Label each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each case write the formula of its conjugate base, and indicate whether the conjugate base is a strong base, a weak base, or a species with negligible basicity: (a) HCOOH

Verified step by step guidance

1. Identify the given species: HCOOH is formic acid.
2. Determine the strength of the acid: HCOOH is a weak acid because it does not completely dissociate in water.
3. Write the formula of the conjugate base: The conjugate base of HCOOH is HCOO⁻.
4. Assess the basicity of the conjugate base: Since HCOOH is a weak acid, its conjugate base, HCOO⁻, is a weak base.
5. Summarize: HCOOH is a weak acid, and its conjugate base, HCOO⁻, is a weak base.

Key Concepts

Acid-Base Theory

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry definition, acids are proton donors, while bases are proton acceptors. This framework helps classify substances based on their ability to donate or accept protons, which is essential for determining the strength of acids and their conjugate bases.

Strength of Acids and Bases

The strength of an acid or base is determined by its ability to dissociate in water. Strong acids, like hydrochloric acid (HCl), completely ionize in solution, while weak acids, such as formic acid (HCOOH), only partially ionize. The strength of the conjugate base is inversely related to the strength of the acid; a strong acid has a weak conjugate base, and vice versa.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of an acid and its corresponding base, which differ by a proton. For example, when HCOOH donates a proton, it forms its conjugate base, HCOO-. Understanding these pairs is crucial for predicting the behavior of acids and bases in reactions, as well as their relative strengths in terms of acidity and basicity.