The ARRHENIUS ACID-BASE THEORY

In 1884, Swedish chemist Svante Arrhenius defined acids as compounds that produce H ions in aqueous solutions, and bases as compounds that produce OH ions in aqueous solutions. For example, HCl and HNO3 are Arrhenius acids. 

NaOH and Ba(OH)2 are examples of Arrhenius bases. These bases release OH ion in aqueous media. 

In water, the H ion of an acid is attracted to a water (H2O) molecule to produce hydronium ion (HgO ). 

The Arrhenius acid-base theory is insufficient to explain the acidic or basic properties of some substances, such as SO2 and NH3, since these don t have H and OH ions in their structures. For these molecules, another theory must be applied, since the Arrhenius acid-base theory can only be applied to aqueous solutions. 

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Our goal in this chapter is to help you understand the equilibrium systems involving acids and bases. If you don t recall the Arrhenius acid-base theory, refer to Chapter 4 on Aqueous Solutions. You will learn a couple of other acid-base theories, the concept of pH, and will apply those basic equilibrium techniques we covered in Chapter 14 to acid-base systems. In addition, you will need to be familiar with the log and 10 functions of your calculator. And, as usual, in order to do well you must Practice, Practice, Practice. 

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