Acid-Base Equilibria and Solubility

In this chapter, we will continue the study of acid-base reactions with a discussion of buffer action and titrations. We will also look at another type of aqueous equilibrium— that between slightly soluble compounds and their ions in solution. 

1 The Ionization of Weak Acids and Bases Is Suppressed by the Addition of a Common Ion 612 

3 The Concentration of an Unknown Acid or Base Can Be Determined by Titration 622 

4 An Acid-Base Indicator Is a Substance That Changes Color at a Specific pH 631 

5 A Precipitation Reaction Occurs when a Reaction in Solution Leads to an Insoluble Product 633 

---

Note that it is general practice not to inclnde nnits for the eqnilibrinm constant. In thermodynamics, K is defined as having no nnits because every concentration (molarity) or pressure (atm) term is actually a ratio to a standard value, which is 1 M or 1 atm. This procedure eliminates all units but does not alter the numerical parts of the concentration or pressure. Consequently, K has no units. Later we will extend this practice to acid-base equilibria and solubility equilibria (to be discussed in Chapters 15 and 16). 

In this part of your study of general chemistry, it is typical to explore how a chemical system comes to equilibrium and how that equilibrium is represented. Interpretation of equilibrium constants, calculation of concentrations in equilibrium systems, equilibrium in gas phase reactions, relationship of enthalpy to equilibrium, acid-base equilibria, and solubility equilibria all fall into this area of study. 

CHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA... 

---