Solutions Chemistry Online Mock Test: NEET PYQ

1. The plot of osmotic pressure (π) vs concentration (mol L⁻¹) for a solution gives a straight line with slope 25.73 L bar mol⁻¹. The temperature at which the osmotic pressure measurement is done is (Use R = 0.083 L bar mol⁻¹ K⁻¹) [NEET 2024]

2. The density of the solution is 2.15 g mL⁻¹, then mass of 2.5 mL solution in correct significant figures is: [NEET Re-2022]

3. Which amongst the following aqueous solution of electrolytes will have minimum elevation in boiling point? Choose the correct option :- [NEET 2023 mpr]

4. 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: [NEET 2021]

5. The Henry's law constant (Kₕ) values of three gases (A, B, C) in water are 145, 2 × 10⁻⁵ and 35 kbar, respectively. The solubility of these gases in water follow the order(decreasing order): [NEET 2024]

6. Gas: K_H / K.bar

Ar → 40.3, CO₂ → 1.67, HCHO → 1.83×10^−5, CH₄ → 0.413

Where K_H is Henry's Law constant in water. The order of their solubility in water is: [NEET Re-2022]

A. HCHO < CH₄ < CO₂ < Ar
B. Ar < CO₂ < CH₄ < HCHO
C. CO₂ < Ar < CH₄ < HCHO
D. HCHO < CO₂ < CH₄ < Ar

7. During the preparation of Mohr's salt solution (Ferrous ammonium sulphate), which of the following acid is added to prevent hydrolysis of Fe²⁺ ion? [NEET 2024]

8.

Arrange the following compounds in increasing order of their solubilities in chloroform: [NEET 2024 Rel] NaCl, CH₃OH, cyclohexane, CH₃CN

A. NaCl < CH₃CN < CH₃OH < Cyclohexane
B. CH₃OH < CH₃CN < NaCl < Cyclohexane
C. NaCl < CH₃OH < CH₃CN < Cyclohexane
D. Cyclohexane < CH₃CN < CH₃OH < NaCl

9.

In one molal solution that contains 0.5 mole of a solute, there is [NEET-2022]

10. Mass of glucose (C₆H₁₂O₆) required to be dissolved to prepare one litre of its solution which is isotonic with 15 g L⁻¹ solution of urea (NH₂CONH₂) is (Given: Molar mass in g mol⁻¹ C:12, H:1, O:16, N:14) [NEET 2024 Rel]

1.

The mixture which shows positive deviation from Raoult's law is (2020)

2. The mixture that forms maximum boiling azeotrope is (NEET 2019)

3.

Which of the following is dependent on temperature? (NEET 2017)

4. 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: [NEET 2021]

5. Which of the following statements is correct regarding a solution of two components A and B exhibiting positive deviation from ideal behaviour? (Odisha NEET 2019)

6. The freezing point depression constant (Kf) 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 up to two decimal places): (2020)

7. In water saturated air, the mole fraction of water vapour is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is (Odisha NEET 2019)

8.

For an ideal solution, the correct option is (NEET 2019)

9. The correct option for the value of vapour pressure of a solution at 45°C with benzene to octane in molar ratio 3 : 2 is: [At 45°C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume ideal solution] [NEET 2021]

10. If molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be (NEET 2017)

1.

Which of them is not equal to zero for an ideal solution? (2015 Cancelled)

2. The boiling point of 0.2 mol kg⁻¹ solution of X in water is greater than equimolar solution of Y in water. Which one of the following statements is true in this case? (2015)

3.

Which one of the following is incorrect for ideal solution? (NEET-II 2016)

4. 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°C. (Given, vapour pressure data at 25°C, benzene = 12.8 kPa, toluene = 3.85 kPa) (NEET-I 2016)

5. 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)? (2015 Cancelled)

6. What is the mole fraction of the solute in a 1.00 m aqueous solution? (2015)

7.

The van't Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is (NEET-II 2016)

8. How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M HNO₃? The concentrated acid is 70% HNO₃ (2013 NEET)

9. Of the following 0.10 m aqueous solutions, which one will exhibit the largest freezing point depression? (2014)

10. At 100°C the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If Kb = 0.52, the boiling point of this solution will be (NEET-I 2016)

1. The van’t Hoff factor i for a compound which undergoes dissociation in one solvent and association in other solvent is respectively (2011)

2. A 0.1 molal aqueous solution of a weak acid is 30% ionized. If KfK_fKf​ for water is 1.86 °C m⁻¹, the freezing point of the solution will be (2011)

3. 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 (2012)

4. 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 × 10^⁻3 bar. The molar mass of protein will be (R = 0.083 L bar mol⁻¹ K⁻¹) [2011]

5. Vapour pressure of chloroform (CHCl₃) and dichloromethane (CH₂Cl₂) at 25°C 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 same temperature will be (Molecular mass of CHCl₃ = 119.5 u and CH₂Cl₂ = 85 u) (2012 Mains)

6.

Mole fraction of the solute in a 1.00 molal aqueous solution is (2011)