Concept:Only carboxylic acids possess sufficient acidity to react with weak bases like sodium bicarbonate and sodium carbonate to release \( \text{CO}_2 \) gas.
Formula:$$ \text{R-COOH} + \text{NaHCO}_3 \longrightarrow \text{R-COONa} + \text{H}_2\text{O} + \text{CO}_2\uparrow $$
Solution:- Option A is an ester (ethyl formate); it is neutral and unreactive with bases under normal conditions.
- Option B is an alcohol (ethanol); it can react with strong metals but not weak bases like \( \text{NaHCO}_3 \).
- Option C is an alkene (propene); it does not undergo acid-base reactions.
- Option D is propanoic acid (\( \text{CH}_3\text{CH}_2\text{COOH} \)), a carboxylic acid that readily neutralizes \( \text{NaOH} \), \( \text{NaHCO}_3 \), and \( \text{Na}_2\text{CO}_3 \).
Why other options are incorrect:Only the molecule containing the carboxyl group (\( -\text{COOH} \)) possesses the necessary acid strength.
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