CHEMISTRY 59-320 ANALYTICAL CHEMISTRY Fall - 2010

1. CHEMISTRY 59-320ANALYTICAL CHEMISTRYFall - 2010 Lecture 10 Chapter 27: Gravimetric and combustion analysis

2. Midterm exam • Time: Oct. 21 between 8:30 and 9:40 AM. • Location: BB121 or CHS 51, depending on your surname (A – J write in room CHS51) • The exam covers chapters 0-7 and chapter 27. • It consists of (1) multiple choice (~ 25%), (2) short answers and analysis (~15%), and (3) calculations (~60%).

3. Gravimetric Analysis • Gravimetric Analysis – one of the most accurate and precise methods of macro-quantitative analysis. • Analyte selectively converted to an insoluble form. • Measurement of mass of material • Correlate with chemical composition • Why choose this technique? -- Simple -- Often required for high precision

4. How to Perform a Successful Gravimetric Analysis • What steps are needed? • Preparation of the solution • Precipitation • Digestion • Filtration • Washing • Drying or igniting • Weighing • Calculation

5. How to Perform a Successful Gravimetric Analysis • Precipitation Techniques • Add precipitating reagent to sample solution • Reacts with analyte to form insoluble material • Precipitate has known composition or can be converted to known composition • Precipitate handling involves • Quantitative collection (no losses) • Isolation of pure product • Measure mass of precipitate (Direct or By difference) • Calculation of original analyte content (concentration). It requires the knowledge of Chemistry, Stoichiometry, and Composition of precipitate

6. How to Perform a Successful Gravimetric Analysis • Desirable properties of analytical precipitates: • Readily filtered and purified • Low solubility, preventing losses during filtration and washing • Stable final form (unreactive) • Known composition after drying or ignition

7. Filterability of Precipitates • Colloidal suspensions • 10-7 to 10-4 cm diameter • Normally remain suspended • Very difficult to filter • Crystalline suspensions • > tenths of mm diameter • Normally settle out spontaneously • Readily filterable

8. 27-1 An example of gravimetric analysis • The determination of Cl- by precipitating with Ag+ : A 10.00 ml solution containing Cl- was treated with excess AgNO3 to precipitate 0.4368 g of AgCl. What was the molarity of Cl- in the unknown. • Solution: The formula mass of AgCl is 143.321 0.4368 g/ (143.321 g/mol) = 3.048 x 10-3 mol Based on 1:1 stoichiometric relationship: [Cl-] = 3.048 x 10-3 mol /(0.01000 L) = 0.3048 M

11. 27.2 Precipitation The ideal product of a gravimetric analysis should be: very pure insoluble easily filterable known composite Nucleation: molecules in solution come together randomly and form small aggregates. Supersaturated: a solution contains more Solute than should be present at equilibrium.

12. Techniques that promote particle growth: -- raising the temperature to increase solubility and thereby decrease supersaturation. -- Adding precipitant slowly with vigorous mixing -- Using a large volume of solution so that the concentrations of analyte and precipitant low • Homogeneous precipitation • Precipitation in the presence of electrolyte.

13. 27.3 Examples of Gravimetric calculations • Problem 27-12: Marie Cure dissolved 0.09192 g of RaCl2 and treated it with excess AgNO3 to precipitate 0.08890 g of AgCl. In her time (1900), the atomic mass of Ag was known to be 107.8 and that of Cl was 35.4. From these values, find the atomic mass of Ra that Marie Curie would have calculated. • Answer: The formula mass of AgCl is (35.4 + 107.8) = 143.2 0.08890 g/(143.2 g/mol) = 6.2081 x10-4 mol. Cl- is 6.2081 x10-4 mol RaCl2 is (6.2081 x10-4)/2 mol the formula mass of RaCl2 is 0.09192/(3.10405x10-4 ) = 296.1292 the atomic mass of Ra = 296.1292 – 2x35.4 = 225.329 = 225.3

14. Example: A problem with two components • Problem 27-22:

15. 27.4 Combustion analysis

16. Combustion analysis (2)

17. Thermal analysis

18. Lab 2:Gravimetric determination of calcium • Prep time for Experiment 2 will begin the week of October 11, 2010.  • For students in Lab Sections 53 - 60, please attend on your regularly scheduled lab day between 12:30 p.m. to 4:30 p.m. during the week of October 11th to prep for Experiment 2.  • Your GA will be in the lab during these hours to assist and answer any questions you may have regarding the experiment.  • For students in Lab Sections 51 and 52, please attend Friday, October 15th between the hours of 9:30 a.m. to 1:30 p.m. to prep for Experiment 2.  • If you have a problem attending the prep session on your regularly scheduled lab day during the hours indicated, please contact your GA for alternative arrangements.

19. A few tips for Lab Preparation • Steps that have great impacts on your final accuracy. • Label your glassware in a way that your partner can easily recognize, such as 52 – 2 -1 ; 52-2-2 … (e.g. section # -- group # -- crucible #). • Standard deviation and Q test? • Discuss with your partner. In case you have a busy week, one can come in to clean and place the three crucibles into the oven, while the other weights the crucibles an hour late.

20. Data analysis • (H2N)2CO + 3H2O + heat ⇌ CO2 + 2NH4+ + 2OH- • Ca2+ + C2O42- + H2O ⇌ CaC2O4 · H2O • The dried precipitate is CaC2O4 with a formula mass of 128 • # mol CaC2O4 = ?? g/(128 g/mol) = yy mol • # mol CaC2O4 = # mol CaO • Mass of CaO = yy mol x 56.0790 g mol-1 = yy2 g • % calcium = yy2/?? =