Consider the titration of 30.0 mL of 0.050 M NH3 with

Problem 17.46Consider the titration of 30.0 mL of 0.050 M NH with 0.03 M HCl. Calculate the pH after thefollowing volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL,(e) 61.0 mL, (f) 65.0 mL. Step-by-step solution Step 1 of 16 The titration of 30.0 mL of 0.050 M NH with 0.023 M HCl is a type of weak base-strong acidtitration. This titration is divided into four regions. They are, 1. Initial point: The pH of the solution is determined by the ionization of weak base (NH ) 3 and K b used to calculate this pH. 2. Between initial point and equivalence point: Prior to reaching the equivalence point, the base (NH ) 3 being neutralized, and its conjugated acid (NH ) is being f4rmed. The pH of this buffer solution is calculated using Henderson-Hasselbalch equation. + 3. Equivalence point: The pH of the solution is determined by the ionization of acid (NH ) 4 Produced from neutralization of weak base (NH ) and K i3used to alculate this pH. 4. After the equivalence point: The pH of the solution is determined by the concentration of + H from the excess acid, HCl.