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SOLUTIONS OF ELECTROLYTES

SOLUTIONS OF ELECTROLYTES. Battery. Electrons. + -. Anode (+) oxidation. Cathode (-) reduction. Cations. +. -. Anions. Electrolysis. Ohm’s law. 1 coul = 3x10 9 esu. transference number. Electrolytic cell. Faraday’s Laws.

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SOLUTIONS OF ELECTROLYTES

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  1. SOLUTIONS OF ELECTROLYTES

  2. Battery Electrons + - Anode (+) oxidation Cathode (-) reduction Cations + - Anions Electrolysis Ohm’s law 1 coul = 3x109 esu transference number Electrolytic cell

  3. Faraday’s Laws The passage of 96,500 coulombs (=F) of electricity through a conductivity cell produces a chemical change of 1 gram equivalent weight of any substance Charge of electron: 1 gram equivalent 6.1023 charges e=96500/ 6.1023 =1.6x10-19 coul/electron =4.8x10-10 esu/electon

  4. + - - + - + + + - - + + + - + - - + - + + - - + - + + - Electrolyte Polar solvent Theory of Electrolytic Dissociation Arrhenius Theory: Strong electrolytes H2O + Na+Cl- = Na+ + Cl- + H2O H2O + HCl = H3O+ + Cl- Weak electrolytes H2O + CH3COOH = H3O+ + CH3COO-

  5. Ionization Degree AB = A+ + B-  = [A+ ]/[AB]o = [B-]/[AB]o [AB]o = [A+ ] + [AB] Strong electrolytes:  0.3 Weak electrolytes:  < 0.3

  6. Weak Electrolytes AB = A+ + B-

  7. Colligative Properties i  2 for NaCl and CaSO4 i  3 for CaCl2 and K2SO4 i  4 for FeCl3 and K3Fe(CN)6

  8. Strong Electrolytes + + - + - Ion “atmosphere” - + + - + - - + - + - + - + - + - - + +

  9. - + + - + - - + - + - + - + - + - - + + Debye-Huckel Theory Ionic Strength Low concentration of electrolyte High concentration of electrolyte

  10. Solubility Product AgClsolid = Ag+ + Cl- • What is the solubility of silver chromate (s, M) in aqueous solution containing 0.04M silver nitrate ? Ag2CrO4 = 2Ag+ + CrO42- Ksp = 2x10-12 (Reference literature) Ksp = [Ag+]2[CrO42-] = (2s + 0.04)2.s s = [Ag2CrO4]  2 x 10-12/1.6 x 10-3 = 1.25 x 10-9 M

  11. Effect of Ionic Strength on Solubility AgClsolid = Ag+ + Cl- Ksp = aAg+.aCl- = +[Ag+]. -[Cl-] [Ag+].[Cl-] = Ksp /2 • Calculate solubility of silver chloride (s, M) in 0.1M ammonium sulfate. Ionic strength of 0.1 M (NH4)2SO4 = 0.3; activity coefficient = 0.7. AgCl = Ag+ + Cl- Ksp = 1.76x10-10 (Reference literature) s2 = Ksp /2 s= (1.76 x 10-10)1/2/0.7= 1.9 x 10-5 M

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