1. Neutralization – Day 1

2. Neutralization Reactions
A neutralization reaction is a reaction in which an acid and a base react to produce a salt and water
Acid + Base  Salt + H2O
A salt is an ionic compound made up of a cation and an anion

3. 3 Types of Acid-Base Reactions

4. Neutralization Reaction
HCl + NaOH 
NaCl
salt
+ H2O
water
acid
base

5. Neutralization Reactions
Mg(OH)2(aq) + 2HCl(aq) 
base acid
Write a balanced formula equation for the following acid base neutralization reaction
Nitric acid and sodium hydroxide
HNO NaOH 
MgCl H2O 2
Salt Water
NaNO H2O
Salt Water

6. Practice Neutralization Reactions
Write a balanced formula equation for the following acid base neutralization reactions:
Barium hydroxide and hydrochloric acid
Ba(OH)2 + HCl 
Sulfuric acid and cesium hydroxide
H2SO4 + CsOH 
Nitirc acid and potassium hydroxide
HNO KOH  2 2
H2O +
BaCl2 2 2
H2O +
Cs2SO4
H2O +
KNO3

7. Question Time What is a neutralization reaction? What is a salt?
Where does the cation in the salt come from?
Where does the anion in the salt come from?

8. Titration Day 2

9. Titration Purpose - To find the unknown concentration of a solution.
Procedure – Add a known amount of solution of known concentration to a solution of unknown concentration.

10. Titration Vocabulary
Buret – A piece of glassware used for dispensing accurate volumes of a solution.
The solution of known concentration is in the buret.

11. Titration Vocabulary
Analyte/Unknown Solution - The solution that is being analyzed. It is the solution of unknown concentration
Titrant/Standard Solution - The solution of known concentration that is added to the analyte

12. Titration Vocabulary
Equivalence Point - when the acid and base are mixed and the number of hydrogen ions equal the number of hydroxide ions.
[H+] = [OH-]

13. Titration
Acid–base indicator – A chemical dye whose colors are affected by acidic and basic solutions. A common acid base indicator for titration is phenolphthalein.
End point is the point which the indicator used in titration changes color.

14. Equivalence Point vs. End Point
The equivalence point is when [H+] = [OH-]. You cannot see this.
The end point is when you see a change in color in the indicator.
The equivalence point should be very close to the end point. To make sure this happens, an appropriate indicator needs to be chosen.

15. Question Time What is the purpose of titration?
What is a standard solution? What is another name for the standard solution?
What is the equivalence point?
What is phenolphthalein?
What is the end point?
What is the difference between the equivalence point and end point

16. You Tube Titrations http://www.youtube.com/watch?v=g8jdCWC10vQ
(1min 10 sec)
ated
(3 min 15 sec)
(4 min 51 sec)
(5min 3 sec)
(8min 50 sec-student video)

17. Titration Calculation Example
HC2H3O2 + NaOH  H2O + NaC2H3O2
In a titration, the volume of base needed was 9.50mL of M NaOH to reach equivalence point. The volume of HC2H3O2 acid titrated was mL. Find the molarity of the acid.

18. What is the standard solution?(the acid or the base)
HC2H3O2 + NaOH  H2O + NaC2H3O2
What is the standard solution?(the acid or the base)
9.50mL NaOH
1 L
0.500 mol NaOH
1 mol HC2H3O2
1000 mL
1 L NaOH
1 mol NaOH
mol HC2H3O2 =
mol HC2H3O2
1000 mL
0.806 mol HC2H3O2 L =
5.89 mL HC2H3O2
1 L
0.806 M HC2H3O2

19. Neutralization with Polyprotic Acids
If you are doing a neutralization where there is more than one hydrogen on the acid, your mole ratio will not be one to one.
Example:
H2SO4 + 2RbOH  2H2O + Rb2SO4
43.21mL RbOH
1 L
mol NaOH
1 mol H2SO4
1000 mL
1 L NaOH
2 mol RbOH
mol H2SO4 =
mol H2SO4
1000 mL
mol H2SO4 L =
30.00 mL H2SO4
1 L
or M H2SO4