Difference between revisions of "Potassium biiodate"

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The biiodate anion is a [[Hydrogen bond|hydrogen-bonded]] species formed from the reaction of an [[iodate]] anion with undissociated [[iodic acid]] (p''K''<sub>a</sub>&nbsp;= 0.75).<ref>{{Greenwood&Earnshaw1st|page=1010}}.</ref>
 
The biiodate anion is a [[Hydrogen bond|hydrogen-bonded]] species formed from the reaction of an [[iodate]] anion with undissociated [[iodic acid]] (p''K''<sub>a</sub>&nbsp;= 0.75).<ref>{{Greenwood&Earnshaw1st|page=1010}}.</ref>
 
:IO{{su|b=3|p=−}} + HIO<sub>3</sub> &rarr; [H(IO<sub>3</sub>)<sub>2</sub>]<sup>−</sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;''K''<sub>c</sub> ≈ 4 dm<sup>3</sup> mol<sup>−1</sup>
 
:IO{{su|b=3|p=−}} + HIO<sub>3</sub> &rarr; [H(IO<sub>3</sub>)<sub>2</sub>]<sup>−</sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;''K''<sub>c</sub> ≈ 4 dm<sup>3</sup> mol<sup>−1</sup>
Hence, in dilute aqueous solutions, potassium biiodate can be considered to be a mixture of [[potassium iodate]] and iodic acid: however, it dissolves and recrystallizes coherently from water.<ref>{{citation | title = Ternary Systems. VIII. Potassium Iodate, Iodic Acid and Water | first = Sterling B. | last = Smith | journal = J. Am. Chem. Soc. | year = 1947 | volume = 69 | issue = 10 | pages = 2285–86 | doi = 10.1021/ja01202a013}}.</ref>
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Hence, in dilute aqueous solutions, potassium biiodate can be considered to be a mixture of [[potassium iodate]] and iodic acid: however, it dissolves and recrystallizes coherently from water.<ref name="Smith">{{citation | title = Ternary Systems. VIII. Potassium Iodate, Iodic Acid and Water | first = Sterling B. | last = Smith | journal = J. Am. Chem. Soc. | year = 1947 | volume = 69 | issue = 10 | pages = 2285–86 | doi = 10.1021/ja01202a013}}.</ref>
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Potassium biiodate loses water on heating to form a compound formulated as 2KIO<sub>3</sub>·I<sub>2</sub>O<sub>5</sub>: quantitative dehydration is described as rapid at 200&nbsp;C, but takes three days at 105&nbsp;C.<ref name="Smith"/>
  
 
===Preparation===
 
===Preparation===
Potassium biiodate is commercially available in analytical grade. However it may be conveniently prepared by simply mixing hot concentrated solutions of potassium iodate and iodic acid and allowing the potassium biiodate to crystallize.
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Potassium biiodate is commercially available in analytical grade. However it may be conveniently prepared by simply mixing hot concentrated solutions of potassium iodate and iodic acid and allowing the potassium biiodate to crystallize. The crystals may be washed with absolute [[ethanol]] and dried in air.<ref name="Smith"/>
  
 
==Ferroelectricity==
 
==Ferroelectricity==

Revision as of 21:03, 9 September 2010

Potassium biiodate
IUPAC name potassium µ-hydridobis(trioxidoiodate)(1−)
Other names potassium hydrogen iodate
Identifiers
InChI InChI=1/2HIO3.K/c2*2-1(3)4;/h2*(H,2,3,4);/q;;+1/p-1
InChIKey ACAYDTMSDROWHW-REWHXWOFAC
Standard InChI InChI=1S/2HIO3.K/c2*2-1(3)4;/h2*(H,2,3,4);/q;;+1/p-1
Standard InChIKey ACAYDTMSDROWHW-UHFFFAOYSA-M
CAS number [13455-24-8]
EC number 236-650-9
ChemSpider 2341255
Properties[1]
Chemical formula KH(IO3)2
Molar mass 389.91 g mol−1
Appearance white crystals
Solubility in water 1.33 g/100 ml (15 °C)
Hazards[2][3][Note 1]
EU index number not listed
GHS pictograms Skin Corr. 1C, Eye Dam. 1Ox. Sol. 2Acute Tox. 4 (oral)
GHS signal word DANGER
GHS hazard statements H272, H302, H314, H318
GHS precautionary statements P210, P220, P221, P260, P264, P270, P280, P301+312, P301+330+331, P303+361+353, P363, P304+340, P310, P321
Flash point Non-flammable
Related compounds
Other compounds Potassium iodate
Iodic acid
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

Potassium biiodate, KH(IO3)2, is a primary standard strong acid in analytical chemistry.[4][5]

Chemistry

The biiodate anion is a hydrogen-bonded species formed from the reaction of an iodate anion with undissociated iodic acid (pKa = 0.75).[6]

IO3 + HIO3 → [H(IO3)2]     Kc ≈ 4 dm3 mol−1

Hence, in dilute aqueous solutions, potassium biiodate can be considered to be a mixture of potassium iodate and iodic acid: however, it dissolves and recrystallizes coherently from water.[7]

Potassium biiodate loses water on heating to form a compound formulated as 2KIO3·I2O5: quantitative dehydration is described as rapid at 200 C, but takes three days at 105 C.[7]

Preparation

Potassium biiodate is commercially available in analytical grade. However it may be conveniently prepared by simply mixing hot concentrated solutions of potassium iodate and iodic acid and allowing the potassium biiodate to crystallize. The crystals may be washed with absolute ethanol and dried in air.[7]

Ferroelectricity

Potassium biiodate forms a ferroelectric phase below the Curie point of TC = 223(2) K.[8] The second-order phase transition appears to be associated with the ordering of the hydrogen bonds in the crystal structure.[9]

Notes and references

Notes

  1. Hazards were assessed as for an equimolar mixture of potassium iodate and iodic acid.

References

  1. CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-133. ISBN 0-8493-0462-8.
  2. HSNO Chemical Classification Information Database, <http://www.ermanz.govt.nz/Chemicals/ChemicalDisplay.aspx?SubstanceID=1913> (accessed 9 September 2010), New Zealand Environmental Risk Management Authority. (potassium iodate)
  3. HSNO Chemical Classification Information Database, <http://www.ermanz.govt.nz/Chemicals/ChemicalDisplay.aspx?SubstanceID=12620> (accessed 9 September 2010), New Zealand Environmental Risk Management Authority. (iodic acid)
  4. Kolthoff, I. M.; van Berk, L. H. The Use of Potassium Bi-iodate as a Standard Substance in Alkalimetric and Iodimetric Titrations. J. Am. Chem. Soc. 1926, 48 (11), 2799–2801. DOI: 10.1021/ja01690a006.
  5. Processing KODAK Motion Picture Films, Module 4 – Potassium Biiodate; Kodak, <http://motion.kodak.com/motion/uploadedFiles/US_plugins_acrobat_en_motion_support_processing_h244_potBiiod.pdf>. (accessed 9 September 2010).
  6. Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; p 1010. ISBN 0-08-022057-6.
  7. 7.0 7.1 7.2 Smith, Sterling B. Ternary Systems. VIII. Potassium Iodate, Iodic Acid and Water. J. Am. Chem. Soc. 1947, 69 (10), 2285–86. DOI: 10.1021/ja01202a013.
  8. Petrosyana, A. M.; Buscha, A. A.; Chechkina, V. V.; Volkova, A. F.; Venevtsev, Yu. N. Ferroelectric phase transition in potassium Bi-iodate. Ferroelectrics 1978, 21 (1), 525–26. DOI: 10.1080/00150197808237316.
  9. Barabash, A.; Baran, J.; Gavrilko, T.; Eshimov, K.; Puchkovskaya, G.; Ratajczak, H. Structure and dynamics of crystal α-modification of potassium biiodate. J. Mol. Struct. 1997, 404 (1–2), 187–91. DOI: 10.1016/S0022-2860(96)09380-5.