Di(2-ethylhexyl)phosphoric acid
Di(2-ethylhexyl)phosphoric acid
Names
Preferred IUPAC name
Bis(2-ethylhexyl) hydrogen phosphate
Other names
Bis(2-ethylhexyl) phosphoric acid
Bis(2-ethylhexyl) phosphate
Bis(2-ethylhexyl) hydrophosphoric acid
BEHPA
BEHP
BEHHPA
BEHHP
Di(2-ethylhexyl) phosphoric acid
DEHPA
D2EHPA
EHPA
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.005.507
UNII
  • InChI=1S/C16H35O4P/c1-5-9-11-15(7-3)13-19-21(17,18)20-14-16(8-4)12-10-6-2/h15-16H,5-14H2,1-4H3,(H,17,18) ☒N
    Key: SEGLCEQVOFDUPX-UHFFFAOYSA-N ☒N
  • InChI=1/C16H35O4P/c1-5-9-11-15(7-3)13-19-21(17,18)20-14-16(8-4)12-10-6-2/h15-16H,5-14H2,1-4H3,(H,17,18)
    Key: SEGLCEQVOFDUPX-UHFFFAOYAP
  • CCCCC(CC)COP(=O)(O)OCC(CC)CCCC
Properties
C16H35O4P
Molar mass 322.43 g/mol
Appearance odorless colorless liquid (impure samples are often yellow)
Density 0.9758 g/mL
Melting point −50 °C (−58 °F; 223 K)
Boiling point 393 °C (739 °F; 666 K)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Di(2-ethylhexyl)phosphoric acid (DEHPA or HDEHP) is an organophosphorus compound with the formula (C8H17O)2PO2H. The colorless liquid is a diester of phosphoric acid and 2-ethylhexanol. It is used in the solvent extraction of uranium, vanadium and the rare-earth metals.[1]

Preparation

DEHPA is prepared through the reaction of phosphorus pentoxide and 2-ethylhexanol:

4 C8H17OH + P4O10 → 2 [(C8H17O)PO(OH)]2O
[(C8H17O)PO(OH)]2O + C8H17OH → (C8H17O)2PO(OH) + (C8H17O)PO(OH)2

These reaction produce a mixture of mono-, di-, and trisubstituted phosphates, from which DEHPA can be isolated based on solubility.[2]

Use in uranium extraction

Extraction

DEHPA is used in the solvent extraction of uranium salts from solutions containing the sulfate, chloride, or perchlorate anions. This extraction is known as the “Dapex procedure” (dialkyl phosphoric extraction). Reminiscent of the behaviours of carboxylic acids, DEHPA generally exists as a hydrogen-bonded dimer in the non-polar organic solvents. For practical applications, the solvent, often called a diluent, is typically kerosene.[3] A complex is formed from two equivalents of the conjugate base of DEHPA and one uranyl ion.[4] Complexes of the formula (UO2)2[(O2P(OR)2]4 also form, and at high concentrations of uranium, polymeric complexes may form.[3]

The extractability of Fe3+ is similar to that of uranium, so it must be reduced to Fe2+ before the extraction.[3]

Stripping

The uranium is then stripped from the DEHPA/kerosene solution with hydrochloric acid, hydrofluoric acid, or carbonate solutions. Sodium carbonate solutions effectively strip uranium from the organic layer, but the sodium salt of DEHPA is somewhat soluble in water, which can lead to loss of the extractant.[2]

Synergistic effects

The extractive capabilities of DEHPA can be increased through synergistic effects by the addition of other organophosphorus compounds. Tributyl phosphate is often used, as well as dibutyl-, diamyl-, and dihexylphosphonates. The synergistic effects are thought to occur by the addition of the trialkylphosphate to the uranyl-DEHPA complex by hydrogen bonding. The synergistic additive may also react with the DEHPA, competing with the uranyl extraction, resulting in a decrease in extraction efficiency past a concentration specific to the compound. [5]

Alternatives to DEHPA

Alternative organophosphorus compounds include trioctylphosphine oxide and bis(2,4,4-trimethyl pentyl)phosphinic acid.[6] Secondary, tertiary, and quaternary amines have also been used for some uranium extractions. Compared to phosphate extractants, amines are more selective for uranium, extract the uranium faster, and are easily stripped with a wider variety of reagents. However, the phosphates are more tolerant of solids in the feed solution and show faster phase separation.[5]

References

  1. ↑ Sato, T. Hydrometallurgy, 1989, volume 22, 121–140. doi:10.1016/0304-386X(89)90045-5
  2. 1 2 Galkin, N.P.; Sudarikov, B.N.; Veryatin, U.D.; Shishkov, Yu.D.; Maiorov, A.A. Technology of Uranium, 1st Ed.; Israel Program for Scientific Translations: Jerusalem, 1966.
  3. 1 2 3 Wilkinson, W.D. Uranium Metallurgy, 1st Ed.; Interscience Publishers: New York, 1962; Vol. 1.
  4. ↑ Lemire, A.E.; Janzen, A.F.; Marat, K. A 31P and 15N Study of the Extraction of Uranyl Nitrate by Di-2-ethylhexyl Phosphoric Acid. Inorg. Chim. Acta, 1985, 110, 234-241. doi:10.1016/S0020-1693(00)82312-9
  5. 1 2 Merritt, R.C. The Extractive Metallurgy of Uranium, 1st Ed.; Colorado School of Mines Research Institution, 1971.
  6. ↑ Kumar, Jyothi Rajesh; Kim, Joon-Soo; Lee, Jin-Young; Yoon, Ho-Sung (18 February 2011). "A Brief Review on Solvent Extraction of Uranium from Acidic Solutions". Separation & Purification Reviews. 40 (2): 77–125. doi:10.1080/15422119.2010.549760. S2CID 95358600.
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