Brønsted-Lowry Base
| Formula / Notation | B + HA → BH⁺ + A⁻ |
|---|---|
| Also Known As | Proton acceptor, Brønsted base, Lewis base (partially overlapping concept) |
What is Brønsted-Lowry Base?
A Brønsted-Lowry base is any species that accepts a proton (H⁺) from another species. This definition, proposed in 1923, is broader than the Arrhenius definition and includes species such as ammonia (NH₃) and carbonate ions that accept protons without producing OH⁻ directly. Every Brønsted-Lowry base has a conjugate acid formed by gaining a proton.
Formula & Notation
Other Names / Synonyms: Proton acceptor, Brønsted base, Lewis base (partially overlapping concept)
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A Brønsted-Lowry base is any species that accepts a proton (H⁺) from another species. This definition, proposed in 1923, is broader than the Arrhenius definition and includes species such as ammonia (NH₃) and carbonate ions that accept protons without producing OH⁻ directly. Every Brønsted-Lowry base has a conjugate acid formed by gaining a proton.
Brønsted-Lowry base theory explains the action of antacids, detergents, biological catalysts, and industrial basic processes (saponification, Haber process NH₃ as base). It is fundamental to pharmaceutical formulation and biochemical pH buffering.
Strong Brønsted bases (NaOH, KOH, Ca(OH)₂) are corrosive and cause deep chemical burns. Splashes cause severe eye damage. Use alkali-resistant PPE, work in ventilated areas, and have eyewash stations readily accessible. Neutralise spills with dilute acid or citric acid.
The formula or notation for Brønsted-Lowry Base is: B + HA → BH⁺ + A⁻