Please be patient as the PDF generation may take up to a minute.

1.

An example of a gas in a solid-type solution is:
1. Solution of hydrogen in palladium
2. Ethanol dissolved in water
3. Camphor vapours in N₂ gas
4. Amalgams

2. The Henry Law constants of four gases P, Q, R, and S in water are 38.5, 10.42, 1.26, and 2.11 bar at 298 K and 1 atm. Identify the gas that will dissolve maximally in water.

1.	P	2.	Q
3.	R	4.	S

3. The property(ies) that is/are shown by an ideal solution:
1. \(\Delta \mathrm{H}_{\operatorname{mix}}=0\)
2. It follows Raoult's law.
3. \(\Delta \mathrm{V}_{\operatorname{mix}}=0\)
4. All of the above

4.

A set of solutions is prepared using 180 g of water as a solvent and 10 g of different non-volatile solutes A, B and C. The relative lowering of vapour pressure in the presence of these solutes are in the order:
[Given, molar mass of A = 100 g ${\mathrm{mol}}^{-1}$; B = 200 g ${\mathrm{mol}}^{-1}$; C = 10,000 g ${\mathrm{mol}}^{-1}$]

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

5. The elevation in boiling point for 1 molal solution of a non-volatile solute A is 3 K. The depression in the freezing point for 2 molal solutions of A in the same solvent is 6 K. The ratio of \(K_b \text { and } K_f \text { i.e., } K_b / K_f~\text{is}~1:X.\) 
The value of \(X\) is:

1.	7	2.	3
3.	1	4.	2

6. When 5 g of non-volatile non-electrolyte solute is dissolved in 100 g of a certain solvent, the freezing point of the solvent decreases by 0.25 K. The molar mass of the solute is:
\([\text{K}_f \) of the given solvent \( =1.2 \mathrm{K ~kg}~ \mathrm{mol}^{-1}] \)

1.	\(242.8 \mathrm{~g} \mathrm{~mol}^{-1}\)	2.	\(238.2 \mathrm{~g} \mathrm{~mol}^{-1}\)
3.	\(241.8 \mathrm{~g} \mathrm{~mol}^{-1}\)	4.	\(240.0 \mathrm{~g} \mathrm{~mol}^{-1}\)

7. What is the correct sequence of osmotic pressure for 0.01 M aqueous solutions of the following compounds? (\(\pi_a​, \pi_b,\) \(\pi_c,\) and \(\pi_d\) represent the osmotic pressures of the respective solutions)

a.	\(\mathrm{Al}_2\left(\mathrm{SO}_4\right)_3\)	b.	\(\mathrm{Na}_3 \mathrm{PO}_4\)
c.	\(\mathrm{BaCl}_2\)	d.	Glucose

1. \(\pi_d>\pi_b>\pi_c>\pi_a\)
2. \(\pi_c>\pi_d>\pi_b>\pi_a\)
3. \(\pi_c>\pi_d>\pi_a>\pi_b\)
4. \(\pi_a>\pi_b>\pi_c>\pi_d\)

8.

The boiling point of an azeotropic mixture of water and ethanol is less than that of water and ethanol individually. The mixture shows:
1. No deviation from Raoult's law
2. Positive deviation from Raoult's law
3. Negative deviation from Raoult's law
4. That the solution is unsaturated

9. The Van't Hoff factor (i) for a dilute solution of \(Al_2(SO_4)_3 \) is:
1.  \(1+\alpha/4 \)
2.  \(1+\alpha \)
3.  \(1-3\alpha \)
4.  \(1+4\alpha \)

10.

Match the terms given in Column I with expressions given in Column II.

Column I (Term)	Column II (Expression)
A. Mass percentage	1. \(\text{Number of moles of the solute component} \over \text{Volume of solution in litres}\)
B. Volume percentage	2. \(\text{Number of moles of the solute component} \over \text{Mass of solvent in kilograms}\)
C. Molarity	3. \(\small{\text{Volume of the solute component in solution} \over \text{Total volume of solution}} \times 100\)
D. Molality	4. \(\small{\text{Mass of the solute component in solution} \over \text{Total Mass of solution}} \times 100\)

Codes:

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