1. Topic: Titration
Do Now:

2. Acid-Base Titration
A procedure used in order to determine the molarity of an acid or base
Known volume of a solution with a known concentration (standard solution) and known volume of unknown concentration and a
MAVA = MBVB
acid-base indicator needed

3. Titration Standard solution slowly added to unknown solution
As solutions mix:
neutralization reaction occurs
Eventually:
enough standard solution is added to neutralize the unknown solution  Equivalence point

4. total # moles H+1 ions donated by acid equals
Equivalence point
total # moles H+1 ions donated by acid equals
total # moles H+1 accepted by base
total moles H+1 = total moles OH-1

5. Titration End-point = point at which indicator changes color
if indicator chosen correctly:
end-point very close to equivalence point

6. Titration of a strong acid with a strong base
14-
Phenolphthalein
Color change:
8.2 to  pH 7-
Equivalence Pt  0-   
Volume of M NaOH added (ml)
0 ml
40ml
20 ml

7. MH+1 VH+1 = MOH-1 VOH-1 MH+1 = molarity of H+1
MOH-1 = molarity of OH-1
VH+1 = volume of H+1
VOH-1 = volume of OH-1

8. Titration Problem #1
In a titration of 40.0 mL of a nitric acid solution, the end point is reached when 35.0mL of M NaOH is added
Calculate the concentration of the nitric acid solution
HNO3 + NaOH  H2O + NaNO3

9. Variables # of H’s = 1 Ma = ? Va = 40.0 mL # of OH’s = 1 Mb = 0.100 M
Vb = 35.0 mL

10. (1)(X) (40.0 mL) = (0.100 M )(35.0mL)(1)
X = M HNO3

11. Titration Problem #2
What is the concentration of a hydrochloric acid solution if 50.0 mL of a 0.250M KOH solution is needed to neutralize 20.0mL of the HCl solution of unknown concentration?
KOH + HCl  H2O + KCl

12. Variables # of H’s = 1 Ma = X Va = 20.0 mL # of OH’s = 1 Mb = 0.250 M
Vb = 50.0 mL

13. (1)(X)(20.0 mL) = (0.250 M) (50.0 mL)(1)
X = M HCl

14. Titration Problem #3
What is the concentration of a sulfuric acid solution if 50.0mL of a M KOH solution is needed to neutralize 20.0mL of the H2SO4 solution of unknown concentration?
H2SO4 + 2 KOH  2 H2O + K2SO4

15. Variables
# of H’s = 2
Ma = X
Va = 20.0mL
# of OH’s = 1
Mb = 0.25M
Vb = 50.0mL

16. (2)(X)(20.0ml) = (0.25M)(50.0ml)(1)
X = M H2SO4(sulfuric acid)