Drug analysis

S.H. Burungale

1. Drug Analysis Dr. S. H. Burungale

2. Definition Drug  is a chemical substance used to  treat, cure, prevent, or diagnose  a disease or to promote well-being Introduction to Drugs

3. Anti hyperlipidemic Anti hypertensive Anti hyperuricemic agents Anti malarial agents Anti metabolites Anti migraine agents Anti neoplastic Anti platelet agents Antipsychotics Anti rheumatics Anti septic and germicides Anti thyroid agents Classification of Drugs

4. Plant sources Animal sources Mineral/ Earth sources Microbiological sources Semi synthetic sources/ Synthetic sources Recombinant DNA technology Sources of the Drugs

5. Raw material employed in Manufacturing Method or the process employed in Manufacturing Chemical Process and Plant materials employed in the process Storage Condition Decomposition Sources of Impurities

6. Limit test is defined as semi quantitative test designed to identify and control small quantities of impurity which is likely to be present in the substance.  Limit test is generally carried out to determine the inorganic impurities present in compound. In short, limit test is nothing but to identify the impurities present in the substance and compare it with standard.  Importance of Limit tests: To find out the harmful amount of impurities To find out the avoidable/unavoidable amount of impurities Limit test of impurities

7. Limit test for Lead 25 ml test solution Maintain pH 3-4 by Acetic acid 10 ml H 2 S Solution 25 ml Standard solution (20 ppm ) Maintain pH 3-4 by Acetic acid 10 ml H 2 S Solution

8. The limit test for Iron is based on the reaction between iron and Thiogycolic acid in ammonical solution to form pink to deep reddish purple coloured complex of iron thioglycollate . Limit Test for Iron

9. Limit Test for Iron 10 ml Test solution 2 ml Citric Acid 0.1 ml Thiogycolic acid Ammonia till alkaline 10 ml Standard solution (20 ppm ) 2 ml Citric Acid 0.1 ml Thiogycolic acid Ammonia till alkaline

10. The limit test for Arsenic is based on the conversion of Arsenic to Arsine gas (AsH 3 ) which when passed over mercuric chloride test paper which produces yellow stain. Step I Arsenic is converted Arsenic acid Step II Arsenic acid is reduced by different reducing agents like potassium iodide, stannous chloride etc. Limit Test for Arsenic

11. Step III The nascent hydrogen produced during the reaction converts arsenious acid to Arsine gas which reacts with mercuric chloride paper and produces yellow stain.

12. Gutzeit Apparatus

13. Estimation of Halide (Oxygen flask Combustion method)

14. Advantages It is suitable for titration of very weak acids and bases It also provides a solvent in which organic compounds are soluble. Non Aqueous Titrations Competition of water with weak acids and bases for protons

15. Types of solvents used in Non aqueous titrations Protogenic solvents Protophilic Amphiprotic

16. Sodium Nitrite titrations are also known as Diazotization Titration Substances containing primary aromatic amino group are assayed by these type of titration Sodium Nitrite Titrations

17. A demonstration of Beer's Law. A  aqueous solution of  rhodamine  (a  fluorescent dye ) is illuminated with a green laser pointer. Note how far the green light travels before it is fully absorbed (the length of the yellow-green line ). The same green laser illuminating an aqueous  rhodamine  solution of lower concentration. Note the laser light is visible to a greater depth than observed in the photo above, because the less concentrated solution absorbs the light less efficiently (i.e., the more dilute solution has lower c). UV and Visible Spectrometry Methods Illustrated Glossary of Organic Chemistry Beer's Law (Beer-Lambert Law):  The amount of energy absorbed or transmitted by a solution is proportional to the solution's  molar  absorptivity and the concentration of  solute . In simple terms, a more concentrated solution absorbs more light than a more dilute solution does. Mathematical statement of Beer's law is A =  ε l c, where: A = absorption;  ε  =  molar  absorptivity (amount of energy absorbed per  mole of substance dissolved),  l  = path length (the thickness of the solution), and c = concentration of the solution.                                                                                                                                                                                                                                                                                                          The amount of energy absorbed or transmitted by a solution is proportional to the solution's  molar  absorptivity and the concentration of solute.

18. Flourimetry