1 / 14

Electrolytes

Electrolytes. Electrolytes. Are substances that form positive(+) and negative (-) ions in water Conduct an electric current. Electrolytes in the Body. Carry messages send to and from the brain as electrical signals Maintain cellular function with the correct concentrations electrolytes.

kelly-caldwell
Download Presentation

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. Electrolytes

  2. Electrolytes • Are substances that form positive(+) and negative (-) ions in water • Conduct an electric current

  3. Electrolytes in the Body • Carry messages send to and from the brain as electrical signals • Maintain cellular function with the correct concentrations electrolytes

  4. Strong Electrolytes are 100% ionized saltsH2O 100%ions NaCl(s) Na+(aq) + Cl-(aq) H2O CaBr2(s) Ca2+(aq) + 2Br- (aq) acidsH2O HCl(g) H3O+(aq) + Cl-(aq)

  5. Weak electrolytes • Most of the solute exists as molecules in solution • Only a few solute particles produce ions HF + H2O  H3O+(aq) + F- (aq) acid NH3 + H2O  NH4+(aq) + OH- (aq) base

  6. Classification of electrolytes • Acids Binary acids • Ternary acids (oxyacids) • Thioacids • Monoprotic acids • Polyprotic acids • Strong acids • Weak acids

  7. Bases Monovalent • Polyvalent • Strong • Weak • Basic oxides – base anhydrides • Oxides of metals • Salts Strong electrolytes!!!

  8. Important Facts • HCl, HNO3 – strong acids • 100% dissociation (no equilibrium, no K) • HCl  H+ + Cl– • 0%HCl, 100% H+, 100% Cl– • H+ is a proton, a subatomic particle and does not exist alone in solution • Really H+ + H2O  H3O+ (hydronium ion) HNO3 + H2O  NO3– + H3O+

  9. conc. of ionic form a = total concentration a ≤1 Strong electrolytes weak electrolytes Degree of dissociation: a Strong electrolyte: a1 Weak electrolyte: a < 0.5

  10. _ +     H H H H+ Cl- H _ O O + H O O H H H Conductivity of electrolytes

  11. H O Na+OH- H O H H H O O H H H 1 Conductivity=  + 1 cm 1 cm ( = resistance) V = 1 cm3

  12. H2SO4 NH4Cl NaCl cc.  =specific conductivity 

  13. v a = inf Equivalent conductivity:  Conductivity of equivalent amount of electrolyte  = V V = equivalent dilution in cm3 ainf = 1 v = a

  14. 400 300 200 100 cc. ( ) 1 10-4 10-5 10-1 10-2 10-3 10 Strong acid Strong base Weak acid Weak base Salt

More Related