Question

Ammonia is a weak base with a Kb of 1.8×10^-5. A 140.0-mL sample of a 0.175 M solution of aqueous ammonia is titrated with a 0.106 M solution of the strong acid HCI. The reaction is

NH3(aq)+HCl(aq)→NH+4(aq)+Ci−(aq)NH3(aq)+HCl(aq)→NH+4(aq)+Ci−(aq)

Compute the pH of the titration solution before any acid is added, when the titration is at the half-equi valence point, when the titration is at the equivalence point, and when the titration is 1.00 mL past the equivalence point

Answer 1

Here is the Solution:

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