1. Neutralization Reactions
Prentice Hall Chapter 19.4
Dr. Yager

2. Objectives Define the products of an acid-base reaction
Explain how acid-base titration is used to calculate the concentration of an acid or a base
Explain the concept of equivalence in a neutralization reaction
Describe the relationship between equivalence point and end point of a titration

3. Reactions of Acids and Bases
In general, the reaction of an acid with a base produces water and one of a class of compounds called salts.
Reactions in which an acid and a base react in an aqueous solution to produce a salt and water are generally called neutralization reactions.

5. Titration
The process of adding a known amount of solution of known concentration to determine the concentration of another solution is called titration.

6. Equivalence Point
When an acid and base are mixed, the equivalence point is when the number of moles of hydrogen ions equals the number of moles of hydroxide ions.

9. H3PO4 +3KOH → K3PO4 +3H2O

10. Doing a Titration
The solution of known concentration is called the standard solution.
Indicators are often used to determine when enough of the standard solution has been added to neutralize the acid or base.
The point at which the indicator changes color is the end point of the titration.
For a titration using a strong acid and a strong base, the point of neutralization is the end point of the titration.

11. Doing a Titration Added base is measured with a buret.
Color change shows neutralization.
Acid solution with indicator

17. H3PO4 + 3NaOH → Na3PO4 + 3H2O

18. 1. When a neutralization takes place, one of the products is always
carbon dioxide.
a salt.
sodium chloride.
a precipitate.

19. 1. When a neutralization takes place, one of the products is always
carbon dioxide.
a salt.
sodium chloride.
a precipitate.

20. 2. In a titration, 45. 0 mL of KOH is neutralized by 75. 0 mL of 0
2. In a titration, 45.0 mL of KOH is neutralized by 75.0 mL of 0.30M HBr. What is the concentration of the KOH solution?
0.18M
0.60M
0.25M
0.50M

21. 2. In a titration, 45. 0 mL of KOH is neutralized by 75. 0 mL of 0
2. In a titration, 45.0 mL of KOH is neutralized by 75.0 mL of 0.30M HBr. What is the concentration of the KOH solution?
0.18M
0.60M
0.25M
0.50M

22. 3. How many moles of HCl are required to neutralize an aqueous solution of 2.0 mol Ca(OH)2?

23. 3. How many moles of HCl are required to neutralize an aqueous solution of 2.0 mol Ca(OH)2?

24. H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(aq)
4. In which of the following neutralization titrations of 1-molar solutions of H2SO4 and NaOH will the equivalence point be reached at the very end of the additions?
H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(aq)
200 mL of H2SO4 is slowly added to 100 mL of NaOH
200 mL of H2SO4 is slowly added to 200 mL of NaOH
100 mL of H2SO4 is slowly added to 200 mL of NaOH
100 mL of H2SO4 is slowly added to 100 mL of NaOH

25. H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(aq)
4. In which of the following neutralization titrations of 1-molar solutions of H2SO4 and NaOH will the equivalence point be reached at the very end of the additions?
H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(aq)
200 mL of H2SO4 is slowly added to 100 mL of NaOH
200 mL of H2SO4 is slowly added to 200 mL of NaOH
100 mL of H2SO4 is slowly added to 200 mL of NaOH
100 mL of H2SO4 is slowly added to 100 mL of NaOH