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Metaperiodates are typically prepared by the dehydration of sodium hydrogen periodate with nitric acid, [2] or by dehydrating orthoperiodic acid by heating it to 100 °C under vacuum. Classically, periodate was most commonly produced in the form of sodium hydrogen periodate ( Na 3H 2IO 6). [3] This is commercially available, but can also be produced by the oxidation of iodates with chlorine and sodium hydroxide. [4] Or, similarly, from iodides by oxidation with bromine and sodium hydroxide: Parsons, Roger (1959). Handbook of electrochemical constants. Butterworths Scientific Publications Ltd. p. 71.

a b Riley, edited by Georg Brauer; translated by Scripta Technica, Inc. Translation editor Reed F. (1963). Handbook of preparative inorganic chemistry. Volume 1 (2nded.). New York, N.Y.: Academic Press. pp.323–324. ISBN 012126601X. {{ cite book}}: |first= has generic name ( help) CS1 maint: multiple names: authors list ( link)Record of Natriumperiodat in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2018-01-08. Jansen, Martin; Rehr, Anette (1988). "Na 2H 3IO 6, eine Variante der Markasitstruktur". Zeitschrift für anorganische und allgemeine Chemie (in German). 567 (1): 95–100. doi: 10.1002/zaac.19885670111. NaIO 3 + NaOCl sodium hypochlorite ⟶ NaIO 4 + NaCl {\displaystyle {\ce {NaIO3{}+{\overset {sodium\ hypochlorite}{NaOCl}}->NaIO4{}+NaCl}}} Forms and interconversion [ edit ]

Modern industrial scale production involves the electrochemical oxidation of iodates, on a lead dioxide ( PbO 2) anode, with the following standard electrode potential: McMurry, John. Organic chemistry (8th ed., [international ed.]ed.). Singapore: Brooks/Cole Cengage Learning. pp.285–286. ISBN 9780840054531. In this regard it is comparable to the tellurate ion from the adjacent group. It can combine with a number of counter ions to form periodates, which may also be regarded as the salts of periodic acid.H 5 IO 6 + H + + 2 e − ⟶ IO 3 − + 3 H 2 O {\displaystyle {\ce {H5IO6 + H+ + 2e- -> IO3- + 3 H2O}}} E° = 1.6 V [4] Andrew G. Wee, Jason Slobodian, Manuel A. Fernández-Rodríguez and Enrique Aguilar "Sodium Periodate" e-EROS Encyclopedia of Reagents for Organic Synthesis 2006. doi: 10.1002/047084289X.rs095.pub2 Na 3 H 2 IO 6 + 2 HNO 3 ⟶ NaIO 4 + 2 NaNO 3 + 2 H 2 O {\displaystyle {\ce {Na3H2IO6 + 2 HNO3 -> NaIO4 + 2 NaNO3 + 2 H2O}}} H 5 IO 6 ⟶ HIO 4 + 2 H 2 O {\displaystyle {\ce {H5IO6 -> HIO4 + 2 H2O}}} Periodates were discovered by Heinrich Gustav Magnus and C. F. Ammermüller; who first synthesised periodic acid in 1833. [1] Synthesis [ edit ]

Classically, periodate was most commonly produced in the form of sodium hydrogen periodate ( Na 3H 2IO 6). [2] This is commercially available, but can also be produced by the oxidation of iodates with chlorine and sodium hydroxide. [3] Or, similarly, from iodides by oxidation with bromine and sodium hydroxide:Hill, Arthur E. (October 1928). "Ternary Systems. VII. The Periodates of the Alkali Metals". Journal of the American Chemical Society. 50 (10): 2678–2692. doi: 10.1021/ja01397a013. ions with average I–O bond distances of 1.775Å; the Na + ions are surrounded by 8 oxygen atoms at distances of 2.54 and 2.60Å. [6] H 5 IO 6 + H + + 2 e − ⟶ IO 3 − + 3 H 2 O {\displaystyle {\ce {H5IO6 + H+ + 2e- -> IO3- + 3 H2O}}} E° = 1.6 V [5] Sodium metaperiodate can be prepared by the dehydration of sodium hydrogen periodate with nitric acid. [3] Na 3 H 2 IO 6 + 2 HNO 3 ⟶ NaIO 4 + 2 NaNO 3 + 2 H 2 O {\displaystyle {\ce {Na3H2IO6 + 2 HNO3 -> NaIO4 + 2 NaNO3 + 2 H2O}}} Structure [ edit ]