1. Lecture 1 contents
The nature of analytical chemistry.
Qualitative and quantitative analysis.
Sensitivity of analysis.
 Solution.  
Electrolytes.
Solubility rules.

2. Quantitative Analysis Qualitative Analysis
Analytical Chemistry
Quantitative Analysis
Qualitative Analysis
Gravimetric Analysis
Instrumental Analysis
Volumetric Analysis

3. It is a Measurements science consisting of a set of powerful ideas and methods that are useful in all field of science and medicine.

5. Qualitative Analysis (identification)
Provides information about the elements and compounds in a sample.
“Identifying what is in unknown”
Quantitative Analysis
provides information about the amount of each substance in a sample .
“Identifying how much is present”

6. Qualitative analysis is what. Quantitative analysis is how much.
©Gary Christian, Analytical Chemistry, 6th Ed. (Wiley)

8. Analyets
Substances being measured
Species
Any chemical of interest in the analysis

9. Sensitivity of analysis
Trace analysis = ppm or wt.%
Ultrtrace analysis = < 1ppm or wt.%
Macro- = >1mg
Micro- = < 1 mg

10. The Role of Analytical Chemistry
Analytical chemistry plays a vital role in the development of science.
Plays a vital role in many research areas in chemistry, biochemistry, biology, geology, physics and the other sciences.
All branches of chemistry draw on the ideas and techniques of analytical chemistry.
All branches of chemistry draw on the ideas and techniques of analytical chemistry

11. Where is Analytical Chemistry used?
1- Clinical laboratories.
2- Forensic laboratories.
3-Environmental laboratories.
4- Manufacturing /industry
5- Research.
6- Others.

12. Analytical chemistry and other branches of sciences

13. Steps in chemical analysis

14. Steps in chemical analysis
1- Formulating the question.
2- Selecting the analytical procedure.

15. Steps in chemical analysis
3- Sampling
Sampling: selecting representative material to analyze

16. Steps in chemical analysis
3- Sample preparation

17. Steps in chemical analysis
4- Interpretation and reporting
5- Drawing conclusions

18. Sample preparation 1- sample storage(e.g. temperature, moisture)
2- Grinding ,extracting analyte ,etc

19. Sample preparation 3- Dissolving sample, dispersing analyte)
4- Concentrating analyte.

20. Sample preparation
5- Eliminate interfering/ “mask” species (drying , ingnition ,isolation).

21. Types of Analysis Gravimetric Methods:
Measure the mass of the analyte or some compound chemically related to it.
Volumetric Methods:
Measure the volume of a solution containing sufficient reagent to react completely with the analyte .

22. Quantitative Analytical Methods
Spectroscopic Methods:
measurement based on interaction between electromagnetic radiation and analyte .
Mass spectrometry
Measure of mass to charge ratio (m/z) of analyte.
Electroanalytical Methods:
measure of electrical properties such as voltage, current, resistance and quantity of electrical charge.
Others :
Radioactive decay, heat of reaction, optical activity, refractive index, rate of reaction

23. Measurements
SI Units (International System of Units)

24. Measurements
Prefixes used with SI Units

25. Mass /amount of substance
Mass kilogram (kg) gram (g)
Amount of substances moles (mol)
1 mole = 6.022×1023 particles (e.g. atoms, molecules, ions) .
Atomic mass = number of grams containing  Avogadro's number (6.022×1023 ) of atoms
Molecular mass = number of grams containing Avogadro's number (6.022×1023 ) of molecules; sum of atomic masses of elements in a molecule

26. Solution
solution
Solution : A homogenous mixture of two or more substances, the solute and the solvent.
A solute is what dissolves or disappears, like salt or sugar.
A solvent is what does the dissolving.
solute
solvent

27. Examples Example: Salt water Example – 70% ethanol solution.
What is the solute?______
What is the solvent?___________
Example – 70% ethanol solution.
Solute _______________
Solvent________________
Why?
Salt
water
Water
ethanol
If 70% is ethanol, then it must be the solvent. The remaining 30% is water, the solute.

28. Solute dissolve to form
Solution
-Solutions can be electrolytes or non- electrolytes .
Solute dissolve to form
Ions
electrolytes
Molecules
Non-electrolytes

29. Some non-electrolytes can also dissolve in water
Solution
Some non-electrolytes can also dissolve in water

30. Solution
e.g. NaCl salt

31. Electrolyte
Electrolytes: A substance that dissociates into ions in aqueous solution and conduct electricity.

33. Like dissolves like

34. Making solutions