Potassium hypochromate
Other names
  • Potassium chromate(V)
3D model (JSmol)
  • O=[Mn-3](=O)(=O)=O.[K+].[K+].[K+]
Molar mass 233.2886 g/mol
Appearance Green solid
Melting point 1,000 °C (1,830 °F; 1,270 K) (decomposes)
Soluble, decomposes (25 °C)[1]
Similar to potassium hypomanganate
-370 ± 2 kcal mol−1[2]
Flash point Not flammable
Related compounds
Other anions
Potassium hypomanganate
Other cations
Sodium hypochromate
Related chromates
Potassium chromate
Potassium perchromate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Potassium hypochromate is a chemical compound with the formula K3CrO4 with the unusual Cr5+ ion. This compound is unstable in water but stable in alkaline solution[1] and was found to have a similar crystal structure to potassium hypomanganate.[2]


This compound is commonly prepared by reacting chromium(III) oxide and potassium hydroxide at 850 °C under argon:[2]

Cr2O3 + 6 KOH → 2 K3CrO4 + H2O + 2 H2

This compound can be prepared other ways such as replacing chromium oxide with potassium chromate. It is important that there is no Fe2+ ions present because it would reduce the Cr(V) ions to Cr(III) ions.[1]


Potassium hypochromate decomposes in water to form chromium(III) oxide and potassium chromate when alkali is not present or low.[1] Potassium hypochromate also reacts with acids such as hydrochloric acid to form chromium(III) oxide, potassium chromate, and potassium chloride:[2]

6 K3CrO4 + 10 HCl → 4 K2CrO4 + Cr2O3 + 5 H2O + 10 KCl

Other reducing agents such as hydroperoxides can reduce the hypochromate ion into chromate ions.[1] At extremely high temperatures, it decomposes into potassium chromate and potassium metal.[2]

This compound is used to synthesize various compounds such as chromyl chlorosulfate by reacting this compound with chlorosulfuric acid.[3]


  1. ^ a b c d e N. Bailey; M. C. R. Symons (1957). "Structure and reactivity of the oxyanions of transition metals. Part III. The hypochromate ion". Journal of the Chemical Society (Resumed). 35: 203–207. doi:10.1039/jr9570000203.
  2. ^ a b c d e Lawrence H. Johnson; Loren G. Hepler; Carlos E. Bamberger; Donald M. Richardson (1978). "The enthalpy of formation of potassium chromate(V), K3CrO4(c)". Canadian Journal of Chemistry. The Ohio State University: National Research Council. 56 (4): 446–449. doi:10.1139/v78-071.
  3. ^ Silvia A. Brandán (2012). "1". A Structural and Vibrational Study of the Chromyl Chlorosulfate, Fluorosulfate, and Nitrate Compounds (Ebook). Springer Netherlands. p. 2. ISBN 9789400757639. Retrieved 15 October 2021.