Bronsted Lowry Acid Definition
Substances which donates a proton or H+ ion to another compound are called Bronsted Lowry Acids.
Acid ⇋ Proton + Conjugate Base
Bronsted Lowry Acids Examples
Some examples of Bronsted Lowry Acids are
- Hydrochloric Acid (HCl): It donates a proton (H⁺ ion) when dissolved in water.
- Sulfuric Acid (H2SO4): Contains two acidic hydrogen atoms and can release two protons sequentially.
- Acetic Acid (CH3COOH): An organic acid that donates a proton from its -COOH group.
- Water (H2O): Acts as both an acid (donating H⁺) and a base (accepting H⁺) in various reactions.
What Is Bronsted–Lowry Theory?
Bronsted-Lowry Theory, also called the Proton Theory of Acid and Base, is a theory that explains the concept of acid and base. It was given by Johannes Nicolaus Bronsted (Danish Chemist) and Thomas Martin Lowry (English Chemist) in 1923.
In this article, we will learn about, Bronsted Lowry’s Theory Definition, Examples, and others in detail.
Table of Content
- What is Bronsted Lowry Theory?
- Bronsted-Lowry Acids and Base
- Advantages of Bronsted Lowry Theory of Acid and Base
- Disadvantages of Bronsted Lowry Theory
- Applications of Bronsted Lowry Theory of Acid and Base
- Difference between Arrhenius Theory, Bronsted-Lowry Theory, and Lewis Acid-Base Theory