Concept:The strength of an acid in aqueous solution is defined solely by its ability to dissociate (ionize) and donate hydrogen ions (\( \text{H}^+ \)).
Formula:$$ \text{Acid Strength} \propto \text{Degree of Ionization } (\alpha) $$
Solution:- Sulfuric acid (\( \text{H}_2\text{SO}_4 \)) is a strong acid that ionizes almost 100% in water.
- Acetic acid (\( \text{CH}_3\text{COOH} \)) is a weak acid that only partially ionizes (typically less than 5% in standard solutions).
- Because it produces far fewer \( \text{H}^+ \) ions per mole dissolved, it is classified as weaker due to its lesser degree of ionization.
Why other options are incorrect:Having a --COOH group defines it as an organic acid, but doesn't explain relative strength against sulfuric acid fundamentally. Decomposition and inductive effects are secondary physical/structural traits, not the primary definition of aqueous acid strength.
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