Official compound of Iodine

Official compound of iodine and iodine contain preparation. Iodine uses, preparation, assay, storage, their physical, chemical properties and deficiency .

1. Official compounds of iodine Presented By Ms. Monika P. Maske M. Pharm (Pharmaceutical Chemistry) Kamla Nehru College of Pharmacy, Butibori , Nagpur

2. Iodine Introduction Iodine (as iodide) is one of essential trace element. Iodide with food after absorption reaches blood circulation. Play important role in synthesis of two important thyroid hormones known as thyroxine & triiodothyronine. Its essential for the normal growth & development Play a important role in energy metabolism

3. Structure of thyroxine & triiodothyronine

4. Iodine Thyroxine important function is to increase the metabolic rate by increasing the oxidative process. Deficiency of thyroid causes “hypothyroidism”, Cretinism. Metabolic processes are slowed down & gaiter characterised by swelling of neck. Male usual requirement of iodine is about 140 micrograms & female about 100 microgram daily usually obtained from diet.

5. Iodine

6. Iodine After internal administered iodide is oxidised to iodine. Then converted to an amino acid tyrosine to form monoiodo and diiodo tyrosine. It again converted to triodo and tetraiodo tyrosine by coupling reactions. Using radioactive iodide, iodine is incorporated in thyroid gland only for forming the thyroid hormones.

7. Iodine 1. Physical properties: Symbol- I 2 Mol. weight- 253.8 Colour- Bluish-black rhombic prism or plates Odour- Irritating odour Taste- Pungent tase Solubility- Insoluble in water - soluble in alcohol, freely soluble in chloroform, ether

8. Iodine 2. Chemical Properties:- At higher temperature iodine gets melt. It combines directly with non-metals & with many metals. 2P + 3I 2 2PI 2 Reducing agents react with aqueous iodine solution & gets oxidised. H 2 S + I 2 2 HI + S

9. Iodine Iodine react with alkali to form iodide & iodate especially when heated. 3I 2 + 6NaOH 5NaI + NaIO 3 + 3H 2 O Potassium iodine dissolves in iodine because of formation of ion KI + I 2 KI 3 Iodine add to unsaturated compounds & unsaturated acids present in oil. This principal reaction used in the preparation of non-staining iodine ointment. RCH = CH-COOH +I 2 RCHICH-COOH

10. Preparation Iodine mfg. by extracting kelp (seaweed ash) with water, the solution is concentrated. The sodium and potassium are crystals out. leaving freely soluble sodium & potassium iodide in the mother liquor. Sulphuric acid is added to mother liquor & sulphur allowed to settle. The mother liquor is decanted and MnO 2 then added and iodine is distilled out.

11. Preparation 2 NaI + 3H 2 SO 4 + MnO 2 MnSO 4 + 2NaHSO 4 + 2 NaHSO 4 + I 2 + 2H 2 O Impurities like ICl , IBr , and ICN are removed by heating crude iodine with potassium iodide. ICl + KI KCl + I 2

12. Assay Iodine is analysed by oxidation-reduction method. 0.5 g of iodine + potassium iodide + 5 ml of water + dissolved +dilute with 50 ml of water. Acidify with 1 ml of acetic acid + using starch as indicator. Titrated with 0.1 N sodium thiosulphate solution.

13. Uses Used as germicide and fungicide Powerful bactericidal Disinfectant of skin, mouth Management of burns and cuts Locating agent Treatment of thyrotoxicosis Purification of drinking water Chemical antidote for alkaloidal poising Analytical chemistry

14. Incompatibilism And Storage Iodine is oxidising agent, it oxidised hypophosphite, sulphites, some metals. It react with ammonia or ammoniated mercury to form explosive iodise of nitrogen. Storage iodine is stored in amber-coloured bottles with a tight stopper and kept in cool place.

15. Compound Containing Iodine Sodium iodide Physical properties:- Symbol- NaI Mol. weight- 149.9 Colour- Colourless crystals or white crystalline powder Odour- Odourless Nature- Hygroscopic Solubility- Soluble in water & alcohol

16. Sodium iodide 2. Chemical properties:- Its stable in dry air but may decompose on storage & develop brown colour. The aqueous solution gives yellow ppt. with sliver nitrate. NaI + AgNO 3 AgI + NaN 3

17. Preparation Take slightly excess amount of iodine + conc. of sodium hydroxide. it gives the mixture of sodium iodate & potassium iodate. The reaction mixture evaporate to dryness. Residue is treated with carbon to convert sodium iodate into sodium iodide. 6 NaOH + 3 I 2 5 NaI + NaIO 3 + 3H 2 O NaIO 3 + 3C NaI + 3CO

18. Assay 1.3 g of sodium iodide + 100 ml of water. 20 ml of this solution + 40 ml concentrated HCl mixed properly. Titrated with 0.05 M potassium iodate until colour changes to yellow. 5 ml of chloroform is added with continues stirring.

19. Potassium iodide Incompatibilities :- both iodides get decomposed in presence of acid with liberation of iodine. Storage :- sodium and potassium iodide stored in well closed container and kept in dry place.

20. Uses Used in treatment of thyroid gland Fibrolytic agent in syphilis and leprosy In fungal infection & actinomycosis As expectorant In asthma and chronic bronchitis

21. Radioactive Iodine & Sodium Iodide Introduction:- 131 I is obtained by neutron irradiation of tellurium. Its used in the form of sodium iodide ( 131 I). In 1988 sodium iodide ( 131 I ) official in B.P. 131 I in the form of sodium iodide and contains sodium thiosulphate or any other reducing agent and may be suitably buffered.

22. Radioactive Iodine & Sodium Iodide Properties:- Colour- Clear colourless solution 131 I having half life of 8.04 days It emits beta and gamma radiations pH between 7 – 10

23. Assay The activity is determined by comparison with a standardised iodine – 131 solution. Using counting instrument. Its also tested for radionuclide purity and Radiochemical purity.

24. Uses Radioactive iodine is most widely used for diagnosis of thyroid function for treatment of hyperthyroidism. Thyroid cancer Diagnosis of hypothyroidism, hyperthyroidism and goitre. Grave’s disease