CEM142 1nd Edition Lecture 6Outline of Last Lecture I. LeChatlier’s PrincipleOutline of Current Lecture II. Aqueous equilibriaIII. ElectrolytesIV. Acids/basesCurrent Lecture-review from last lecture-K = [products]/[reactants]-Q = [products]/[reactants] -same equation as for K, but used with a reaction that is not at equilibrium-electrolytes: something that can yield ions-strong electrolytes: complete dissociation-NaCl Na+ + Cl--weak electrolytes: only dissociate partially-CH3COOH CH3COO- + H+-extremely weak electrolyte: non-electrolyte-CH4 CH3- + H+ (reaction rarely/never occurs)-most important electrolyte: H2O-H2O H+ + OH--H2O + H2O H3O+ + OH--K = [H3O+][OH-]/[H2O]2These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.-Kw=equilibrium constant of water = [H3O+][OH-] = 10-14-with pure water at 25 degrees Celsius… [H3O+] = [OH-]-pH-pH = -log[H3O+]-pOH = -log[OH-]-pKw = pH + pOH-strong acids:-HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4-strong bases: -NaOH, KOH-weak acids: -HCN, HF, H3PO4, H2CO3-weak
View Full Document
Unlocking...