What is the Bronsted-Lowry definition of acid and base?

By the Brønsted–Lowry definition, an acid is a proton (H⁺) donor and a base is a proton acceptor. This is broader than the Arrhenius idea of acids giving H⁺ and bases giving OH⁻ in water.

What happens when an acid reacts with a base?

An acid and a base undergo a neutralisation reaction to form a salt and water, and the process releases heat (it is exothermic).

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Difference Between Acid and Base

Acids and bases are two classes of compounds that behave oppositely in water and neutralise each other.

In short

An acid donates hydrogen ions (H⁺), tastes sour and has a pH below 7; a base accepts H⁺ (or donates OH⁻ ions), tastes bitter, feels soapy and has a pH above 7.

Acid vs Base - Comparison Table

Basis	Acid	Base
Ions released in water	H⁺ (hydrogen ions)	OH⁻ (hydroxide ions)
pH value	Less than 7	Greater than 7
Taste	Sour	Bitter
Litmus test	Turns blue litmus red	Turns red litmus blue
Feel	-	Soapy / slippery
Examples	HCl, H₂SO₄, vinegar	NaOH, NH₃, soap

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Frequently Asked Questions - Acid vs Base

What is the Bronsted-Lowry definition of acid and base?: By the Brønsted–Lowry definition, an acid is a proton (H⁺) donor and a base is a proton acceptor. This is broader than the Arrhenius idea of acids giving H⁺ and bases giving OH⁻ in water.
What happens when an acid reacts with a base?: An acid and a base undergo a neutralisation reaction to form a salt and water, and the process releases heat (it is exothermic).

Difference Between Acid and Base

Acid vs Base - Comparison Table

Frequently Asked Questions - Acid vs Base

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