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MCQ (More than One Correct Answer)

Which of the following aqueous solution will exhibit highest boiling point?

MCQ (Single Correct Answer)

Match List-I with List-II

	List - I (Exsample)		List - II (Type of Solution)
A	Humidity	I	Solid in solid
B	Alloys	II	Liquid in gas
C	Amalgams	III	Solid in gas
D	Smoke	IV	Liquid in solid

Choose the correct answer from the options given below:

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?

Mass of glucose $$(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6)$$ required to be dissolved to prepare one litre of its solution which is isotonic with $$15 \mathrm{~g} \mathrm{~L}^{-1}$$ solution of urea $$(\mathrm{NH}_3 \mathrm{CONH}_2)$$ is (Given: Molar mass in $$\mathrm{g} \mathrm{mol}^{-1} \mathrm{C}: 12, \mathrm{H}: 1, \mathrm{O}: 16, \mathrm{~N}: 14$$)

NEET 2024 (Re-Examination)

The Henry's law constant $$(\mathrm{K}_{\mathrm{H}})$$ values of three gases $$(\mathrm{A}, \mathrm{B}, \mathrm{C})$$ in water are $$145, 2 \times 10^{-5}$$ and $$35 \mathrm{~kbar}$$ respectively. The solubility of these gases in water follow the order:

The plot of osmotic pressure (П) vs concentration $$(\mathrm{mol} \mathrm{~L}^{-1})$$ for a solution gives a straight line with slope $$25.73 \mathrm{~L} \mathrm{~bar} \mathrm{~mol}^{-1}$$. The temperature at which the osmotic pressure measurement is done is

(Use $$\mathrm{R}=0.083 \mathrm{~L} \mathrm{~bar} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$$)

Which amongst the following aqueous solution of electrolytes will have minimum elevation in boiling point? Choose the correct option :-

NEET 2023 Manipur

K_H value for some gases at the same temperature 'T' are given :

Gas	K$$_H$$/k bar
Ar	40.3
CO$$_2$$	1.67
HCHO	1.83 $$\times$$ 10$$^{ - 5}$$
CH$$_4$$	0.413

where K_H is Henry's Law constant in water. The order of their solubility in water is :

NEET 2022 Phase 2

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 :

The correct option for the value of vapour pressure of a solution at 45$$^\circ$$C with benzene to octane in molar ratio 3 : 2 is :

[At 45$$^\circ$$C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume Ideal gas]

The freezing point depression constant (K_r) 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 :

NEET 2020 Phase 1

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

NEET 2020 Phase 1

For an ideal solution, the correct option is :

The mixture that forms maximum boiling azeotrope is :

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

Which one of the following is incorrect for ideal solution?

NEET 2016 Phase 2

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

NEET 2016 Phase 2

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

NEET 2016 Phase 1

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^oC. (Given, vapour pressure data at 25^oC, benzene = 12.8 kPa, toluene = 3.85 kPa)

NEET 2016 Phase 1

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)?

AIPMT 2015 Cancelled Paper

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

AIPMT 2015 Cancelled Paper

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?

AIPMT 2015 Cancelled Paper

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

Which condition is not satisfied by an ideal solution?

NEET 2013 (Karnataka)

Vapour pressure of chloroform (CHCl₃) and dichloromethane (CH₂Cl₂) at 25^oC 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)

AIPMT 2012 Mains

p_A and p_B are the vapour pressure of pure liquid components, A and B, respectively of an ideal binary solution. If x_A represents the mole fraction of component A, the total pressure of the solution will be

AIPMT 2012 Prelims

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_f for water is 1.86^oC/m, the freezing point of the solution will be

AIPMT 2011 Mains

200 mL of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at 300 K is found to be 2.57 $$ \times $$ 10^$$-$$3 bar. The molar mass of protein will be (R = 0.083 L bar mol^$$-$$1 K^$$-$$1)

AIPMT 2011 Mains

The freezing point depression constant for water is $$-$$1.86^o C m^$$-$$1. If 5.00 g Na₂SO₄ is dissolved in 45.0 g H₂O, the freezing point is changed by $$-$$3.82^oC. Calculate the van't Hoff factor for Na₂SO₄.

AIPMT 2011 Prelims

The van't Hoff factor $$i$$ for a compound which undergoes dissociation in one solvent and association in other solvent is respectively

AIPMT 2011 Prelims

A solution of sucrose (molar mass = 342 g mol^$$-$$) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be (K_f for water = 1.86 K kg mol^$$-$$1)

AIPMT 2010 Prelims

An aqueous solution is 1.00 molal in KI. Which change will cause the vapour pressure of the solution to increase?

AIPMT 2010 Prelims

A 0.0020 m aqueous solution of an ionic compound [Co(NH₃)₅(NO₂)]Cl freezes at $$-$$ 0.00732^oC. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (K_f = $$-$$1.86^oC/m)

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_f for water is 1.86 K kg mol^$$-$$1, the lowering in freezing point of the solution is

A solution containing 10 g per dm³ of urea (molecular mass = 60 g mol^$$-$$1) is isotonic with a 5% solution of a nonvolatile solute is

During osmosis, flow of water through a semipermeable membrane is

A solution of acetone in ethanol

1.00 g of a non-electrolyte solute (molar mass 250 g mol^$$-$$1) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K_f of benzene is 5.12 K kg mol^$$-$$1, the freezing point of benzene will be lowered by

A solution of urea (mol. mass 56 g mol^$$-$$1) boils at 100.18^oC at the atmospheric pressure. If K_f and K_b for water are 1.86 and 0.512 K kg mol^$$-$$1 respectively, the above solution will freeze at

A solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressures of the pure hydrocarbons at 20^oC are 440 mm Hg for pentane and 120 mm Hg for hexane. The mole fraction of pentane in the vapour phase would be

The vapour pressure of two liquids P and Q are 80 and 60 torr, respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mole of Q would be

A solution contains non volatile solute of molecular mass M₂. Which of the following can be used to calculate the molecular mass of solute in terms of osmotic pressure?

A solution containing components A and B folloes Raoult's law

Pure water can be obtained from sea water by

From the colligative properties of solution, which one is the best method for the determination of molecular weight of proteins and polymers?