Concept:The strength of an acid is defined strictly by its ability to dissociate (ionize) and donate protons (\( \text{H}^+ \)) in an aqueous solution.
Solution:- Sulfuric acid (\( \text{H}_2\text{SO}_4 \)) is a strong mineral acid that ionizes nearly 100% in water, yielding a high concentration of protons.
- Acetic acid (\( \text{CH}_3\text{COOH} \)) is an organic acid with a very low acid dissociation constant (\( \text{K}_a \approx 1.8 \times 10^{-5} \)).
- This means it only partially dissociates (has a less degree of ionization), making it a much weaker acid.
Why other options are incorrect:Having a \( -\text{COOH} \) group defines its class but does not scientifically define
why it's weaker than a mineral acid. Thermal decomposition and inductive effects are irrelevant to the core definition of its weak electrolytic nature compared to \( \text{H}_2\text{SO}_4 \).
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