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

2. Neutralization Reactions
Brønsted-Lowry Acids and Bases
Neutralization
Examples

3. 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)

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

5. 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

7. - 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

8. 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