The conjugate base of hydrazoic acid is the azide ion (N₃⁻¹).
Understanding Conjugate Bases
In acid-base chemistry, according to the Brønsted-Lowry theory, an acid is a proton (H⁺) donor, and a base is a proton acceptor. When an acid donates a proton, the remaining species is called its conjugate base. Conversely, when a base accepts a proton, it forms its conjugate acid.
This relationship can be represented by a reversible reaction:
Acid ⇌ Conjugate Base + H⁺
Hydrazoic Acid (HN₃) and its Conjugate Base
Hydrazoic acid, with the chemical formula HN₃, is a weak acid. When it dissociates in a solution, it donates a proton (H⁺), forming its corresponding conjugate base.
The dissociation reaction for hydrazoic acid is:
HN₃ (aq) ⇌ N₃⁻¹ (aq) + H⁺ (aq)
Here's a breakdown:
- Hydrazoic Acid (HN₃): The acid, which donates a proton.
- Azide Ion (N₃⁻¹): The conjugate base, which is formed after HN₃ loses its proton. It is known specifically as the azide ion.
Why Azide Ion is a Base
The azide ion (N₃⁻¹) has a negative charge. This negative charge signifies an excess of electrons, giving the ion a greater ability to donate electrons. According to the definition of a base (specifically a Lewis base, which donates an electron pair), this enhanced electron-donating capability contributes to its higher basicity compared to the neutral hydrazoic acid molecule.
Summary of the Acid-Base Pair
For clarity, here's the relationship between hydrazoic acid and its conjugate base:
| Acid | Conjugate Base |
|---|---|
| Hydrazoic acid (HN₃) | Azide ion (N₃⁻¹) |
Understanding this relationship is fundamental to predicting the behavior of these chemical species in various reactions and environments.
