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Chem. 31 – 9/3 Lecture

Chem. 31 – 9/3 Lecture. 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:

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Chem. 31 – 9/3 Lecture

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  1. Chem. 31 – 9/3 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 (passed out in lab and 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) oligosaccharides protein Oligosaccharides from protein in Xenopus laevis egg glycoproteins Glucose oligomer standard

  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 + H2) Chromatogram (each peak = 1 compound)

  9. Traditional vs. Modern Methods

  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) Measure Unit_____ Length meter (m) Mass kilogram (kg) (only one with multiplier) Time second (s) Temperature Kelvin (K) Amount Mole (mol)

  12. Units of Measure • Directly Derived from Base Units • Volume: cube volume = l3 so units = m3 • Density = m/V so kg/m3 • Pressure = force(kg·m/s2)/area(m2) = kg/(s2·m) l

  13. Units of Measure • Other metric units (not directly in SI units) • Density (g/cm3) • Pressure (Pascals or Pa = kg/(s2·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) Name Abbreviation Multiplier Kilo k x103 Centi c x10-2 Milli m x10-3 Micro m x10-6 Nano n x10-9 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)

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