The correct definition of an acid and a base that states an acid is an electron-pair acceptor and a base is an electron-pair donor is known as the Bronsted-Lowry definition.
Here's a breakdown to help you understand:
1. **Bronsted-Lowry Definition**:
- According to the Bronsted-Lowry definition, an acid is a substance that can donate a proton (H+) while a base is a substance that can accept a proton.
- In this context, acids and bases are related to the transfer of protons (hydrogen ions) between molecules.
- For example, in the reaction HCl (hydrochloric acid) + H2O (water) → Cl- (chloride ion) + H3O+ (hydronium ion), HCl donates a proton and acts as an acid, while water accepts the proton and acts as a base.
Understanding the Bronsted-Lowry definition is important in the study of acids and bases as it provides a more inclusive and versatile understanding compared to the Arrhenius definition, which defines acids as substances that release H+ ions in water and bases as substances that release OH- ions in water.
