Title 02. SOLUTIONS.pdf ✅

PAPER 1 (1.) The osmotic pressure of 0.2 molar solution of urea at 300 K R 0.082 ( = ) litre atm ) 1 1 mol K − − is : (1) 4.92 atm (2) 1 atm (3) 0.25 atm (4) 27 atm (2.) A 5% solution of cane sugar is isotonic with 0.877% of X . The molecular weight of substance X is : (1) 59.98 (2) 119.96 (3) 95.58 (4) 126.98 (3.) A 0.01M solution of glucose in water freezes at −0.186 C . A 0.01M solution of KCl in water will freeze at temperature : (1) higher than −0.0186 C (2) 0C (3) 0.0186 C (4) lower than −0.0186 C (4.) Equivalent mass of crystalline oxalic acid is : (1) 90 (2) 63 (3) 53 (4) 45 (5.) The volume of 2 4 0.1MH SO required to neutralise completely 40 mL of 0.2MNaOH solution is : (1) 10 mL (2) 40 mL (3) 20 mL (4) 80 mL (6.) An aqueous solution freezes at ( f − = 0.186 C K 1.86 ; K 0.512 b = ). What is the elevation in boiling point: (1) 0.186 (2) 0.512 (3) 0.512 1.86 (4) 0.0512 (7.) Relative lowering in vapour pressure of solution containing non-volatile solute is directly proportional to mole fraction of solute. Above statement is : (1) Henry law (2) Dulong and Petit law (3) Raoult's law (4) Le-Chatelier's principle (8.) If  is the degree of dissociation of Na SO2 4 the van't Hoff's factor (i) used for calculating the molecular mass is : (1) 1+ (2) 1− (3) 1 2 +  (4) 1 2 −  (9.) The depression in freezing point of 0.1M aqueous solutions of HCl,CuSO4 and K SO2 4 are in the ratio: (1) 1:1:1 (2) 1: 2:3 (3) 1:1:1.5 (4) 2: 4:3 (10.) The colligative properties depend upon :
(1) relative number of solute molecules irrespective of the nature of the solute and solvent (2) relative number of solute molecules in solution and nature of solvent (3) relative number of solute molecules and the nature of solute and solvent (4) relative number of solvent molecules. (11.) Which one of the following solutions exhibits the maximum elevation in boiling point : (1) 0.1 mNaCl (2) 2 0.1 mCaCl (3) 2 0.1 mBaCl (4) 3 0.1 mFeCl (12.) What will molality of 1 liter solution of 2 4 93%H SO (weight/volume) The density of the solution 1.84 g Iml: (1) 10.43M (2) 0.1043M (3) 104.3M (4) 0.00143M (13.) When mercuric iodide is added to the aqueous solution of potassium iodide : (1) Freezing point is raised (2) Freezing point is lowered (3) Freezing point does not change (4) Boiling point does not change (14.) Which will form maximum boiling azeotrope : (1) HNO H O 3 2 + solution (2) C H OH H O 2 5 2 + solution (3) C H C H CH 6 6 6 5 3 + solution (4) None of these. (15.) One kilogram of a sea water sample contains 6 mg of dissolved O2 . The concentration of O2 in the sample in ppm is : (1) 0.6 (2) 6.0 (3) 60.0 (4) 16.0 (16.) 0.1MNaCl and 2 0.05MBaCl solutions are separated by a semi-permeable membrane in a container. For this system, choose the correct answer : (1) There is no movement of any solution across the membrane (2) Water flows from BaCl2 solution towards NaC solution (3) Water flows from NaCl solution towards BaCl solution (4) Osmotic pressure of 0.1MNaCl is lower than the osmotic pressure of BaCl2 (Assume complete dissociation) (17.) The osmotic pressure of a solution at 27 C , which is prepared by dissolving 6.0gm of urea, 18gm glucose and 34.2gm sucrose to make 500ml of the solution: (1) 10.72 atm (2) 12.18 atm (3) 14.76 atm (4) 16.96 atm
(18.) 1.0 molal aqueous solution of the electrolyte 3 4 ( ) Mg PO 2 is 25% ionized. If Kb for H O2 is 0.52 K kg / mol , the boiling point of the solution is : (1) 375.5 K (2) 374.04 K (3) 377.12 K (4) 373.25k (19.) When the two liquids ( 0 A PA 300 = torr ) and ( 0 B PB = 800 torr), are mixed to prepare an ideal solution , its vapour pressure is observed to be 0.55 atm . The percentage mole fraction of B in the solution will be : (1) 24% (2) 48% (3) 72% (4) 86% (20.) A 0.6% solution of urea would be isotonic with which of the following solution : (1) 0.1M Glucose solution (2) 0.1MKCl solution (3) 0.6% Glucose solution (4) All of these (21.) During freezing of an aqueous solution of sodium chloride, there exists an equilibrium between : (1) Solid solute and solid solvent (2) Solid solvent and liquid solvent (3) Liquid solute and liquid solvent (4) Liquid solute and solid solvent (22.) The value of Van't Hoff factor (i) for aqueous solution of K Fe(CN) 4 6   , if the degree of ionisation of salt is  : (1) i 1 4 = +  (2) i 1 5 = +  (3) i 1 6 = +  (4) i 1 8 = +  (23.) The von't Hoff factor for 2 4 0.1MCs SO solution is 2.74. The degree of dissociation of salt will be : (1) 34.8% (2) 87.0% (3) 91.3% (4) 98.4% (24.) The vapour pressure of two liquids P and Q are 80 and 60 torr, respectively. The total vapour pressure of solution obtained by mixing 3 moles of P and 2 moles of Q would be : (1) 140 torr (2) 20 torr (3) 68 torr (4) 72 torr (25.) 0.5 molal aqueous solution of a weak acid HX is 20% ionised. If Kf for water is 1 1.86 K kg mol− , the lowering of freezing point of solution will be : (1) 0.56 K (2) 1.12 K (3) −0.56 K (4) −1.12 K (26.) For equal molar concentrations of glucose, NaCl, BaCl2 and AlCl3 , the decreasing order of measured colligative property is : (1) Glucose    AlCl BaCl NaCl 3 2 (2) AlCl BaCl NaCl 3 2    Glucose (3) Glucose    NaCl BaCl AlCl 2 3 (4) AlCl BaCl NaCl 3 2   = Glucose
(27.) Which of the following will have highest measure of any coligative property : (1) 1% sucrose solution (2) 1% glucose solution (3) 1% glycerol solution (4) 1% urea solution (28.) How are O.P. of 6% urea 1 and 6% glucose 2  related to each other : (1) 1 2    (2) 1 2    (3) 1 2   = (4) 1 2 1   = (29.) 0.2 molal aqueous solutions of each of NaCl,BaCl2 and AlCl3 have boiling points 1 2 T T, and T3 respectively. Which of the of following is correct : (1) T T T 1 2 3   (2) T T T 3 2 1   (3) T T T 2 1 3   (4) T T T 1 3 2   (30.) The relationship between osmotic pressure at 273 K when 10 g glucose (P ,10 g 1 ) urea ( ) P2 and 10 g sucrose ( ) P3 are dissolved in 250 mL of water is : (1) P P P 1 2 3   (2) P P P 3 1 2   (3) P P P 2 1 3   (4) P P P 2 3 1   (31.) An X molal solution of a compound in benzene has mole fraction of solute equal to 0.2 . The value of X is nearly : (1) 14 (2) 3.2 (3) 1.4 (4) 0.8 (32.) The example of positive deviation of : (1) CH COOH 3 and water (2) NaOH and water (3) Ethyl alcohol & water (4) Nitric acid and water (33.) The vapour pressure of water depends upon : (1) Amount of liquid (2) Surface area of container (3) Temperature (4) All of these (34.) When 1.04 g of BaCl2 is present in 5 10 g of solution the concentration of solution is : (1) 0.104ppm (2) 10.4ppm (3) 0.0104ppm (4) 104ppm (35.) The boiling point of 1 molal aq. solution of KCl is: ( Kb for water .52 k-kg/mole) (1) 102.0 C (2) 100.52 (3) 101.04 C (4) 100.25 C (36.) When acetone and chloroform are mixed together, which of the following observations is correct :