1. burette clamp ring stand burette erlenmeyer flask Titration

2.  Describe an acid/base titration.  Compare and contrast the end point and the equivalence point of a titration.  Determine the concentration of an unknown acid or base using titration data.  Determine the mass of an unknown acid or base using titration data

3. Titration – controlled neutralization reaction. Used to measure [ ] of unknown acid or base. A standard solution is required. Standard solution – solution of a strong acid or base of known concentration. **pH does not indicate concentration because weak acids/bases do not dissociate completely. HA + BOH  BA + H 2 O salt water

4. ring stand burette clamp erlenmeyer flask burette Titration Apparatus buret

5. Equivalence point – amount of standard added neutralizes the unknown sample. Endpoint – the indicator changes colour. Determined by adding a pH indicator. moles H + = moles OH - Eq. point - defined by reaction stoichiometry. Endpoint - determined by the choice of indicator. (pH = 7)

7. 1.Measured amount of acid of unknown concentration is added to the flask. 2.An appropriate indicator is added to the unknown. 3. Measured amount of base of known concentration is added slowly to the flask. 4. The titration is stopped when a colour change has occurred (end point). 5.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 25.00 mL is just neutralized by 40.00 ml of a 0.150 mol/L sodium hydroxide solution. HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O (l) 1:1 ratio0.00600 moles of HCl = 0.006 moles NaOH 0.150 mol0.04 L 1 L = 0.240 M HCl 0.006 mol 0.025 L

9. What volume of a 0.250 mol/L solution of carbonic acid is needed to neutralize 30.0 g of sodium hydroxide. H 2 CO 3(aq) + 2 NaOH (aq) Na 2 CO 3(aq) + 2 H 2 O (l) = 0.750 moles NaOH 30.0 g1 mole 40.0 g Molar mass of NaOH = 40.0 g

10. 1.5 L of 0.250 mol/L H 2 CO 3 will neutralize 30.0 g of NaOH = 0.375 moles H 2 CO 3 0.750 mol1 H 2 CO 3 2 NaOH = 1.5 L H 2 CO 3 0.375 mol1 L 0.250 mol 2:1 ratio

11. Determine the concentration of a hydrochloric acid solution using a 0.100 mol/L solution of NaOH Indicator - phenolphthalein (endpoint turns pink) HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O (l)

12. 1. Calculate the moles of base used: 1:1 ratio0.001383 moles of HCl = 0.001383 mol NaOH 0.100 mol0.01383 L 1 L = 0.121 M HCl 0.001383 mol 0.01144 L 2. Use stoich to determine moles of acid used: 3. Calculate unknown value.

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. 2. Strong base titrated with strong acid. 3. Weak acid titrated with strong base. 4. Weak base titrated with strong acid.

15. The equivalence point is the centre of the steepest portion of the curve. SA - SB

16. SB - SA

17. WA - SB Phenolphthalein not suitable indicator.

18. WB - SA

19.  Eqv pt of a SA-SB / SB-SA titration is at pH = 7.  Eqv pt of a WA-SB titration had a pH > 7.  Eqv pt of a WB-SA titration has a pH < 7.  Chose indicator that changes colour (end point) near the expected Eqv pt.