Chemistry_Class-12_Ch-1_Solution_Topic-7_Colligative Properties of Electrolyte 1 / 30 1. Consider separate solution of 0.500 M C₂H5OH(aq), 0.100 M Mg3(PO4)2(aq), 0.250 M KBr(aq) and 0.125 M Na3PO4(aq) at 25°C. Which statement is true about these solution, assuming all salts to be strong electrolytes A) They all have the same osmotic pressure B) 0.100 Mg3(PO4)2(aq) has the highest osmotic pressure C) 0.125 M Na₃PO₄(aq) has the highest osmotic pressure D) 0.500 M C2H5OH(aq) has the highest osmotic pressure 2 / 30 2. The highest osmotic pressure corresponds to the following solution A) M/10 urea B) M/10 glucose C) M/10 HCI D) M/10 BaCl2 3 / 30 3. In equimolar solution of glucose, NaCl and BaCl2, the order of osmotic pressure is as follow A) Glucose > NaCl > BaCl2 B) NaCl > BaCl2 > Glucose C) BaCl2 > NaCl > Glucose D) Glucose > BaCl2 > NaCl 4 / 30 4. The osmotic pressure of which solution is maximum (consider that deci-molar solution of each 90% dissociated) A) Aluminium sulphate B) Barium chloride C) Sodium sulphate D) A mixture of equal volumes of (b) and (c) 5 / 30 5. At 25°C, the highest osmotic pressure is exhibited by 0.1M solution of A) CaCl2 B) KCI C) Glucose D) Urea 6 / 30 6. Which of the following will have the highest boiling point at 1 atm pressure A) 0.1 M NaCl B) 0.1M sucrose C) 0.1M BaCl2 D) 0.1M glucose 7 / 30 7. Which one of the following aqueous solutions will exhibit highest boiling point A) 0.015 M urea B) 0.01 Μ ΚΝΟ3 C) 0.01 M Na2SO4 D) 0.015 M glucose 8 / 30 8. 0.01 molar solutions of glucose, phenol and potassium chloride were prepared in water. The boiling points of A) Glucose solution = Phenol solution = Potassium chloride solution B) Potassium chloride solution > Glucose solution > Phenol solution C) Phenol solution > Potassium chloride solution > Glucose solution D) Potassium chloride solution > Phenol solution > Glucose solution 9 / 30 9. Which one has the highest boiling point A) 0.1N Na₂SO₄ B) 0.1N MgSO₄ C) 0.1M Al₂(SO₄)₃ D) 0.1M BaSO₄ 10 / 30 10) 0.01M solution each of urea, common salt and Na2SO4 are taken, the ratio of depression of freezing point is A) 1:1:1 B) 1:2:1 C) 2:2:3 D) 1:2:3 11 / 30 11. Which has the minimum freezing point A) One molal NaCl solution B) One molal KCI solution C) One molal CaCl₂ solution D) One molal urea solution 12 / 30 12) The freezing points of equimolar solutions of glucose, KNO3 and AICI3 are in the order of A) AlCl₃ < KNO₃ < Glucose B) Glucose < KNO₃ < AlCl₃ C) Glucose < AlCl₃ < KNO₃ D) AlCl₃ < Glucose < KNO₃ 13 / 30 13. Which of the following will have the highest F.P. at one atmosphere A) 0.1M NaCl solution B) 0.1 M sugar solution C) 0.1 M BaCl2 solution D) 0.1 M FeCl3 solution 14 / 30 14. Which of the following 0.10m aqueous solution will have the lowest freezing point A) Al₂(SO₄)₃ B) C₅H₁₀O₅ C) KI D) C₁₂H₂₂O₁₁ 15 / 30 15) The correct order of increasing boiling points of the following aqueous solutions 0.0001 M NaCl (I), 0.0001 M Urea (II), 0.001 M MgCl2 (III), 0.01 M NaCl (IV) is A) I < II < III < IV B) IV < III < II < I C) II < I < III < IV D) III < II < IV < I 16 / 30 16) Identify the compound amongst the following of which 0.1 M aqueous solution has highest boiling point A) Glucose B) Sodium chloride C) Calcium chloride D) ) Ferric chloride 17 / 30 17) When 20 g of naphthoic acid (C11H8O2) is dissolved in 50 g of benzene (Kf = 1.72Kkgmol), a freezing point depression of 2K is observed. The van't Hoff factor (i) is A) 0.5 B) 1 C) 2 D) 3 18 / 30 18. Which of the following salt has the same value of Van't Hoff factor i as that of K4[Fe(CN)6] A) Al₂(SO₄)₃ B) NaCl C) Na₂SO₄ D) Al(NO₃)₃ 19 / 30 19. Observe the following abbreviations πobs = observed colligative property πcal = theoretical colligative property assuming normal behaviour of solute. Van't Haff factor (i) is given by A) i = πobs × πcal B) i = πobs + πcal C) i = πobs - πcal D) i = πobs / πcal 20 / 30 20. The Van't Hoff factor i for a 0.2 molal aqueous solution of urea is A) 0.2 B) 0.1 C) 1.2 D) 1.0 21 / 30 21. If the various terms in the given below expressions have usual meaning, the van’t Hoff factor (i) cannot be calculated by which one of the expressions. A) πV = √inRT B) ∆Tf = i.kf.m C) ∆Tb = i.kb.m D) 22 / 30 22) The freezing point depression constant for water is -1.86° Cm-1. If 5.00g 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 A) 0.381 B) 2.05 C) 2.63 D) 3.11 23 / 30 23. The van't Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is A) 3 B) 0 C) 1 D) 2 24 / 30 24) A 1.2 g/L of solution of NaCl is isotonic with 7.2 g/L of solution of glucose. Calculate the van't Hoff's factor of NaCl solution A) 2.36 B) 1.50 C) 1.95 D) 1.00 25 / 30 25. The freezing point of equimolal aqueous solution will be highest for A) C₆H₅NH₃⁺Cl⁻ (aniline hydrochloride) B) Ca(NO₃)₂ C) La(NO₃)₃ D) C₆H₁₂O₆ (glucose) 26 / 30 26. In comparison to a 0.01 m solution of glucose, the depression in freezing point of a 0.01 m MgCl2 solution A) The same B) About twice C) About three times D) About six times 27 / 30 27. The values of van't Hoff factors for KCl, NaCl and K₂SO₄ respectively are........ A) 2, 2 and 2 B) 2, 2 and 3 C) 1. 1 and 2 D) 1, 1 and 1 28 / 30 28. Which of the following has the lowest freezing point A) 0.1 m sucrose B) 0.1 m urea C) 0.1 m ethanol D) 0.1 m glucose 29 / 30 29) An aqueous solution is 1.00 molal Kl. Which change will cause the vapour pressure of the solution to increase A) Addition of water B) Addition of NaCl C) Addition of Na2SO4 D) Addition of 1.00 molal KI 30 / 30 30) The degree of dissociation (α) of a weak electrolyte, Ax By is related to van't Hoff factor (i) by the expression(AIEEE -2011) A) B) C) D) Your score isThe average score is 0% 0% Exit
