Given that the pH of a 0.1 M monobasic acid is 2, what is the osmotic pressure at a given temperature T?

1. 0.1RT

2. 0.11RT

3. 1.1RT

4. 0.01RT

The vapour pressure of pure water at 298K is 23.76mm. The vapour pressure of a solution of sucrose(C₁₂H₂₂O₁₁) in 5.56 moles of water is 23.392mm Hg. The mass of sucrose in the solution is

1. 15 g

2. 45 g

3. 30 g

4. 37.5 g

Which of the following 0.1 M aqueous solutions will have the lowest freezing point?

The vapour pressure of toluene is 59.1 torr at 313.75 K and 298.7 torr at 353.15 K. Calculate, the molar heat of vaporisation.

1. 37888 J mol^-1

2. 27188 J mol^-1

3.  12834 J mol^-1

4. 571328 J mol^-1

The vapour pressure of a pure liquid solvent A is 0.80 atm. When a non-volatile substance B is added to the solvent, its vapour pressure drops to 0.60 atm.
Mole fraction of the component B in the solution is:

The lowest boiling point, if concentration is fixed at 0.1 M in aqueous solution, is given by which of the following solutions?

a. K₂SO₄

b. NaCl

c. Urea

d. Glucose

1. a, b

2. b, c

3. c, d

4. d, a

The boiling point of acetic acid is 118.1$°\mathrm{C}$ and its latent heat of vaporisation is 121 cal/gm. A solution containing 0.4344 gm anthracene in 44.16 gm acetic acid boils at 118.24$°\mathrm{C}$. What is the molecular wt. of anthracene ?

1. 122

2. 178

3. 105

4. 154

Which solution will have the highest boiling point ?

1. 1 (M) C₆H₁₂O₆ solution

2. 1 (M) NaCl solution

3. 1 (M) BaCl₂ solution

4. 1 (M) CO(NH₂)₂ solution

A 2.0% solution by weight of urea in water shows a boiling point elevation of 0.18 deg [Molecular weight of urea=60]. Calculate the latent heat of vaporization per gram of water.

1. 495.3 cal/g

2. 560.3 cal/g

3. 525.8 cal/g

4. 501.3 cal/g

A solution of 18 g of glucose in 1000 g of water is cooled to -0.2 ^oC. The amount of ice separating out from this solution is -

[K_f(H₂O) = 1.86 K molal^-1]