Acids, Bases, and Brønsted-Lowry Definitions

This set explores the fundamental definitions and chemical representations of acids and bases, including Br%f8nsted-Lowry theory and specific examples from the IGCSE Chemistry syllabus.

Acid (Arrhenius)

A substance that produces hydrogen ions, $H^{+}(aq)$, when dissolved in water.

Hydrochloric acid dissociation

$$HCl(aq) \rightarrow H^{+}(aq) + Cl^{-}(aq)$$

Nitric acid dissociation

$$HNO_{3}(aq) \rightarrow H^{+}(aq) + NO_{3}^{-}(aq)$$

Brønsted-Lowry Acid

A substance that acts as a proton donor.

Proton

In the context of acid-base chemistry, a proton is an $H^{+}$ ion.

Acid Reaction Example ($HCl$)

$HCl + H_{2}O \rightarrow H_{3}O^{+} + Cl^{-}$, where $HCl$ donates an $H^{+}$ ion.

Base (General)

An oxide or hydroxide of a metal that neutralizes an acid.

Metal Oxide Bases

Examples include Copper(II) oxide ($CuO$) and Magnesium oxide ($MgO$).

Metal Hydroxide Bases

Examples include Sodium hydroxide ($NaOH$) and Calcium hydroxide ($Ca(OH)_{2}$).

Brønsted-Lowry Base

A substance that acts as a proton acceptor.

Base Reaction Example ($NH_{3}$)

$NH_{3} + H_{2}O \rightleftharpoons NH_{4}^{+} + OH^{-}$, where $NH_{3}$ accepts an $H^{+}$ ion from water.