This post will be an introduction to the Bronsted-Lowry Model of acids and bases for QCE Chemistry.
What Model of Acids and Bases do we Use?
3.1.4 – Brønsted-Lowry Model
- Recognise that the relationship between acids and bases in equilibrium systems can be explained using the Brønsted-Lowry model and represented using chemical equations that illustrate the transfer of hydrogen ions (protons) between conjugate acid-base pairs
The Bronsted-Lowry Model
This video will introduce you to the Brønsted-Lowry Theory of Acids and Bases. You will learn that acids are proton donors and bases are proton acceptors.
The Bronsted-Lowry Model is a widely used concept in the field of Chemistry that defines the nature of acids and bases. It considers an acid as a substance that donates a hydrogen ion (H+) to a solution, while a base is defined as a substance that can accept a hydrogen ion. This model can be applied to a wide range of chemical reactions, making it a flexible definition for both strong and weak acids and bases. In a reaction between an acid and a base, the acid donates a hydrogen ion to the base, creating a new substance.
This video goes through the definition in a little more depth.
This model can be used in both gaseous and aqueous phases, providing a comprehensive understanding of the behavior of acids and bases in different environments. The Bronsted-Lowry Model provides a fundamental basis for understanding a range of chemical reactions, from simple proton transfer reactions to complex chemical processes in living organisms. This model’s versatility and wide application make it a crucial concept in the study of chemistry.
Want to learn more in order to prepare for your Chemistry exam at the end of the year? Check out more of our QCE Chemistry resources here!
