The conjugate base of HBr is Br⁻, also known as the bromide ion.
Understanding Conjugate Bases
In chemistry, particularly within the Brønsted-Lowry acid-base theory, an acid is defined as a substance that donates a proton (H⁺). When an acid donates its proton, the species that remains is called its conjugate base. This conjugate base is capable of accepting a proton in the reverse reaction.
HBr as an Acid
- HBr is the chemical formula for hydrobromic acid. It is a strong acid, meaning it readily donates its proton in solution.
- When hydrobromic acid (HBr) acts as an acid, it donates a proton (H⁺) to another substance (a base).
- The process can be visualized as HBr losing its H⁺ ion:
HBr → H⁺ + Br⁻ - What is left behind after HBr donates its proton is the Br⁻ ion. This bromide ion is therefore the conjugate base of HBr.
Acid-Conjugate Base Pair Summary
The relationship between an acid and its conjugate base can be summarized in the following table:
| Acid (Proton Donor) | Conjugate Base (Proton Acceptor) |
|---|---|
| HBr (Hydrobromic Acid) | Br⁻ (Bromide Ion) |
This illustrates that when HBr donates a proton, it forms its corresponding conjugate base, Br⁻. The bromide ion can then potentially act as a base by accepting a proton.
