✓✗The molality of a solution containing 9.8 g of H₂SO₄ (molar mass 98 g mol⁻¹) in 250 g of water is

✓✗Statement I: The van't Hoff equation π = CRT holds well only for dilute solutions.
Statement II: Osmotic pressure is a colligative property.

✓✗If the partial pressure of a gas above its solution is doubled at constant temperature, its mole fraction in the solution becomes

✓✗The modified formula for depression of freezing point when the solute dissociates or associates is

✓✗Pressure has no significant effect on the solubility of solids in liquids because

✓✗A mixture of ethanol and water shows positive deviation from Raoult's law. Its azeotrope is a

✓✗Which of the following salts has the same value of van't Hoff factor (i) as that of K₃[Fe(CN)₆]?

✓✗Which of the following statements about Henry's law are correct?
A. K_H is a function of the nature of the gas.
B. The higher the value of K_H, the higher the solubility of the gas.
C. K_H for a gas generally increases with temperature.
D. Henry's law is obeyed when the gas does not react with the solvent.
Choose the correct answer from the options given below.

✓✗In the ideal benzene−toluene solution described with 0.5 mol of each (benzene 95 mm Hg, toluene 28 mm Hg), the mole fraction of benzene in the vapour is

✓✗The vapour pressure of a 5% (by mass) aqueous solution of a non-volatile solute at 373 K is 745 mm Hg. Using the exact Raoult expression, its molar mass is close to

✓✗Ethylene glycol (62 g mol⁻¹) is preferred to methanol as an antifreeze mainly because

✓✗Which of the following aqueous solutions has the highest osmotic pressure at the same temperature?

✓✗The concentration unit that is independent of temperature is

✓✗An antifreeze solution is prepared from 222.6 g of ethylene glycol (C₂H₆O₂, molar mass 62 g mol⁻¹) and 200 g of water. The molality of the solution is

✓✗The density of a 3 M aqueous NaCl solution is 1.25 g mL⁻¹. Its molality is (molar mass of NaCl 58.5 g mol⁻¹)