This is from my textbook:
Carboxylic acids owe their acidity ($\mathrm pK_\mathrm a$ of about $5$) to the resonance-stabilized carboxylate anions formed by deprotonation.
Why are they such weak acids? If the anions are resonance-stabilized, I would expect them to be much stronger acids.
Stated another way: this screenshot of the textbook page shows a representative protonation/deprotonation equilibrium for a carboxylic acid:
Why is the reaction favoured in the reverse direction if the carboxylate ion is more stable than the reactant?