Target DPP Test

1.

One molal solution of a carboxylic acid in benzene shows the elevation of boiling point of 1.518 K. The degree of association for dimerisation of the acid in benzene is
(Kb for benzene = 2.53 K kgmol^-1)
(1) 60%
(2) 70%
(3) 75%
(4) 80 %

2.

Determining the normality of a solution with a density of 0.6 g/ml and composed of 35% NH₄OH by mass.

1. 4.8 N
2. 10 N
3. 0.5 N
4. 6 N

3.

Which of the following pairs exhibit positive deviation from Raoult's law?

(i) Chloroform and Acetone
(ii) Carbon disulphide and Acetone
(iii) Ethanol and Acetone
(iv) Phenol and Aniline
1. i and ii
2. ii and iii
3. i and iv
4. ii and iv

4.

What amount of CaCl₂(i=2.47) is dissolved in 2L water so that its osmotic pressure is 0.5 atm at 27 $° C$ ?
1. 13.42 g
2. 19.24 g
3. 8.834 g
4. 1.820 g

5.

The total vapor of a solution of liquid A and liquid B is 600 torr. The mole fraction of component A in the liquid phase is 0.7 and in the vapor phase is 0.35. The vapor pressure of pure A and B are respectively
(1) 300 torr, 130 torr
(2) 1300 torr, 130 torr
(3) 300 torr, 1300 torr
(4) 300 torr, 300 torr

6.

Which one of the following elctrolytes has the same value of van't Hoff's factor(i) as
that of Al₂(SO₄)₃(if all are 100% ionised)?
1. K₂SO₄
2. K₃[Fe(CN)₆]
3. Al(NO₃)₃
4. K₄[Fe(CN)₆]

7.

Isotonic solutions have the same
(1) vapor pressure
(2) freezing temperature
(3) osmotic pressure
(4) boiling temperature

8.

At a given temperature, osmotic pressure of a concentrated solution of a substance:

1.	Is higher than that of a dilute solution.
2.	Is lower than that of a dilute solution.
3.	Is same as that of a dilute solution.
4.	Cannot be compared with osmotic pressure of dilute solution.

9.

The value of Henry's constant, K_H is ......... .

1.	Greater for gases with higher solubility.
2.	Greater for gases with lower solubility.
3.	Constant for all gases.
4.	Not related to the solubility of gases.

10.

Consider the figure and mark the correct option.

1.	Water will move from the side (B) to side (A) if pressure is lower than the osmotic pressure is applied on piston (B).
2.	Water will move from side (B) to side (A) if a pressure greater than osmotic pressure is applied on piston (B).
3.	Water will move from side (B) to side (A) if a pressure equal to osmotic pressure is applied on piston (B).
4.	Water will move from side (A) to side (B) if pressure equal to osmotic pressure is applied on piston (A).

11.

The partial pressure of ethane over a solution containing 6.56 × 10^–2 g of ethane is 1 bar. If the solution contains 5.00 × 10^–2g of ethane, the partial pressure of the gas will be:
1. 0.66 bar
2. 0.96 bar
3. 0.76 bar
4. 0.19 bar

12.

The mass percentage of aspirin (C₉H₈O₄) in acetonitrile (CH₃CN) when 6.5 g of C₉H₈O₄ is dissolved in 450 g of CH₃CN will be:
1. 1.424%
2. 4.424%
3. 5.124%
4. 2.124%

13.

The vapour pressure of water in the solution having 50 g of urea dissolved in 850 g of water is:
(Vapor pressure of pure water at 298 K is 23.8 mm Hg)
1. 23.40 mm of Hg
2. 33.46 mm of Hg
3. 12.76 mm of Hg
4. 87.12 mm of Hg

14. The correct match for the below table is:

Type of solution	Example
a. Solid in gas	i. Aerated water
b. Gas in liquid	ii. Smoke
c. Liquid in solid	iii. Solution of hydrogen in palladium
d. Gas in solid	iv. Amalgams

	a	b	c	d
1.	i	iii	iv	ii
2.	ii	i	iv	iii
3.	iii	i	iv	ii
4.	iv	i	ii	iii

15.

The density of 68 % nitric acid by mass in an aqueous solution is 1.504 g mL^–¹. The molarity of the acid solution would be:
1. 15.24 M
2. 16.23 M
3. 14.52 M
4. 13.45 M

16.

Points A and B in the below-mentioned graph represent, respectively:

1.	Partial pressures of first and second components
2.	Vapour pressures of the pure second and first components
3.	Partial pressures of second and first components
4.	Vapour pressures of the pure first and second components

17.

The graph, amongst the following, that represents depression in the freezing point is:

1.
2.
3.
4.	None of the above

18. If the boiling point of water at 750 mm Hg is 99.63°C, what quantity of sucrose is needed to be dissolved in 500 g of water to achieve a boiling point of 100°C?
(Molal elevation constant for water is 0.52 K kg mol⁻¹ )
1. 128.17 g
2. 121.67 g
3. 125.57 g
4. 116.27 g

19. 3% (W/V) solution of glucose is isotonic with 1% (W/V) solution of a non-volatile and non-electrolyte substance. The molecular mass of the substance would be:
1. 180 g/mol
2. 360 g/mol
3. 420 g/mol
4. 60 g/mol

20. 2 grams of non-volatile solute dissolves in 200 grams each of two different solvents A and B to attain the same molality. If the ratio of $K_b $ of solvent A and B is 1:8 and the ratio of elevation in boiling points is x:y, then the value of y is:
1. 4
2. 6
3. 10
4. 8

21.

Assertion (A):	When an ideal binary solution is in equilibrium with its vapour, molar ratio of the two components in the solution and in the vapour phase may or may not be the same.
Reason (R):	Vapour pressure of solution depends upon the vapour pressures of volatile components.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

22. An aqueous solution contains 37.92% Na₂S₂O₃by weight. In this solution, the mole fraction of $Na_2S_2O_3 $ is:
(Total weight of solution = 1250 g)

1.	0.051	2.	0.510
3.	0.065	4.	0.65

23. On dissolving urea in 500 g of water and cooling up to 272.65 K, 128 g of ice separates out of the solution. The amount of dissolved urea is :
$(K_f = 1.86 \ K ~ \text {kg} / \text {mol}) $
1. 0.06 g
2. 0.6 g
3. 6.0 g
4. 60 g

24.

Assertion (A):	A mixture of chloroform and acetone forms a solution with a negative deviation from Raoult's Law.
Reason (R):	In such solutions, the intermolecular forces of attraction between the molecules of the solution (A-B attractions) are weaker than those of either of the pure components (A-A attractions or B-B attractions).

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

25. Which of the following aqueous solutions exhibits the highest boiling point?

1.	1.0 M NaOH	2.	1.0 M $Na_2SO_4~~~~~~$
3.	1.0 M $NH_4NO_3~~~~$	4.	1.0 M KNO₃

26. What amount of urea should be dissolved in 400 g of water to attain a solution with a
vapour pressure 2% lower than pure water?
1. 32.4 g
2. 27.2 g
3. 21.4 g
4. 24. 5 g

27. The correct increasing order of solubility of the following gases is:
($\mathrm{K_H}$ values for $\mathrm{Ar_(g), CO_{2(g)} , HCHO_{(g)}}$ and $\mathrm{CH_{4(g)}}$ are 40.39, 1.67, $1.83 \times 10^{-5}$ and 0.413 respectively.)
1. $\mathrm{HCHO < CH_4 < CO_2 < Ar}$
2. $\mathrm{HCHO < CO_2 < CH_4 < Ar}$
3. $\mathrm{Ar < CO_2 < CH_4 < HCHO}$
4. $\mathrm{Ar < CH_4 <CO_2< HCHO}$

28.

What will be the molarity of a solution prepared by mixing 750 mL of 0.5 M HCl with 250 mL of 2 M HCl?

1. 0.875 M
2. 1.00 M
3. 1.75 M
4. 0.975 M

29. The Henry's law constant K_H values of three gases (A, B, C) in water are 145, 2 × 10^–5, and 35 kbar, respectively. Determine the order of solubility of these gases in water from highest to lowest:

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

30. The plot of osmotic pressure $(\pi)$ vs concentration $(mol L^{-1})$ for a solution gives a straight line with slope 25.73 L bar mol^-1. The temperature at which osmotic pressure measurement is done is: $(\text {Use} \left.\mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$

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

Fill OMR Sheet*

*If above link doesn't work, please go to test link from where you got the pdf and fill OMR from there

CLICK HERE to get FREE ACCESS for 2 days of ANY NEETprep course

1.	1.0 M NaOH	2.	1.0 M \(Na_2SO_4~~~~~~\)
3.	1.0 M \(NH_4NO_3~~~~\)	4.	1.0 M KNO₃

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

Fill OMR Sheet*