1. Review cation Ion charges anion
Ionic compounds are made of cations and anions. The cation is always first followed by the anion. Ionic compounds are NEUTRAL, so you may have to criss cross the charges of your ions. Ex: Mg2+ Cl-
MgCl2

2. Neutralization

3. 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

4. Example: NaCl + H2O salt water HCl + NaOH  Mg(OH)2(aq) + 2HCl(aq) 
acid
base
Mg(OH)2(aq) + 2HCl(aq) 
HNO NaOH 
Ba(OH)2 + HCl 
H2SO4 + CsOH 
HNO KOH 

5. Practice Problem #1 C
NH HCl  NH4+ + Cl-
base acid

6. Reading a Buret

10. Titrations

11. 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.

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

13. Analyte/Unknown Solution - The solution that is being analyzed
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

14. Titrant or Standard Solution (known concentration)
stopcock
Analyte (unknown concentration)

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

16. 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.

17. 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.

18. Titration Youtube Explanation of titration
Titration using pheonthalein

21. At the Endpoint
Past the endpoint
(overshot)
Before the endpoint

23. Calculations: Example 1
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.

24. HC2H3O2 + NaOH  H2O + NaC2H3O2

25. Example 2
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