Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (a) CH3COO-

Key Concepts

Acid-Base Theory

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, acids are proton donors, while bases are proton acceptors. Understanding this theory is essential for classifying substances like CH3COO- and determining their conjugate acids.

Conjugate Acid-Base Pairs

A conjugate acid-base pair consists of two species that differ by the presence or absence of a proton (H+). For example, when a base accepts a proton, it forms its conjugate acid. Recognizing these pairs helps in identifying the strength of acids and bases, such as determining the nature of CH3COO- and its conjugate acid, CH3COOH.

Strength of Acids and Bases

The strength of acids and bases is determined by their ability to dissociate in water. Strong acids completely ionize, while weak acids only partially ionize. Similarly, strong bases fully dissociate in solution, whereas weak bases do not. This concept is crucial for classifying CH3COO- and its conjugate acid, CH3COOH, in terms of their basicity and acidity.