Ammonia is a weak base with a K of 1.8 X 10-5. A 140.0-mL sample of a 0.200 M solution of aqueous ammonia is titrated with a 0.100 M solution of the strong acid HCI at 25 °C. The reaction is NH3 (aq) + HCI (aq) NH4+ (aq) Calculate the pH of the titration solution for each case. (a) Before any acid is added. (b) When the titration is at the half-equivalence point. (c) When the titration is at the equivalence point. (d) When the titration is 1.00 mL past the equivalence point. + CI (aq)

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Ammonia is a weak base with a K₂ of 1.8 X 10-5. A 140.0-mL sample of a 0.200 M solution of
aqueous ammonia is titrated with a 0.100 M solution of the strong acid HCI at 25 °C. The
reaction is
NH3 (aq) +
HCI (aq)
NH4+ (aq)
Calculate the pH of the titration solution for each case.
(a) Before any acid is added.
(b) When the titration is at the half-equivalence point.
(c) When the titration is at the equivalence point.
(d) When the titration is 1.00 mL past the equivalence point.
+ CI (aq)
Transcribed Image Text:Ammonia is a weak base with a K₂ of 1.8 X 10-5. A 140.0-mL sample of a 0.200 M solution of aqueous ammonia is titrated with a 0.100 M solution of the strong acid HCI at 25 °C. The reaction is NH3 (aq) + HCI (aq) NH4+ (aq) Calculate the pH of the titration solution for each case. (a) Before any acid is added. (b) When the titration is at the half-equivalence point. (c) When the titration is at the equivalence point. (d) When the titration is 1.00 mL past the equivalence point. + CI (aq)
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