Arsenous acid

Arsenous acid (or arsenious acid) is the inorganic compound with the formula H3AsO3. It is known to occur in aqueous solutions, but it has not been isolated as a pure material, although this fact does not detract from the significance of As(OH)3.[2]

Arsenous acid
Names
IUPAC name
Arsorous acid
Other names
Arsenious acid
Arsenic oxide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
DrugBank
UNII
Properties
H3AsO3
Molar mass 125.94 g/mol
Appearance Only exists in aqueous solutions
Conjugate base Arsenite
-51.2·10−6 cm3/mol
Hazards
Main hazards Toxic, corrosive
NIOSH (US health exposure limits):
PEL (Permissible)
 [1910.1018] TWA 0.010 mg/m3[1]
REL (Recommended)
 Ca C 0.002 mg/m3 [15-minute][1]
IDLH (Immediate danger)
 Ca [5 mg/m3 (as As)][1]
Related compounds
Related compounds
 Arsenic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is YN ?)
Infobox references

Properties

As(OH)3 is a pyramidal molecule consisting of three hydroxyl groups bonded to arsenic. The 1H NMR spectrum of arsenous acid solutions consists of a single signal consistent with the molecule's high symmetry.[3] In contrast, the nominally related phosphorous acid H3PO3 adopts the structure HPO(OH)2. The structural analogue of arsenous acid (P(OH)3) is a very minor equilibrium component of such solutions. The differing behaviors of the As and P compounds reflect a trend whereby high oxidation states are more stable for lighter members of main group elements than their heavier congeners.[4]

One tautomer of arsenous acid is HAsO(OH)2, which is called arsonic acid. It has not been isolated or well-characterized.

Phosphorous acid exists in as the dihydroxy tautomer in contrast to arsenous acid.

Synthesis

The preparation of As(OH)3 involves a slow hydrolysis of arsenic trioxide in water. Addition of base converts arsenous acid to the arsenite ions [AsO(OH)2]−, [AsO2(OH)]2−, and [AsO3]3−.

Reactions

With its first pKa being 9.2, As(OH)3 is a weak acid.[4] Reactions attributed to aqueous arsenic trioxide are due to arsenous acid and its conjugate bases.

Like arsenic trioxide, arsenous acid is sometimes amphoteric. For example, it reacts with hydrochloric, hydrobromic, and hydroiodic acids to produce arsenic trichloride, tribromide, and triiodide.

As(OH)3 + 3 HCl ⇌ AsCl3 + 3 H2O
As(OH)3 + 3 HBr ⇌ AsBr3 + 3 H2O
As(OH)3 + 3 HI ⇌ AsI3 + 3 H2O

Reaction of arsenous acid with methyl iodide gives methylarsonic acid. This historically significant conversion is the Meyer reaction:[5]

As(OH)3 + CH3I + NaOH ⇌ CH3AsO(OH)2 + NaI + H2O

Alkylation occurs at As, and the oxidation state of As increases from III to V.

Toxicology

Arsenic-containing compounds are highly toxic and carcinogenic. The anhydride form of arsenous acid, arsenic trioxide, is used as a herbicide, pesticide, and rodenticide.

gollark: 🌵 🦀
gollark: Make an Embedded HQ9+ interpreter.
gollark: Oh, right, rightclick to erase.
gollark: There are other controls, documented somewhere... copy paste work as usual... stamps are available via ctrl+S, k can access saved stamps.
gollark: Well, you can use [ and ] to adjust cursor size, z to zoom in on a bit of space, and ctrl/shift/ctrl+shift for different ways to draw.

References
  1. NIOSH Pocket Guide to Chemical Hazards. "#0038". National Institute for Occupational Safety and Health (NIOSH).
  2. Munoz-Hernandez, M.-A. (1994). "Arsenic: Inorganic Chemistry". In King, R. B. (ed.). Encyclopedia of Inorganic Chemistry. Chichester: John Wiley & Sons.
  3. Kolozsi, A.; Lakatos, A.; Galbács, G.; Madsen, A. Ø.; Larsen, E.; Gyurcsik, B. (2008). "A pH-Metric, UV, NMR, and X-ray Crystallographic Study on Arsenous Acid Reacting with Dithioerythritol" (PDF). Inorganic Chemistry. 47: 3832–3840. doi:10.1021/ic7024439. PMID 18380458. Archived from the original (pdf) on 2012-04-25. Retrieved 2011-12-18.
  4. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  5. G. Meyer (1883). "Ueber einige anomale Reaktionen". Berichte der deutschen chemischen Gesellschaft. 13: 1439–1443. doi:10.1002/cber.188301601316.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.