Write the formula for the conjugate base of each acid. b. HBr

Verified step by step guidance

1. Identify the acid in the problem: HBr.
2. Recall that a conjugate base is formed by removing a proton (H⁺) from the acid.
3. Remove one hydrogen ion (H⁺) from HBr.
4. After removing H⁺, the remaining species is Br⁻.
5. Thus, the conjugate base of HBr is Br⁻.

Key Concepts

Conjugate Acid-Base Pairs

In acid-base chemistry, a conjugate acid-base pair consists of two species that differ by the presence of a proton (H+). When an acid donates a proton, it transforms into its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding this relationship is crucial for identifying the conjugate base of any given acid.

Strong Acids and Their Conjugate Bases

Strong acids, such as HBr, completely dissociate in water, meaning they release all their protons. The conjugate base of a strong acid is typically a weak base, as it has a low tendency to re-accept the proton. Recognizing that HBr is a strong acid helps in determining that its conjugate base, Br-, is relatively stable and does not readily accept protons.

Chemical Formulas and Ion Representation

Chemical formulas represent the composition of substances, including ions. The conjugate base of an acid can be represented by its chemical formula, which indicates the remaining species after the acid has lost a proton. For HBr, the conjugate base is Br-, highlighting the importance of understanding how to write and interpret chemical formulas in acid-base reactions.