|IUPAC name||Hydrogen iodide|
|Other names||hydroiodic acid|
|Molar mass||127.904 g/mol|
|Density||2.85 g/mL (-47 °C)|
–50.80 °C (184.55 K)
–35.36 °C (237.79 K)
|Dipole moment||0.38 D|
|MSDS|| hydrogen iodide|
|Main hazards||Toxic, corrosive.|
|R-phrases||, , ,|
|S-phrases||, , ,|
|Other anions|| Flouride|
| Except where noted otherwise, data are given for|
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references
Hydrogen iodide (HI) is a diatomic molecule. Aqueous solutions of HI are known as hydroiodic acid or hydriodic acid, a strong acid. Hydrogen iodide and hydroiodic acid are, however, different in that the former is a gas under standard conditions; whereas, the other is an aqueous solution of said gas. They are interconvertible. HI is used in organic and inorganic synthesis as one of the primary sources of iodine and as a reducing agent.
Properties of hydrogen iodide
HI is a colorless gas that reacts with oxygen to give water and iodine. With moist air, HI gives a mist (or fumes) of hydroiodic acid. It is exceptionally soluble in water, giving hydroiodic acid. One liter of water will dissolve 425 liters of HI, the final solution having only four water molecules per molecule of HI.
Once again, although chemically related, hydroiodic acid is not pure HI but a mixture containing it. Commercial "concentrated" hydroiodic acid usually contains 48% - 57% HI by mass. The solution forms an azeotrope boiling at 127 °C with 57% HI, 43% water. Hydroiodidic acid is one of the strongest of all the common halide acids because the electronegativity of iodine is weaker than the rest of the other common halides. The high acidity is caused by the dispersal of the ionic charge over the anion. The iodide ion is much larger than the other common halides which results in the negative charge being dispersed over a large space. By contrast, a chloride ion is much smaller, meaning its negative charge is more concentrated, leading to a stronger interaction between the proton and the chloride ion. This weaker H+---I− interaction in HI facilitates dissociation of the proton from the anion..
- 2 I2 + N2H4 → 4 HI + N2
When performed in water, the HI must be distilled.
HI can also be distilled from a solution of NaI or other alkali iodide in concentrated phosphoric acid (note that sulfuric acid will not work for acidifying iodides as it will oxidize the iodide to elemental iodine).
Additionally HI can be prepared by simply combining H2 and I2. This method is usually employed to generate high purity samples.
- H2 + I2 → 2 HI
For many years, this reaction was considered to involve a simple bimolecular reaction between molecules of H2 and I2. However, when a mixture of the gases is irradiated with the wavelength of light equal to the dissociation energy of I2, about 578 nm, the rate increases significantly. This supports a mechanism whereby I2 first dissociates into 2 iodine atoms, which each attach themselves to a side of an H2 molecule and break the H -- H bond:
- H2 + I2 + 578 nm radiation → H2 + 2 I → I - - - H - - - H - - - I → 2 HI
In the laboratory, another method involves hydrolysis of PI3, the iodine equivalent of PBr3. In this method, I2 reacts with phosphorus to create phosphorus triiodide, which then reacts with water to form HI and phosphorous acid.
- 3 I2 + 2 P + 6 H2O → 2 PI3 + 6 H2O → 6 HI + 2 H3PO3
Key reactions and applications
- HI will undergo oxidation if left open to air according to the following pathway:'
- 4 HI + O2 → 2H2O + 2 I2
- HI + I2 → HI3
HI3 is dark brown in color, which makes aged solutions of HI often appear dark brown.
- HI + H2C=CH2 → H3CCH2I
HI is subject to the same Markovnikov and anti-Markovnikov guidelines as HCl and HBr.
- HI reduces certain α-substituted ketones and alcohols replacing the α substituent with a hydrogen atom.
- ↑ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ↑ Greenwood, N.N. and A. Earnshaw. The Chemistry of the Elements. 2nd ed. Oxford: Butterworth-Heineman. p 809-815. 1997.
- ↑ Holleman, A.F. Wiberg, E. Inorganic Chemistry. San Diego: Academic Press. p 371, 432-433. 2001.
- ↑ 4.0 4.1 Breton, G. W., P. J. Kropp, P. J.; Harvey, R. G. “Hydrogen Iodide” in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.
See also: Nishikata, E., T.; Ishii, and T. Ohta. “Viscosities of Aqueous Hydrochloric Acid Solutions, and Densities and Viscosities of Aqueous Hydroiodic Acid Solutions”. J. Chem. Eng. Data. 26. 254-256. 1981.
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