CHEM 1062 Lecture Notes - Lecture 18: Sulfuric Acid, Electronegativity, Sodium Hydroxide
Document Summary
Acid - arrhenius dissociates to give a proton h+which is hydronium. Base - arrhenius dissociates to make an oh- Chapter 18 lecture notes - acids and bases. Works in water, not inclusive definition because it only looks at h. Bronsted lowry definition - valid in every solvent; default definition. Lewis definition - examines electron movement instead of protons (more encompassing) Use bronsted lowry definition - acids and bases are equilibrium involve the transfer of an h+ Conj acid/base pair differ only by one h+ Nh3(aq) + h2o (l) < --- > nh4. Ch3cooh (aq) + h2o(l) < --- > ch3coo- (aq) + h3o+(aq) Water(l) as a solvent can be an acid or base. H2o (l) + h2o (l) < --- > oh-(aq) + h3o+(aq) Kw = [oh-][h3o+] = 1. 0 * 10-14 m2 at 25 degrees c. Pure water: [oh-] = [h3o+] = 1. 0 * 10 -7 m2 at 25 degrees c ph = -log[h3o+]
