1. Titration
burette clamp
ring stand
burette
erlenmeyer
flask

2. Calculate the concentration or volume of an acid or base from the concentration and volume of an acid or base required for neutralization.
Using a standardized acid or base, determine the concentration of an unknown base or acid.
Additional KEY Terms
standard solution equivalence point
end point titration

3. HA + BOH  BA + H2O Titration – quantitative chemical reaction.
unknown reacted with a standard solution
used to find [ ] of unknown solution
Standard solution – solution of known concentration which is compared to unknown.
HA + BOH  BA + H2O
2.0 M ???
**pH does not indicate concentration because weak acids/bases do not dissociate completely.

4. Acid / Base Titration Apparatus
burette clamp
burette
buret
ring stand
erlenmeyer
flask

5. amount of standard needed to neutralize the unknown sample
Equivalence point
amount of standard needed to neutralize the unknown sample
moles H+ = moles OH-
(pH = 7)
Eq. point - defined by balanced reaction
End point
point in the reaction when indicator turns colour.
Endpoint - determined by the choice of indicator

6. Goal is to pick the indicator with an end point at the same pH as the equivalence piont

7. Measured amount of unknown
concentration is added to the flask.
An appropriate indicator is added to the
unknown.
3. Measured amount of known concentration is added slowly from the buret.
The titration is stopped when a colour
change has occurred (end point).
Concentration of the acid is calculated.
**Titration can also be preformed with a calculated volume of standard in the flask, and the unknown in the buret.

8. Calculate the concentration of hydrochloric acid, if 25
Calculate the concentration of hydrochloric acid, if mL is just neutralized by ml of a mol/L sodium hydroxide solution.
NaCl(aq) + H2O(l)
HCl(aq) + NaOH(aq)
0.150 mol
0.04 L
= moles NaOH
1 L
1:1 ratio moles of HCl
0.006 mol
= M HCl
0.025 L

9. What volume of a mol/L solution of carbonic acid is needed to neutralize 30.0 g of sodium hydroxide.
H2CO3(aq) + 2 NaOH(aq)
Na2CO3(aq) + 2 H2O(l)
Molar mass of NaOH = 40.0 g
30.0 g
1 mole
= moles NaOH
40.0 g
1:2 ratio moles of H2CO3

10. 1.5 L of 0.250 mol/L H2CO3 will neutralize
1:2 ratio
0.750 mol
1 H2CO3
= moles H2CO3
2 NaOH
0.375 mol
1 L
= 1.5 L H2CO3
0.250 mol
1.5 L of mol/L H2CO3 will neutralize
30.0 g of NaOH

11. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
Determine the concentration of a hydrochloric acid solution using a mol/L solution of NaOH
Indicator - phenolphthalein (endpoint turns pink)
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

12. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
1. Calculate the moles of base used:
0.100 mol L
= mol NaOH
1 L
2. Use stoich to determine moles of acid used:
1:1 ratio moles of HCl
3. Calculate unknown value.
mol
= M HCl L

13. Titration Curves

14. Plotting pH values during a titration gives a titration curve.
Type of curve produced accounts for 2 classes of titrations:
1. Strong acid titrated with strong base.
Strong base titrated with strong acid.
2. Weak acid titrated with strong base.
Weak base titrated with strong acid.

15. SB - SA Strong w/ Strong titrations produce well defined,
steep s-curves

16. SA - SB Eq point is the centre of the steepest portion of the curve
Eq point is at a pH = 7

17. WA - SB
Strong w/ weak titrations produce sloppy s-curves

18. WB - SA Eq point not at pH = 7
due to secondary reaction with acidic or basic salt

19. CAN YOU / HAVE YOU?
Calculate the concentration or volume of an acid or base from the concentration and volume of an acid or base required for neutralization.
Using a standardized acid or base, determine the concentration of an unknown base or acid.
Additional KEY Terms
standard solution equivalence point
end point titration