1 / 11

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.

maik
Download Presentation

SOLUTIONS OF ELECTROLYTES

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  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

More Related