Which indicators could you use for a titration of \(0.20 \mathrm{M}\) ammonia with \(0.20 \mathrm{M} \mathrm{HCl}(\mathrm{aq}):\) (a) bromocresol green; (b) methyl red; (c) phenol red; (d) thymol blue? Fxplain your selections.

Understanding the titration endpoint is key to successfully conducting a titration. The endpoint refers to the point in titration at which the reactants have been mixed in exactly the right proportions according to the stoichiometry of the reaction. This is different from the equivalence point, which is a theoretical point where the number of moles of acid equals the number of moles of base. It's at the endpoint that the indicator, which is added to the analyte, changes color to signal the completion of the reaction.

For instance, in the titration of ammonia with hydrochloric acid, the endpoint is reached when the color of the indicator changes, signaling that the amount of acid added is stoichiometrically equivalent to the amount of ammonia present. It's important to choose an indicator with a color change that occurs close to the equivalence point pH, in this case, an acidic pH, as that will give the most accurate representation of the endpoint.

Titration indicators are substances that provide a visual cue, typically a color change, during a titration, marking the endpoint of the procedure. The choice of an indicator depends largely on the pH range over which it changes color, which should be near the expected pH at the titration's equivalence point.

For acid-base titrations, indicators are chosen based on whether the reaction involves a strong acid or base and a weak base or acid. As ammonia is a weak base and HCl is a strong acid, we expect the equivalence point pH to be on the acidic side of the pH scale. Therefore, indicators that change color in an acidic environment are necessary. In the exercise, bromocresol green and methyl red are suitable because their color change occurs in the acidic pH range, closely matching the expected pH at the equivalence point of this specific titration.

Choosing the correct indicator is critical for accurate results. If an indicator that changes color at a pH far from the equivalence point was used, it would lead to an inaccurate determination of the titration's endpoint, resulting in systematic errors.

The pH at the equivalence point of a titration depends on the nature of the acid and base involved in the reaction. For the titration of a weak base with a strong acid, as is the case with ammonia and hydrochloric acid, the pH at the equivalence point will be less than 7. This is because the reaction produces ammonium chloride, where the ammonium ion (\( \text{NH}_4^+ \)) acts as a weak acid, slightly lowering the pH.

The pH equivalence point can also be estimated using the pKa of the conjugate acid (in this case, ammonium). Since the pKa for the ammonium ion is around 9.25, the Henderson-Hasselbalch equation could be used to estimate the pH at which a given concentration of ammonia would be neutralized by hydrochloric acid. This helps in selecting the right indicator. For instance, bromocresol green and methyl red, with their pH transition ranges falling below 7, are apt choices precisely because they align with the acidic pH we expect at the equivalence point for the chosen system.