Pick the stronger base from each pair. c. F^– or ClO^–

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Identify the concept of base strength: A stronger base is better at accepting protons (H+).

Consider the conjugate acid: The strength of a base is inversely related to the strength of its conjugate acid.

Compare the conjugate acids: HF (conjugate acid of F-) and HClO (conjugate acid of ClO-).

Determine the acid strength: HF is a weak acid, while HClO is a stronger acid.

Conclude the base strength: Since HF is weaker, F- is a stronger base than ClO-.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Theory

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. Understanding this concept is crucial for determining the strength of bases, as it helps identify which species can effectively accept protons in a reaction.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of two species that differ by the presence of a proton. When a base accepts a proton, it forms its conjugate acid. The strength of a base can often be inferred from the stability of its conjugate acid; a weaker conjugate acid indicates a stronger base. This concept is essential for comparing the basicity of F- and ClO-.

Electronegativity and Basicity

Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the context of basicity, a more electronegative atom in a conjugate base can stabilize the negative charge, making it a weaker base. Comparing the electronegativities of fluorine and chlorine helps determine which anion, F- or ClO-, is the stronger base, as the less electronegative atom will generally be a stronger base.