HW15-G1- Solution Properties

# HW15-G1- Solution Properties - 1. 4. 5. CO 10. Exercise Set...

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Unformatted text preview: 1. 4. 5. CO 10. Exercise Set 1 5 Solution Properties CHM 2045 HW12-Gi~Liq—Sol.wpd why does fresh water evaporate faster than seawater under the same condi‘ tions? The concentrations of two solutions (nonvolatile, nonelectrolytic solutes) are as follows: N0. 1, 5.0 g of ethylene glycol, C2H602, in 100 g of water; NO. 2, 8.0 g of glucose, C5H1206, in 100 g of water Which solution has the higher (a) vapor pressure, (b) boiling point, (c) freezing POlnt? What are the freezing and boiling points of a solution prepared by dissolv— ing 10.0 g of glucose, C6H1206’ in 40-0 9 H20? The freezing point of an aqueous solution of a nonelectrolyte is -0.160°C. What would be the expected normal boiling point of the same solution? Arrange the following aqueous solutions in the expected order of decreasing freezing points: 0.01 m NaCl, 0.02 m Mg504, 0.01 m MgClZ, 0.005 m KBr, 0.025 m HCl, 0.015 m CZHSOH Calculate the freezing point of a 0.700 m solution of K2304. _The percentage ionization of weak acid HX in water is known to be 10.0 per— cent for a 0.200 m solution. What is the freezing point of the solution? The freezing point of a 0.010 m solution of H2504 is 0.0047°C. Show that this is consistent with 100 percent ionization of the acid according to the reaction H2304 -as~H+1 + Hso4-1 and 50 percent ionization of the resultant H304— Hso4—1 .—e> n+1 + 504-2 l The addition of 1.10 g of an unknown compound reduces the freezing point of 78.22 g benzene from 5.51°C to 4.90°C. What is the molecular weight of the 0 unknown compound? k§C£*“§M*3 =‘ 53'1 é% Arrange the following aqueous solutions in order of their increasing vapor pressures: (a) 0.1 m NaCl (a) 0.1 m CH3OH (c) 0.1 m CaClg , (d) 0.2 m KCl 11. 12. 13. 14. 16. 17. Benzene, C5H6, and toluene, C7H8, form ideal solutions. At 60°C the vapor pressure of pure benzene is 0.507 atm and the vapor pressure of pure tolu- ene is 0.184 atm. What is the vapor pressure at 60°C of a solution con— taining 6.5 g of benzene and 23.0 g of toluene? Liquids A and B ionn ideal solutions. The vapor pressure of pure 8 is 0.650 atm at the boiling point of a solution prepared from 0.200 mole of B and 0.600 mole of A. (a) What is the vapor pressure of pure A at this temperature? (b) What is the mole fraction of A in the vapor that is in equilibrium with this solution when the solution first begins to boil? A solution containing 1 mole of chloroform and 4 moles of acetone has a vapor pressure of 0.400 atm at 35°C. At this temperature the vapor pres» sure of pure chloroform is 0.359 atm and that of acetone is 0.453 atm. (a) What would the vapor pressure of the solution be it chloroform and acetone formed ideal solutions? (b) Does the vapor pressure of the solution show a positive or negative deviation from that predicted by Raoult's law? (c) Is heat evolved or absorbed when this solution is prepared? Describe the composition changes of the distillate and the residue as a 50—50 mixture of benzene (8P 80°C) and toluene (BP 111°C) is distilled. Which of the following solutions exhibits the largest osmotic pressure? (a) 0.1 M C12H22011 (b) 0.1 M NaCl (C) 0.1 M CH3C02H What is the osmotic pressure of 1.00 g of aspirin (C9H804) in 100 ml of solution at 25°C? The average osmotic pressure of blood is 7.7 atm at 37°C (human body tem— perature). What concentration of glucose, C5H1205, Will be isotonic with blood? ...
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## This note was uploaded on 11/16/2011 for the course CHM 2045 taught by Professor Mitchell during the Fall '07 term at University of Florida.

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HW15-G1- Solution Properties - 1. 4. 5. CO 10. Exercise Set...

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