1. Chapter 15(a) Applications of Aqueous Equilibria

2. A digital pH meter shows the pH of the buffered solution to be 4.740.

3. Copyright © Houghton Mifflin Company. All rights reserved.15a–3 (left) Pure water at pH 7.000. (right) When 0.01 mol NaOH is added to 1.0 L of pure water, the pH jumps to 12.000.

4. Copyright © Houghton Mifflin Company. All rights reserved.15a–4

5. Copyright © Houghton Mifflin Company. All rights reserved.15a–5 Figure 15.1: The pH curve for the titration of 50.0 mL of 0.200 M HNO 3 with 0.100 M NaOH.

6. Copyright © Houghton Mifflin Company. All rights reserved.15a–6 Figure 15.2: The pH curve for the titration of 100.0 mL of 0.50 M NaOH with 1.0 M HCl.

7. Copyright © Houghton Mifflin Company. All rights reserved.15a–7 Figure 15.3: The pH curve for the titration of 50.0 mL of 0.100 M HC 2 H 3 O 2 with 0.100 M NaOH.

8. Copyright © Houghton Mifflin Company. All rights reserved.15a–8 Comparison of strong and weak acid titration curves.

9. Figure 15.4: The pH curves for the titrations of 50.0-mL samples of 0.10 M acids with various K a values with 0.10 M NaOH.

10. Copyright © Houghton Mifflin Company. All rights reserved.15a–10

11. Copyright © Houghton Mifflin Company. All rights reserved.15a–11 Figure 15.5: The pH curve for the titration of 100.0 mL of 0.050 M NH 3 with 0.10 M HCl.

12. Figure 15.6: The acid and base forms of the indicator phenolphthalein. In the acid form (Hln), the molecule is colorless. When a proton (plus H 2 O) is removed to give the base form (ln-), the color changes to pink.

13. Copyright © Houghton Mifflin Company. All rights reserved.15a–13 Methyl orange indicator is yellow in basic solution and red in acidic solution.

14. Copyright © Houghton Mifflin Company. All rights reserved.15a–14 Figure 15.7: (a) Yellow acid form of bromthymol blue; (b) a greenish tint is seen when the solution contains 1 part blue and 10 parts yellow; (c) blue basic form.