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Lecture 1 first day(1)
- 1. Quantitative Analysis (CHEM309) Basic Information Office: Temple 4429 Office hours: MTWR Morning(or by appt) Instructor: Dr. Collinson Email: mmcollinson@vcu.edu Text: Harris, Quantitative Chemical Analysis, 8th ed. Course Information: Located on Blackboard Purchase and Register Clicker (Rf) via Blackboard
- 2. Quantitative Analysis Basic Information Grade tests(5): 70% **No Make up tests* final : 20% homework: 10% Bring clicker to class everyday and participate. Attendance at each and every class is very important
- 3. Class Objectives Students ShouldLearn 1. How to Solve Problems (Acid-Base Chemistry) 2. Apply chemical concepts to chemical analysis 3. Different Analytical Techniques and Methods 4. Appreciation for Analytical Measurements 5. Appreciation for error in chemical analysis
- 4. First Law ofReality: Second Law of Reality: What you put in determines what you get out! “Learning is a choice – your choice!”
- 5. Keys to Success •Attendand participate in EVERY class •Do homework each night •Read the book each night; outline chapters as needed •Seek help when needed
- 6. Classroom Etiquette Do nottalk when the instructor is talking Laptops can be used to take notes, not for surfing the web Silence cell phones Abide by the VCU Honor Code
- 7. Chapter 1: Introduction AnalyticalChemistry • Making Chemical Measurements Quantitative Analysis Determine how much is present Qualitative Analysis Determine what is present
- 8. Classification of AnalyticalMethods Classical methods • gravimetric • Titrimetric Instrumental methods • Spectroscopy (light – sample interactions) • Electroanalytical (interaction of charges and ions) • Chromatography (purification and qualification)
- 9. First: The Basics VeryImportant: Memorize! Know SI Base Units (Very Important)
- 10. Clicker Question: Express thefollowing number in units of picomoles: 300 nm
- 11. Concentrations Examples • Molarity (M) •Formality (F) • Molality (m) • Normality (N) • Percent Composition • Density • ppm/ppb • p-functions
- 12. Concentrations Examples • Molarity (M) molesof solute / liter of solution mmoles of solute / mL of solution Very important
- 13. Concentrations Examples • Molarity • Formality(F) ex. KCl Your book loves using formality
- 14. Concentrations Examples • Molarity (M) •Formality (F) • Molality (m) • Normality
- 15. Concentrations Examples • Molarity • Formality(F) • Molality • Normality • Percent Composition (1) wt % : mass of solute (g) / mass of soln (g) x 100% (2) vol% : vol of solute (mL) / vol of soln (mL) x 100% (3) wt/vol % : mass of solute (g) / vol of soln (mL) x 100% Very important
- 16. Concentrated ammonium hydroxidecontains 27.0% (w/w) NH3. The density is 0.90 g/mL. What is the molarity of this concentrated solution. Example 1
- 17. Concentrations Examples • Molarity • Formality(F) • Molality • Normality • Percent Composition • Density density mass/volume (units: g/mL or Kg/L) Very important
- 18. Concentrations Examples • Molarity • Formality(F) • Molality • Normality • Percent Composition • Density/Specific Gravity • ppm/ppb mass of solute / mass of solution x 106 mass of solute / mass of solution x 109 Very important
- 19. Concentrations Examples • Molarity • Formality(F) • Molality • Normality • Percent Composition • Density • ppm/ppb • p-functions Very important
- 20. Saltwater contains 17.8ppm NO3 - . The density of the solution is 1.02 g/mL. Calculate the Molarity. Example 2
- 21. Concentrations Other Concepts: Review •Balance Equations • Stoichiometry • Limiting Reagent • Convert btwn solution conc. (ex. M to %comp or ppm) • Dilutions (M1V1 = M2V2) …it’s all about the units…