Ionic Equilibria in Aqueous Systems

Creating Coral Many remarkable natural formations, such as caves and reefs, arise through the subtle interplay of the aqueous ionic equilibria that you ll study in this 

The dissolution in water of a slightly soluble ionic compound reaches an equilibrium characterized by a solubility-product constant, Kgp, that is much less than 1. Addition of a common ion lowers such a compound s solubility. Lowering the pH (adding HsO ) increases the solubility if the anion of the ionic compound is that of a weak acid. 

A complex ion consists of a central metal ion bonded to molecules or anions called ligands. Complex ions form in a stepwise process characterized by a formation constant, K, that is much greater than 1. Adding a ligand increases the solubility of a slightly soluble ionic compound if the ligand forms a complex ion with the ionic compound s cation. 

The Common-Ion Effect The Henderson-Hasselbalch Equation Buffer Capacity and Range Preparing a Buffer 

Acid-Base Indicators Strong Acid-Strong Base Titrations Weak Acid-Strong Base Titrations Weak Base-Strong Acid Titrations 

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Of the numerous definitions of acids and bases that have been employed over the years, the 1923 definitions of J. N. Brpnsted and T. M. Lowry have proven to be the most useful for discussions of ionic equilibria in aqueous systems. According to the Brpnsted-Lowry model, an acid is a substance capable of donating a proton to another substance, such as water ... 

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