A mixture of liquid X and liquid Y forms a maximum boiling azeotrope. What can be inferred about the intermolecular forces between X and Y compared to the forces within pure X and pure Y?

Solution A contains 7 g/L of $MgC{l_2}$ and solution B contains 7 g/L of $NaCl$. At room temperature, the osmotic pressure of

Henry's law constant for CO2 in water at 298 K is $1.67 imes 10^8$ Pa. Calculate the mass of CO2 that can be dissolved in 500 mL of water at 298 K and a CO2 partial pressure of 2.5 atm.

At 25°C, the vapor pressures of pure benzene and toluene are 12.8 kPa and 3.85 kPa, respectively. If an ideal solution is prepared with 2 moles of benzene and 1 mole of toluene, what is the total vapor pressure above the solution?

Which of the following is NOT an application of Henry's law?

Relative lowering of vapour pressure of a dilute solution is 0.2. What is the mole fraction of the non-volatile solute ?

Lowering of vapour pressure is highest for

The vapour pressure $(VP)$ of a dilute solution of non-volatile solute is $P$ and the $VP$ of pure solvent is ${P_0}$, the lowering of the $VP$ is :

An aqueous solution is 1.0 molal in KI. Which change will cause the vapour pressure of solution to increase :

A solution showing a large positive deviation from Raoult's law forms a:

The vapour pressure of a pure liquid A is 70 mm Hg at 300 K. When a non-volatile solute B is added to A, the vapour pressure of the solution becomes 63 mm Hg. What is the mole fraction of B in the solution?