Example of Brønsted – Lowry acid-base:
HCl (aq) + H2O (l) → Cl− (aq) + H3O + (aq)
When viewed with the Brønsted-Lowry theory, in the ionization reaction of HCl when dissolved in water, HCl acts as an acid and H2O as a base. The HCl turns into a Cl− ion after giving a proton (H +) to H2O. H2O accepts protons by using a pair of free electrons in the O atom to bind to H + to form hydronium ions (H3O +).
Examples of Lewis Acid Bases:
H ++ NH3 → NH4 +
Ion H + (Proton) is a Lewis Acid because it can accept Electron Pairs, while NH3 is a Lewis Base.
<h2>Further Explanation
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Acid is a compound that makes a sour taste. A base may be a compound that reacts with acids.
The Brønsted – Lowry acid-base theory
The Brønsted-Lowry Theory is an acid-base reaction theory proposed separately by Johannes Nicolaus Brønsted and Thomas Martin Lowry in 1923. The basic concept of this theory is that when an acid and a base react with each other, acids will form their conjugate bases, and bases form their conjugate acids through proton exchange (hydrogen cations, or H +). This theory could be a generalization of the Arrhenius theory.
Lewis Acid-Base Theory
In 1923, G. N. Lewis proposed a broader acid-base theory compared to the two previous theories by emphasizing the electron pair associated with structure and bonding. According to the definition of Lewis acid-base:
- acid is an electron pair acceptor.
- bases are electron-pair donors.
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Grade: College
Subject: Chemistry
keywords: The Brønsted – Lowry acid-base theory, Lewis Acid-Base Theory
