Which of the following changes would result in greater solubility of a gas in a liquid?

1.	Increasing temperature
2.	Increasing the amount of liquid
3.	Decreasing temperature
4.	Reducing gas pressure

Which of the following solution would exhibit abnormal colligative properties?

1. 1 M glucose

2. 0.1 M NaCl

3. 0.1 M sucrose 

4. 10 gram glass powder in water 

The number of moles of sodium hydroxide present in 2.5 L and 0.5 M aqueous solution will be

(1) 1.25

(2) 0.5

(3) 12.5

(4) 5

Maximum freezing point will be for 1 molal solution of assuming equal ionization in each case:

(1) [Fe(H${}_2$O)${}_6$]Cl${}_3$

(2) [Fe(H${}_2$O)${}_5$Cl] Cl${}_2$.H${}_2$O

(3) [Fe(H${}_2$O)${}_4$Cl${}_2$]Cl.2H${}_2$O

(4) [Fe(H${}_2$O)${}_3$Cl${}_3$].3H${}_2$O

The solution which has the lowest freezing point is 

(1) 0.1 M potassium nitrate

(2) 0.1 M aluminium sulphate

(3) 0.1 M potassium chloride

(4) 0.1 M potassium sulphate

The vant Hoff factor 'i' accounts for

1. the extent of dissociation of solute

2. the extent of dissolution of solute

3. the degree of decomposition of solution

4. degree of solubilization of solute

The azeotropic mixture of water and ethanol boils at 78.15 ^oC. When this mixture is distilled, it is possible to obtain-

1. Pure H₂O

2. Pure C₂H₅OH

3. Pure H₂O as well as pure C₂HOH

4. Neither H₂O nor C₂H₅OH in their pure state 

Which of the following changes with a change in temperature?

(1) Mole fraction

(2) Formality

(3) %(W/W)

(4) Molality

When the solute is present in trace quantities the following expression is used

1. Gram per million

2. Nanogram percent

3. Microgram percent

4. parts per million

Increasing the temperature of an aqueous solution will cause

(1) Decrease in molality

(2) Decrease in molarity

(3) Decrease in mole fraction

(4) Decrease in % (w/w)