Write the formula for the conjugate base of each acid. a. HCl

Verified step by step guidance

1. Identify the acid in the problem: HCl.
2. Recall that a conjugate base is formed by removing a proton (H⁺) from the acid.
3. Remove one hydrogen ion (H⁺) from HCl, which leaves you with Cl⁻.
4. Recognize that the remaining species, Cl⁻, is the conjugate base of HCl.
5. Write the formula for the conjugate base: Cl⁻.

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 hydrochloric acid (HCl), completely dissociate in water, meaning they release all their protons. The conjugate base of a strong acid is typically a weak base, which does not readily accept protons. For HCl, the conjugate base is Cl-, which is stable and does not react significantly with water to form HCl again.

Chemical Notation and Formulas

Chemical notation is a system of symbols used to represent elements and compounds. The formula for a conjugate base is derived from the acid's formula by removing one hydrogen atom and adjusting the charge accordingly. For HCl, the removal of H+ results in the formula Cl-, indicating the chloride ion as the conjugate base.