//M1//QN1//MCQ//DL0//EQ

(i) In bromoethane and chloroethane mixture intermolecular interactions of A-A and B-B type are nearly same as A-B type interactions. (ii) In ethanol and acetone mixture A-A or B-B type intermolecular interactions are stronger than A-B type interactions. (iii) In chloroform and acetone mixture A-A or B-B type intermolecular interactions are weaker than A-B type interactions.21. We have three aqueous solutions of NaCl labelled as ‘A’, ‘B’ and ‘C’ with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of Van't Hoff factor for these solutions will be in the order ________.22. Two beakers of capacity 500 mL were taken. One of these beakers, labelled as “A”, was filled with 400 mL water, whereas the beaker labelled “B” was filled with 400 mL of 2 M solution of NaCl. At the same temperature both the beakers were placed in closed containers of same material and same capacity as shown in Figure. At a given temperature, which of the following statement is correct about the vapour pressure of pure water and that of NaCl solution.

23. If two liquids A and B form minimum boiling azeotrope at some specific composition

then ________.24. 4 L of 0.02 M aqueous solution of NaCl was diluted by adding one litre of water. The molality of the resultant solution is ________.25. On the basis of information given below mark the correct option. On adding acetone to methanol some of the hydrogen bonds between methanol molecules break.26. KH value for Ar(g), CO2(g), HCHO(g) and CH4(g) are 40.39, 1.67, 1.83 × 10–5 and 0.413 respectively. Arrange these gases in the order of their increasing solubility.1. An alloy of copper and zinc is called? 2. Camphor in N2 gas is an example of?3. Which of the following is a true solution?4. Which of the following fluoride is used as rat poison?5. An example of a solution having liquid in gas is:6. Which of the following solid solutions has a solute that is a gas?7. Which of the following is example of solution?8. What type of solution does soda form by dissolving CO2 in water?9. State the molecular mass and formula mass of potash alum.10. When a solute is present in trace quantities the following expression is used:11. The atmospheric pollution is generally measured in the units of.12. If 2 g of NaOH is present is 200 ml of its solution, its molarity will be ....13. Dilute 1 L one molar H2SO4 solution by 5 L water, the Normality of that solution is14. 2.5 L of NaCl solution contain 5 moles of the solute, What is the molarity?15. 6.02 × 1020 molecules of urea are present in

100 mL of its solution. The concentration of urea solution is ... 16. Which of the following solutions has the highest normality? 17. 100 mL of 0.3 N HCl is mixed with 200 ml of 0.6 N H2SO4. The final Normality of the resulting solution will be 18. Molecular weight of glucose is 180. A solution of glucose which contains 18 g/L, is 19. In a solution of 7.8 g benzene (C6H6) and 46.0 g toluene (C6H5CH3), the mole-fraction of benzene  is20. How much of 0.1 M H2SO4 Solution is required to neutralize 50mL of 0.2 M NaOH Solution?21. Molarity of 0.2 N H2SO4 is ...22. The amount of anhydrous Na2CO3 present in 250 mL of 0.25 M solution is ...23. How many gram of NaOH will be required to prepare 500 g solution containing NaOH solution?24. 5 L of a solution contains 25 mg of CaCO3,

What is its concentration in ppm?

(mol. wt. of CaCO3 is 100)25. Which of the following concentration term is/are independent of temperature?26. What amount of water is added in 40 mL of NaOH (0.1 N) which is neutralised by 50 mL of HCl (0.2 N)? 27. The Normality of 2.3 M H2SO4 solution is ...28. A 5 molar solution of H2SO4 is diluted from 1 L to 10 L. What is the Normality of the solution?29. Molarity of a given orthophosphoric acid solution is 3 M. Its Normality is:30. Molarity of solution prepared by dissolving 75.5 g of pure KOH in 540 ml solution is:31. Volume of 0.6 M NaOH required to neutralise 30 cm3 of 0.4 M HCl is:32. The volume of 10 N and 4 N HCl required to make 1 L of 7 N HCl are:33. 1 M, 2.5 litre NaOH solution is mixed with another 0.5 M, 3 litre NaOH solution. Then find out the molarity of resultant solution:34. Molality of 30% W/W NaOH aq. solution _________ .35. In 100 ml solution 5  10–5 gm CO2 is dissolved. What will be its concentration in ppm units?36. State the value of [H+] in 0.01 M KOH solution.37. How many grams of urea are required to make 150 grams of 20% W/W solution of urea?38. The partial pressure of ethane over a saturated solution containing 6.56 × 10-2g of ethane is

1 bar. If the solution contains 5.0 × 10-2 g of ethane, the partial pressure of ethane will be: 39. The solubility order for the following gases is:40. How does the solubility of gas change in a liquid, as described?41. Which of the following best describes the difficulty in breathing as one climbs to higher altitudes?42. The law which indicates the relationship between solubility of a gas in liquid and pressure.43. The solubility of gas in water depends on:44. The solubility of a gaseous solute in a liquid solvent does not depend on which factor?45. Which of the following compounds will be more soluble in water?46. Which gas will have the highest solubility in ethyl alcohol?47. Find the constant of Henry's law for O2 if

2 milli mole of O2 gas dissolve in 540 ml of water at 27°C. The partial pressure of the

O2 gas is 2 × 10–8 bar.48. Which of the given option is correct when KCl is soluble in water?49. Solvent + solute = solution ∆H > 0. What will be the change in solubility of a substance when the temperature is raised at equilibrium in the process?50. Vapour pressure of pure liquid A at 27°C is

70 mm. Hg. Adding another liquid B to it forms an ideal solution. If the mole fraction of B is 0.2 and the total vapour pressure of the solution at 27°C is 84 mm Hg, find the vapour pressure of pure liquid B at 27°C.51. A liquid has a vapour pressure of 70 mm at 27°C. Adding another liquid (mole fraction 0.2) to this liquid at 27°C has a vapour pressure of 95 mm. Hg. Then find the vapour pressure of the other liquid.52. The vapour pressure of two liquids X and Y are 80 and 60 torr respectively. The total vapour pressure of the ideal solution obtained by mixing 3 moles of X and 2 moles of

Y would be53. Vapour pressure of pure A = 100 torr,

moles = 2; vapour pressure of pure B = 80 torr, moles = 3. Total vapour pressure of the

mixture is:54. Vapour pressure of a solvent containing non-volatile solute is: 55. Vapour pressure of pure ‘A’ is 70 mm Hg at 25oC. It form an ideal solution with ‘B’ in which mole fraction of A is 0.8. If the vapour pressure of the solution is 84 mm Hg at 25oC, the vapour pressure of pure ‘B’ at 25oC is.56. A mixture of ethyl alcohol and propyl alcohol has a vapour pressure of 290 mm at 300K. the vapour pressure of propyl alcohol is

200 mm Hg. If the mole fraction of ethyl alcohol is 0.6, it's vapour pressure (in mm) at the same temperature will be :57. On mixing, heptane and octane form an ideal solution. At 373K, the vapour pressures of the two liquid components (heptane and octanes) are

105 kPa and 45 kPa respectively. Vapour pressure of the solution obtained by mixing 25 g of heptane and 35 g of octane will be (molar mass of heptane = 100 g mol-1 and of octane = 114 g.mol-1)58. A solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressure of pure hydrocarbons at 20°C are 440 mm Hg for pentane and 120 mm Hg for hexane. The mole fraction of pentane in vapour phase would be:59. Which of the following is true when components forming an ideal solution are mixed?60. Which of the following is not correct for ideal solution?61. Azeotropic mixture are:62. Which of the following liquid pair shows a positive deviation from Raoult's law?63. In a mixture of A and B, components show negative deviation when64. Which of the following mixture does not show positive deviation from the Raoult’s law? 65. A binary liquid solution is prepared by mixing n-heptane and ethanol. Which one of the following statements is correct regarding the behaviour of the solution?66. An ideal solution is that which67. In a mixture A and B components show negative deviation as: 68. Which of the following is an example of a non-ideal solution showing positive deviation?69. What deviation is shown by a mixture of equimolar phenol and aniline?70. Colligative properties of a solution depend upon:71. At 25°C, the highest osmotic pressure is exhibited by 0.1 M solution of72. Which one of the following aqueous solutions will exhibit highest boiling point?73. The molal elevation constant of water is 0.52oC. The boiling point of 1.0 Molal aqueous KCl solution (assuming complete dissociation of KCl), therefore, should be74. The increase in boiling point of a solution containing 0.6 g urea in 200 g water is 0.50oC. Find the molal elevation constant. 75. In an osmotic pressure measurement experiment, a 5% solution of compound 'X' is found to be isotonic with a 2% acetic acid solution. The gram molecular mass of 'X' is76. Which is a colligative property?77. Kf for water is 1.86 K.kg.mol-1. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol (C2H6O2) must you add to get the freezing point of the solution lowered to -2.8°C?78. Which of the following solution has highest boiling point?79. If for a sucrose solution elevation in boiling point is 0.1oC then what will be boiling point of NaCl solution for the same molal concentration?80. In two solutions having different osmotic pressure, the solution of higher osmotic pressure is called: 81. Isotonic solution have the same82. Two solutions have different osmotic pressure. The solution of lower osmotic pressure is called:83. The osmotic pressure (at 27oC) of an aqueous solution (200 ml) containing 6 g of a protein is 2 × 10-3atm . If R = 0.080L.atm.mol-1.K-1, the molecular weight of protein is84. A 5% solution of cane sugar (molar mass 342) is isotonic with 1% of a solution of an unknown solute. The molar mass of unknown solute in

g/mole is85. Osmotic pressure is 0.0821 atm at temperature of 300K. Find concentration in mole per litre86. The elevation in boiling point for one molal solution of a solute in a solvent is called:87. The depression in freezing point of 0.01 m aqueous solution of urea, sodium chloride and sodium sulphate is in the ratio:88. Colligative properties are used for the determination of:89. The osmotic pressure of 0.4% urea solution is 1.66 atm and that of a solutions of sugar of 3.42% is 2.46 atm. When both the solutions are mixed then the osmotic pressure of the resultant solution will be:90. The freezing point (in oC) of solution containing 0.1 g of K3[Fe(CN)6] (mol . wt 329) in 100 g of water (Kf= 1.86 K.kg.mol-1) is 91. The vapour pressure of water at 20°C is 17.54 mm. When 20 g of a non-ionic. substance is dissolved in 100g of water, the vapour pressure is lowered by 0.30 mm. What is the molecular mass of the substance?92. Boiling point of water is defined as the temperature at which:93. The molal elevation constant for water is 0.52. What is the boiling point of 2 molar sucrose solution at 1 atm pressure? (Assume b.p. of pure water is 100oC)94. When 10 g of a non-volatile solute is dissolved in 100 g of benzene, it raises boiling point by 1oC then molecular mass of the solute is

(Kb for C6H6 = 2.53 K.kg.mol-1)95. Depression in freezing point is 6K for NaCl solution if Kf for water is 1.86 K.kg.mol–1, amount of NaCl dissolved in 1 kg water is96. Which of the following is not a colligative property?97. Vapour pressure of dilute aqueous solution of glucose is 750 mm Hg at 373 K. The mole fraction of solute is98. Which solution will have least vapour pressure?99. The relative lowering of vapour pressure produced by dissolving 71.5 g of a substance in 1000 g of water is 0.00713. The molecular weight of the substance will be:100. The molal boiling point constant of water is 0.53oC. When 2 mole of glucose are dissolved in 4000 g of water, the solution will boil at:101. Calculate the molal depression constant of a solvent which has freezing point 16.6°C and latent heat of fusion 180.75 Jg-1.102. The movement of solvent molecules through a semipermeable membrane is called:103. Molal elevation/depression constant depends upon:104. 1.0 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 of benzene is 5.12 K.kg.mol-1, the lowering in freezing point will be: 105. The vapour pressure of water at 20oC is

17.5 mmHg. If 18 g of glucose (C6H12O6) is added to 178.2 g of water at 20oC, the vapour pressure of the resulting solution will be106. What is the molality of ethyl alcohol

(mol. wt. = 46) in aqueous solution which freezes at -10oC?. (Kf for water = 1.86 K.molality-1)107. Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg water to prevent it from freezing at -6oC will be (Kf for water = 1.86 K.kg.mol-1 and molar mass of ethylene glycol = 62 g mol-1)108. The process of getting fresh water from sea water is known as:109. If 0.15 g of a solute dissolved in 15 g of solvent is boiled at temperature higher by 0.216oC than that of the pure solvent, the molecular weight of the substance is (molal elevation constant for the solvent is 2.16 K.kg.mol–1)110. The osmatic pressure of 5% (wt./vol) solution of cane sugar at 150oC is 111. Which of the following solutions will have highest boiling point:112. Osmotic pressure of a solution at a given temperature:113. When a non-volatile solute is dissolved in a solvent, the relative lowering of vapour pressure is equal to:114. From the colligative properties of solution which one is the best method for the determination of molecular weight of proteins and polymers:115. Which has the highest freezing point at one atmosphere?116. An aqueous solution of glucose was prepared by dissolving 18 g of glucose in 90 g of water. The relative lowering in vapour pressure is117. Solutions A, B, C and D are respectively

0.1 M glucose, 0.05 M NaCl, 0.05 M BaCl2 and 0.1 M AlCl3 which one of the following pairs isotonic?118. The relationship between the values of osmotic pressure of 0.1 M solution of KNO3(p1) and CH3 COOH(p2) is119. The order of osmotic pressure of isomolar solution of BaCl2, NaCl and sucrose is:120. The relationship between osmotic pressure at

273K when 10 g glucose (p1), 10 g urea (p2) and

10 g sucrose (p3) are dissolved in 250 mL of

water is:121. Blood cells retain their normal shapes in solutions which are:122. Which has the minimum freezing point? 123. Which of the following solution is hypotonic?124. A 1.5% urea solution is isotonic with 5.25% of an unknown solution. The molar mass of unknown solute is.125. What will be the osmotic pressure (π) of a 6% W/V glucose aqueous solution at 300K?

(R = 0.082) (molecular weight of glucose = 180 g/mol)126. If the relative decrease in vapour pressure of a solution is 0.8, state the mole fraction of solvent present in that solution.127. Calculate the boiling point of the solution formed by dissolving 6 g of urea in 2 kg of water. (Kb = 3.2 K.Kg.mol–1)128. What process is required to convert sea water into pure water?129. Which of the following has the lowest vapour pressure?130. State the relative lowering in vapour pressure of the solution when 6 g of urea is dissolved in 90 g of water.131. The freezing point of an aqueous solution is -0.170°C. So, what is the boiling point elevation for that solution?132. Solutions A, B, C and D contain 0.1 M glucose, 0.05 M NaCl, 0.05 M BaCl2 and 0.1 M AlCl3 respectively. So, which of the following pairs of solutions will be isotonic?133. A 3% glucose solution is isotonic with 1% of

an unknown solution. The molar mass of unknown solute is.134. Which of the given solutions is hypertonic compared to the liquid in the blood cell at a fixed temperature?135. Van't Hoff factor more than unity indicates that the solution has:136. Which of the following shows maximum depression in freezing point?137. 20 g of binary electrolyte (mol. wt. = 100) are dissolved in 500 g of water. The depression in freezing point of the solution is 0.74°C

(kf = 1.86 K.m-1) the degree of ionisation of the electrolyte is138. If α is the degree of dissociation of Na2SO4 the Van't Hoff factor (i) used for calculating the molecular mass is139. Two solution of KNO3 and CH3COOH are prepared separately. Molarity of both is 0.1 M and osmotic pressures are p1 and p2 respectively. The correct relationship between the osmotic pressure is140. What is the freezing point of a solution containing 8.1 g HBr in 100 g water assuming the acid to be 90% ionised (kf for water = 1.86 K.kg.mol-1)? 141. A 0.5 molal aqueous solution of weak acid (HX) is 20 percent ionized. The lowering in freezing point of this solution is: (Kf = 1.86 K/m for water)142. When 20 g of naphthoic acid (C11H8O2)

is dissolved in 50 g benzene (Kf = 1.72

K.kg. mol-1), a freezing point depression of 2K is observed. The Van't Hoff factor (i) is:143. A solution of 4.5 g of a pure non-electrolyte in 100 g of water was found to freeze at 0.465°C. The molecular weight of the solute closest to (Kf = 1.86 K.kg.mol–1)144. The Van't Hoff factor i for a compound which undergoes dissociation in one solvent and association in other solvent is respectively:145. Phenol dimerises in benzene having Van't Hoff factor 0.54. What is the degree of association?146. Van't Hoff factor of Ca (NO3)2 is:147. The freezing point depression of 0.001 m, Kx[Fe(CN)6] is 7.10 × 10-3K. If for water, Kf is 1.86 K.kg.mol-1 value of x will be:148. 0.1 Molal aqueous solution of NaBr freezes at –0.335oC at atmospheric pressure Kf for water is 1.86 K.kg.mol–1. The percentage of dissociation of the salt in solution is 149. Which of the following compounds correspond to maximum Van't Hoff factor for dilute solution?150. The freezing point of one molal NaCl solution assuming NaCl to be 100% dissociated in water is (molal depression constant = 1.86)151. If the various terms in the below given expressions have usual meanings, the Van't Hoff factor (i) cannot be calculated by which one of the expressions?152. The Van't Hoff factor for 0.1 M Ba(NO3)2 solution is 2.74. The degree of dissociation is:153. Value of Van't Hoff factor when solute

dissociate is:154. Value of Van't Hoff factor when solute

associate is:155. Van't Hoff factor of K4 [Fe(CN)6] is:156. What amount of CaCl2 (i=2.47) is dissolved in 2 litres of water so that its osmotic pressure is 0.5 atm at 27°C?157. The Van't Hoff factor will be highest for158. Assertion : Molarity of a solution in liquid state changes with temperature. Reason : The volume of a solution changes with change in temperature.159. Assertion : In an ideal solution, ∆Hmix and ∆Vmix both are zero. Reason : In an ideal solution, A−B interactions are similar to A−A and B−B interactions.160. Assertion : When NaCl is added to water a depression in freezing point is observed. Reason : The Lowering of vapour pressure of a solution causes depression in the freezing point.161. Assertion : One molar aqueous solution has always higher concentration than one molal. Reason : The molality of a solution depends upon the density of the solution whereas molarity does not.162. Assertion : If a concentrated solution is diluted by adding more water, the molarity of the solution does not change. Reason : The ratio of moles of solute to volume is called molarity.163. Assertion : Increasing the pressure on water decreases its boiling point. Reason : Density of water is maximum at 273K.164. Assertion : One molal aqueous solution of glucose contains 180 g of glucose in 1 kg water. Reason : The solution containing one mole of solute in 1000 g of solvent is called one molal solution.165. Assertion : The molecular weight of acetic acid determined by depression in freezing point method in benzene and water was found to be different. Reason : Water is polar while benzene is non-polar.166. Assertion : A mixture of benzene and toluene forms an ideal solution. Reason : Mixing 50 ml of benzene and 50 ml of toluene gives a total volume of solution of 100 ml i.e. ∆V = 0 and

∆H = 0.167. Assertion : Cooking time is reduced in pressure cooker. Reason : Boiling point of water inside the pressure cooker is lowered.168. Assertion : Isotonic solution do not show the phenomenon of osmosis. Reason : Isotonic solutions have equal osmotic pressure.169. Assertion : Iodine is more soluble in CCl4 than in water. Reason : Non-polar solutes are more soluble in non-polar solvents. 170. Assertion : Osmotic pressure 0.1 M urea solution is less than that of 0.1 M NaCl solution. Reason : Osmotic pressure is not a colligative property.171. Assertion : Sodium chloride (NaCI) is useful for de-icing the road. Reason : Sodiumt chloride lowers the boiling point of water.172. Assertion : Molality of solution does not change with change in temperature. Reason : Molality is defined as number of moles of solute per 1000 g. of solvent.173. Assertion : The boiling point of 0.1 m glucose solution is lower than that of 0.1 m KCl solution. Reason : Boiling point elevation is inversely proportional to the number of constituent particles present in the solution.174. Assertion : When a non-volatile solute is dissolved in a solvent the rise in both boiling point and freezing point is equal to 2K. Reason : The increase in boiling point and decrease in freezing point depend on the no. of particles of the volatile solute. 175. Assertion : The boiling point of water increases when methyl alcohol is added to water. Reason : An increase in boiling point is observed when a volatile solute is added to a volatile solvent.176. Assertion : When solute and solvent are separated by a semipermeable membrane, the solvent molecules move towards the solution. Reason : Spontaneous flow of solvent from concentrated solution to dilute solution is called osmosis.177. Select the correct option for the true/false statements with reference to the given figure. Assume complete dissociation of ionic substance in aqueous solution. {[Fe(CNS)]+2 has a red colour.} (i) Concentration of aqueous solution of FeCl3 increase with time. (ii) Aqueous solution of FeCl3 gradually turns red. (iii) Concentration of aqueous solution of KCNS increases with time. (iv) Aqueous solution of KCNS remains colourless.178. Select the correct option for the true/false statements: (i) As the partial pressure of a gas increases, the solubility of a gas in a liquid increases. (ii) The solubility of gas in liquid increases as temperature increases. (iii) A gas for which the value of KH is low at a given temperature is less soluble in a liquid. (iv) As partial pressure of gas decreases and temperature increases the solubility of gas in liquid increases.179. Choose the correct option for the true/false statements with respect to the given graph of mole fraction versus vapour pressure. (i) The boiling point of an azeotropic mixture of liquid-A and liquid-B will be maximum. (ii) In mixture vapour pressures of both liquids are equal then xA < xB. (iii) The given mixture shows positive deviation in terms of Raoult's law. (iv) xA = xB then pA < pB180. Select the correct option for the true-false statements with reference to the given figure: (Assume complete dissociation of ionic substances in aqueous solution) (i) Adding water to an aqueous solution of CuSO4 increases the osmotic pressure of the system. (ii) Concentration of glucose solution increases with time. (iii) Addition of glucose to a glucose solution decreases the osmotic pressure of the system. (iv) Concentration of solution of CuSO4 increases with time.181. Choose the correct option using T (True) and F (False) notation for the following statements. (i) The vapour pressure of a solution containing a non-volatile solute is proportional to the mole-fraction of the solvent. (ii) A solution of 0.1 M Ba(NO2)2 is isotonic with 0.1 M Na2SO4 solution. (iii) Boiling point is a Colligative property. (iv) When the solute is associated the value of Van't Hoff factor (i) is greater than one.182. Choose the correct option using T (True) and F (False) notation for the following statements. (i) For CH3COCH3 and C6H6 mixed solution ∆H > 0 and ∆V > 0 becomes pTotal = p0A ⋅ xA + p0B ⋅ xB (ii) If the density of a 5% W/W solution is 1.043 g/ml, its molality will be 0.549 m. (iii) A liquid which has a low vapour pressure has a high boiling point. (iv) Two solutions A and B are separated by a semipermeable membrane, if the liquid moves from A to B the concentration of A is greater than that of B.183. Decide whether the following statements are true or false: (i) At a given temperature, 2 g/liter urea solution and 2 g/liter glucose solution separated by a semipermeable membrane are isotonic. (ii) A solution of KCI is hypotonic if it is separated by a semipermeable membrane from a solution of 0.01 M KCl and 0.001 M NaCl. (iii) 1 mole of glucose mix with 3 moles of water the relative lowering in vapour pressure is 0.25. (iv) 100 g of sugar is required to make 2 liters of 5% concentration of solution.184. For the following statements select the correct option using T (for true) and F (for false). (i) Dissolving two molecules of benzoic acid in benzene show association. (ii) Fe2(SO4)3 and NaCl dissociate in water. (iii) The number of solute particles in a solution increases during association. (iv) Colligative properties of solutions apply only to concentrated solutions.185. Choose the correct option using the true and false from the following statement. (i) The decrease in vapour pressure is equal to the mole fraction of solute. (ii) Relative decreases in vapour pressure is proportional to amount of salute. (iii) Relative decreases in vapour pressure is proportional to mole fraction of solute . (iv) Vapour pressure of a solution is equal to the mole fraction of solvent.186. For an ideal solution containing liquid-A and liquid-B choose the correct option using the symbol T (True) or F (False) according to the following statements. (i) p = p0A · xA + p0B · xB (ii) p = p0A · xB + p0B · xB (iii) p = p0A + (p0B – p0A) xB (iv) p = p0B + (p0A · p0B) xA187. Choose the correct option using T (True) and F (False) notation for the following statements. (i) The values of KH at a given temperature are different for different gaseous solutes. (ii) The value of KH change with temperature change for each component (for gas solutes). (iii) As the value of KH increases, the solubility of gaseous solute in liquid increases. (iv) The value of KH decreases with decreasing temperature.188. Choose the correct option using T (True) and F (False) notation for the following statements. (i) The solubility of a gas in a liquid solvent decreases as temperature increases. (ii) The value of KH increases as the temperature increases. (iii) Divers use a mixture of 2% He and 98% O2 while diving in the sea. (iv) Partial pressure of gas in a solution is proportional to mole fraction of that gas.189. Select the correct option using T (True) and F (False) notation for the following statements. (i) An aqueous solution of 5% NaCl and KCI is equimolar. (ii) 1 M H2SO4 means 1 N H2SO4. (iii) Aqueous solutions of 1 M sucrose and 1 M glucose are isotonic. (iv) The Van't Hoff factor for BaCl2(aq) is 3.190. Choose the correct option using T (True) and F (False) notation for the following statements.. (i) Mathematical form of Raoult's law (ii) Increase in boiling point of 1M aqueous solution is called molal elevation constant. (iii) An aqueous solution of urea has a value of Van't Hoff factor less than one. (iv) Placing a plant cell in a hypertonic solution causes it to swell.

(A) FTTT    (B) TFFF    (C) FTFF    (D) TTFF

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