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Class 11 · Chemistry
→If AB2 dissociates completely into A2+ and 2B− ions, what is the ideal value of the van’t Hoff factor, i?
Class 12 · Chemistry
→In which situation is osmotic pressure more useful than freezing-point depression for determining molar mass?
Class 11 · Chemistry
→Which of the following properties depends on the number of solute particles rather than on their chemical nature?
Class 12 · Chemistry
→A solution contains 0.1 mol of NaCl, which dissociates completely into ions. At the same molality, how will the boiling-point elevation of the NaCl solution compare with that of a urea solution?
Class 12 · Chemistry
→In a numerical problem on colligative properties, what should be done first to obtain the correct answer?
Class 12 · Chemistry
→If two solutions have the same molality but the solute ionises in one of them, which solution will show the greater colligative effect?
Class 12 · Chemistry
→If two non-electrolyte solutions have the same molality and the same solvent, how will their ΔT_f values compare?
Class 12 · Chemistry
→If a solute completely dissociates into three ions in solution, what is the ideal van’t Hoff factor, i?
Class 12 · Chemistry
→Which statement gives the correct understanding of colligative properties?
Class 12 · Chemistry
→If 0.2 mol of a non-electrolyte solute is dissolved in 400 g of solvent and K_b = 0.5 K kg mol⁻¹, what is the elevation in boiling point, ΔT_b?
Class 12 · Chemistry
→If 0.1 mol of a non-electrolyte solute is dissolved in 200 g of solvent and K_f = 1.8 K kg mol⁻¹, what is the depression in freezing point, ΔT_f?
Class 12 · Chemistry
→For a solution with van’t Hoff factor i = 0.5, cryoscopic constant K_f = 2 K kg mol⁻¹, and molality m = 1 mol kg⁻¹, what is the depression in freezing point, ΔT_f?
Class 12 · Chemistry
→If the molality of a non-electrolyte solution is 0.5 mol kg⁻¹ and the ebullioscopic constant is K_b = 0.52 K kg mol⁻¹, what is the elevation in boiling point, ΔT_b?
Class 12 · Chemistry
→Why is the freezing point of a solution lower than that of the pure solvent?
Class 12 · Chemistry
→Why does the boiling point of a solution become higher than that of the pure solvent when a non-volatile solute is added?
Class 12 · Chemistry
→If the effective number of solute particles in a solution increases, what happens to the lowering of vapour pressure?
Class 12 · Chemistry
→Why must temperature be expressed in kelvin in the osmotic-pressure equation π = iCRT?
Class 12 · Chemistry
→If the concentration of a dilute solution remains constant and its temperature is increased, what happens to its osmotic pressure?
Class 12 · Chemistry
→If two solutions are separated by a semipermeable membrane and have equal osmotic pressure at the same temperature, what will happen?
Class 12 · Chemistry
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