1. Chem. 31 – 1/26 Lecture

2. What is Quantitative Analysis? (and Why is it important?) Quantitative Analysis is the determination of a compound’s concentration (or mass or amount) in a sample Some examples of where a compound’s concentration is important: –level of intoxication from blood alcohol content –determine whether a compound (e.g. F - in drinking water) is beneficial or harmful –risk of having health problems (such as from high LDL concentrations or low HDL concentrations)

3. Roll Call

4. Handouts Syllabus Homework Set #1 Laboratory Report Schedule (discussed more in lab)

5. Typical Lecture Style Mix of white board or document camera and powerpoint slides Use white board/document camera for working out detailed problems Use Powerpoint slides for covering review material (e.g. Chapter 1) or material where having good graphics helps Powerpoint slides will be made available on website Announcements given in first few minutes

6. Why is This Course Valuable? Analysis of chemicals is common in other chemistry classes (e.g. Chem. 25, Chem. 125, Chem. 141, Chem. 161, etc.). Many of the jobs both within chemical industry/pharmaceutical industry and in applied areas (e.g. environmental service and biotech) involve chemical analysis.

7. Research Projects - some examples of chemical analysis Quantitation of glycoprotein oligosaccharides (joint with Dr. Peavy) protein oligosaccharides Glucose oligomer standard Oligosaccharides from protein in Xenopus laevis egg glycoproteins

8. Research Projects - some examples of chemical analysis Measurement of new diesel fuels –biodiesel (on-campus effort to use waste fryer oil to fuel lawn mowers) –synthetic diesel (made from CO + H 2 ) Chromatogram (each peak = 1 compound)

9. Traditional vs. Modern Methods CharacteristicTraditionalModern EquipmentGlassware and balances (low cost) Instruments (high cost) PrecisionHighModerate Speedslowfast Sensitivitylowhigh SelectivityminimalGood to great

10. Chapter 1 – Measurements and Titrations No measurement is valuable unless it is given with units and some measure of uncertainty Units – Chapter 1 Uncertainty – Chapters 3 and 4

11. Units of Measure Most Basic – SI base units (important ones) MeasureUnit_____ Lengthmeter (m) Masskilogram (kg) (only one with multiplier) Timesecond (s) TemperatureKelvin (K) AmountMole (mol)

12. Units of Measure Directly Derived from Base Units –Volume: cube volume = l 3 so units = m 3 –Density = m/V so kg/m 3 –Pressure = force(kg·m/s 2 )/area(m 2 ) = kg/(s 2 ·m) l

13. Units of Measure Other metric units (not directly in SI units) –Density (g/cm 3 ) –Pressure (Pascals or Pa = kg/(s 2 ·m)) Non-metric units (used commonly) –For pressure 1 atmosphere (atm) = 101300 Pa –English/Other system (not emphasized here)

14. Units of Measure Metric Multipliers (ones you should know) NameAbbreviationMultiplier Kilokx10 3 Centicx10 -2 Millim x10 -3 Micro  x10 -6 Nanonx10 -9 Analytical chemists like small quantities. An instrument that can detect 1 fg (1 x 10 -15 g) is better than an instrument that can detect 1 pg (1 x 10 -12 g)