Chapter 16: Acid-Base Equilibria. 16.1. Acids and Bases: A Brief Review 16.2 Brønsted -Lowry Acids and Bases 16.3 The Autoionization of Water 16.4 The pH Scale 16.5 Strong Acids and Bases 16.6 Weak Acids 16.7 Weak Bases 16.8 Relationship Between Ka and Kb
Arrhenius defined an acid as a substance that produces H+ ions in water; he defined a base as a substance that produces OH– ions in water. HCl—one of the strong acids—is an Arrhenius acid. Potassium hydroxide—one of the strong bases—is an Arrhenius base.
What is the pH of a 1.75 10–3M nitrous acid solution?
The ionization equilibrium expression for nitrous acid is
ClO- + H2O HClO + OH-
3.3 x 10-7 =
= 46 g NaClO