Oxyacids are acids that contain hydrogen, oxygen, and another element (the central atom). They dissociate in water to produce H+ ions and the corresponding oxyanion.
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Oxyacids are named based on the central atom and its oxidation state; for example, HClO4 is perchloric acid.
The strength of an oxyacid depends on the electronegativity of the central atom and the number of oxygen atoms bonded to it.
In oxyacids, as the number of oxygen atoms increases, the acid strength generally increases due to increased electron withdrawal from hydrogen.
Common examples include sulfuric acid (H2SO4), nitric acid (HNO3), and phosphoric acid (H3PO4).
Oxyacids can be monoprotic or polyprotic depending on how many protons they can donate.
Review Questions
What factors influence the strength of an oxyacid?
How does the structure of an oxyacid affect its dissociation in water?
Name three common examples of oxyacids and their chemical formulas.
Related terms
Acid-Base Equilibria: The balance between acids and bases in a solution, often described by equilibrium constants such as Ka for acids and Kb for bases.
Electronegativity: A measure of an atom's ability to attract shared electrons in a chemical bond. Higher electronegativity often correlates with stronger acids in oxyacids.
Oxyanion: An ion containing oxygen and another element, typically formed when an oxyacid loses one or more hydrogen ions.