Topic: Colligative Property O 3

Transcription

1 PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Topic: Colligative Property 1. What is the mole fraction of C 3 O 3 in a solution prepared from 1.01 moles of C 3 O 3 and 2.00 moles of water? (Atomic weights : C = 12.01, H = 1.008, O = 16.00) a) b) c) d) e) What is the mole fraction of CH 3 OH in a solution prepared from 1.74 moles of CH 3 OH and 2.44 moles of water? (Atomic weights : C = 12.01, H = 1.008, O = 16.00) a) b) c) d) e) What is the mole fraction of CsCl in a solution prepared from moles of CsCl and 2.78 moles of water? (Atomic weights : Cs = 132.9, Cl = 35.45, H = 1.008, O = 16.00) a) b) c) d) e) What is the mole fraction of urea, (NH 2 CO in an aqueous solution that is 10.0% urea by mass? (Atomic weights : C = 12.01, N = H = 1.008, O = 16.00) a) b) c) d) e) A lead glass is prepared by melting 20.0 g of silica (SiO 2 ) and 80.0 g of lead (II) oxide (PbO). What is the mole fraction of SiO 2 in the glass? (Atomic weights : Si = 28.08, Pb = 207.2, O = 16.00) a) b) c) d) e) What is the mole fraction of methanol in a solution that is 40% methanol (CH 3 OH), 40% ethanol (C 2 H 5 OH) and 20% H 2 O by mass? (Atomic weights : C = 12.01, H = 1.008, O = 16.00) a) 0.39 b) 0.49 c) 0.30 d) 0.45 e) 0.35 Page No.: 1

2 7. Plumber s solder contains 67.0% lead and 33.0% tin by weight. What is the mole fraction of tin? (Atomic weights: Pb = , Sn = ). a) b) c) d) e) Molybdenum steel contains 98.0% iron and 2.0% molybdenum by weight. What is the mole fraction of molybdenum? (Atomic weights: Fe = 55.85, Mo = 95.94). a) b) c) d) e) Sterling silver contains 92.5% silver and 7.5% copper by weight. What is the mole fraction of silver? (Atomic weights: Ag = , Cu = 63.55). a) b) c) d) e) Babbitt metal contains 90.0% tin, 7.0% antimony, and 3.0 carbon by weight. What is the mole fraction of antimony? (Atomic weights: Sn = , Sb = , C = 12.01). a) b) c) d) e) Duralumin contains 95.5% aluminum, 4.0% copper and 0.5% magnesium by weight. What is the mole fraction of copper? (Atomic weights: Al = 26.98, Cu = 63.55, Mg = 24.31). a) b) c) d) e) Type metal contains 82.0% lead, 15.0% antimony and 3.0% copper by weight. What is the mole fraction of copper? (Atomic weights: Pb = 207.2, Sb = , Cu = 63.55). a) b) c) d) e) Babbitt metal is 69.0% zinc, 19.0% tin, 4.0% copper, 3.0% antimony and 5.0% lead by weight.what is the mole fraction of copper? (Atomic weights: Zn = 65.39, Sn = , Cu = 63.55, Sb = , Pb = 207.2) a) b) c) d) e) Babbitt metal is 69.0% zinc, 19.0% tin, 4.0% copper, 3.0% antimony and 5.0% lead by weight. What is the mole fraction of zinc? (Atomic weights: Zn = 65.39, Sn = , Cu = 63.55, Sb = , Pb = 207.2) Page No.: 2

3 e) a) b) c) d) e) Pewter contains 85.0% tin, 6.8% copper, 6.5% bismuth and 1.7% antimony by weight. What is the mole fraction of bismuth?(atomic weights: Sn = , Cu = 63.55, Bi = , Sb = ). a) b) c) d) e) A solution prepared by dissolving 50.0 g of cesium chloride (CsCl) in 50.0 g of water has a density of 1.58 g/cm 3. What is the mole fraction of CsCl of the solution? (Atomic weights: Cs = 132.9, Cl = 35.45, H = 1.008, O = 16.00). a) b) c) d) e) What is the mole fraction of a 18.0% by weight of a Pb (NO 3 solution if the density is 1.18 g/cm 3? (Atomic weights: Pb = 207.2, N = 14.01, O = 16.00). a) b) c) d) e) The density of a 48.0% by weight aqueous solution of H 2 is g/cm 3. What is the mole fraction of the compound? (Atomic weights: H = 1.008, S = 32.06, O = 16.00). a) b) c) d) e) What is the mole fraction of AgNO 3 in a 1.66 molal aqueous solution? (Atomic weights: Ag = , N = 14.01, O = 16.00, H = 1.008). a) b) c) d) e) What is the mole fraction of H 3 C 6 H 5 O 7 in a 1.63 molal aqueous solution? (Atomic weights: C = 12.01, O = 16.00, H = 1.008). a) b) c) d) e) What is the mole fraction of H 2 in a 9.41 molal aqueous solution? (Atomic weights: H = 1.008, S = 32.06, O = 16.00). a) b) c) d) Page No.: 3

4 22. In a solution of ethanol and water, the mole fraction of ethanol is What is the mole fraction of water? The molecular weights of ethanol and water are 46 and 18 amu respectively. a) 0.36 b) 0.72 c) 0.55 d) 0.45 e) A solution is prepared by mixing 2.2 moles of CH 2 Cl 2, 1.2 moles of CH 2 Br 2 and 1.8 moles of CHCl 3 and 1.0 mole of CHBr 3. What is the mole fraction of CHBr 3? (Atomic weights: C = 12.01, H = 1.008, Cl = 35.45, Br = 79.9). a) 0.11 b) 0.22 c) 0.19 d) 0.13 e) A solution is prepared by mixing 2.2 moles of CH 2 Cl 2, 1.2 moles of CH 2 Br 2 and 1.8 moles of CHCl 3. What is the mole fraction of CH 2 Br 2? (At. Wt. C=12.01, H=1.008, Cl=35.45, Br = 79.9). a) 0.58 b) 0.18 c) 0.35 d) 0.42 e) What is the vapor pressure (atm) of a 1.00 m solution of a nonvolatile, nondissociating solute in water at 50 C? The vapor pressure of water at 50 C is atm. a) b) c) d) e) Ethylene glycol (C 2 O 2 ) is only slightly volatile at 100 C. Determine the vapor pressure (torr) of water at 100 C in a solution of 1.90 x 10 3 g of water and 625 g of ethylene glycol. The vapor pressure of pure water is 760 torr at 100 C. (Atomic weights: C = 12.01, H = 1.008, O = 16.00). a) 682 b) 671 c) 705 d) 694 e) What is the vapor pressure above an aqueous solution at 25 C in which 25.0 g of the nonvolatile compound urea, CO(NH 2 is dissolved in 525 g of H 2 O? The vapor pressure of water at 25 C is 23.8 mm Hg. (Atomic weights: C = 12.01, H = 1.008, O = 16.00, N = 14.01). a2.0 b3.0 c2.8 d3.5 e Which of the following aqueous solutions having the indicated mole fraction of solute should have the lowest vapor pressure of water assuming ideality? a) X(ScCl 3 ) at 25 C b) X(NH 4 ) at 25 C c) X(NaCl) at 50 C d) X(NaCl) at 25 C e) X(ScCl 3 ) at 50 C Page No.: 4

5 e) Which of the following aqueous solutions having the indicated mole fraction of solute should have the highest vapor pressure of water assuming ideality? a) X(CaCl 2 ) at 25 C b) 0.02 X(NaCl) at 50 C c) 0.02 X(NaCl) at 25 C d) X(CaCl 2 ) at 50 C e) 0.03 X(sucrose) at 15 C 30. Which of the following aqueous solutions having the indicated mole fraction of solute should have the lowest vapor pressure of water assuming ideality? a) X(CaCl 2 ) at 50 C b) 0.01 X(NaCl) at 50 C c) 0.01 X(NaCl) at 25 C d) 0.02 X(sucrose) at 15 C e) X(CaCl 2 ) at 25 C 31. What is the total pressure at 25 C of a solution of 25 g of C 6 H 14 and 50 g of C 6 H 12 at 25 C if the vapor pressures of the pure solvents are 151 and 98 mm Hg respectively at 25 C? (Atomic weights: C = 12.01, H = 1.008, Cl = 35.45). a) 134 b) 128 c) 115 d) 103 e) What is the total pressure at 25 C of a solution of 10.0 g of CH 2 Cl 2 and 1.00 g C 6 H 12 at 25 C if the vapor pressures of the pure solvents are 435 and 166 mm Hg respectively at 25 C? (Atomic weights: C = 12.01, H = 1.008, Cl = 35.45). a) 382 b) 398 c) 410 d) 402 e) Heptane, C 7 H 16, and octane, C 8 H 18, have vapor pressures of 791 torr and 352 torr at 100 C respectively. What is the vapor pressure (torr) of a solution of 25.0 g of C 7 H 16 and 35.0 g of C 8 H 18? (Atomic weights: C = 12.01, H = 1.008, O = 16.00). a) 485 b) 512 c) 549 d) 586 e) What is the mole fraction of CBr 4 in the vapor above a solution of g of CBr 4 and g C 7 at 100 C. The vapor pressure of pure CBr 4 and pure C 7 are and torr respectively at 100 C? (Atomic weights: C = 12.01, H = 1.008, Br = 79.90). a) b) c) d) e) What is the mole fraction of C 6 in the vapor above a solution of 50.0 g of benzene, C 6 and 50.0 g of toluene, C 7, at 25 C. The vapor pressure of pure benzene and toluene at this temperature are 95.1 and 28.4 mm Hg respectively. (Atomic weights : C = 12.01, H = 1.008). a) b) c) d) Page No.: 5

6 36. What is the mole fraction of CCl 4 in the vapor a solution of 50.0 g of CCl 4 and 50.0 g of CHCl3 at 25 C. The vapor pressures at 25 C for pure CCl 4 and CHCl 3 are 98.3 and torr respectively. (Atomic weights: C = 12.01, H = 1.008, Cl = 35.45). a) b) c) d) e) Azulene has the empirical formula C 5 H 4. A solution of g of azulene in g of benzene (C 6 ) boils at C. The normal boiling point of benzene is C; the K b is 2.53 C/molal. What is the molecular formula of azulene? (Atomic weights: C = 12.01, H = 1.008). a) C 5 H 4 b) C 8 H 5 c) C 15 H 12 d) C 10 e) C 3 H Acenapthalene has the empirical formula C 6 H 5. A solution of g of acenapthalene in 15.0 g CHCl 3 boils at 62.5 C. The normal boiling point of CHCl 3 is 61.7 C; the K b is 3.63 C/molal. (Atomic weights: C = 12.01, H = 1.008, Cl = 35.45). a) C 18 H 15 b) C 9 H 7 c) C 6 H 5 d) C 12 H 10 e) C A compound has the empirical formula C 10 Fe. A solution of g of the compound in g of benzene (C 6 ) boils at C. The boiling point of benzene is 80.10; the K b is 2.53 C/molal. What is the molecular formula of the compound? (At. Wt.: C = 12.01, H = 1.008, Fe = 55.85). a) C 5 H 4 Fe b) C 30 H 24 Fe 3 c) C 15 H 12 Fe d) C 20 H 16 Fe 2 e) C 10 Fe 40. A solution of g of a germicidal agent dissolved in 25.0 g of chloroform boils at C. The normal boiling point of chloroform is C and its K b is 3.63 C/molal. What is the molecular weight of the compound? a) 364 b) 404 c) 322 d) 382 e) A solution of g of a nonelectrolyte in 40.0 g of water freezes at C. What is the molecular weight of the nonelectrolyte? (K f = 1.86 C/m). a) 44.0 b) 40.0 c) 100 d) 36.0 e) The freezing point of p-dichlorobenzene is 53.1 C; its K f value is C/m. A solution of 1.26 of a sulfa drug in 10.0 g of p-dichlorobenzene freezes at 47.9 C. What is the molecular weight of the sulfa drug? Page No.: 6

7 a) 178 b) 172 c) 164 d) 186 e) The boiling point of a solution of 2.40 g of biphenyl (C 12 H 10 ) in 75.0 g of benzene (C 6 ) is C. The normal boiling point of benzene is 80.10ºC. What is the molal boiling point constant ( C/m) for benzene? (Atomic weights: C = 12.01, H = 1.008). a.7 b.3 c.2 d.0 e The freezing point of a solution of 2.40 g of biphenyl (C 12 H 10 ) in 75.0 g of benzene (C 6 ) is 4.40 C. The normal freezing point of benzene is 5.50 C. What is the molal freezing point constant ( C/m) for benzene? (Atomic weights: C = 12.01, H = 1.008). a) -4.8 b) -4.6 c) -5.6 d) -5.1 e) The freezing point of a solution of g of azulene (C 10 ) in g of camphor freezes at C. The freezing point of pure camphor is What is the molar freezing point constant (deg/molal) of camphor? Atomic weights: C = 12.01, H = 1.008). a) b) c) d) e) Which of the following solutions should have the highest freezing point? a) m ScCl 3 b) m NaCl c) m (NH 4 d) m Ce(NO 3 ) 3 e) m KNO Which of the following solutions should have the lowest boiling point? a) m Mg(OH b) 0.01 m sucrose c) m Na 2 d) m CaCl 2 e) 0.01 m NaCl 48. Which of the following solutions should have the highest boiling point? a) 0.012m ScCl 3 b) m (Ce(NO 3 ) 4 c) 0.02 m KNO 3 d) m (NH 4 e) 0.02 m NaCl 49. A m solution of K 2 in water freezes at C. What is the van t Hoff factor (i) for K 2? (K f = -186 C/m). a.49 b.10 c.20 d.00 e.32 Page No.: 7

8 50. A 1.00 g sample of Co(NH 2 CH 2 CH 2 NH 2 Cl 3 is dissolved in 25.0 g of water and the freezing point of the solution is C. How many ions are produced per mole of compound? The K f of water is -186 C/molal. (Atomic weights: Co = 58.93, C = 12.01, N = 14.01, H = 1.008, Cl = 35.45) a) 1 b) 4 c) 3 d) 5 e 51. The compound K 3 Fe(CN) 6 dissolves in water according to the following equation. A m solution of K 3 Fe(CN) 6 freezes at C. What is the van t Hoff factor (i) for K 3 Fe(CN) 6? (K f = C/m). K 3 Fe(CN) 6 3 K Fe(CN) 6 a.40 b.70 c.55 d) 3.00 e Dextran, a polymeric carbohydrate, is used as a blood plasma substitute. An aqueous solution contining g of dextran in 106 ml of solution at 21 C has an osmotic pressure of 1.47 mm Hg. What is the molecular weight of the dextran? a) 6.86 x 10 5 b) 6.85 x 10 4 c) 5.21 x 10 7 d) 7.86 x 10 5 e) 7.86 x A 0.15 g sample of a protein dissolved to give 2.0 ml of solution has an osmotic pressure of 18.6 torr at 25 C. What is the molecular weight of the protein? a) 3.8 x b) 7.5 x 10 4 c) 7.5 x 10 3 d) 1.5 x 10 5 e) 3.8 x Insulin controls glucose metabolism. A solution of 2.0 g of insulin in ml of water has an oamotic pressure of 26.1 torr at 30 C. What is the molecular weight of insulin? a) 6.8 x 10 3 b) 5.8 x 10 3 c) 3.4 x 10 3 d) 7.5 x 10 3 e) 4.2 x A g sample of an ionic compound with the formula Cr(NH 3 ) 5 Cl 3 is dissolved in water to give 25.0 ml of solution at 25 C. The osmotic pressure of the solution is 119 mm Hg. How many moles of ions are obtained from each formula unit of the compound when it is dissolved in water? (Atomic weights: Cr = 52.0, N = 14.01, H = 1.008, Cl = 35.45). a) 4 b) 3 c d) 8 e) A g sample of Cr(NH 3 ) 4 Cl 4 is dissolved in 25.0 ml of water and the osmotic pressure of the solution is 84.9 mm Hg at 25 C. How many moles of ions are produced per mole of compound? (Atomic weights: Cr = 52.00, N = 14.01, H = 1.008, Cl = 35.45). Page No.: 8

9 e) 8.19 a b) 3 c) 1 d) 5 e) A g sample of Co(NH 2 CH 2 CH 2 NH 2 Cl 3 is dissolved in 25.0 ml of water and the osmotic pressure of the solution is 52.1 mm Hg at 25 C. How many moles of ions are produced per mole of compound? (Atomic weights: Co = 58.93, C = 12.01, N = 14.01, H = 1.008, Cl = 35.45) a) 3 b c) 1 d) 5 e) Which of the following aqueous solutions should have the highest osmaotic pressure? a) 0.02 M sucrose at 15 C b) M CaCl 2 at 50 C c) 0.01 M NaCl at 25 C d) 0.01M NaCl at 50 C e) M CaCl 2 at 25 C 59. Which of the following solutions should have the highest osmotic pressure assuming ideality? a) M Na 2 b) M CaCl 2 c) 0.01 M NaCl d) M Mg(OH e) 0.01 M sucrose 60. Which of the following aqueous solutions should have the highest osmotic pressure? a) 0.008M NaCl at 25 C b) M CaCl 2 at 50 C c) 0.02 M sucrose at 25 C d) 0.02M sucrose at 50 C e) M CaCl 2 at 25 C 61. A concentrated solution of AgNO 3 is 21.9% by weight and the density is g/cm 3. How many grams of the solution are required to prepare ml of a M solution? (Atomic weights: Ag = 108, N =14, O = 16). a5.3 b1.3 c3.3 d) 19.2 e A concentrated solution of K 2 CrO 4 is 15.0% by weight and the density is g/cm 3. How many grams of the solution are required to prepare ml of a M solution? (Atomic weights: K = 39, Cr = 52, O = 16). a) 34.2 b) 41.4 c) 38.8 d) 40.5 e) A concentrated solution of (NH 4 is 36.0% by weight and the density is g/cm 3. How many grams of the solution are required to prepare ml of a M solution? (Atomic weights: N = 14, S = 32, O = 16, H = 1). a) 5.46 b) 5.93 c) 7.73 d) 6.82 Page No.: 9

10 64. Concentrated HNO 3 is 70.0% HNO 3 by mass and has a density of 1.42 g/ml. How many milliliters of this solution are required to prepare ml of a 1.20 M HNO 3 solution? (Atomic weights: H = 1, O = 16, N = 14). a) 18.0 b) 19.0 c0.0 d7.0 e Concentrated HF is 30.0% HF by mass and has a density of g/ml. How many milliliters of this solution are required to prepare ml of a 1.50 M HF solution? (At. Wt.: H = 1, F = 19). a) 39.1 b) 36.4 c) 38.2 d) 40.0 e) Concentrated H 3 PO 4 is 85.0% H 3 PO 4 by mass and has a density of 1.70 g/ml. How many milliliters of this solution are required to prepare ml of a 2.00 M H 3 PO 4 solution? (Atomic weights: H = 1, O = 16, P = 31). a) 36.2 b) 33.9 c) 38.2 d) 40.1 e) A 10.0 ml sample of concentrated HNO 3 (15.8 M) is diluted to a final volume of ml. What is the molarity of the final solution? (Atomic weights: H = 1, N = 14, O =16). a) b) c) d) e) A 10.0 ml sample of concentrated HF (16.5 M) is diluted to a final volume of ml. What is the molarity of the final solution? (Atomic weights: H = 1, F = 19). a) b) c) d) e) What volume (ml) of M Pb(NO 3 should be used to prepare 50.0 ml of a M solution? (Atomic weights: Pb = 207, N = 14, O =16). a) 4.7 b) 3.3 c) 4.4 d.9 e) What volume (ml) of M K 2 CrO 4 should be used to prepare ml of a M solution? Atomic weights: K = 39, Cr = 52, O =16). a) 13.5 b) 14.9 c) 13.9 d) 14.8 e) 14.3 Page No.: 10

11 71. What volume (ml) of concentrated HNO 3 (15.8 M) should be used to prepare ml of a M solution? (Atomic weights: H = 1, N = 14, O = 16). a) 5.83 b) 6.05 c) 6.59 d) 6.78 e) A 25.0 ml sample of a 47.0% HI solution has a density of 1.50 g/ml. The sample is diluted to a volume of L. What is the molarity of the final solution? (Atomic weights : H = 1, I = 127). a) b) c) d) e) A 50.0 ml sample of a 70.0% HNO 3 solution has a density of 1.42 g/ml. The sample is diluted to a volume of L. What is the molarity of the final solution? (Atomic weights : H = 1, N = 14, O = 16). a.48 b) 3.15 c) 4.51 d) 3.54 e A 50.0 ml sample of a 40.0% NaBr solution has a density of 1.42 g/ml. The sample is diluted to a volume of L. What is the molarity of the final solution? (Atomic weights : Na = 23, Br = 80). a) 1.97 b) c) d) e) The calcium ion content of a blood sample is mg in 1.0 ml. What is the molarity of the calcium ion? (Atomic weight : Ca = 40). a) b) c) d) e) Gatorade Thirst Quencher contains 23 mg of K + in a 250 ml glass. What is the molarity of K +? (Atomic weight : K = 39). a.4 x 10 3 b) 1.2 x 10 4 c) 3.6 x 10 2 d) 3.6 x 10 3 e.4 x Household ammonia contains 4.25 g NH 3 in a L of solution. What is the molarity of ammonia? (Atomic weights : N = 14, H = 1) a) b) 1.00 c) d) e) Page No.: 11

12 78. A solution prepared by dissolving 50.0 g cesium chloride (CsCl) in 50.0 g of water has a density of 1.58 g/cm 3. What is the molarity of the solution? (At. Wt.: Cs = 133, Cl = 35.5, H =1, O = 16). a) 5.21 b) 5.94 c) 4.69 d) 4.08 e) The density of a 32.0% by weight aqueous solution of acetone (C 3 O) is g/cm 3. What is the molarity of the compound? (Atomic weights : C = 12, H =1, O = 16). a) 7.80 b) 7.12 c) 5.74 d) 8.10 e) The density of a 56.0% by weight aqueous solution of 1-propanol (CH 3 CH 2 CH 2 OH) is g/cm 3. What is the molarity of the compound? (Atomic weights : C = 12, H = 1, O = 16). a) 13.5 b) 17.2 c) 8.36 d) 7.40 e How many moles of NaCN are in ml of 3.8 x 10 5 M NaCN (a lethal concentration of sodium cyanide in the blood)? (Atomic weights: Na = 23, N = 14, C = 12). a) 3.8 x 10 6 b) 3.8 x 10 7 c.6 x 10 5 d.6 x 10 6 e) 3.8 x How many moles of lithium chlorate (LiClO 3 ) are in 153 ml of a M soluiton? a) b) c) d) e) Determine the number of moles of solute present in 416 ml of 3.75 M HBr solution. (Atomic weights: Br = 80, H = 1). a) 1.56 b) 1.71 c) 1.89 d) 1.98 e) An iron content of 0.1 mg/l in drinking water can be detected by taste. What is the mass (mg) of iron in 1.00 L of a water sample with an iron carbonate, FeCO 3, concentration of 5.25 x 10 7 M. (Atomic weights : Fe = 56, C = 12, O =16). a.93 x 10 2 b) 4.52 x 10 2 c) 1.46 x 10 2 d) 3.89 x 10 2 e.15 x How many grams of glucose are contained in ml of 0.30 M glucose, C 6 H 12 O 6, used in intravenous injection? (Atomic weights: C = 12, H = 1, O = 16). a7 b.7 c) 1.5 d) 0.15 Page No.: 12

13 86. Determine the mass (g) of solute required to form ml of a M NaCN. (Atomic weights : Na = 23, C = 12, N = 14). a) 3.06 b.91 c.72 d.51 e) An aqueous solution of HF is 30.0% HF by mass and has a density equal to g/cm 3. What is the molality of HF in the solution? (Atomic weights : F = 19, H = 1). a) 19.2 b) 17.1 c3.6 d1.4 e) The density of a 28.0% by weight aqueous solution of LiCl is g/cm 3. What is the molality of the compound? (Atomic weights: Li = 7, Cl = 35.5). a) 9.32 b) 9.73 c) 9.01 d) 9.17 e) A 40.0% NaBr solution has a density of 1.42 g/ml. What is the molality of this solution? (Atomic weights : Na = 23, Br = 80). a) 6.21 b) 5.58 c) 6.01 d) 6.61 e) What is the molality of a solution of 25 g of ethyl alcohol (C 2 H 5 OH) in ml of benzene, C 6? The density of benzene is g/ml. (Atomic weights : C = 12, H = 1, O = 16). a) 0.62 b) 3.1 c) 0.31 d) 0.45 e) What is the molality of a solution prepared by dissolving 8.87 g of methanol, CH 3 OH, in 20.0 g of water? (Atomic weights : C = 12, H =1, O =1). a) 15.0 b) 13.8 c) 12.2 d) 13.0 e) How many grams of I 2 must be dissolved in ml of CCl 4, whose density is g/cm 3, to produce m I 2 solution? (Atomic weights : C = 12, Cl = 35.5, I = 127). Page No.: 13

14 a) 4.42 b) 17.7 c) 5.55 d) 11.1 e) The density of a M aqueous solution of K 2 CrO 4 is g/cm 3? What is the molality of the solution? (Atomic weights : K =39, Cr = 52, O =16). a) b) c) d) The density of a 1.57 M aqueous solution of AgNO 3 is g/cm 3? What is the molality of the solution? (Atomic weights : Ag = 108, N = 14, O =16). a) 1.65 b) c) 1.42 d) 1.58 e) A solution of vinegar is M in acetic acid, C 2 H 4 O 2. The density of vinegar is g/ml. What os tje molal concentration of acetic acid? (Atomic weights : C =12, H = 1, O = 16). a) b) c) d) e) What is the molality of a AgNO 3 solution with a mole fraction of ? (Atomic weights: Ag = 108, N = 14. O = 16, H = 1) a) 1.75 b) 1.65 c) 1.52 d) 1.82 e) Concentrated hydrochloric acid contains 1.00 mole of HCl dissolved in 3.31 mole of H 2 O. What is the molal concentration of HCl? (Atomic weights : Cl = 35.5, H = 1). a) 15.9 b) 16.8 c) 14.6 d) 16.3 e) A solution of methylene chloride (CH 2 Cl 2 ) in benzene (C 6 ) has a mole fraction of What is the molality of CH 2 Cl 2? (Atomic weights : C = 12, H = 1, Cl = 35.5) a) 0.32 b) 3.20 c) 3.00 d) 0.28 e.80 Page No.: 14

15 A N S W E R S 1. e 16. d 31. c 46. b 61. c 2. e 17. d 32. c 47. b 62. c 3. e 18. d 33. c 48. b 63. c 4. a 19. d 34. b 49. e 64. b 5. a 20. d 35. b 50. e 65. b 6. a 21. d 36. b 51. e 66. b 7. c 22. e 37. d 52. b 67. e 8. c 23. e 38. d 53. b 68. e 9. c 24. e 39. d 54. b 69. e 10. c 25. d 40. b 55. b 70. e 11. c 26. d 41. b 56. b 71. e 12. c 27. d 42. b 57. b 72. b 13. c 28. d 43. e 58. b 73. b 14. c 29. d 44. e 59. b 74. b 15. c 30. d 45. e 60. b 75. a 76. a 91. b 77. a 92. b 78. c 93. a 79. c 94. a 80. c 95. a 81. a 96. b 82. a 97. b 83. a 98. b 84. a 85. a 86. a 87. d 88. d 89. d 90. b Page No.: 15