Equilibrium chemistry

1 Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry Model 1. Acids are proton donors 2. Bases are proton acceptors 3. H3O+ is called the hydronium ion C. Conjugate Acid-Base Pairs 1. A conjugate base is what remains after an acid has donated a proton a. Cl- is the conjugate base of HCl 2. A conjugate acid is what is formed when a base accepts a proton base acid acid base 3. HCl is a stronger base than H3O+ (H+) so the equilibrium lies far to the right D. Acid Dissociation Constant 1. ][ ]][[ HCl ClHKa -+ = a. water is not included because, in dilute solution, the concentration of

AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's is low (2.1) 2. Water is a bent molecule 3. Water is a polar molecule B. Hydration of Ionic Solute Molecules 1. Positive ions attracted to the oxygen end of water 2. Negative ions attracted to the hydrogen end of water C. Hydration of Polar Solute Molecules 1. Negative end of polar solute molecules are attracted to water's hydrogen 2. Positive end of polar solute molecules are attracted to water's oxygen D. "Like Dissolves Like" 1. Polar and ionic compounds dissolve in polar solvents like water 2. Nonpolar compounds like fats dissolve in nonpolar solvents like ____ ?_____