You titrate 25.0 mL of 0.10 M NH₃ with 0.10 M HCl.
(a) What is the pH of the NH₃ solution before the titration begins?
(b) What is the pH at the equivalence point?
(c) What is the pH at the halfway point of the titration?
(d) What indicator in Figure 17.11 could be used to detect the equivalence point?
(e) Calculate the pH of the solution after adding 5.00, 15.0, 20.0, 22.0, and 30.0 mL of the acid. Combine this information with that in parts (a)–(c) and plot the titration curve.

Data given in Figure 17.11

Transcribed Image Text:

2 3 Crystal violet Cresol red Thymol blue 5 6 Erythrosin B 2,4-Dinitrophenol Bromphenol blue Methyl orange Bromcresol green Methyl red 8 Eriochrome black T Bromcresol purple Alizarin 10 Bromthymol blue Phenol red 10 I m-Nitrophenol 11 o-Cresolphthalein Phenolphthalein 12 Thymolphthalein 13 14 Alizarin yellow GG Figure 17.11 Common acid-base indicators. The color changes occur over a range of pH values. Notice that a few indicators have color changes over two different pH ranges.