Difference between revisions of "Iodic acid"
Physchim62 (talk | contribs) |
Physchim62 (talk | contribs) |
||
| Line 1: | Line 1: | ||
| + | {{Chembox | ||
| + | | Name = | ||
| + | | ImageFile = | ||
| + | | ImageSize = | ||
| + | | IUPACName = iodic acid | ||
| + | | OtherNames = | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | CASNo = 7782-68-5 | ||
| + | | EINECS = 231-962-1 | ||
| + | | ChemSpiderID = 22761 | ||
| + | | InChI = InChI=1S/HIO3/c2-1(3)4/h(H,2,3,4) | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | Reference = <ref name="G&E">{{Greenwood&Earnshaw1st|page=1010}}.</ref> | ||
| + | | Formula = HIO<sub>3</sub> | ||
| + | | MolarMass = 175.91 g mol<sup>−1</sup> | ||
| + | | Appearance = white crystals | ||
| + | | Density = | ||
| + | | MeltingPt = 100 °C ''decomp.'' | ||
| + | | Solubility = | ||
| + | | SolubleOther = | ||
| + | | Solvent = | ||
| + | | pKa = 0.804 | ||
| + | }} | ||
| + | | Section3 = {{Chembox Structure | ||
| + | | Reference = <ref name="G&E"/> | ||
| + | | CrystalStruct = | ||
| + | | Coordination = | ||
| + | | MolShape = pyramidal; ''r''(I=O) = 181 pm, ''r''(I–OH) = 189 pm, O=I=O = 101.4°, O=I–OH = 97° | ||
| + | }} | ||
| + | | Section7 = {{Chembox Hazards | ||
| + | | ExternalMSDS = | ||
| + | | EUIndex = not listed | ||
| + | | FlashPt = non-flammable | ||
| + | }} | ||
| + | | Section8 = {{Chembox Related | ||
| + | | OtherAnions = [[Hydriodic acid]]<br/>[[Periodic acid]] | ||
| + | | OtherCpds = [[Chloric acid]]<br/>[[Bromic acid]] | ||
| + | }} | ||
| + | }} | ||
'''Iodic acid''', HIO<sub>3</sub>, is a moderately strong [[oxoacid]] of [[iodine]]. It forms a series of salts called [[iodate]]s. | '''Iodic acid''', HIO<sub>3</sub>, is a moderately strong [[oxoacid]] of [[iodine]]. It forms a series of salts called [[iodate]]s. | ||
| − | Iodic acid may be prepared by the oxidation of suspensions of iodine in water, either by [[electrolysis]] or with [[nitric acid]].<ref name="G&E" | + | Iodic acid may be prepared by the oxidation of suspensions of iodine in water, either by [[electrolysis]] or with [[nitric acid]].<ref name="G&E"/> Unlike [[Chloric acid|chloric]] and [[bromic acid]]s, it can be isolated as a white crystalline air-stable solid. The solid decomposes on heating, first to HIO<sub>3</sub>·I<sub>2</sub>O<sub>5</sub> at about 100 °C, then to [[iodine pentoxide]] at about 200 °C.<ref name="G&E"/> |
==Notes and references== | ==Notes and references== | ||
Revision as of 10:17, 10 September 2010
| IUPAC name | iodic acid |
| Identifiers | |
| InChI | InChI=InChI=1S/HIO3/c2-1(3)4/h(H,2,3,4) |
| CAS number | [] |
| EC number | |
| ChemSpider | |
| Properties[1] | |
| Chemical formula | HIO3 |
| Molar mass | 175.91 g mol−1 |
| Appearance | white crystals |
| Melting point |
100 °C decomp. |
| Acidity (pKa) | 0.804 |
| Structure[1] | |
| Molecular geometry | pyramidal; r(I=O) = 181 pm, r(I–OH) = 189 pm, O=I=O = 101.4°, O=I–OH = 97° |
| Hazards | |
| EU index number | not listed |
| Flash point | non-flammable |
| Related compounds | |
| Other anions | Hydriodic acid Periodic acid |
| Other compounds | Chloric acid Bromic acid |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Iodic acid, HIO3, is a moderately strong oxoacid of iodine. It forms a series of salts called iodates.
Iodic acid may be prepared by the oxidation of suspensions of iodine in water, either by electrolysis or with nitric acid.[1] Unlike chloric and bromic acids, it can be isolated as a white crystalline air-stable solid. The solid decomposes on heating, first to HIO3·I2O5 at about 100 °C, then to iodine pentoxide at about 200 °C.[1]
Notes and references
Notes
References
External links
 |
See also the corresponding article on Wikipedia. |
| Error creating thumbnail: Unable to save thumbnail to destination |
This page is currently licensed under the Creative Commons Attribution 3.0 Unported license and any later versions of that license. |
