Test: Colligative Properties - 1 - Chemistry MCQ

Raoult’s law is obeyed by each constituent of a binary liquid solution when:

For a binary ideal liquid solution, the total pressure of the solution is given as:

For an ideal binary liquid solution with , which relation between X_A (mole fraction of A in liquid phase) and Y_A (mole fraction of A in vapour phase) is correct?

An ideal solution is formed by mixing two volatile liquids A and B, X_A and X_B are the mole fractions of A and B respectively in the solution and Y_A and Y_B are the mole fractions of A and B respectively in the vapour phase. A plot of along y–axis against  along x–axis gives a straight line. What is the slope of the straight line?

For a dilute solut ion, Raoult’s law states that:

The solubility of a specific non–volatile salt is 4 g in 100 g of water at 25°C. If 2.0 g, 4.0 g and 6.0 g of the salt added of 100 g of water at 25°C, in system X, Y, and Z. The vapour pressure would be in the order:

The boiling point of C₆H₆, CH₃OH, C₆H₅NH₂ and C₆H₅NO₂ are 80°C, 65ºC, 184°C and 212°C respectively. Which will show highest vapour pressure at room temperature:

6.0 g of urea was dissolved in 9.9 moles of water. If the vapour pressure of pure water is P°, the vapour pressure of solution is:

An ideal solution was found to have a vapour pressure of 80 torr when the mole fraction of a non– volatile solute was 0.2. What would be the vapour pressure of the pure solvent at the same temperature?

The vapour pressure of an aqueous solution of sucrose at 373 K is found to be 750 mm Hg. The molality of the solution at the same temperature will be:

Estimate the lowering of vapour pressure due to the solute (glucose) in a 1.0 M aqueous solution at 100°C:

Calculate the mass of a non-volatile solute (molar mass 40 g mol^-1) which should be dissolved in 114 g octane to reduce its vapour pressure to 80%.

Equal weight of a solute are dissolved in equal weight of two solvents A and B formed very dilute solution. The relative lowering of vapour pressure for the solution B has twice the relative lowering of vapour pressure for the solut ion A. If M_A and M_B are the mo lecular weights of so lvents A and B respectively, then:

An ideal solution has two components A and B. A is more volatile than B, i. e., and also If X_A and Y_A are mole fractions of components A in liquid and vapour phases, then

At 25°C, the vapour pressure of pure liquid A (mol. wt. = 40) is 100 torr, while that of pure liquid B is 40 torr, (mol. wt. = 80). The vapour pressure at 25°C of a solution containing 20 g of each A and B is:

Two liquids A and B from ideal solutions. At 300 K, the vapour pressure of solution containing 1 mole of A and 3 mole of B is 550 mm Hg. At the same temperature, if one more mole of B is added this solution, the vapour pressure of the solution increases by 10 mm Hg. Determine the vapour pressure of A and B in their pure states (in mm Hg):

Two liquids A and B have vapour pressure in the ratio  at a certain temperature. Assume A and B form an ideal solution and the ratio of mole fractions A and B in the vapour phase is 4:3. Then the mole fraction of B in the solution at the same temperature is: