Analytical chemistry involves qualitative and quantitative analysis. Qualitative analysis identifies elements and compounds in a sample, while quantitative analysis determines the amount present. Analytical chemistry plays a vital role across many fields by measuring substances at trace levels down to parts per million. It uses a variety of methods like gravimetric, volumetric, spectroscopic, electroanalytical and others to prepare samples and conduct analyses important for research, manufacturing, clinical labs, forensics and more.

1. • The nature of analytical chemistry.
•]
• Qualitative and quantitative analysis.
• Sensitivity of analysis.
• Solution.
• Electrolytes.
• Solubility rules.
CHAPTER 1 BOOK OF
ANALYTICAL CHEMISTRY-
ANALYTICAL CHEMISTRY
Lecture 1 contents

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

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

9. Sensitivity of analysis
Trace analysis = 1-1000 ppm or 0.0001-0.1 wt.%
Ultrtrace analysis = < 1ppm or 0.0001 wt.%
Macro- = >1mg
Micro- = < 1 mg

10. 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.
The Role 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. 1- Formulating the question.
2- Selecting the analytical procedure.
Steps in chemical analysis

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

16. • 3- Sample preparation
Steps in chemical analysis

17. 3- Analysis
4- Interpretation and reporting
5- Drawing conclusions
Steps in chemical analysis

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

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

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

21. • 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 .
Types of Analysis

22. 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
Quantitative Analytical Methods

23. SI Units (International System of Units)
Measurements

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. solvent
solute
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.

27. • Example: Salt water
– 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.
Examples

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

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

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