Solutions · Question 4

Which of the following aqueous solution will exhibit highest boiling point?

1. 0.01 M Na2SO4
2. 0.015 M C6H12O6
3. 0.01 M Urea
4. 0.01 M KNO3

Match List-I with List-II Choose the correct answer from the options given below:

1. A-III, B-I, C-IV, D-II
2. A-III, B-II, C-I, D-IV
3. A-II, B-IV, C-I, D-III
4. A-II, B-I, C-IV, D-III

5 moles of liquid X and 10 moles of liquid Y make a solution having a vapour pressure of 70 torr. The vapour pressures of pure X and Y are 63 torr and 78 torr respectively. Which of the following is true regarding the described solution?

1. The solution is ideal.
2. The solution has volume greater than the sum of individual volumes.
3. The solution shows positive deviation.
4. The solution shows negative deviation.

The Henry's law constant (KH) values of three gases (A, B, C) in water are 145, 2 10-5 and 35 kbar respectively. The solubility of these gases in water follows the order:

1. B > A > C
2. B > C > A
3. A > C > B
4. A > B > C

The plot of osmotic pressure ( ) vs concentration ( mol L-1) for a solution gives a straight line with slope 25.73 L bar mol-1. The temperature at which the osmotic pressure measurement is done is (Use R = 0.083 L bar mol-1 K-1)

1. 37
2. 310
3. 25.73
4. 12.05

Arrange the following compounds in increasing order of their solubilities in chloroform: NaCl, CH3OH, cyclohexane, CH3CN

1. NaCl < CH3CN < CH3OH < Cyclohexane
2. CH3OH < CH3CN < NaCl < Cyclohexane
3. NaCl < CH3OH < CH3CN < Cyclohexane
4. Cyclohexane < CH3CN < CH3OH < NaCl

Mass of glucose ( C6H12O6) required to be dissolved to prepare one litre of its solution which is isotonic with 15 g L-1 solution of urea (NH2CONH2) is (Given: Molar mass in g mol-1 C : 12, H : 1, O : 16, N : 14)

1. 55 g
2. 15 g
3. 30 g
4. 45 g

KH value for some gases at the same temperature 'T' are given : [figure] where KH is Henry's Law constant in water. The order of their solubility in water is :

1. HCHO < CH4 < CO2 < Ar
2. Ar < CO2 < CH4 < HCHO
3. Ar < CH4 < CO2 < HCHO
4. HCHO < CO2 < CH4 < Ar

The following solutions were prepared by dissolving 10 g of glucose ( C6H12O6) in 250 ml of water (P1), 10 g of urea (CH4N2O) in 250 ml of water (P2) and 10 g of sucrose ( C12H22O11) in 250 ml of water (P3). The right option for the decreasing order of osmotic pressure of these solutions is :

1. P3 > P1 > P2
2. P2 > P1 > P3
3. P1 > P2 > P3
4. P2 > P3 > P1

The correct option for the value of vapour pressure of a solution at 45 C with benzene to octane in molar ratio 3 : 2 is : [At 45 C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume ideal solution]

1. 350 mm of Hg
2. 160 mm of Hg
3. 168 mm of Hg
4. 336 mm of Hg