The conjugate base of chlorous acid is chlorite, with the chemical formula ClO₂⁻.
Understanding Conjugate Bases
In chemistry, an acid-base reaction involves the transfer of a proton (H⁺). When an acid donates a proton, the species remaining is called its conjugate base. Conversely, when a base accepts a proton, it forms its conjugate acid. This relationship is fundamental to Brønsted-Lowry acid-base theory.
Chlorous acid acts as a proton donor. When it loses a hydrogen ion (H⁺), it transforms into its corresponding conjugate base, the chlorite ion.
Properties of Chlorous Acid
Chlorous acid is an inorganic compound known for its acidic properties. Its key characteristics include:
- Chemical Formula: HClO₂
- Molar Mass: 68.46 g/mol
- Acidity (pKa): 1.96
The pKa value of 1.96 indicates that chlorous acid is a relatively weak acid, meaning it does not fully dissociate in water.
Formation of Chlorite
The dissociation of chlorous acid (HClO₂) into its conjugate base, the chlorite ion (ClO₂⁻), can be represented by the following reversible reaction:
HClO₂(aq) ⇌ H⁺(aq) + ClO₂⁻(aq)
In this equilibrium, chlorous acid (HClO₂) donates a proton (H⁺) to form the chlorite ion (ClO₂⁻), which is capable of accepting a proton to reform chlorous acid.
Overview of Chlorous Acid and Chlorite
Here's a quick summary of the acid and its conjugate base:
| Compound | Chemical Formula | Type | Key Property |
|---|---|---|---|
| Chlorous Acid | HClO₂ | Acid | Proton donor (pKa = 1.96) |
| Chlorite (ion) | ClO₂⁻ | Conjugate Base | Proton acceptor, derived from HClO₂ |
The chlorite ion (ClO₂⁻) is a stable anion that plays a role in various chemical processes, including its use in some industrial applications.
