Final answer:
The titration curve of NH3 (a weak base) with HCl (a strong acid) shows an equivalence point pH of less than 7.00 and is the reverse of the curve for a weak acid titrated with a strong base.
Step-by-step explanation:
The titration curve corresponding to the titration of ammonia (NH3), which is a weak base, with hydrochloric acid (HCl), a strong acid, will showcase specific characteristics. As noted in LibreTexts and depicted in various figures such as part (b) in Figure 15.6.3 or Figure 18.4.3, the pH at the equivalence point of such a titration is less than 7.00. This is because the titration of NH3 with HCl results in the formation of NH4Cl, which slightly dissociates to give NH4+ and Cl-, leading to an acidic solution at the equivalence point. This titration curve is the reverse of that seen for a weak acid like acetic acid (CH3CO2H) titrated with a strong base like NaOH. Additionally, the identity of the weak base being titrated influences the shape of the titration curve, and as NH3 is a weaker base, the pH change around the equivalence point will not be as dramatic compared to strong acid-strong base titrations, like HCl with NaOH.