Predicting Stronger Acids in Acid Pairs

Which factors can help us predict the stronger acid within pairs of acids? The stronger acid within pairs can be predicted by considering factors such as electronegativity, oxidation states, and the stability of the conjugate base.

When determining which acid is stronger within a pair, we look at various factors to make our prediction. These factors include:

Electronegativity:

Acids with more electronegative atoms tend to be stronger, as they are better able to stabilize the negative charge that results from donating a proton.

Oxidation State:

The oxidation state of the central atom in an acid can also impact its strength. Generally, higher oxidation states lead to stronger acids.

Conjugate Base Stability:

The stability of the conjugate base formed after donating a proton can influence the strength of an acid. A more stable conjugate base indicates a stronger acid.

For example:

H₂SO₃ or H₂SeO₃:

Sulfur is more electronegative than selenium, making H₂SO₃ the stronger acid in this pair.

H₂SeO₄ or H₂SeO₃:

H₂SeO₄ is the stronger acid due to its additional oxygen atoms, leading to greater electron-withdrawing effects.

HBr or H₂S:

HBr is stronger than H₂S because of bromine's higher electronegativity.

H₂SO₄ or H₂SeO₄:

H₂SO₄ is stronger as sulfur is more electronegative than selenium.

HF or HBr:

HBr is the stronger acid because bromine is less electronegative than fluorine.

By considering these factors, we can make informed predictions about the relative strengths of acids within pairs.

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