Difference between revisions of "Iodic acid"
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+ | {{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 09:17, 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. |
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