Predict the stronger acid in each pair: (c) HBrO₃ or HBrO₂

Verified step by step guidance

1. Identify the acids in the pair: HBrO3 and HBrO2.
2. Recognize that both acids are oxyacids, which means they contain hydrogen, oxygen, and another element (bromine in this case).
3. Understand that the strength of oxyacids generally increases with the number of oxygen atoms bonded to the central atom, as more oxygen atoms can stabilize the negative charge on the conjugate base through resonance.
4. Compare the number of oxygen atoms in each acid: HBrO3 has three oxygen atoms, while HBrO2 has two oxygen atoms.
5. Conclude that HBrO3 is the stronger acid because it has more oxygen atoms, which allows for greater stabilization of the conjugate base.

Key Concepts

Acid Strength and Structure

The strength of an acid is influenced by its molecular structure, particularly the electronegativity of atoms and the stability of the conjugate base. In oxyacids, the number of oxygen atoms bonded to the central atom typically increases acid strength, as more oxygen atoms can stabilize the negative charge on the conjugate base through resonance.

Oxyacids

Oxyacids are acids that contain oxygen, hydrogen, and another element (the central atom). The general formula is HnXOm, where X is the central atom. The strength of oxyacids often increases with the number of oxygen atoms attached to the central atom, as these additional oxygens can help stabilize the conjugate base formed after deprotonation.

Conjugate Base Stability

The stability of the conjugate base formed when an acid donates a proton is crucial in determining acid strength. A more stable conjugate base corresponds to a stronger acid. In the case of HBrO3 and HBrO2, the conjugate base of HBrO3 is more stable due to the presence of an additional oxygen atom, which allows for greater resonance stabilization.