Explain the principles behind an acid-base titration. What is an indicator?

Understanding the equivalence point is crucial for grasping acid-base titrations. It is the precise moment during the titration when the amount of titrant added causes the moles of the base to be stoichiometrically equivalent to the moles of the acid in the solution. At the equivalence point, the reactants have completely neutralized each other, there's no excess hydrogen or hydroxide ions, and the solution should ideally contain only the salt and water.
Equivalence point detection often requires careful monitoring since it signifies the exact completion of the reaction per the balanced chemical equation used in the stoichiometric calculations. It is not always discernible by the naked eye, and hence, indicators or pH meters are typically used to detect it. The change observed at the equivalence point depends on the nature of the reactants and the titration curve's progression.

The titrant plays a pivotal role in acid-base titrations. It is the solution of a known concentration that is gradually added to a solution of unknown concentration to achieve the reaction. The characteristics of the titrant are essential for accurate titrations: it must react quickly and completely with the substance being titrated, and its concentration must be known with accuracy and precision.
Additionally, proper titrant handling is important to prevent contamination or concentration changes, which can significantly impact the titration outcome. The burette, which is used to deliver the titrant, should always be clean, and any air bubbles present must be eliminated to ensure the volume added is precise. The titrant addition proceeds until reaching the equivalence point, signifying the analytical goal of the titration.

Indicators are the heralds of the titration's end point. These are chemicals that display a color change at a particular pH level, signifying that an acid-base reaction's end point has been reached, or is very close. Selecting the appropriate indicator is a critical step; it requires understanding the nature of the acid and base being titrated and their corresponding pH at the equivalence point.
A well-chosen indicator will change color at a pH that is very close to the equivalence point, minimizing the difference between the end point and the equivalence point, thus yielding accurate titration results. Some common indicators include phenolphthalein, which turns pink in basic solutions, and methyl orange, which transitions from red to yellow across its pH change range.

Stoichiometry is the backbone of quantitative chemical analysis, such as an acid-base titration. It involves the calculation of reactants and products in chemical reactions. In the context of titrations, stoichiometry is used to determine the relationship between the quantity of titrant and the substance being titrated, often through a balanced chemical equation.
To achieve accurate results from a titration, it's essential to account for the stoichiometry - this includes understanding the mole-to-mole ratios and considering the mass-to-mass conversions if needed. Applying stoichiometric principles allows us to interpret the point of equivalence and to calculate the unknown concentration, fully elucidating the purpose of the titration.