Apply the general method for solution equilibrium calculations outlined on page 720 to determine the pH values of the following solutions. In applying the method, look for valid assumptions that may simplify the numerical calculations. (a) a solution that is 0.315 M and 0.250 M (b) a solution that contains 1.55 g and 12.5 g in 375 mL (c) 1.0 M NH4CN1aq2
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. H 3 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
