Titration of NH3 with HClO4 Solution

What happens when a 100.00ml solution of 0.20 M NH3 is titrated with 0.20 M HClO4?

What is the pH of the solution after 100.00ml of HClO4 have been added?

Explanation:

When a 100.00ml solution of 0.20 M NH3 is titrated with 0.20 M HClO4, a neutral solution is formed after adding 100.00ml of HClO4. This is because NH3 and HClO4 are both monoprotic and have equal concentrations, resulting in the formation of an ammonium chloride solution.

In this titration scenario, NH3 (ammonia) and HClO4 (perchloric acid) are being titrated together. The resulting solution becomes neutral once 100ml of HClO4 is added, as the mole ratio between NH3 and HClO4 is 1:1 due to the monoprotic nature of both substances with equal concentrations. As a result, an ammonium chloride (NH4Cl) solution is produced.

The pH of this solution is influenced by the temperature of the system. To accurately determine the pH, we would need the Ka value for NH4+ or the Kb value for ammonia (NH3).

Without knowing the temperature or the specific Ka or Kb values, it is not possible to provide an exact pH value. If the reaction did not proceed to completion, the Henderson-Hasselbalch equation could be used with the Ka or Kb values to determine the pH.