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Sodium Iodide

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sodium iodide [′sōd·ē·əm ′ī·ə‚dīd]
(inorganic chemistry)
NaI A white, air-sensitive powder, deliquescent, with bitter taste; soluble in water, alcohol, and glycerin; melts at 653°C; used in photography and in medicine and as an analytical reagent.

Sodium Iodide 

Nal, a salt; colorless crystals. Density, 3.665 g/cm3; melting point, 662°C. Upon prolonged exposure to light, it turns yellow because of oxidation by atmospheric oxygen and liberation of free iodine. Sodium iodide is hygroscopic. Solubility in water, 64.1 percent at 20°C and 75.1 percent at 100°C. At ordinary temperature, NaI · 2H2O crystallizes from aqueous solutions. Sodium iodide is obtained by means of an exchange reaction between Fe3 I8 and Na2CO3 and is used for medicinal purposes as an iodine preparation.



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David Marine administered what we now recognize as a very large dose of iodine: 170-340 mg (170,000 -340,000 micrograms or mcg) sodium iodide per day for a period of 10 days, repeated every 6 months for 2.
Usual treatment is sodium iodide into the jugular vein, repeated in 10 days.
In the latest version of their experiment, known as DAMA/LIBRA, Bernabei and her colleagues analyzed faint flashes of light from 25 sodium iodide detectors at the Gran Sasso National Laboratory beneath the Apennines east of Rome.
 
 
 
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