Chemistry Exercise -1

Solution Solubility 1. 2. Method of expressing concentration of solution 6. 5 ml of N HCl, 20 ml of N/2 H 2 SO4 and 30 ml (C) Viscosity is higher than H 2O at 25o 7. of N/3 HNO3 are mixed together and volume made to one litre. The normally of the resulting solution is N N (A) (B) 5 10 N N (C) (D) 20 40 The amount of K 2Cr2O7 (eq. wt. 49.04) (D) Solubility of NaCl in it is more than H 2O required to prepare 100 ml of its 0.05 N solution is (A) 2.9424 g (B) 0.4904 g (C) 1.4712 g (D) 0.2452 g 8. With increase of temperature, which of these changes (A) Molality (B) Weight fraction of solute (C) Fraction of solute present in water (D) Mole fraction 9. 25ml of a solution of barium hydroxide on titration with a 0.1molar solution of hydrochloric acid gave a litre value of 35 ml. The molarity of barium hydroxide solution was (A) 0.07 (B) 0.14 (C) 0.28 (D) 0.35 10. 2.0 molar solution is obtained , when 0.5 mole solute is dissolved in (A) 250 ml solvent (B) 250 g solvent (C) 250 ml solution (D) 1000 ml solvent 11. How many gram of HCl will be present in 150 ml of its 0.52 M solution (A) 2.84 gm (B) 5.70 gm (C) 8.50 gm (D) 3.65 gm 12. The number of moles present in 2 litre of 0.5 M NaOH is (A) 0.5 (B) 0.1 (C) 1 (D) 2 The solubility of a gas in water depends on (A) Nature of the gas (B) Temperature (C) Pressure of the gas (D) All of the above Which of the following is not correct for D2O (A) Boiling point is higher than H 2O (B) D2O reacts slowly than H 2O 3. The statement “ The mass of a gas dissolved in a given mass of a solvent at any temperature is proportional to the pressure of the gas above the solvent” is (A) Dalton’s Law of Partial Pressures (B) Law of Mass Action (C) Henry’s Law (D) None of these 4. Which is correct about Henry’s law (A) The gas in contact with the liquid should behave as an ideal gas (B) There should not be any chemical interaction between the gas and liquid (C) The pressure applied should be high (D) All of these 5. The statement “If 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atmosphere, 0.006 moles will be dissolved under a pressure of 2 atmospheres”, illustrates (A) Dalton’s law of partial pressure (B) Graham’s law (C) Raoult’s law (D) Henry’s law 13. 36g water and 828g ethyl alcohol form an ideal solution. The mole fraction of water in it, is (A) 1.0 (B) 0.7 (C) 0.4 (D) 0.1 14. What will be the normality of a solution containing 4.9 g. H 3 PO4 dissolved in 500 ml 15. 16. 17. 18. 19. water (A) 0.3 (B) 1.0 (C) 3.0 (D) 0.1 3.0 molal NaOH solution has a density of 1.110 g/ml. The molarity of the solution is (A) 3.0504 (B) 3.64 (C) 3.05 (D) 2.9732 The number of moles of solute per kg of a solvent is called its (A) Molarity (B) Normality (C) Molar fraction (D) Molality 1.0 gm of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of the HCl solution is given by (A) 4 N (B) 2 N (C) 0.4 N (D) 0.2 N Molecular weight of glucose is 180. A solution of glucose which contains 18 gms per litre is (A) 2 molal (B) 1 molal (C) 0.1 molal (D) 18 molal 0.5 M of H 2 SO4 is diluted from 1 litre to 10 litre, normality of resulting solution is (A) 1 N (B) 0.1 N (C) 10 N (D) 11 N 20. If one mole of a substance is present in 1kg of solvent, then (A) It shows molar concentration (B) It shows molal concentration (C) It shows normality (D) It shows strength gm / gm 21. The molality of 90% H 2 SO4 solution is [density=1.8 gm/ml] (A) 1.8 (C) 9.18 (B) 48.4 (D) 94.6 Solution 22. The volume of water to be added to 100cm3 of 0.5 N H 2 SO4 to get decinormal concentration is (A) 400 cm3 (B) 500 cm3 (C) 450 cm3 (D) 100 cm3 23. If 25 ml of 0.25 M NaCl solution is diluted with water to a volume of 500ml the new concentration of the solution is (A) 0.167 M (B) 0.0125 M (C) 0.833 M (D) 0.0167 M 24. 10 grams of a solute is dissolved in 90 grams of a solvent. Its mass percent in solution is (A) 0.01 (B) 11.1 (C) 10 (D) 9 25. What is the molality of a solution which contains 18 g of glucose (C6 H12O6 ) in 250 g of water (A) 4.0 m (B) 0.4 m (C) 4.2 m (D) 0.8 m 26. On dissolving 1 mole of each of the following acids in 1 litre water, the acid which does not give a solution of strength 1N is (A) HCl (B) Perchloric acid (C) HNO3 (D) Phosphoric acid 27. How many grams of NaOH will be required to neutralize 12.2 grams of benzoic acid (A) 40 gms (B) 4gms (C) 16gms (D) 12.2 gms 28. 10ml of conc. H 2 SO4 (18 molar) is diluted to 1 litre. The approximate strength of dilute acid could be (A) 0.18 N (B) 0.09 N (C) 0.36 N (D) 1800 N 29. The normality of 10 lit. volume hydrogen peroxide is (A) 0.176 (B) 3.52 (C) 1.78 (D) 0.88 30. Essential quantity of ammonium sulphate taken for preparation of 1 molar solution in 2 litres is (A) 132 gm (B) 264 gm (C) 198 gm (D) 212 gm Colligative properties 31. Which of the following is not a colligative property (A) Optical activity (B) Elevation in boiling point (C) Osmotic pressure (D) Lowering of vapour pressure 32. Colligative properties of a solution depends upon (A) Nature of both solvent and solute (B) The relative number of solute and solvent particles (C) Nature of solute only (D) Nature of solvent only 33. Which is not a colligative property (A) Refractive index (B) Lowering of vapour pressure (C) Depression of freezing point (D) Elevation of boiling point 34. Which of the following is a colligative property (A) Surface tension (B) Viscosity (C) Osmotic pressure (D) Optical rotation 35. Colligative properties are used for the determination of (A) Molar Mass (B) Equivalent weight (C) Arrangement of molecules (D) Melting point and boiling point 38. 39. 40. 41. Lowering of vapour pressure 42. 36. Lowering of vapour pressure is highest for (A) Urea (B) 0.1M glucose (C) 0.1M MgSO4 (D) 0.1M BaCl2 37. An aqueous solution of glucose was prepared by dissolving 18 g of glucose in 90 g of water. The relative lowering in vapour pressure is (A) 0.02 (B) 1 (C) 20 (D) 180 Solution “Relative lowering in vapour pressure of solution containing non-volatile solute is directly proportional to mole fraction of solute”. Above statement is (A) Henry law (B) Dulong and Petit law (C) Raoult's law (D) Le-Chatelier's principle An ideal solution was obtained by mixing methanol and ethanol. If the partial vapour pressure of methanol and ethanol are 2.619kPa and 4.556 kPa respectively, the composition of the vapour (in terms of mole fraction) will be (A) 0.635 methanol, 0.365 ethanol (B) 0.365 methanol, 0.635 ethanol (C) 0.574 methanol, 0.326 ethanol (D) 0.173 methanol, 0.827 ethanol The vapour pressure of two liquids P and Q are 80 and 600 torr, respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mole of Q would be (A) 140 torr (B) 20 torr (C) 68 torr (D) 72 torr The vapour pressure of benzene at a certain temperature is 640 mm of Hg . A non-volatile and non-electrolyte solid weighing 2.175g is added to 39.08g of benzene. The vapour pressure of the solution is 600mm of Hg . What is the molecular weight of solid substance (A) 49.50 (B) 59.6 (C) 69.5 (D) 79.8 Which one of the following is the expression of Raoult's law p  ps p p n N (A) (B) s   p nN p N n p  ps p  p N n N (C)  (D) s  ps N n ps N p  vapour pressure of pure solvent ps  vapour pressure of the solution n  number of moles of the solute N  number of moles of the solvent 43. Which has maximum vapour pressure (A) HI (B) HBr (C) HCl (D) HF 44. When a non-volatile solute is dissolved in a solvent, the relative lowering of vapour pressure is equal to (A) Mole fraction of solute (B) Mole fraction of solvent (C) Concentration of the solute in grams per litre (D) Concentration of the solute in grams 100 ml 45. 60 gm of Urea (Mol. wt 60) was dissolved in 9.9 moles, of water. If the vapour pressure of pure water is Po , the vapour pressure of solution is (A) 0.10 Po (B) 1.10 Po (C) 0.90 Po Ideal and Non-ideal solution (C) CHCl3  (C2 H 5 ) 2 O (C) (C2 H 5 )2 O  CHCl3 (D) (CH 3 ) 2 CO  C6 H 5 NH 2 50. All form ideal solution except (A) C2 H 5 Br and C2 H 5 I (B) C2 H 5Cl and C6 H 5 Br (C) C6 H 6 0,1 and C6 H 5CH 3 (D) C2 H 5 I and C2 H 5OH  separated solvent (ii) Pure solute  separated solute molecules H2 (iii) Separated solvent and solute molecules  solution H3 Solution so formed will be ideal if (A) H soln  H 3  H1  H 2 (B) H soln  H1  H 2  H 3 (C) H soln  H1  H 2  H 3 (D) H soln  H1  H 2  H 3 (A) CHCl3  (CH 3 ) 2 CO 46. In which case Raoult's law is not applicable (A) 1M NaCl (B) 1 M urea (C) 1 M glucose (D) 1 M sucrose 47. A solution that obeys Raoult's law is (A) Normal (B) Molar (C) Ideal (D) Saturated 48. An example of near ideal solution is (A) n -heptane and n -hexane (B) CH 3COOH  C5 H 5 N (B) (CH 3 ) 2 CO  CHCl3 (i) Pure solvent molecules H1 52. Identify the mixture that shows positive deviation from Raoult’s law (D) 0.99 Po (D) H 2O  HNO3 49. A mixture of liquid showing deviation in Raoult's law is (A) (CH 3 ) 2 CO  C2 H 5 OH Solution 51. Formation of a solution from two components can be considered as positive (B) (CH 3 ) 2 CO  C6 H 5 NH 2 (C) CHCl3  C6 H 6 (D) (CH 3 ) 2 CO  CS 2 53. When acetone is added to chloroform, then hydrogen bond is formed between them.These liquids show (A) Positive deviation from Raoult's law (B) Negative deviation from Raoult's law (C) No deviation from Raoult's law (D) Volume is slightly increased 54. Which of the following is true when components forming an ideal solution are mixed (A) H m  Vm  0 (B) H m  Vm (C) H m  Vm (D) H m  Vm  1 55. The liquid pair benzene-toluene shows (A) Irregular deviation from Raoult's law (B) Negative deviation from Raoult's law (C) Positive deviation from Raoult's law (D) Practically no deviation from Raoult's law Azeotropic mixture 56. The azeotropic mixture of water (b. p.100 o C ) and HCl (b. p.85o C ) boils at 108.5o C . When this mixture is distilled it is possible to obtain (A) Pure HCl (B) Pure water (C) Pure water as well as pure HCl (D) Neither HCl nor H 2O in their pure states 57. An azeotropic solution of two liquids has boiling point lower than either when it (A) Shows a negative deviation from Raoult's law (B) Shows no deviation from Raoult's law (C) Shows positive deviation from Raoult's law (D) Is saturated 58. A liquid mixture boils without changing constituent is called (A) Stable structure complex (B) Binary liquid mixture (C) Zeotropic liquid mixture (D) Azeotropic liquid mixture 59. Azeotropic mixture are (A) Constant temperature boiling mixtures (B) Those which boils at different temperatures (C) Mixture of two solids (D) None of the above 60. A mixture of two completely miscible nonideal liquids which distil as such without change in its composition at a constant temperature as though it were a pure liquid. This mixture is known as (A) Binary liquid mixture (B) Azeotropic mixture (C) Eutectic mixture (D) Ideal mixture Solution Osmosis and Osmotic pressure of the solution 61. If 20 g of a solute was dissolved in 500 ml of water and osmotic pressure of the solution was found to be 600 mm of Hg at 15o C , then molecular weight of the solute is (A) 1000 (B) 1200 (C) 1400 (D) 1800 62. The osmotic pressure of 0.4% urea solution is 1.66 atm and. that of a solution of suger of 3.42 % is 2.46 atm. When both the solution are mixed then the osmotic pressure of the resultant solution will be (A) 1.64 atm (B) 2.46 atm (C) 2.06 atm (D) 0.82 atm 63. Blood is isotonic with (A) 0.16 M NaCl (B) Conc. NaCl (C) 50 % NaCl (D) 30 % NaCl 64. Which inorganic precipitate acts as semipermeable membrane or The chemical composition of semipermeable membrane is (A) Calcium sulphate (B) Barium oxalate (C) Nickel phosphate (D) Copper ferrocyanide 65. The osmotic pressure of 1m solution at 27 o C is (A) 2.46 atm (B) 24.6 atm (C) 1.21 atm (D) 12.1 atm 66. Osmotic pressure of a solution can be measured quickly and accurately by (A) Berkeley and Hartley's method (B) Morse's method (C) Pfeffer's method (D) De Vries method 67. The solution in which the blood cells retain their normal form are with regard to the blood (A) Isotonic (B) Isomotic (C) Hypertonic (D) Equinormal 68. The osmotic pressure of a solution is given by the relation RT CT (A) P  (B) P  R C RC P (C) P  (D)  RT T C 69. The osmotic pressure of a solution is directly proportional to (A) The molecular concentration of solute (B) The absolute temperature at a given concentration (C) The lowering of vapour pressure (D) All of the above 70. What would happen if a thin slice of sugar beet is placed in a concentrated solution of NaCl (A) Sugar beet will lose water from its cells (B) Sugar beet will absorb water from solution (C) Sugar beet will neither absorb nor lose water (D) Sugar beet will dissolve in solution Elevation of boiling boint of the solvent 71. The molal elevation constant is the ratio of the elevation in B.P. to (A) Molarity (B) Molality (C) Mole fraction of solute (D) Mole fraction of solvent 72. The molal boiling point constant for water is 0.513o C kg mol 1 . When 0.1 mole of sugar is dissolved in 200ml of water, the solution boils under a pressure of one atmosphere at (A) 100.513o C (B) 100.0513o C (C) 100.256 o C (D) 101.025o C 73. Value of gas constant R is (A) 0.082 litre atm (B) 0.987 cal mol 1 K 1 (C) 8.3 J mol 1 K 1 (D) 83 erg mol 1 K 1 Solution 74. The temperature, at which the vapour pressure of a liquid becomes equal to the atmospheric pressure is known as (A) Freezing point (B) Boiling point (C) Absolute temperature (D) None of these 75. The elevation in boiling point of a solution of 13.44g of CuCl2 in 1kg of water using the following information will be (Molecular weight of CuCl2 = 134.4 and Kb = 0.52 K molal1) (A) 0.16 (B) 0.05 (C) 0.1 (D) 0.2 Depression of freezing point of the solvent 76. Given that T f is the depression in freezing point of the solvent in a solution of a nonvolatile solute of molality m , the quantity  T f  lim   is equal to m0  m  (A) Zero (B) One (C) Three (D) None of the above 77. The freezing point of 1 percent solution of lead nitrate in water will be (A) Below 0o C (B) 0o C (C) 1o C (D) 2o C 78. What is the effect of the addition of sugar on the boiling and freezing points of water (A) Both boiling point and freezing point increases (B) Both boiling point and freezing point decreases (C) Boiling point increases and freezing point decreases (D) Boiling point decreases and freezing point increases 79. During depression of freezing point in a solution the following are in equilibrium (A) Liquid solvent, solid solvent (B) Liquid solvent, solid solute (C) Liquid solute, solid solute (D) Liquid solute solid solvent 80. 1.00 gm of a non-electrolyte solute dissolved in 50 gm of benzene lowered the freezing point of benzene by 0.40 K. K f for benzene is 5.12 kg mol–1. Molecular mass of the solute will be (A) 256 g mol 1 (B) 2.56 g mol 1 (C) 512 103 g mol 1 (D) 2.56 104 g mol 1 81. 0.440 g of a substance dissolved in 22.2 g of benzene lowered the freezing point of benzene by 0.567o C . The molecular mass of the substance ( K f  5.12o C mol 1 ) (A) 178.9 (B) 177.8 (C) 176.7 (D) 175.6 82. Which of the following aqueous molal solution have highest freezing point (A) Urea (B) Barium chloride (C) Potassium bromide (D) Aluminium sulphate 83. Which will show maximum depression in freezing point when concentration is 0.1M (A) NaCl (B) Urea (C) Glucose (D) K 2 SO4 84. The freezing point of a 0.01M aqueous glucose solution at 1 atmosphere is 0.18o C . To it, an addition of equal volume of 0.002 M glucose solution will; produce a solution with freezing point of nearly (A) 0.036o C (B) 0.108o C (C) 0.216o C (D) 0.422o C 85. What should be the freezing point of aqueous solution containing 17 gm of C2 H 5OH in 1000gm of water (water K f = 1.86 deg  kg mol 1 (A) 0.69o C (C) 0.0o C (B) 0.34o C (D) 0.34o C Solution Colligative properties of electrolyte 86. Which of the following will have the highest boiling point at 1 atm pressure (A) 0.1M NaCl (B) 0.1M sucrose (C) 0.1M BaCl2 (D) 0.1M glucose 87. Which one of the following would produce maximum elevation in boiling point (A) 0.1 M glucose (B) 0.2 M sucrose (C) 0.1 M barium chloride (D) 0.1 M magnesium sulphate 88. Which of the following solutions will have the highest boiling point (A) 1% glucose (B) 1% sucrose (C) 1% NaCl (D) 1% CaCl2 89. Which one of the following aqueous solutions will exhibit highest boiling point (A) 0.015 M urea (B) 0.01M KNO3 (C) 0.01M Na2 SO4 (D) 0.015 M glucose 90. Which of the following aqueous solutions containing 10 gm of solute in each case has highest B.P. (A) NaCl solution (B) KCl solution (C) Sugar solution (D) Glucose solution 91. 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 92. Which one has the highest boiling point (A) 0.1N Na2 SO4 (B) 0.1N MgSO4 (C) 0.1M Al2 ( SO4 )3 (D) 0.1M BaSO4 93. Which of the following solutions boils at the highest temperature (A) 0.1 M glucose (B) 0.1 M NaCl (C) 0.1 M BaCl2 (D) 0.1 M Urea 94. 0.01M solution each of urea, common salt and Na2 SO4 are taken, the ratio of depression of freezing point is (A) 1 : 1 : 1 (B) 1 : 2 : 1 (C) 1 : 2 : 3 (D) 2 : 2 : 3 95. Which has the minimum freezing point (A) One molal NaCl solution (B) One molal KCl solution (C) One molal CaCl2 solution (D) One molal urea solution Solution 98. Acetic acid dissolved in benzene shows a molecular weight of (A) 60 (B) 120 (C) 180 (D) 240 99. The observed osmotic pressure of a solution of benzoic acid in benzene is less than its expected value because (A) Benzene is a non-polar solvent (B) Benzoic acid molecules are associated in benzene (C) Benzoic acid molecules are dissociated in benzene (D) Benzoic acid is an organic compound 100.The experimental molecular weight of an electrolyte will always be less than its Abnormal molecular mass 96. 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 97. One mole of a solute A is dissolved in a given volume of a solvent. The association of the solute take place according to nA ⇄ ( A) n . The Van't Hoff factor i is expressed as x (A) i  1  x (B) i  1  n x 1 x  n (C) i  (D) i  1 1 calculated value because the value of Van't Hoff factor “i” is (A) Less than 1 (B) Greater than 1 (C) Equivalent to one (D) Zero