Solid iodine reacts slowly with sodium hydroxide to form a salt of sodium iodide, sodium iodate(I) and water. Sodium iodide exhibits high solubility in some organic solvents, unlike sodium chloride or even bromide: Iodides (including sodium iodide) are detectably oxidized by atmospheric oxygen (O2) to molecular iodine (I2). This makes it well-suited as a pH regulator in many industries, like water treatment, because of its ability to neutralise or control acidity.NaOH reacts with acid to produce a water and an ionic compound. The black iodine crystals dissolve slowly in sodium hydroxide, forming a colourless solution. This is because fluorine is so reactive that it will react with most of the substance it comes into contact with. Some radioactive iodide salts of sodium, including Na125I and Na131I, have radiopharmaceutical uses, such as in the treatment of thyroid cancer and hyperthyroidism or as radiolabeling tracers in imaging (see Isotopes of iodine > Radioiodines I-123, I-124, I-125, and I-131 in medicine and biology). Crystals with a higher level of doping are used in X-ray detectors with high spectrometric quality. It is produced industrially as the salt formed when acidic iodides react with sodium hydroxide. The crystals are usually coupled with a photomultiplier tube, in a hermetically sealed assembly, as sodium iodide is hygroscopic. Therefore all the experiments involving these gases should be carried out in a fume chamber. The reaction is exothermic. It is produced industrially as the salt formed when acidic iodides react with sodium hydroxide. The sodium iodide formula is NaI. Except where otherwise noted, data are given for materials in their, Isotopes of iodine > Radioiodines I-123, I-124, I-125, and I-131 in medicine and biology, Ullmann's Encyclopedia of Industrial Chemistry, "Single-atom electron energy loss spectroscopy of light elements", "Darstellung organischer Jodide aus den entsprechenden Bromiden und Chloriden", Journal of the Chemical Society, Faraday Transactions 1, "Material Safety Data Sheet (MSDS) – Safety data for sodium iodide", "Sodium iodide (Oral route, Injection route, Intravenous route)", https://en.wikipedia.org/w/index.php?title=Sodium_iodide&oldid=967359815, Chemical articles with multiple compound IDs, Multiple chemicals in an infobox that need indexing, Chemical articles with multiple CAS registry numbers, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Creative Commons Attribution-ShareAlike License, This page was last edited on 12 July 2020, at 20:02. Iodized table salt contains 10 ppm iodide. Sodium iodide can be used both as single crystals and as polycrystals for this purpose. The greenish chlorine gas dissolves quickly in sodium hydroxide, forming a colourless solution. The wavelength of maximum emission is 415 nm.. Chlorine gas reacts with sodium hydroxide to form a salt of sodium chloride, sodium chlorate(I) and water. Under standard conditions, it is a white, water-soluble solid comprising a 1:1 mix of sodium cations and iodide anions in a crystal lattice. The reaction is least reactive among the three.  It is a chaotropic salt. NaI(Tl) is the most widely used scintillation material. 03 Concept of Mole, Formulae and Equations. Sodium iodide is an ionic compound formed from the chemical reaction of sodium metal and iodine. Sodium hydroxide - concentrated, heated solution. Sodium iodide, as well as potassium iodide, is commonly used to treat and prevent iodine deficiency. Under standard conditions, it is a white, soluble solid which includes a 1:1 blend of sodium cations (Na+) and iodide anions (I−) in a lattice grid. During the reaction, the sodium metal may well become so hot that it catches fire and burns with a characteristic orange colour.