Properties of Solutions. Solution
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1 Properties of Solutions Solution Formed when one substance is uniformly dispersed throughout another Solutions form when solute-solvent intermolecular forces are comparable to those between the solute-solute and solvent-solvent molecules
2 Enthalpy of solution can be either Exothermic MgSO + ( x + y )H O Mg (H O) + SO (H O) x 4 2 y H = 91. 2kJ / mol soln or Endothermic NH NO + ( x + y )H O NH ( H O ) + NO ( H O ) x 3 2 y H = kJ / mol soln Both are spontaneous!
3 Spontaneity & Disorder Processes in which the energy content of the system decreases tend to occur spontaneously Exothermic processes tend to be spontaneous Endothermic processes can be spontaneous if the entropy change is positive Entropy measures disorder Criterion for spontaneity is G < 0 G = H T S
4 Solubility Given that one material dissolves in another what determines how much? Solubility of NaCl 35.7 grams in 100 ml water
5 Enthalpy of Solution-Components Hsoln = H1+ H2 + H 3 Solubility (continued)
6 Polar liquids tend to dissolve in polar solvents Non-polar liquids tend to be insoluble in polar solvents Non-polar liquids tend to be soluble in non-polar solvents Liquids that mix in all proportions are miscible Liquids that do not dissolve in one another are immiscible like dissolves like
7 Entropy of Mixing S = R( η lnx + η lnx ) mix a a b b
8 Saturated Solution
9 Pressure & Temperature Effects
10 Pressure has no effect on the solubility of liquids & solids Pressure has a large effect on the solubility of gases Henry s Law
11 The solubility of a gas is directly proportional to the partial pressure of the gas above the solution S (mol / L) = kp (atm) gas gas k depends on the solvent as well as the dissolved gas k for N 2 in water at 25 0 C is 6.8 x 10-4 mol/l-atm Solubility of ionic solids in water increases with increasing temperature
12 Colligative Properties Depends on the concentration of the solute but not on its identity Vapor pressure lowering
13 Adding a non-volatile solute to a solvent always lowers the vapor pressure of the solution P = X P 0 A A A Raoult s law 0 P A vapor pressure of pure A X A mole fraction of A in solution P A vapor pressure of A above solution
14 Example of Raoult s Law What is the vapor pressure of a solution made by adding 50.0 ml of glycerin (non-volatile) to ml of water at 25 0 C? Density of glycerin (C 3 H 8 O 3 ) 1.26g/mL Vapor pressure of pure water at 25 0 C 23.8 torr Ideal Solution
15 A mixture of two or more volatile components, each of which obeys Raoult s law = soln 0 = soln 0 A A A B B B P X P & P X P Ptotal = PA + PB X A + X = B 1 Mole fraction of A and B in Vapor vapor A P = A = X & X P total vapor B P P B total
16 Solution of benzene (C 6 H 6 ) and toluene (C 7 H 8 ) made by mixing 1.0 mol benzene and 2.0 mol toluene soln soln X = 1/ 3 & X = 2/ 3 B P = 75torr & P = 22torr 0 0 B T 75torr PB = = 25torr 3 2 PT = 22 torr = torr 3 T P = P + P = 39. 7torr X total B T Vapor B = P B 25.torr 0 P = 39. 7torr = total 063. Boiling Point Elevation
17 Consequence of the lowering of the vapor pressure of a solvent by the addition of a non-volatile solute T = K m b b b m the molality K the molal boiling point elevation constant Freezing Point Depression
18 Consequence of the lowering of the vapor pressure of a solvent by the addition of a non-volatile solute T = K m f f m the molality f K the molal freezing-point depression constant Boiling Point Elevation
19 & Freezing Point Depression What is the boiling-point and the freezing-point of a 25% by mass aqueous solution of ethylene glycol (C 2 H 6 O 2 )? Osmosis Net movement of a solvent through a semipermeable membrane from a region of low solute concentration to one of high solute concentration
20
21 Osmotic Pressure Osmotic pressure given by π V = nrt or n π = RT = MRT V What is the osmotic pressure of a M aqueous solution of sucrose (C 12 H 22 O 11 ) at 20 0 C?
22 hypotonic, isotonic & hypertonic Solution A is hypotonic relative to B if Π A is greater than Π B Solution A is isotonic relative to B if Π A = Π B Solution A is hypertonic relative to B if Π A is less than Π B
23 Reverse Osmosis One can stop the flow of solvent into the more concentrated solution by applying pressure to the concentrated solution equal to its Osmotic pressure One can even drive the process in the opposite direction by increasing the pressure on the concentrated solution in excess of the Osmotic pressure Used to desalinate water
24 All colligative properties can be used to determine the molecular mass of a material A solution contains 3.50mg of protein dissolved in water so that the volume of the solution is 5.00mL. The osmotic pressure at 25 0 C was measured to be 1.54 torr. What is the molecular weight of the protein? Example of Molality & Molarity Solution contains equal masses of water and glycerol (C 3 H 8 O 3 ) and has a density of 1.10g/mL. Calculate
25 molality of glycerol mole fraction of glycerol molarity of glycerol
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