The vapour pressure of water at room temperature is 30mm of Hg. If the mole fraction of the water is 0.9, the
vapour pressure of the solution will be
What is the osmotic pressure of the solution obtained by mixing 300 cm3 of 2% (mass-volume) solution of urea with 300 cm3 of 3.42% solution of sucrose of 27°C? (R = 0.082 L atm K–1mol–1)
Elevation in boiling point was 0.52°C when 6 g of a compound X was dissolved in 100 g of water. Molecular
weight of X is (Kb for H2O is 0.52)
0.5 molal aqueous solution of a weak acid(HX) is 20% ionised. If Kf for water is 1.86 K kg mol–1, the lowering in freezing point of the solution is
Two beakers have equal volumes of solutions. One contains 60 g of glucose and other contains 60 g of
urea. Which one of the following is true about two solutions ?
For an ideal solution with , which of the following is true ?
Two beakers of capacity 500 mL were taken. One of these beakers, labelled as “A”, was filled with
400 mL water whereas the beaker labelled “B” was filled with 400 mL of 2 M solution of NaCl. At the same
temperature both the beakers were placed in closed containers of same material and same capacity as in
At the given temperature, which of the following statement is correct about the vapour pressure of pure
water and that of NaCl solution.
The vapour pressure of a pure liquid ‘A’ is 70 torr at 27°C. It forms an ideal solution with another liquid B.
The mole fraction of B is 0.2 and total pressure of the solution is 84 torr at 27°C. The vapour pressure of pure
liquid B at 27°C is
A 0.004 M solution of Na2SO4 is isotonic with a 0.010 M solution of glucose at same temperature. The apparent degree of dissociation of Na2SO4 is
At 40°C, the vapour pressure in torr of methanol and ethanol solution is P = 119x + 135 (where x is the mole
fraction of methanol).Hence,
Concentrated aqueous sulphuric acid is 98% H2SO4 by mass and has a density of 1.80 g mol–1. The volume
of acid required to make one litre of 0.1 M H2SO4 solution
Two liquids A and B have and in the ratio of 1 : 3. If the ratio of number of moles of A and B are
1 : 3, the mole fraction of ‘A’ in vapour phase in equilibrium with the solution is equal to
The molal elevation constant of water is 0.51. The boiling point of 0.1 molal aqueous NaCl solution is
The freezing point of a solution prepared from 1.25 g of non-electrolyte and 20 g of water is 271.9 K. If
molar depression constant is 1.86 K mol–1 then molar mass of the solute will be
An aqueous solution freezes at –0.186°C,what will be elevation in boiling point of the solution? (Kf = 1.860,
Kb = 0.512°)
Benzene and toluene form nearly ideal solutions. At 20o C, the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The partial vapour pressure of benzene at 20o C for a solution containing 78 g of benzene and 46 g of toluene in torr is
When a solute B is added to a solution of A then solution appears hotter. Which of the following graph correctly represent nature of solution ?
How many gram of dibasic acid(mol. mass 200) should be present in 100 mL of the aqueous solution to give
0.1 N solution ?
At 800C, the vapour pressure of pure liquid ‘A’ is 520 mm Hg and that of pure liquid ‘B’ is 1000 mm Hg. If a
mixture solution of ‘A’ and ‘B’ boils at 800C and 1 atm pressure , then amount of ‘A’ in the mixture is (1 atm =
760 mm Hg)