Tritiated water

Tritium oxide
All types of isotopically substituted water molecules have this structure.
All types of isotopically substituted water molecules have this structure.
Names
IUPAC name
[3H]2-water
Systematic IUPAC name
(3H2)Water
Other names
  • Super-heavy water
  • Tritium oxide
  • Ditritium oxide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
MeSH tritium+oxide
  • InChI=1S/H2O/h1H2/i/hT2
    Key: XLYOFNOQVPJJNP-PWCQTSIFSA-N
  • [3H]O[3H]
Properties
T2O or 3H2O
Molar mass 22.0315 g·mol−1
Appearance Colorless liquid
Density 1.21 g/mL
Melting point 4.48 °C (40.06 °F; 277.63 K)
Boiling point 101.51 °C (214.72 °F; 374.66 K)
Acidity (pKa) 15.21
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Tritium oxide (T₂O), also called tritiated water or super-heavy water, is a radioactive form of water in which the hydrogen atoms are replaced by tritium (^3H), a radioactive isotope of hydrogen.[1] It is chemically similar to normal water but exhibits radioactivity due to beta decay from tritium.[2]

Properties

Tritium oxide is a colorless liquid with a density of 1.21 g/mL, a melting point of 4.48 °C, and a boiling point of 101.51 °C.[3] It is chemically similar to normal water but radioactive due to the presence of tritium. Tritium emits low-energy beta particles during decay, leading to self-radiolysis of the water and formation of radicals such as OH· and OT·.[4]

Production

Tritium oxide can be produced through several methods. Catalytic oxidation of tritium gas (T₂) with oxygen results in tritium gas reacting with molecular oxygen over a catalyst to form tritiated water (T₂O).[5][6]

Electrolysis of water in the presence of tritium allows tritium atoms in water to be concentrated during electrolysis, producing tritiated water.[7]

Isotopic exchange between tritiated hydrogen and water permits tritium to exchange with hydrogen in normal water to form tritiated water.[8]

Uses

Tritiated water is used in:

  • Tracer studies in biology, physiology, and environmental science.[9]
  • Radio-luminescent devices, such as watches, exit signs, and instrument dials.[10]
  • Fusion research as a component of fuel for deuterium–tritium reactions.[11]
  • Environmental tracing of water movement and turnover studies.

Safety and Environmental Impact

Tritium oxide is radioactive and may pose internal contamination risks through ingestion, inhalation, or skin absorption.[12] It occurs naturally in small amounts due to cosmic ray interactions and is also released from nuclear reactors, weapons testing, and certain consumer products.[13] The biological half-life of tritiated water in humans is typically 7–14 days, depending on age, activity, and environmental conditions.[14] Safety procedures include limiting exposure, replacing contaminated water with uncontaminated sources, and monitoring environmental release.

References

  1. ^ "Tritium oxide". PubChem. Retrieved 2025-08-19.
  2. ^ Heinze, Sylver; Stolz, Thibaut; Ducret, Didier; Colson, Jean-Claude (2005). "Self-Radiolysis of Tritiated Water: Experimental Study and Simulation". Fusion Science and Technology. 48 (1): 673–679. doi:10.13182/FST05-A1014.
  3. ^ "Tritium oxide". PubChem.
  4. ^ Heinze, Sylver; Stolz, Thibaut; Ducret, Didier; Colson, Jean-Claude (2005). "Self-Radiolysis of Tritiated Water: Experimental Study and Simulation". Fusion Science and Technology. 48 (1): 673–679. doi:10.13182/FST05-A1014.
  5. ^ "Tritium gas oxidation". INIS. Retrieved 19 August 2025.
  6. ^ Shmayda, William T. (2015). "Oxidation of Tritium" (PDF). LLE Review. 157.
  7. ^ "Electrolytic enrichment of tritiated water". Fusion Engineering and Design. 12: 55–61. 1986.
  8. ^ "Tritium isotopic exchange". OSTI. Retrieved 19 August 2025.
  9. ^ Holmes, J.A. (1971). "Tritiated Water as a Tracer in Biological Studies". Journal of Applied Ecology. 8: 669–676.
  10. ^ Glass, David (2010). Radioluminescent Materials. Springer. ISBN 978-3-540-58019-5.
  11. ^ Fowler, Michael (2014). "Tritium Handling in Fusion Reactors". Fusion Engineering and Design. 89: 20–25.
  12. ^ "Radiation Protection: Tritium". EPA.
  13. ^ Leclaire, Simon (2008). "Environmental Levels of Tritium". Journal of Environmental Radioactivity. 99: 1180–1189.
  14. ^ Chou, C. (1985). "Biological Half-life of Tritium in Humans". Health Physics. 48: 87–92.

Further reading

  • International Atomic Energy Agency (IAEA). Tritium Handling and Safe Storage. Vienna: IAEA.
  • Health Physics Society. Tritium Fact Sheet. 2024.
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