Hydrogen iodide

Hydrogen iodide
Names
	IUPAC name Iodane
	Other names Hydroiodic acid (aqueous solution) ; Iodine hydride
Identifiers
CAS Number	10034-85-2 ;
3D model (JSmol)	Interactive image;
ChemSpider	23224 ;
ECHA InfoCard	100.030.087
PubChem CID	16109203;
RTECS number	MW3760000;
UNII	694C0EFT9Q ;
CompTox Dashboard (EPA)	DTXSID2044349 ;
	SMILES I;
Properties
Chemical formula	HI
Molar mass	127.904 g/mol
Appearance	Colorless gas
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)
Structure
Molecular shape	Terminus
Dipole moment	0.38 D
Hazards
Main hazards	Toxic, corrosive, Harmful and Irritant
	0 3 1
R-phrases	R20, R21, R22, R35
S-phrases	S7, S9, S26, S45
Flash point	Non-flammable
Related compounds
Other anions	Hydrogen fluoride; Hydrogen chloride; Hydrogen bromide; Hydrogen astatide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	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[change | change source]

References[change | change source]

↑ 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

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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

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