Brønsted–Lowry acid–base theory

The Brønsted–Lowry theory, also known as the proton theory of acids and bases, helps us understand how acids and bases work together. This theory was created in 1923 by two scientists: Johannes Nicolaus Brønsted from Denmark and Thomas Martin Lowry from the United Kingdom.

In simple terms, when an acid and a base react, the acid gives away a proton (a tiny part of an atom called a hydrogen cation, written as H⁺), and the base accepts it. After this, the acid becomes its conjugate base, and the base becomes its conjugate acid.

This theory helps us understand acid–base reactions better than the older Arrhenius theory. It shows that acids and bases are linked through the sharing of protons, which is important in many chemical processes.

Definitions of acids and bases

Johannes Nicolaus Brønsted and Thomas Martin Lowry had an idea about acids and bases. They said that acids give away tiny parts called protons (H⁺), and bases take those protons.

Before this, the Arrhenius theory said acids are things that break apart in water to make H⁺ (hydrogen cations or protons), and bases are things that break apart to make OH⁻ (hydroxide ions).

Brønsted and Lowry’s theory, made in 1923 by physical chemists, looks at how acids and bases react together. When they react, the acid becomes something called its conjugate base, and the base becomes its conjugate acid. This happens by sharing a proton. For example, if you have an acid called HA and a base called B, they can react like this:

HA + B ⇌ A⁻ + HB⁺

The double arrow (⇌) shows the reaction can go both ways. The acid HA gives away a proton to become A⁻, and the base B takes the proton to become HB⁺. Most of these reactions happen quickly and the substances stay balanced with each other.

Aqueous solutions

Acids and bases can react by sharing a tiny part called a proton. For example, acetic acid, written as CH₃COOH, gives a proton to water, H₂O. After this, acetic acid becomes its conjugate base, the acetate ion (CH₃COO⁻). Water becomes its conjugate acid, the hydronium ion (H₃O⁺).

The reverse can also happen. The hydronium ion can give a proton back to the acetate ion, and they return to acetic acid and water. This shows that acids and bases can work in both directions.

Amphoteric substances

In Brønsted–Lowry theory, an acid works only when it meets a base, and a base works only when it meets an acid. Water is special because it can act like either an acid or a base. For example, one water molecule can take a hydrogen ion (H⁺) to become H₃O⁺, while another water molecule can give away a hydrogen ion to become OH⁻.

Another example is aluminium hydroxide, Al(OH)₃. It can act as an acid or a base depending on what it meets.

Comparison with Lewis acid–base theory

See also: Lewis acids and bases

In 1923, the same year Brønsted and Lowry shared their ideas about acids and bases, another scientist named G. N. Lewis offered a different way to understand these reactions. Lewis looked at how tiny parts of atoms, called electrons, behave. In his idea, a base is something that can share a pair of electrons, and an acid is something that can accept that pair.

Lewis’s idea helps explain Brønsted and Lowry’s work by looking at electrons. This shows that even though the two theories describe acids and bases differently, they often agree on what happens in reactions.

Comparison with the Lux–Flood theory

The Brønsted–Lowry theory does not explain reactions between solids or liquids, like oxides. For example, it cannot explain why magnesium oxide and silicon dioxide form a new compound.

But, magnesium oxide can act like a base when mixed with an acid in water. In this case, we can use a different idea called Lewis acid-base reactions.

Dissolved silicon dioxide can act like a weak acid under the Brønsted–Lowry theory. The Lux–Flood theory says that oxides like magnesium oxide and silicon dioxide in solid form can be acids or bases. For example, the mineral olivine is made from magnesium oxide, which acts like a base, and silicon dioxide, which acts like an acid. This helps scientists study Earth’s chemistry.