Ch 14 Outline Acid and Bases

Chapter 14 Outline * 14.1 The Nature of Acid and Bases * Acid-Base Theories * Arrhenius- Acid is a hydrogen producer and a base is a hydroxide producer * Bronsted-Lowry- Acid is a proton donor and a base a proton acceptor * Lewis- An acid is an electron pair acceptor, and I base is an electron pair donor * Conjugate base & acids * Ka= [products]/[reactants] * Acid dissociation constant * 14.2 Acid Strength * In a strong acid dissociate almost 100% * Ka is large * Strong acid yields weak conjugate base * Weak Acid * Does not dissociate much * The weaker the acid, the stronger conjugate base * H2SO4(aq)--->H+(aq) +H SO4- * Oxyacid * Acidic proton attached to an oxygen atom * Amphoteric * Water is the most amphoteric substance * Kw- 1.0 x 10^-14 * 14.3 The pH scale * pH scale * Provides a convenient way to represent solution acidity * The number of decimal places is equal to the number of sig figs in the original number * pH decreases as [H+] increases * pH + pOH= 14 * 14.4 Calculating the Ph of a Strong Acid Solution * Major species * HCl major species are H+ Cl- H20 * 14.5 Calculation the pH of a weak acid * Always write the major species first * THE WEAK EAT RICE * Reaction
Initial
Change
Equilibrium
* Validate * [x]/[initial concentration] X 100 * It HAS to be less than 5% * The equation of validity is the same as percent dissociation * 14.6 Bases * Strong Bases * LiOH * NaOH * KOH * Ca(OH)2 Slaked lime * Sr(OH)2 * Ba(OH)2 * Weak bases… everything else with an OH- * Amines * Methylamine- CH3 * Dimethylamine-(CH3)2NH *