Neutralization reactions occur whenever an acid reacts with a base, including titrations involving weak acids and strong bases. During these reactions, the weak acid partially dissociates, and as hydroxide ions (OH-) react with hydrogen ions (H+), the concentration of H+ decreases. According to Le Chatelier's principle, this leads to further dissociation of the weak acid to maintain equilibrium, potentially resulting in complete dissociation. However, the final solution does not achieve a neutral pH of 7, particularly at 25 ºC, as it contains a salt and may have a different pH depending on the strength of the acid and base involved. Thus, while neutralization can occur in these titrations, it does not always result in a neutral solution, and the term "neutralization reaction" is more accurately applied to titrations involving strong acids and strong bases.
