1. Indicators and pH Meters
Section 2 Determining pH and Titrations
Chapter 15
Indicators and pH Meters
Acid-base indicators - compounds whose colors are sensitive to pH.
Indicators change colors because they are either weak acids or weak bases.
HIn and In are different colors.
In acidic solutions, most of the indicator is HIn
In basic solutions, most of the indicator is In–

2. Indicators and pH Meters
Section 2 Determining pH and Titrations
Chapter 15
Indicators and pH Meters
Transition interval - pH range over which an indicator changes color
Indicators that change color at pH lower than 7 are stronger acids than the other types of indicators.
They tend to ionize more than the others.
Indicators that undergo transition in the higher pH range are weaker acids.

3. Indicators and pH Meters
Section 2 Determining pH and Titrations
Chapter 15
Indicators and pH Meters
pH meter - determines the pH of a solution by measuring the voltage between the two electrodes that are placed in the solution.
The voltage changes as the hydronium ion concentration in the solution changes.
Measures pH more precisely than indicators

4. Color Ranges of Indicators
Section 2 Determining pH and Titrations
Chapter 15
Color Ranges of Indicators

5. Color Ranges of Indicators
Section 2 Determining pH and Titrations
Chapter 15
Color Ranges of Indicators

6. Color Ranges of Indicators
Section 2 Determining pH and Titrations
Chapter 15
Color Ranges of Indicators

7. H3O+(aq) + OH(aq) 2H2O(l)
Section 2 Determining pH and Titrations
Chapter 15
Titration
Neutralization occurs when hydronium ions and hydroxide ions are supplied in equal numbers by reactants.
H3O+(aq) + OH(aq) 2H2O(l)
Titration - controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration.

8. Chapter 15 Equivalence Point
Section 2 Determining pH and Titrations
Chapter 15
Equivalence Point
Equivalence point - point at which the two solutions used in a titration are present in chemically equivalent amounts
End point - point in a titration at which an indicator changes color

9. Chapter 15 Equivalence Point
Section 2 Determining pH and Titrations
Chapter 15
Equivalence Point
Indicators that undergo transition at about pH 7 are used to determine the equivalence point of strong-acid/strong base titrations.
The neutralization of strong acids with strong bases produces a salt solution with a pH of 7.

10. Chapter 15 Equivalence Point
Section 2 Determining pH and Titrations
Chapter 15
Equivalence Point
Indicators that change color at pH lower than 7 are used to determine the equivalence point of strong-acid/weak-base titrations.
The equivalence point of a strong-acid/weak-base titration is acidic.

11. Chapter 15 Equivalence Point
Section 2 Determining pH and Titrations
Chapter 15
Equivalence Point
Indicators that change color at pH higher than 7 are used to determine the equivalence point of weak-acid/strong-base titrations.
The equivalence point of a weak-acid/strong-base titration is basic.

12. Titration Curve for a Strong Acid and a Strong Base
Section 2 Determining pH and Titrations
Chapter 15
Titration Curve for a Strong Acid and a Strong Base

13. Titration Curve for a Weak Acid and a Strong Base
Section 2 Determining pH and Titrations
Chapter 15
Titration Curve for a Weak Acid and a Strong Base

14. Molarity and Titration
Section 2 Determining pH and Titrations
Chapter 15
Molarity and Titration
Standard solution - solution that contains the precisely known concentration of a solute
Primary standard - highly purified solid compound used to check the concentration of the known solution in a titration
The standard solution can be used to determine the molarity of another solution by titration.

15. Performing a Titration, Part 1
Section 2 Determining pH and Titrations
Chapter 15
Performing a Titration, Part 1

16. Performing a Titration, Part 1
Section 2 Determining pH and Titrations
Chapter 15
Performing a Titration, Part 1

17. Performing a Titration, Part 1
Section 2 Determining pH and Titrations
Chapter 15
Performing a Titration, Part 1

18. Performing a Titration, Part 2
Section 2 Determining pH and Titrations
Chapter 15
Performing a Titration, Part 2

19. Performing a Titration, Part 2
Section 2 Determining pH and Titrations
Chapter 15
Performing a Titration, Part 2

20. Performing a Titration, Part 2
Section 2 Determining pH and Titrations
Chapter 15
Performing a Titration, Part 2

21. Molarity and Titration
Section 2 Determining pH and Titrations
Chapter 15
Molarity and Titration
To determine the molarity of an acidic solution, 10 mL HCl, by titration
Titrate acid with a standard base solution mL of 5.0  103 M NaOH was titrated
Write the balanced neutralization reaction equation.
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
1 mol mol mol mol
Determine the chemically equivalent amounts of HCl and NaOH.

22. Molarity and Titration
Section 2 Determining pH and Titrations
Chapter 15
Molarity and Titration
Calculate the number of moles of NaOH used in the titration.
20.0 mL of 5.0  103 M NaOH is needed to reach the end point
amount of HCl = mol NaOH = 1.0  104 mol
Calculate the molarity of the HCl solution

23. Molarity and Titration
Section 2 Determining pH and Titrations
Chapter 15
Molarity and Titration
Start with the balanced equation for the neutralization reaction, and determine the chemically equivalent amounts of the acid and base.
2. Determine the moles of acid (or base) from the known solution used during the titration.
3. Determine the moles of solute of the unknown solution used during the titration.
4. Determine the molarity of the unknown solution.

24. Chapter 15 Sample Problem F
Section 2 Determining pH and Titrations
Chapter 15
Sample Problem F
In a titration, 27.4 mL of M Ba(OH)2 is added to a 20.0 mL sample of HCl solution of unknown concentration until the equivalence point is reached. What is the molarity of the acid solution?

25. Chapter 15 Antacid Visual Concepts
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Visual Concept