1. Chem. 31 – 8/28 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. Course Instructors Dr. Roy Dixon (lecture and sect. 2 of lab)
I have been teaching this class for over 20 years
My educational and research background is in analytical chemistry (with work on environmental and biological problems)
Now, I’m teaching less as Department Chair
Dr. Jahansooz Toofan (lab – sect. 4, 6, and 7), Dr. Alexander Gunn (lab – sect. 2) Dr. Justin Miller Schulze (lab – sect. 3) and Ms. Heidi Van Atta (lab – sect. 5)

4. Roll Call
Sign in to sheet being passed around

5. Handouts
Syllabus
Other materials will be posted online

6. Typical Lecture Style Mix of whiteboard and Powerpoint slides
Use whiteboard 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

7. 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.

8. Examples of Chemical Analysis from Term Projects in Chemical Instrumentation (Chem 133 – S’16)
Biodiesel Analysis (3 projects)
Biodiesel is being produced on campus from waste cooking oil
Composition can affect lifetime and use in cold weather
In addition, analysis is needed for problematic compounds (methanol, glycerol, other glycerides, free fatty acids)
Example fatty acid: CH3(CH2)7CH=CH(CH2)7CO2H
= Oleic = C18:1
C18:3
C18:2
C18:1
C18
C17
C16
triglyceride
fatty acid methyl esters (FAMEs)

9. Traditional vs. Modern Methods
Characteristic
Traditional
Modern
Equipment
Glassware and balances (low cost)
Instruments
(high cost)
Precision
High
Moderate
Speed
slow
fast
Sensitivity
low
high
Selectivity
minimal
Good 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)
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) = 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 g) is better than an instrument that can detect 1 pg (1 x g)

15. Unit Conversion – Example Problem
Convert the density of lead from g/cm3 to kg m-3 if density = 11.7 g cm-3.

16. Concentration Units General form
Note: sometimes, volume is required in the denominator to be strictly considered “concentration”, but for this class mass ratios or mole ratios will be considered to be an expression of concentration