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: (c) O2-

검증된 단계별 안내

First, identify the given species. In this case, it is O2-.

Next, determine the basicity of the given species. O2- is a strong base because it readily accepts protons (H+ ions) to form OH-.

Then, write the formula of its conjugate acid. The conjugate acid of a base is formed by adding a proton (H+) to the base. Therefore, the conjugate acid of O2- is OH-.

Finally, determine the acidity of the conjugate acid. OH- is a weak acid because it does not readily donate protons (H+ ions).

Summarize your findings: O2- is a strong base, its conjugate acid is OH-, and OH- is a weak acid.

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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. This framework helps classify substances based on their ability to donate or accept protons, which is essential for determining the strength of acids and bases.

Conjugate Acid-Base Pairs

A conjugate acid-base pair consists of two species that differ by the presence of a proton (H+). When a base accepts a proton, it forms its conjugate acid, while the acid that donates the proton becomes its conjugate base. Understanding these pairs is crucial for predicting the strength of acids and bases, as strong bases yield weak conjugate acids and vice versa.

Strength of Acids and Bases

The strength of an acid or base is determined by its 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 vital for classifying substances like O2- and understanding the nature of their conjugate acids.