Hydrogen iodide - Simple English Wikipedia, the free encyclopedia

Hydrogen iodide
Names
	IUPAC name Hydrogen iodide
	Systematic IUPAC name Iodane
	Other names Hydroiodic acid (aqueous solution); Iodine hydride
Identifiers
CAS Number	10034-85-2 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:43451;
ChemSpider	23224 ;
ECHA InfoCard	100.030.087
EC Number	233-109-9;
KEGG	C05590;
PubChem CID	24841;
RTECS number	MW3760000;
UNII	694C0EFT9Q ;
UN number	1787 2197
CompTox Dashboard (EPA)	DTXSID2044349 ;
	SMILES I;
Properties
Chemical formula	HI
Molar mass	127.91 g·mol−1
Appearance	Colorless gas
Odor	acrid
Density	2.85 g/mL (−47 °C)
Melting point	−50.80 °C (−59.44 °F; 222.35 K)
Boiling point	−35.36 °C (−31.65 °F; 237.79 K)
Solubility in water	approximately 245 g/100 ml
Acidity (pKa)	−10 (in water, estimate); −9.5 (±1.0); 2.8 (in acetonitrile)
Conjugate acid	Iodonium
Conjugate base	Iodide
Refractive index (nD)	1.466 (16 °C)
Structure
Molecular shape	Terminus
Dipole moment	0.38 D
Thermochemistry
Standard molar; entropy So298	206.6 J·mol−1·K−1
Specific heat capacity, C	29.2 J·mol−1·K−1
Hazards
Main hazards	Toxic, corrosive, harmful and irritant
	0 3 1
Flash point	Non-flammable
Related compounds
Other anions	{{{value}}}
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Hydrogen iodide (HI) is a chemical compound. Its chemical formula is HI. It is a colorless odorous gas. It reacts with oxygen to make iodine and water. It can be made by reducing iodine with hydrazine. It can also be made by reacting iodides with non-oxidizing acids such as phosphoric acid. It can also be made by reacting hydrogen sulfide with iodine. Very pure hydrogen iodide can be made by combining hydrogen and iodine, but this is very slow. It will break down if exposed to air. It can be used to make illegal drugs and various chemical compounds of iodine. It dissolves in water to produce hydroiodic acid. Hydroiodic acid is a strong acid that is used to make iodides.

Related pages

References

↑ Bell, R.P. The Proton in Chemistry. 2nd ed., Cornell University Press, Ithaca, NY, 1973.
↑ Trummal, A.; Lipping, L.; Kaljurand, I.; Koppel, I. A.; Leito, I. "Acidity of Strong Acids in Water and Dimethyl Sulfoxide" J. Phys. Chem. A. 2016, 120, 3663-3669. doi:10.1021/acs.jpca.6b02253
↑ Raamat, E.; Kaupmees, K.; Ovsjannikov, G.; Trummal, A.; Kütt, A.; Saame, J.; Koppel, I.; Kaljurand, I.; Lipping, L.; Rodima, T.; Pihl, V.; Koppel, I. A.; Leito, I. "Acidities of strong neutral Brønsted acids in different media." J. Phys. Org. Chem. 2013, 26, 162-170. doi:10.1002/poc.2946
↑ CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN 978-1-4987-5428-6. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)

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International Chemical Safety Card 1326

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[1] Bell, R.P. The Proton in Chemistry. 2nd ed., Cornell University Press, Ithaca, NY, 1973.

[2] Trummal, A.; Lipping, L.; Kaljurand, I.; Koppel, I. A.; Leito, I. "Acidity of Strong Acids in Water and Dimethyl Sulfoxide" J. Phys. Chem. A. 2016, 120, 3663-3669. doi:10.1021/acs.jpca.6b02253

[3] Raamat, E.; Kaupmees, K.; Ovsjannikov, G.; Trummal, A.; Kütt, A.; Saame, J.; Koppel, I.; Kaljurand, I.; Lipping, L.; Rodima, T.; Pihl, V.; Koppel, I. A.; Leito, I. "Acidities of strong neutral Brønsted acids in different media." J. Phys. Org. Chem. 2013, 26, 162-170. doi:10.1002/poc.2946

[CRC97-4] CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN 978-1-4987-5428-6. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)

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