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An acid's strength is determined by how stable its conjugate base (anion) is after deprotonation. A stable anion is a weak base, making the corresponding acid strong. Conversely, an unstable anion indicates a weak acid. To predict acid strength, chemists analyze the stability of the conjugate base using factors like size, electronegativity, resonance, induction, and hybridization.

When comparing acids from elements in the same column, larger atoms stabilize negative charge better by spreading it over a greater volume. This increased stability of the anion makes the corresponding acid stronger. For example, HI is a stronger acid than HF because iodine is larger than fluorine, allowing better charge delocalization in the conjugate base.

For acids formed from elements in the same periodic row, electronegativity dominates anion stability. More electronegative atoms stabilize the negative charge more effectively, producing a stable conjugate base and a stronger acid. This charge effect explains why HClO₄ is stronger than HBrO₄, as chlorine is more electronegative than bromine.

When anions have the negative charge on the same atom, resonance structures determine stability. Anions with multiple resonance structures delocalize charge over several atoms, increasing stability and acid strength. Methanesulfonic acid is stronger than ethanol because its conjugate base has three resonance structures, whereas ethoxide has none, demonstrating how resonance-stabilized conjugate bases correspond to stronger acids.

Electronegative substituents adjacent to a negatively charged region withdraw electron density through induction, stabilizing the anion and strengthening the acid. As the substituent moves farther from the charged region, this stabilizing effect weakens. For example, 2-chlorobutanoic acid is stronger than 4-chlorobutanoic acid because chlorine is closer to the carboxylate group in the former.

Acidity in these hydrocarbons depends on the hybridization of carbon in the conjugate base. Electrons in sp-hybridized carbon are closest to the nucleus, stabilizing the negative charge most effectively. Therefore, alkynes are strongest acids, followed by alkenes, then alkanes. This ordering reflects the s-character: sp orbitals have 50% s-character, sp² has 33.3%, and sp³ has 25%.

When compounds lack resonance, electronegative substituents, or have charge on identical atoms, hybridization becomes the determining factor. For compounds with equal resonance, the induction effect is analyzed by examining electronegative element proximity to the acidic hydrogen. Understanding acid strength requires systematically evaluating size, electronegativity, resonance, induction, and hybridization effects in order of relevance.