Neutralization Reactions Main Concept: In a neutralization reaction protons are transferred from an acid to a base.

Neutralization Reactions Brønsted-Lowry Acids and Bases Neutralization Examples

Brønsted-Lowry acid/base definition: - Acids: species that are able to donate protons (often in the form of H+) - Bases: species that are able to accept protons OR produce ions that can accept protons (ex: NaOH, KOH, etc)

acid + base ↔ conjugate base + conjugate acid In any neutralization reaction, we see… acid + base ↔ conjugate base + conjugate acid

Examples of acids and conjugate bases: HCl  Cl- H2O  OH- H2SO3  HSO3- HSO3  SO32- Examples of bases and conjugate acids: NH3  NH4+ H2O  H3O+ HSO3-  H2SO3

- The amphoteric* nature of water plays an important role in the chemistry of aqueous solutions, since water can both accept protons from and donate protons to dissolved species. * Able to act as both an acid and a base

In acid-base reactions: - Only reactions in aqueous solutions are considered - When an acid or base ionizes in water, conjugate acid-base pairs can be identified and relative strengths compared