NEET Chemistry Solutions Online Test Set C

1. 1.00 g of a non-electrolyte solute (molar mass 250g 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

2. A solution containing 10g per dm³ of urea (molecular mass = 60 g mol^-1) is isotonic with a 5% solution of a nonvolatile solute. The molecular mass of this non-volatile solute is

3. 0.5 molal aqueous solution of a weak acid (HX) is 20% ionized. If Kf for water is 1.86 K kg mol sup-1, the lowering in freezing point of the solution is

4. A 0.0020 m aqueous solution of an ionic compound Co(NH₃)₅(NO₂)Cl freezes at -0.00732°C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (k1= -.86°C /m)

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

6. A solution of sucrose (molar mass = 342 g mol^-1) 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)

7. 200 mL of an aqueous solution of a protein contains its 1.26g. The osmotic pressure of this solution at 300 K is found to be 2.57 x 10^-3 bar. The molar mass of protein will be (R = 0.083 L bar mol^-1 K^-1)

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

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

10. 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

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

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

13. Which one of the following electrolytes has the same value of van't Hoff's factor (i) as that of Al₂(SO₄)₃ (if all are 100% ionised)?

14. 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?

15. What is the mole fraction of the solute in a 1.00 m aqueous solution?

16. Which one is not equal to zero for an ideal solution?

17. K₄[Fe(CN)₆] is supposed to be 40% dissociated when 1M solution prepared. Its boiling point is equal to another 20% mass by volume of non-electrolytic solution A. Considering molality = molarity. The molecular weight of A is

18. Substance A tetramerises in water to the extent of 80%. A solution of 2.5 g of A in 100 g of water lowers the freezing point by 0.3°C. The molar mass of A is

19. If any solute 'A' dimerises in water at 1 atm pressure and the boiling point of this solution is 100.52°C. If 2 moles of A is added to 1 kg of water and k_b for water is 0.52°C/molal, calculate the percentage association of A

20. What is the concentration of NO₃^- ions when equal volumes of 0.1 M AgNO₃ and 0.1 M NaCl are mixed together?

21. During evaporation of liquid

22. At higher altitude, the boiling point of water is lowered because

23. Vapour pressure diagram of some liquids plotted against temperature are shown below Most volatile liquid

24. Boiling point of 0.01 M AB₂ which is 10% dissociated in aqueous medium as A⁺² and B^-

25. Correct order of freezing point of given solution
I. 0.1 M glucose II. 0.2 M urea
III. 0.1 M NaCl IV. 0.5 M CaCl₂

26. van't Hoff factor for acetic acid in aqueous medium at infinite dilution is

27. Freezing point of solution is marked as

28. Which is having highest elevation in boiling point?

29. Which gas is most soluble in water?

30. Osmotic pressure of solution containing 0.6 g urea and 3.42 g sugar in 100 ml at 27°C