Pick the stronger base from each pair. a. ClO₄^– or ClO₂^– b. Cl^– or H₂O c. CN^– or ClO^–

Verified step by step guidance

1. Step 1: Understand the concept of base strength. A stronger base is more willing to accept protons (H+ ions) or donate electron pairs. The strength of a base is often related to the stability of its conjugate acid.
2. Step 2: Analyze the conjugate acids of each pair. For example, the conjugate acid of ClO4– is HClO4, and the conjugate acid of ClO2– is HClO2. Compare the acid strengths to determine the base strengths.
3. Step 3: Use the concept of acid strength to infer base strength. A weaker acid has a stronger conjugate base. For instance, if HClO4 is a stronger acid than HClO2, then ClO2– is a stronger base than ClO4–.
4. Step 4: Consider the electronegativity and size of atoms involved. For example, Cl– is the conjugate base of HCl, a strong acid, making Cl– a very weak base. Compare this with H2O, which is a weak acid, making it a relatively stronger base than Cl–.
5. Step 5: Evaluate the stability of the base. For CN– and ClO–, consider the resonance and electronegativity. CN– has resonance stabilization and is a stronger base compared to ClO–, which has less resonance stabilization.

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 concept is crucial for determining the strength of bases in given pairs, as it allows for the evaluation of their ability to accept protons.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of two species that differ by the presence of a proton (H+). The strength of a base can often be inferred from its conjugate acid; a weaker conjugate acid corresponds to a stronger base. This relationship is essential for comparing the strength of bases in the provided pairs.

Electronegativity and Stability

Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the context of bases, a more electronegative atom can stabilize negative charge better, making the corresponding base weaker. Evaluating the electronegativity of atoms in the anions helps determine which base is stronger in each pair.