Solutions

Mixture of chloroform and acetone forms a solution with negative deviation from Raoult's law due to :

1. Stronger intermolecular forces between chloroform molecules than those between chloroform and acetone molecules
2. Formation of hydrogen bonding between acetone and chloroform
3. Repulsive forces
4. Increase in escaping tendency of molecules of each component

Identify the correct statements : Choose the correct answer from the options given below :

1. A, B and C only
2. A, D and E only
3. A and B only
4. A and C only

Consider the following statements about the solutions formed by mixing two liquids.

1. A and C only
2. A and B only
3. B and C only
4. A only

In the light of the above statements, choose the most appropriate answer from the options given below.

1. A is not correct but R is correct
2. Both A and R are correct and R is the correct explanation of A
3. Both A and R are correct but R is NOT the correct explanation of A
4. A is correct but R is not correct

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

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

The freezing point depression constant (Kf) of benzene is 5.12 K kg mol-1. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is rounded off upto two decimal places :

1. 0.80 K
2. 0.40 K
3. 0.60 K
4. 0.20 K

The mixture which shows positive deviation from Raoult's law is :

1. Benzene + Toluene
2. Acetone + Chloroform
3. Chloroethane + Bromoethane
4. Ethanol + Acetone

For an ideal solution, the correct option is :

1. mix H = 0 at constant T and P
2. mix G = 0 at constant T and P
3. mix S = 0 at constant T and P
4. mix V 0 at constant T and P

The mixture that forms maximum boiling azeotrope is :

1. Ethanol + Water
2. Acetone + Carbon disulphide
3. Heptane + Octane
4. Water + Nitric acid

If molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be

1. halved
2. tripled
3. unchanged
4. doubled.

Which of the following is dependent on temperature?

1. Molarity
2. Mole fraction
3. Weight percentage
4. Molality

Which of the following statements about the composition of the vapour over an ideal 1 : 1 molar mixture of benzene and toluene is correct? Assume that the temperature is constant at 25 . (Given, vapour pressure data at 25 , benzene = 12.8 kPa, toluene = 3.85 kPa)

1. The vapour will contain equal amounts of benzene and toluene.
2. Not enough information is given to make a prediction.
3. The vapour will contain a higher percentage of benzene.
4. The vapour will contain a higher percentage of toluene

At 100 the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If Kb = 0.52, the boiling point of this solution will be

1. 102
2. 103
3. 101
4. 100

The van't Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is

1. 0
2. 1
3. 2
4. 3

Which one of the following is incorrect for ideal solution?

1. Hmix = 0
2. Umix = 0
3. P = Pobs - Pcalculated by Raoult's law = 0
4. Gmix = 0

What is the mole fraction of the solute in a 1.00 m aqueous solution?

1. 1.770
2. 0.0354
3. 0.0177
4. 0.177

The boiling point of 0.2 mol kg-1 solution of X in water is greater than equimolal solution of Y in water. Which one of the following statements is true in this case?

1. Molecular mass of X is less than the molecular mass of Y.
2. Y is undergoing dissociation in water while X undergoes no change.
3. X is undergoing dissociation in water.
4. Molecular mass of X is greater than the molecular mass of Y.

Which one of the following electrolytes has the same value of van't Hoff factor (i) as that of Al2(SO4)3 (if all are 100% ionised)?

1. Al(NO3)3
2. K4[Fe(CN)6]
3. K2SO4
4. K3[Fe(CN)6]

Which of them is not equal to zero for an ideal solution?

1. Vmix
2. P = Pobserved - PRaoult
3. Hmix
4. Smix

Of the following 0.10 m aqueous solutions, which one will exhibit the largest freezing point depression?

1. KCl
2. C6H12O6
3. Al2(SO4)3
4. K2SO4

Which condition is not satisfied by an ideal solution?

1. mixV = 0
2. mixS = 0
3. Obeyance to Raoult's Law
4. mixH = 0

Vapour pressure of chloroform (CHCl3) and dichloromethane (CH2Cl2) at 25 are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of CHCl3 and 40 g of CH2Cl2 at the same temperature will be (Molecular mass of CHCl3 = 119.5 u and molecular mass of CH2Cl2 = 85 u)

1. 173.9 mm Hg
2. 615.0 mm Hg
3. 90.6 mm Hg
4. 285.5 mm Hg