Potassium Iodate

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POTASSIUM IODATE Prepared at the 33rd JECFA (1988), published in FNP 38 (1988) and in FNP 52 (1992). Metals and arsenic specifications revised at the 63rd JECFA (2004). Use not recommended as Flour treatment agent 9th JECFA (1965) SYNONYMS INS No. 917 DEFINITION Chemical names Potassium iodate C.A.S. number 7758-05-6 Chemical formula KIO3 Formula weight 214.02 Assay Not less than 99.0% and not more than 101.0% on the dried basis DESCRIPTION White, odourless crystalline powder FUNCTIONAL USES Flour treatment agent, oxidizing agent CHARACTERISTICS IDENTIFICATION Solubility (Vol. 4) Soluble in water; insoluble in ethanol Test for potassium Passes test (Vol. 4) Test for iodate To a 1 in 20 solution of the sample add one drop of starch TS and a few drops of 20% hypophosphorous acid. A transient blue colour appears PURITY Loss on drying (Vol. 4) Not more than 0.5% (150o, 3 h) Acidity or alkalinity Dissolve by warming 5 g of the sample in 40 ml of freshly boiled and cooled water, cool and add 3 drops of phenol- phthalein TS; observe colour: If the solution is pink, add 0.4 ml of 0.01 N hydro chloric acid. The pink colour disappears. If the solution is colourless, add 1.2 ml of 0.01 N sodium hydroxide. The solution turns pink. Lead (Vol. 4) Not more than 2 mg/kg Determine using an atomic absorption technique appropriate to the specified level. The selection of sample size and method of sample preparation may be based on the principles of the method described in Volume 4, “Instrumental Methods.” METHOD OF Weigh accurately about 100 mg of the sample, previously dried at 105o for 3 ASSAY h, and dissolve in 50 ml of water contained in a 250 ml glass-stoppered conical flask. Add 3 g of potassium iodide, followed by 3 ml of dilute hydrochloric acid (3 in 10), and stopper the flask. Allow the mixture to stand for 5 min., add 100 ml of cold water, and titrate the liberated iodine with 0.1 N sodium thiosulfate, adding starch TS as the end-point is approached. Perform a blank determination. Each ml of 0.1 N sodium thiosulfate is equivalent to 3.567 mg of KIO3. .

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Determination of Iodate in Iodised Salt by Redox Titration
College of Science Determination of Iodate in Iodised Salt by Redox Titration Safety • 0.6 M potassium iodide solution (10 g solid KI made up to 100 mL with distilled water) • 0.5% starch indicator solution Lab coats, safety glasses and enclosed footwear must (see below for preparation) be worn at all times in the laboratory. • 250 mL volumetric flask Introduction • 50 mL pipette (or 20 and 10 mL pipettes) • 250 mL conical flasks New Zealand soil is low in iodine and hence New Zealand food is low in iodine. Until iodised salt was • 10 mL measuring cylinder commonly used (starting in 1924), a large proportion • burette and stand of school children were reported as being affected • distilled water by iodine deficiency – as high as 60% in Canterbury schools, and averaging 20 − 40% overall. In the worst cases this deficiency can lead to disorders such as Method goitre, and impaired physical and mental development. 1. Preparation of 0.002 mol L−1 sodium thiosulfate In earlier times salt was “iodised” by the addition of solution: Accurately weigh about 2.5 g of solid potassium iodide; however, nowadays iodine is more sodium thiosulfate (NaS2O3•5H2O) and dissolve in commonly added in the form of potassium iodate 100 mL of distilled water in a volumetric flask. (This gives a 0.1 mol L−1 solution). Then use a pipette to (KIO3). The Australia New Zealand Food Standards Code specifies that iodised salt must contain: “equivalent to transfer 10 mL of this solution to a 500 mL volumetric no less than 25 mg/kg of iodine; and no more than 65 flask and dilute by adding distilled water up to the mg/kg of iodine”.
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Potassium Iodate, 0.00564N (0.00094M) Safety Data Sheet according to Federal Register / Vol. 77, No. 58 / Monday, March 26, 2012 / Rules and Regulations Date of issue: 04/15/2015 Revision date: 02/08/2018 Supersedes: 02/08/2018 Version: 1.1 SECTION 1: Identification 1.1. Identification Product form : Mixtures Product name : Potassium Iodate, 0.00564N (0.00094M) Product code : LC19600 1.2. Recommended use and restrictions on use Use of the substance/mixture : For laboratory and manufacturing use only. Recommended use : Laboratory chemicals Restrictions on use : Not for food, drug or household use 1.3. Supplier LabChem Inc Jackson's Pointe Commerce Park Building 1000, 1010 Jackson's Pointe Court Zelienople, PA 16063 - USA T 412-826-5230 - F 724-473-0647 [email protected] - www.labchem.com 1.4. Emergency telephone number Emergency number : CHEMTREC: 1-800-424-9300 or 011-703-527-3887 SECTION 2: Hazard(s) identification 2.1. Classification of the substance or mixture GHS-US classification Not classified 2.2. GHS Label elements, including precautionary statements Not classified as a hazardous chemical. Other hazards not contributing to the : None under normal conditions. classification 2.4. Unknown acute toxicity (GHS US) Not applicable SECTION 3: Composition/Information on ingredients 3.1. Substances Not applicable 3.2. Mixtures Name Product identifier % GHS -US classification Water (CAS-No.) 7732-18-5 99.98 Not classified Potassium Iodate (CAS-No.) 7758-05-6 0.02 Ox. Sol. 3, H272 Full text of hazard classes and H-statements : see section 16 SECTION 4: First-aid measures 4.1.
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TITRATIONS with POTASSIUM IODATE Potassium Iodate Is a Fairly
TITRATIONS WITH POTASSIUM IODATE Potassium iodate is a fairly strong oxidizing agent that may be used in the assay of a number of pharmaceutical substances, for instance : benzalkonium chloride, cetrimide, hydralazine hydrochloride, potassium iodide, phenylhydrazine hydrochloride, semicarbazide hydrochloride and the like. Under appropriate experimental parameters the iodate reacts quantitatively with both iodides and iodine. It is, however, interesting to observe here that the iodate titrations may be carried out effectively in the presence of saturated organic acids, alcohol and a host of other organic substances. The oxidation-reduction methods with potassium iodate invariably based on the formation of iodine monochloride (ICl) in a medium of strong hydrochloric acid solution. Preparation of 0.05 M Potassium Iodate Potassium iodate is dried to a constant weight at 110°C to make it completely free from moisture and then brought to room temperature in a desiccator. It is pertinent to mention here that KIO3 is a very stable salt and may be obtained in a very pure form. Therefore, it is possible to prepare the standard solutions of KIO3 by dissolving the calculated weight of the salt in water and diluting the same to an approximate volume. Since, the normality of iodate solution varies significantly depending on the nature of the reaction, therefore, in usual practice standard iodate solutions of known molarity are used. The reduction of potassium iodate to iodide is usually not feasible in a direct titrimetric method (unlike the reduction of potassium bromate to bromide) and hence, has no viable application in the official procedures ...........................(a) In this type of reaction, 1 mol of KIO3 is 6 equivalent and a 0.05 M solution would be 0.3 N.
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Consideration of Mandatory Fortification with Iodine for Australia and New Zealand Food Technology Report
CONSIDERATION OF MANDATORY FORTIFICATION WITH IODINE FOR AUSTRALIA AND NEW ZEALAND FOOD TECHNOLOGY REPORT December 2007 1 Introduction Food Standards Australia New Zealand is considering mandatory fortification of the food supply in Australia and New Zealand with iodine. Generally, the addition of iodine to foods is technologically feasible. However, in some instances the addition of iodine can lead to quality changes in food products such as appearance, taste, odour, texture and shelf life. These changes will depend on the chemical form of iodine used as a fortificant, the chemistry of the food that is being fortified, the food processes involved in manufacture and possible processing interactions that could occur during distribution and storage. Many foods have been fortified with iodine and the potassium salts of iodine compounds have been used as the preferred form. 2 Forms of Iodine Iodine is normally introduced, or supplemented, as the iodide or iodate of potassium, calcium or sodium. The following table lists different chemical forms of iodine along with their important physical properties. Table 1: Physical Properties of Iodine and its Compounds Name Chemical Formula % Iodine Solubility in water (g/L) 0°C 20°C 30°C 40°C 60°C Iodine I2 100 - - 0.3 0.4 0.6 Calcium iodide CaI2 86.5 646 676 690 708 740 Calcium iodate Ca(IO3)2.6H2O 65.0 - 1.0 4.2 6.1 13.6 Potassium iodide KI 76.5 1280 1440 1520 1600 1760 Potassium iodate KIO3 59.5 47.3 81.3 117 128 185 Sodium iodide NaI.2H20 85.0 1590 1790 1900 2050 2570 Sodium iodate NaIO3 64.0 - 25.0 90.0 150 210 Adapted from Mannar and Dunn (1995) 2.1 Potassium Iodide Potassium iodide (KI) is highly soluble in water.
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Potassium Iodate
374 Potassium Iodate COHPONENTS: EVALUATOR: (1) Potassium iodate; KI03; [7758-05-6] H. Miyamoto Niigata University Niigata, Japan (2) Water; H20; [7732-18-5] and Mark Salomon US Army ET & DL Fort Monmouth, NJ, USA June, 1986 CRITICAL EVALUATION: THE BINARY SYSTEM Solubility data for KI03 in pure water have been reported in 30 publications (1-28, 35, 36). A summary of the solubility data over the temperature range 273-373 K is given in Table 1. Note that the data from references (15, 16, 20 and 31) have been compiled in the LiI03 chapter, and the data in reference (3) have been compiled in the NaI03 chapter. With the exception of the high temperature study of Benrath et al. (7) which employed the synthetic method, all other studies are based on the isothermal method. From Table 1 it is seen that a number of authors reported identical solubilities in more than one publication, and the evaluators have therefore treated these results as one independent measurement. Thus, at 298.2 K, the data in (3, 8, 10) have been treated as one independent solubility value as have the data reported in (17, 19, 23), and at 323.2 K in (18, 21, 26). Most authors reported the solid phase over the temperature range of 278-323 K as the anhydrous salt, and although Breusov et al. (11) and Benrath et al. (7) did not report the nature of the solid phases over the temperature range of 273-573 K, it probably is the anhydrous salt in all cases. In fitting the solubility data to the two smoothing equations, a number of data points were rejected as the differences in smoothed (calculated) solubilities differed from the experi mental values by more than 20 (where a is the standard error of estimate).
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