concentration value.<\/li>\n            
    • (C) Molality is a ratio of moles to the total volume of the solution, making it inherently more stable than mass-based units.<\/li>\n            
    • (D) The number of moles of solute actually increases at higher temperatures, but this effect is mathematically cancelled out in molality calculations.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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      Q3.<\/strong> Consider three 0.1 m aqueous solutions: Glucose, Sodium Chloride, and Aluminium Sulfate. Which statement accurately compares their freezing points?<\/p>\n        
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      • (A) All three solutions will freeze at exactly the same temperature because they have the same molality.<\/li>\n            
      • (B) Glucose will have the lowest freezing point because it has the largest molecular weight among the three solutes.<\/li>\n            
      • (C) Aluminium Sulfate will have the lowest freezing point because it dissociates into the highest number of particles per formula unit.<\/li>\n            
      • (D) Sodium Chloride will have a lower freezing point than Aluminium Sulfate because the smaller size of its ions allows for faster freezing.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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        Q4.<\/strong> In a scuba diving scenario, ‘the bends’ is a painful condition caused by nitrogen bubbles forming in the blood. How does Henry\u2019s Law explain the prevention of this condition using Heliox (Helium-Oxygen mixture)?<\/p>\n        
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        • (A) Helium has a higher Henry\u2019s Law constant (KH<\/sub>) than Nitrogen, meaning it is less soluble in blood at high pressures.<\/li>\n            
        • (B) Helium is more soluble than Nitrogen at high pressures, ensuring that no gas escapes the blood during rapid ascent.<\/li>\n            
        • (C) The pressure of Helium is independent of the depth of the diver, preventing any changes in gas concentration in the tissues.<\/li>\n            
        • (D) Helium reacts chemically with hemoglobin to prevent other gases from dissolving in the plasma under extreme pressure.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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          Q5.<\/strong> An azeotropic mixture of Ethanol and Water (95.4% ethanol) cannot be separated further by simple fractional distillation. This is primarily because:<\/p>\n        
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          • (A) The boiling points of the two pure components have become identical due to the high concentration of ethanol.<\/li>\n            
          • (B) The composition of the liquid phase is identical to the composition of the vapor phase at this specific concentration.<\/li>\n            
          • (C) Ethanol and Water form a solid complex at this ratio, which prevents the liquid from evaporating at all.<\/li>\n            
          • (D) The mixture shows a large negative deviation from Raoult’s Law, making the vapor pressure extremely low.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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            Q6.<\/strong> If a non-volatile solute undergoes 80% dissociation in an aqueous solution, how does this specifically impact the calculated Osmotic Pressure compared to a non-electrolyte?<\/p>\n        
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            • (A) The osmotic pressure will be exactly double because dissociation always implies a two-fold increase in particle count.<\/li>\n            
            • (B) The osmotic pressure will be significantly higher than calculated for a non-electrolyte, as the Van’t Hoff factor (i) will be greater than 1.<\/li>\n            
            • (C) The osmotic pressure will decrease because the total volume of the solution increases when ions move apart.<\/li>\n            
            • (D) There will be no change in osmotic pressure because the total mass of the solute remains the same regardless of dissociation.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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              Q7.<\/strong> Which of the following conditions must be met for a solution to be considered ‘Ideal’ across the entire range of concentrations?<\/p>\n        
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              • (A) The heat of mixing must be negative to ensure that the molecules are strongly attracted to one another.<\/li>\n            
              • (B) The total volume of the solution must be exactly equal to the sum of the volumes of the two pure components.<\/li>\n            
              • (C) The solute must be significantly more volatile than the solvent to ensure rapid equilibration in the vapor phase.<\/li>\n            
              • (D) The mixture must form a maximum-boiling azeotrope to stabilize the vapor pressure against external fluctuations.<\/li>\n        <\/ul>\n    <\/div>\n\n    \n    
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                Q8.<\/strong> When salt is spread on icy roads in cold climates, the ice melts. What is the underlying physical chemistry principle behind this practical application?<\/p>\n