Hydrogen iodide
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.
| Hydrogen iodide | |
|---|---|
| |
| |
| IUPAC name | Iodane |
| Other names | Hydroiodic acid (aqueous solution) Iodine hydride |
| Identifiers | |
| CAS number | |
| PubChem | |
| RTECS number | MW3760000 |
| SMILES | I |
| Properties | |
| Molecular formula | HI |
| Molar mass | 127.91 g mol-1 |
| Appearance | Colorless gas |
| Density | 2.85 g/mL (−47 °C) |
| Melting point |
-50.80 °C, 222 K, -59 °F |
| Boiling point | |
| Solubility in water | approximately 245 g/100 ml |
| Acidity (pKa) | −10 (in water, estimate);[1] -9.5 (±1.0) [2] 2.8 (in acetonitrile)[3] |
| Structure | |
| Molecular shape | Terminus |
| Dipole moment | 0.38 D |
| Hazards | |
| Main hazards | Toxic, corrosive, Harmful and Irritant |
| NFPA 704 |
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 noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Hydrogen Iodide Media
Conversion of 1-propanol to 1-iodopropane with HI
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.
- ↑ 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.
