Identify the weakest acid in each of the following sets. Explain your reasoning. (a) H₂SO₃, HClO₃, HClO₄

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Identify the structure and stability of the conjugate bases of each acid. The stability of the conjugate base often determines the strength of the acid.

Consider the oxidation state of the central atom in each oxyacid. Higher oxidation states generally correlate with stronger acids because they stabilize the negative charge on the conjugate base more effectively.

Examine the electronegativity and electron withdrawing effects of the atoms surrounding the central atom. More electronegative atoms or groups that are better at withdrawing electrons will generally stabilize the conjugate base, leading to a stronger acid.

Compare the number of oxygen atoms bonded to the central atom in each acid. More oxygen atoms usually indicate stronger acids due to better stabilization of the conjugate base through resonance and inductive effects.

Based on the above considerations, determine which acid has the least effective stabilization of its conjugate base, indicating it is the weakest acid among the given options.

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Key Concepts

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

Acid Strength

Acid strength refers to the ability of an acid to donate protons (H+) in a solution. Strong acids completely dissociate in water, while weak acids only partially dissociate. The strength of an acid is often determined by its dissociation constant (Ka), with larger values indicating stronger acids.

Oxidation States

The oxidation state of an element in a compound indicates its degree of oxidation or reduction. In oxyacids, the oxidation state of the central atom can influence acid strength; higher oxidation states typically lead to stronger acids due to increased positive charge, which stabilizes the conjugate base after proton donation.

Comparative Analysis of Oxyacids

When comparing oxyacids, the number of oxygen atoms bonded to the central atom plays a crucial role in determining acid strength. More oxygen atoms generally lead to stronger acids because they stabilize the negative charge on the conjugate base through resonance. Thus, in a set of oxyacids, the one with fewer oxygen atoms is often the weakest.

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