Solution BFP

1. What is the concentration of a glucose solution in intravenous injection in gram/lit which is isotonic with blood solution which has osmotic pressure 15.93 bar at 300 K?
1. 162 g/L
2. 0.64 g/L
3. 115.3 g/L
4. 58 g/L

2. Which of the following is the correct statement?

1.	Relative lowering of vapor pressure is independent of temperature.
2.	Osmotic pressure always depends on the nature of the solute.
3.	Elevation of boiling point is independent of the nature of the solvent.
4.	Lowering of freezing point is proportional to the molar concentration of solute.

3.

A 0.03 M aqueous solution of a weak acid HX has an acid dissociation constant $K_a = 1.2 \times 10^{-5}$, for the dissociation$\mathrm{HX}_{(\mathrm{aq})} \rightleftharpoons \mathrm{H}_{(\mathrm{aq})}^{+}+\mathrm{X}_{(\mathrm{aq})}^{-} $. Calculate the osmotic pressure (in atm) of the solution at 300 K.

1.	4 atm	2.	2 atm
3.	1 atm	4.	6 atm

4. When mercuric iodide is added to the aqueous solution of potassium iodide then:

1.	The freezing point is raised.
2.	The freezing point is lowered.
3.	The freezing point does not change.
4.	The boiling point does not change.

5. Which one of the following are in equilibrium during the depression of the freezing point in a solution?
1. Liquid solvent, Solid solvent
2. Liquid solvent, Solid solute
3. Liquid solute, Solid solute
4. Liquid solute, Solid solvent

6. The elevation in boiling point of a solution of 13.44 g of CuCl₂ in 1 kg of water using the following information will be:
(Molecular weight of CuCl₂ = 134.4 and K_b = 0.52 K molal⁻¹)
1. 0.16
2. 0.05
3. 0.9
4. 0.4

7. An open beaker of water in equilibrium with water vapour is in a sealed container.
When a few grams of glucose are added to the beaker of water,
the rate at which water molecules :

1.	Leaves the vapour increases
2.	Leaves the solution increases
3.	Leaves the solution decreases
4.	Leaves the vapour decreases

8. Given below are two statements :

Statement I:	The proportionality constant, K_f, depends on the nature of the solvent as well as the solute.
Statement II:	When blood cells are placed in water containing less than 0.9 % (mass/volume) salt, blood cells shrink due to osmosis.

In light of the above statements choose the correct answer from the options given below:

1.	Statement I is correct; Statement II is incorrect
2.	Statement I is incorrect; Statement II is incorrect
3.	Statement I is incorrect; Statement II is correct
4.	Statement I is correct; Statement II is correct

9. Which of the following is/are not a colligative property?
(a) Optical activity
(b) Elevation in boiling point
(c) Osmotic pressure
(d) Lowering of vapour pressure
1. Only (a)
2. (a) and (d)
3. (a), (d) and (c)
4. (b) and (c)

10. Which of the following is the correct statement about Henry's law?

1.	The gas in contact with the liquid should behave as an ideal gas.
2.	There should not be any chemical interaction between the gas and the liquid.
3.	The pressure applied should be high.
4.	All of the above.

11. Azeotropic mixture of HCl and water has:
1. 20.2% HCl
2. 22.2% of HCl
3. 63% HCl
4. 84% HCl

12.

What is the molality of Na⁺ in a solution containing 3.00 g NaCl (M=58.4), 9.00 g glucose (M=180.0), and 168 g H₂O (M=18.0)?
1. 5.50 × 10^-3 m
2. 0.285 m
3. 0.306 m
4. 0.777 m

13.

Density of 3 M solution of NaCl is 1.25 g/mL. Calculate the volume of water required to make 1000 mL of this NaCl solution. [Consider the density of water as 1 g/mL].
1. 1074.5 mL
2. 824.5 mL
3. 1250 mL
4. 1000 mL

14. The vapour pressures of pure liquids A and B are 100 bar and 200 bar, respectively. If the vapour pressures of A and B in their binary solution are equal, then the total vapour pressure of the solution is:
1. 150 bar
2. 166.6 bar
3. 133.3 bar
4. 250 bar

15.

The difference between the boiling point and freezing point of an aqueous solution of 1% (w/w) NaOH solution will be:
(For $H_2O ~~K_f = 1.86~K~kg~mol^{-1},K_b = 0.52 ~K ~kg~mol^{-1} $)
1. 100.24
2. 101.20
3. 100.72
4. 100.96

16.

The osmotic pressure of the solution formed by mixing 25 ml of 0.1 M MgCl₂ and 25 ml of 0.1 M Urea at 300 K will be:
(R=0.0821 lit atm K^-1mol^-1)

1.	2.463 atm	2.	1.231 atm
3.	4.926 atm	4.	369 atm

17. Choose the correct statement from the following:

1.	Nitric acid (68%) and water (32%) mixture is an example of the minimum boiling azeotrope.
2.	Osmosis can be reversed if pressure lower than the osmotic pressure is applied to the solution.
3.	As compared to other colligative properties, the magnitude of osmotic pressure is large even for very dilute solutions.
4.	The condition of anoxia in mountain climbers is an application of Raoult's law.

18. Which substances exhibit the highest solubility in the specified liquid at 298 K and 1 atm pressure?

1.	Sodium chloride in liquid cyclohexane
2.	Bromine in liquid hexane
3.	Hydrogen in liquid water
4.	Potassium bromide in liquid tetrachloromethane

19. 40 cm³of a solution of sodium hydroxide is exactly neutralized by 25 cm³ of 0.40 mol L^–1 sulphuric acid.
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O
What is the concentration, in g L^–1, of the sodium hydroxide solution?
[Molecular mass value: NaOH = 40]
1. 20 gL^-1
2. 5 gL^-1
3. 0.25 gL^-1
4. 10 gL^-1

20.

Assertion (A):	The preservation of meat by salting and fruits by adding sugar is done to protect them from bacterial action.
Reason (R):	Due to reverse osmosis.

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.	(A) is false but (R) is true.

21. Consider the given two statements:

Assertion(A):	For 0.1 M aq. NaOH and for 0.1 M aq. CH₃COOH solution, the ebulioscopic constant is different.
Reason(R):	The ebulioscopic constant depends on the nature of the solute.

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

22.

Assertion (A):	0.1 M solution of glucose has the same decrement in the freezing point as 0.1 M solution of urea.
Reason (R):	K_f for both has the same value.

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.

23. Given below are two statements:

Assertion (A):	The solubility of all solutes in water generally increases with higher temperatures.
Reason (R):	The solubility of the solutes is dependent on temperature.

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.	(A) is False but (R) is True.

24. Which of the following aqueous solutions has the minimum freezing point?
1. 4% solution of $NaCl$
2. 10% solution of sugar
3. 6% solution of Urea
4. 2% solution of $MgCl_2$

25.

Which of the following solutions has the highest osmotic pressure?
1. 1% glucose solution
2. 1% urea solution
3. 1% sucrose solution
4. All of the above have the same osmotic pressure

26. Two compartments, A and B, are separated by a semipermeable membrane. Compartment A contains 0.01 M Na₂SO₄ solution, and compartment B contains 0.02 M BaCl₂ solution. In which compartment will the precipitate of BaSO₄ be formed?
1. Compartment A
2. Compartment B
3. No precipitate is formed in any compartment
4. Precipitate forms in both compartments A and B

27. 9.5 gram MgCl₂is dissolved in 500 g of water. The difference in boiling point and freezing point of the solution will be (K_bfor H₂O = 0.52 K/m, K_ffor H₂O = 1.86 K/m, Molar weight of MgCl₂ = 95) (assume that MgCl₂ is 100% dissociated)

1.	103.57 ^oC	2.	101.428 ^oC
3.	374.428 K	4.	372.196 K

28. The correct formula of Roult's law for non-volatile and electrolyte solute is:
(P = Vapour pressure of pure solvent
P_s = vapour pressure of solution
i = Van't Hoff Factor
n = Moles of solute
N = Moles of solvent)

1.	$P-P_s \over P $ = i ($n \over n+N$)	2.	$P-P_s \over P_s$ = i ($n \over n+N$)
3.	$P-P_s \over P $ = $i n \over in+N$	4.	$P-P_s \over P_s$ = $in \over in+N$

29. Which of the following solutions has the highest freezing point?
1. 0.02 M NaCl
2. 0.05 M Urea
3. 0.01 M MgCl₂
4. 0.01 M KCl

30.

The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K. If the total vapour pressure is 600 mm Hg then the composition of the vapour phase are:
1. X_A=0.30; X_B=0.70
2. X_A=0.40; X_B=0.60
3. X_A=0.20; X_B=0.90
4. X_A=0.50; X_B=0.50

31. Henry’s law constant for CO₂ in water is 1.67 × 10⁸ Pa at 298 K. The quantity of CO₂ in 500 mL of soda water when packed under 2.5 atm CO₂ pressure at 298 K is:

1.	1.24 g	2.	1.45 g
3.	1.65 g	4.	1.85 g

32.

Solution A contains 7 g/L of MgCl₂ and solution B contains 7 g/L of NaCl. At room temperature, the osmotic pressure of:
1. Solution A is greater than B
2. Both have the same osmotic pressure
3. Solution B is greater than A
4. Cannot be determined

33.

The boiling point of 1M Urea solution is 101^o C. The boiling point of 1M NaCl solution will be (Assume that NaCl is 100% dissociated):
1. 101^oC
2. 275 K
3. 375 K
4. 202^oC

34.

The boiling point of an aqueous solution is $102 ° C$ . The freezing point of this solution will be:
(Given: K_b = 0.52 k/m, K_f = 1.86 k/m)
1. $- 3.58 ° C$
2. $- 7.15 ° C$
3. $- 1.86 ° C$
4. $3.58 ° C$

35.

1 mole NaCl is mixed with 6 mole of H₂O. As a result, relative lowering in vapour pressure is observed to be 0.2. In these conditions, percentage ionisation of NaCl will be
1. 25
2. 50
3. 75
4. 100

36.

0.6 mL of acetic acid (CH₃COOH), having density 1.06 g mL^–1, is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205°C. The value of van’t Hoff factor and the dissociation constant of acid are respectively:
1. 1.041; 1.86 × 10^–5
2. 2.073; 1.86 × 10^–5
3. 0.091; 1.76 × 10^–5
4. 1.041; 1.76 × 10^–5

37.

The solubility of $H_2S$ in water at STP is 0.195 m. The value of Henry's constant is:

1.	274 atm	2.	285 atm
3.	295 atm	4.	278 atm

38.

Match the following type of intermolecular interactions present in the pair of compounds given:

(a)	Methanol and Acetone	(i)	Van der Waal’s forces of attraction
(b)	Acetonitrile and Acetone	(ii)	Ion-dipole interaction
		(iii)	Dipole-dipole interaction

	(a)	(b)
1.	(iii)	(ii)
2.	(ii)	(ii)
3.	(iii)	(iii)
4.	(iii)	(i)

39.

When 19.5 g of fluoroacetic acid (CH₂FCOOH) is dissolved in 500 g of water, the observed depression in the freezing point was found to be 1.00 K. The Van’t Hoff factor and the dissociation constant of the fluoroacetic acid, respectively are: (Given: $K_f$ for water = 1.86 K kg mol⁻¹, Molar mass of CH₂FCOOH = 78 g mol⁻¹)

1.	20.75 , 4.77 × 10^–3	2.	1.075 , 4.77 × 10^–2
3.	2.073 , 3.07 × 10^–4	4.	1.075 , 3.07 × 10^–3

40.

A solution containing 30 g of non-volatile solute in 90 g of water has a vapour pressure of 2.8 kPa at 298 K. Further, 18 g of water is then added to the solution and the new vapour pressure becomes 2.9 kPa at 298 K.
The molar mass of the solute will be :
1. 23 g mol⁻¹
2. 34 g mol⁻¹
3. 15 g mol⁻¹
4. 46 g mol⁻¹

41.

Camphor is often used in molecular mass determination because:
1. It has a very high cryoscopic constant
2. It is volatile
3. It is a solvent for organic substances
4. It is readily available

42.

The vapour pressure of a solvent decreased by 10 mm of Hg when a non-volatile solute was added to the solvent. The mole fraction of the solute in solution is 0.2. What would be the mole fraction of the solvent if the decrease in vapour pressure is 20 mm of Hg:
1. 0.2
2. 0.4
3. 0.6
4 0.8

43.

The addition of water vapour does not change the density of:
1. CCl₄
2. CS₂
3. Ether
4. Coke

44.

Select the correct option based on statements below:

Assertion (A):	When methyl alcohol is added to water, boiling point of water increases.
Reason (R):	When a volatile solute is added to a volatile solvent, elevation in boiling point is observed.

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.

45.

Which of the following binary mixtures will have the same composition in the liquid and the vapour phase?

(a)	Benzene-toluene	(b)	Water-nitric acid
(c)	Water-ethanol	(d)	n-Hexane-n-heptane

The correct option is:

1.	a and b	2.	b and c
3.	c and d	4.	a and d

46.

Three aqueous solutions of NaCl are labelled as ‘A', ‘B’ and ‘C with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of van’t Hoff factor for these solutions will be in the order of :
1. i_A < i_B < i_C
2. i_A > i_B > i_C
3. i_A = i_B = i_C
4. i_A < i_B > i_C

47.

The boiling point of water at 750 mm Hg is 99.63°C. How much sucrose is to be added to 400 g of water such that it boils at 100°C?
( K_b H₂O = 0.52 K kg mol⁻¹)
1. 97.33g
2. 121.67g
3. 145.14g
4. 124.79g

48.

Benzene and toluene form an ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at 300 K are 50.71 mm Hg and 32.06 mm Hg respectively.
The mole fraction of benzene in vapour phase, if 80 g of benzene is mixed with 100 g of toluene, would be:
1. 0.41
2. 0.68
3. 0.72
4. 0.59

49.

The mass of a non-volatile solute (molar mass 40 g mol^–1) that should be dissolved in 114 g octane to reduce its vapour pressure to 80 % would be:
1. 6 g
2. 7 g
3. 8 g
4. 10 g

50.

Which of the following represents a metastable system?
1. an unsaturated solution
2. a dilute solution
3. a saturated solution
4. a supersaturated solution

51.

A solution of acetone in ethanol :
1. Shows a negative deviation from Raoult's law.
2. Shows a positive deviation from Raoult's law.
3. Behaves like a near-ideal solution.
4. Obeys Raoult's law.

52.

During osmosis.flow of water through a semipermeable membrane is
(1) from both sides of semi-permeable membrane with unequal flow rates
(2) from solution having lower concentration only
(3) from solution having higher concentration only
(4) from both sides of semi-permeable membrane with equal flow rates

53.

Which of the following graph is correct for an ideal binary liquid solution containing non-volatile solute?

1.		2.
3.		4.	All are correct

54.

The latent heat of vaporization of water is 540 cal g^-1at 100 ^oC. K_b for water is:
1. $0 . 562 K m^{- 1}$
2. $1 . 86 K m^{- 1}$
3. $0 . 515 K m^{- 1}$
4. $5 . 12 K m^{- 1}$

55.

The partial pressure of ethane over a saturated solution containing 3.56 X 10^-2 g of ethane is 3 bar. If the solution contains 9.00 X 10^-2 g of ethane, then what will be the partial pressure of the gas?

1.	0.76 bar	2.	0.16 bar
3.	7.82 bar	4.	3.12 bar

56.

Sodium chloride (relative molecular mass=58.5) has a solubility of 36.0 g per 100 g of water. The density of the solution is 1.13 g/ml. Which of the following calculations would give the solubility in moles per litre?
1. 36.0 × 10/58.5
2. 36.0 × 1000/(58.5 × 1.13)
3. 36.0 × 10 × 1.13/58.5
4. 36.0 × 1000 × 1.13/(58.5 × 136)

57.

Mole of K₂SO4 to be dissolved in 12 moles water
to lower its vapour pressure by 10 mm of Hg at a
temperature at which vapour pressure of pure
water is 50 mm of Hg is
1. 3 mol
2. 0.5 mol
3. 1 mol
4. 2 mol

58.

A dilute sulphuric acid (H₂SO₄) solution has pH = 0.
Assuming complete dissociation, what is the molarity of the solution?
1. 1M
2. M/2
3. M/10
4. Cannot be determined

59.

A mixture of CO & CO2 has a density of 1.5 gL–1 at
20°C and 740 mm Hg. The mole fraction of CO in the
mixture is around
1. 0.65
2. 0.56
3. 0.43
4. 1

60.

A metal oxide contains 40% oxygen by weight. Its
equivalent weight is
1. 12
2. 20
3. 40
4. 60

61.

If the relative decrease in vapour pressure is 0.4 for a solution containing 1 mol NaCl in 3 mol of $H_{2} O$ , then percentage ionisation of NaCl will be -
1. 60%
2. 80%
3. 40%
4. 100%

62.

60 g m of Urea is dissolved in 1100 gm solution. To keep $∆ T_{f} / k_{f}$ as 1 mol/g, water separated in the form of ice is
1. 40 gm
2. 60 gm
3. 100 gm
4. 200 gm

63.

When mercuric iodide is added to the aqueous solution of potassium iodide is
(1) Freezing point is raised
(2) Freezing point is lowered
(3) Freezing point does not change
(4) Boiling point does not change

64.

Mole of $K_{2} S O_{4}$ to be dissolved in 12 moles water to lower its vapour pressure by 10 mm of Hg at a temperature at which vapour pressure of pure water is 50 mm of Hg is
(1) 3 mol
(2) 0.5 mol
(3) 1 mol
(4) 2 mol

65.

Equal volumes of 0.1 M $A g N O_{3}$ and 0.2 M NaCl are mixed. The concentration of $N O_{3}^{-}$ ions in the mixture will be:

1.	0.1 M	2.	0.05 M
3.	0.2 M	4.	0.15 M

66.

The Henry's law constant for the solubility of N₂ gas in water at 298 K is 1.0 × 10⁵ atm. The mole fraction of N₂ in air is 0.8. The number of moles of N₂ formed from air dissolved in 10 moles of water at 298 K and 5 atm pressure is-

1.	4.0 × 10^–4 mol	2.	4.0 × 10^–5 mol
3.	5.0 × 10^–4 mol	4.	4.0 × 10^–6 mol

67.

The solubility of a specific non-volatile salt is 4 g in 100 g of water at 25 $°$ C. If 2.0 g , 4.0 g and 6.0 g of the salt added of 100 g of water at 25 $°$ C, in system X,Y and Z. The vapour pressure would be in the oreder :
1. X < Y < Z
2. X > Y > Z
3. Z > X = Y
4. X > Y = Z

68.

Dimer of acetic acid in liquid benzene is in equilibrium with acetic acid monomer at certain temperature and pressure. If 25% of the dimer molecules are separated out then
1. Freezing point of the solution reduces
2. Average molar mass of solute increases
3. Boiling point of solution increases
4. Molar mass of solute decreases

69.

How much ethyl alcohol must be added to 1.0 L of water so that solution will not freeze at -4 $°$ F ? (K_f = 1.86 $°$ C/m)
1. < 20 g
2. < 10.75 g
3. < 494.5 g
4. > 494.5 g

70.

Water and chlorobenzene are immiscible liquids. Their mixture boils at 89^oC under a reduced pressure of $7.7 \times 10^{4} Pa$ . The vapour pressure of pure water at 89^oC is $7 \times 10^{4} Pa$ . Weight percent of chlorobenzene in the distillate is :
1. 50
2. 60
3. 78.3
4. 38.46

71.

If two liquids A $(P_{A}^{0} = 100 torr)$ and B $(P_{B}^{0} = 200 torr)$ are completely immiscible with each other ( each one will behave independtly of the other ) are present in a closed vessel. The total vapour pressure of the system will be :
1. less than 100 torr
2. greater than 200 torr
3. between 100 to 200 torr
4. 300 torr

72.

An aqueous solution of 2% non volatile solute
exerts a pressure of 1.004bar at the normal
boiling point of the solvent.What is the
molecular mass of the solute?
1. 4.135g / mol
2. 22.1g / mol
3. 90.1g / mol
4. 41.35g / mol

73.

During osmosis, the flow of water through a semi-permeable membrane is:

1.	From a solution having higher concentration only.
2.	From both sides of the semi-permeable membrane with equal flow rates.
3.	From both sides of the semi-permeable membrane with unequal flow rates.
4.	From a solution having lower concentration only.

74.

100 mL of liquid A was mixed with 25 mL of liquid B to give a non-ideal solution of A-B. The volume of this mixture will be:
1. 75 mL
2. Exact 125 mL
3. Between 75 mL and 125 mL
4. Close to 125 mL but will not exceed 125 mL

75. Consider the following liquid-vapor equilibrium
Liquid ↔ Vapour
Which of the following relation is correct?

1.	$\dfrac{dlnp}{dT}=\frac{-\Delta H_v}{RT}$	2.	$\dfrac{dlnp}{dT^2}=\frac{-\Delta H_v}{T^2}$
3.	$\dfrac{dlnp}{dT}=\frac{\Delta H_v}{RT^2}$	4.	$\dfrac{dlnG}{dT^2}=\frac{-\Delta H_v}{RT^2}$

76.

The density of dry air containing only $N_{2}$ and $O_{2}$ is 1.15 g/L at 740 mm and 300 K. What is % composition of $N_{2}$ by weight in the air:
1. 78%
2. 75.5%
3. 70.08%
4. 72.25%

77.

0.1 M KI and 0.2 M ${AgNO}_{3}$ are mixe in a 3:1 volume ratio. The depression of the freezing point of the resulting solution will be [ $k_{r} (H_{2} O)$ = 1.86 K kg ${mol}^{- 1}$ ]
1. 3.72 K
2. 1.86 K
3. 0.93 K
4. 0.279 K.

78.

A saturated solution of ${XCl}_{3}$ has a vapor pressure of 17.20 mm Hg at 20°C, while pure water vapor pressure is 17.25 mm Hg. Solubility product ( $K_{sp}$ ) of ${XCl}_{3}$ at 20°C
1. 9.8x $10^{- 2}$
2. $10^{- 5}$
3. 2.56x $10^{- 6}$
4. 7x $10^{- 5}$

79.

At 300 K, 40 mL of $O_{3}$ (g) dissolved in 100 g of water at 1.0 atm. What mass of ozone dissolved in 400 g of water at a pressure of 4.0 atm at 300 K?
1. 0.1 g
2. 1.2 g
3. 0.48 g
4. 4.8 g

80.

A sample of liquid $H_{2} O$ of mass 18.0 g is injected into an evacuated 7.6 L flask maintained at 27.0 $°$ C. If vapour pressure of $H_{2} O$ at 27 $°$ C is 24.63 mm Hg. What weight percentage of the water will be vapourised when the system comes to equilibrium? Assume water vapours behave as an ideal gas. The volume occupied by the liquid water is negligible compared to the volume of the container :
1. 1%
2. 10%
3. 18%
4. 20%

81.

Which has highest freezing point?
1. 0.01 M NaCl
2. 0.05 M Urea
3. 0.01 M MgCl₂
4. 0.02 M NaCl

82.

The boiling point of an aqueous solution of a non-volatile solute is 100.15 $°$ C. What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The value of Kb and Kf for water are 0.512 $°$ C and 1.86 $°$ CK molality $— 1$
:
(1) $— 0.544 ° C$
(2) $— 0.512 ° C$
(3) $— 0272 ° C$
(4) $— 1.86 ° C$

83.

At Abu mountains, water boils at 96 $° C$ . What amount of NaCl be added in 1 kg water so that it boils at 100 $° C$ . $K_{b} for H_{2} O = 0.52 K {molality}^{- 1}$ .
1. 225 g
2. 450 g
3. 200 g
4. 125 g

84.

Two solutions $A$ containing ${FeCl}_{3} (aq)$ and $B$ semipermeable membrane as shown below. If ${FeCl}_{3}$ on reaction with $K_{4} [Fe {(CN)}_{6}]$ $$ produces blue colour of ${Fe}_{4} [Fe {(CN)}_{6}]$ $,$ the blue colour will be noticed in:

(1) $(A)$
(2) $(B)$
(3) in both $(A)$ and $(B)$
(4) neither in $(A)$ nor in $(B)$

85.

Elevation in boiling point for 1 molal $C r C l_{3} . x N H_{3}$ is three times of one molal aqueous solution of urea. Calculate the value of x, assuming 100% ionization of complex salt. $K_{b} for H_{2} O = 0.51 K {mol}^{- 1}$ solvent.
1. 5
2. 4
3. 1
4. 6

86.

During osmosis, the flow of water through a semi-permeable membrane is :
1. From solution having higher concentration only
2. From both sides of the semi-permeable membrane with equal flow rates
3. From both sides of the semi-permeable membrane with unequal flow rates
4. From solution having lower concentration only

87.

When mercuric iodide is added to the aqueous solution of potassium iodide is
1. Freezing point is raised
2. Freezing point is lowered
3. Freezing point does not change
4. The boiling point does not change

88.

Which has the highest freezing point?
1. 0.01 M NaCl
2. 0.05M Urea
3. 0.01 M MgCl₂
4. 0.02 M NaCl

89.

What is the required amount of K₂SO₄ in moles to dissolve in 12 moles of water to decrease
the vapour pressure by 10 mmHg, if the vapour pressure of pure water is 50 mmHg?

1. 3 mol
2. 0.5 mol
3. 1 mol
4. 2 mol

90.

If partial pressure of oxygen is 0.5 atm and K_H= 1.4 × 10^-3 M/atm, then the amount of oxygen dissolved in 100 ml water at 298K is-

1.	22.4 mg	2.	22.4 g
3.	2.24 g	4.	2.24 mg

91.

Which solution has highest freezing point?
1. 1% glucose solution
2. 1% urea solution
3. 1% sucrose solution
4. All have same freezing

92.

The salt that possesses the highest freezing point
1. 0.01 M NaCl
2. 0.05 M Urea
3. 0.01 M MgCl₂
4. 0.02 M NaCl

93.

The mole(s) of K₂SO₄ to be dissolved in 12 moles of water to lower its vapor pressure by 10 mm of Hg at a temperature at which vapor pressure of pure water is 50 mm of Hg is :

1.	3 mol	2.	0.5 mol
3.	1 mol	4.	2 mol

94.

A solution is prepared by dissolving 18 g of glucose in 1000 g of water. When this solution is cooled to –0.2 °C,
some ice separates. Calculate the amount of ice that separates from the solution.
[Freezing point depression constant of water, K_f(H₂O) = 1.86 K molal^-1]

1.	70 g	2.	140 g
3.	90 g	4.	210 g

95.

Given that the pH of a 0.1 M monobasic acid is 2, what is the osmotic pressure at a given temperature T?
1. 0.1RT
2. 0.11RT
3. 1.1RT
4. 0.01RT

96.

The latent heat of vapourisation of water is 540 cal g^-1 at 100 $° C$ . K_b for water is
1. 0.56 K.mole^-1
2. 1.86 K.mole^-1
3. 0.51 K.mole^-1
4. 5.12 K.mole^-1

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.	\(P-P_s \over P \) = i (\(n \over n+N\))	2.	\(P-P_s \over P_s\) = i (\(n \over n+N\))
3.	\(P-P_s \over P \) = \(i n \over in+N\)	4.	\(P-P_s \over P_s\) = \(in \over in+N\)

1.	\(\dfrac{dlnp}{dT}=\frac{-\Delta H_v}{RT}\)	2.	\(\dfrac{dlnp}{dT^2}=\frac{-\Delta H_v}{T^2}\)
3.	\(\dfrac{dlnp}{dT}=\frac{\Delta H_v}{RT^2}\)	4.	\(\dfrac{dlnG}{dT^2}=\frac{-\Delta H_v}{RT^2}\)

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

Fill OMR Sheet*