Consider a weak base-strong acid titration in which 25 mL of0.160 M ammonia is titrated with 0.160 M HCl.
a) What is the pH of the ammonia solution before the addition ofHCl? pKb of ammonia= 4.75
b) Calculate the pH after the addtion of 3 mL of HCl.
c) Calculate the pH after the addition of 12.5mL of HCl. This isthe half-neutralization point: the partial neutralization ofammonia converts some of the NH3 molecules to NH4+ ions andproduces a buffer whose pH depends on the acid/base ratio(NH4+/NH3).
d)Calculate the pH after the addition of 25mL of HCl(equivalence point).
e) Calculate the pH after the addition of 35mL of HCl.
f) Suggest an indicator, other then methyl red, that would besuitable for this titration, and explain why it would beeffective.
Thanks alot
