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Title: Edds  
Author: World Heritage Encyclopedia
Language: English
Subject: S-Nitrosoglutathione, Nitrilotriacetic acid, Chelating agents, Carboxylic acids, Amines
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Skeletal formula of EDDS
CAS number  YesY
PubChem ,  2-[(2-{[(1S)-1-Carboxyethyl]amino}ethyl)amino],  (2R)-2-[(2-{[(1R)-1-Carboxyethyl]amino}ethyl)amino],  (2S)-2-[(2-{[(1S)-1-Carboxyethyl]amino}ethyl)amino],  (2S)-2-[(2-{[(1R)-1-Carboxyethyl]amino}ethyl)amino]
ChemSpider  N,  2-[(2-{[(1S)-1-Carboxyethyl]amino}ethyl)amino] YesY,  (2R)-2-[(2-{[(1R)-1-Carboxyethyl]amino}ethyl)amino] YesY,  (2S)-2-[(2-{[(1S)-1-Carboxyethyl]amino}ethyl)amino] YesY
Jmol-3D images Image 1
Image 2
Molecular formula C10H16N2O8
Molar mass 292.24 g mol−1
Density 1.44 g mL−1
Melting point 220 to 222 °C (428 to 432 °F; 493 to 495 K)
Acidity (pKa) 2.4
Basicity (pKb) 11.6
Std enthalpy of
−1.9541–−1.9463 MJ mol−1
Std enthalpy of
−4.2755–−4.2677 MJ mol−1
Related compounds
Related alkanoic acids EDTA
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 N   YesY/N?)

Ethylenediamine-N,N'-disuccinic acid (EDDS) is an aminopolycarboxylic acid. It is a colourless solid that is used as chelating agent that may offer a biodegradable alternative to EDTA, which is currently used on a large scale in numerous applications.


  • Structure and properties 1
  • Synthesis 2
    • From aspartic acid 2.1
  • Coordination chemistry 3
  • Uses 4
  • External links 5
  • References 6

Structure and properties

EDDS has two chiral centers, and as such three stereoisomers.[1] These are the enantiomeric (R,R) and (S,S) isomers and the achiral meso (R,S) isomer. As a biodegradable replacement for EDTA, only the (S,S) stereoisomer is of interest. The (R,S) and (R,R) stereoisomers are less biodegradable, whereas the (S,S) stereoisomer has been shown to be very effectively biodegraded even in highly polluted soils.[2]


EDDS was first synthesized from

  1. ^ Neal, J. A.; Rose, N. J. (1968). "Stereospecific Ligands and Their Complexes. I. A Cobalt(III) Complex of Ethylenediaminedisuccinic Acid". Inorganic Chemistry 7 (11): 2405–2412.  
  2. ^ Tandy, S.; Ammann, A.; Schulin, R.; Nowack, B. (2006). "Biodegredation and speciation of residual SS-ethylenediaminedisuccinic acid (EDDS) in soil solution left after soil washing". Environmental Pollution 142 (2): 191–199.  
  3. ^ Barbier, M. et al. (1963). "Synthese und Eigenschaften eines Analogen des Lycomarasmins und der Aspergillomarasmine". Liebigs Annalen 668: 132.  
  4. ^ US patent 3158635, Kezerian, Charles; Ramsey, William M., "Bisadducts of diamines and unsaturated acids", issued 1964-11-24 
  5. ^ Takahashi, R. et al. (1999). "Production of (S,S)-Ethylenediamine-N,N'-disuccinic Acid from Ethylenediamine and Fumaric Acid by Bacteria". Biosci. Biotechnol. Biochem. 63 (7): 1269–1273.  
  6. ^ Orama, M.; Hyvönen, H.; Saarinen, H.; Aksela, R. (2002). "Complexation of [S,S] and mixed stereoisomers of N,N’-ethylenediaminedisuccinic acid (EDDS) with Fe(III), Cu(II), Zn(II) and Mn(II) ions in aqueous solution". J. Chem. Soc., Dalton Trans. (24): 4644–4648.  
  7. ^ Pavelčík, F and Majer, J. (1978). "The crystal and molecular structure of lithium [(S,S)-N,N'-ethylenediaminedisuccinato]cobaltate(III) trihydrate". Acta Crystallographica B 34 (12): 3582–3585.  
  8. ^ Yuan, Z. and VanBriesen, J. M. (2006). "The Formation of Intermediates in EDTA and NTA Biodegradation". Environmental Engineering Science 23 (3): 533–544.  
  9. ^ Yip, T.C.M.; Tsang, D.C.W.; Ng, K.T.W.; Lo, I.M.C. (2009). "Kinetic interactions of EDDS with soils. 1. Metal resorption and competition under EDDS deficiency". Environ. Sci. Technol. 43 (3): 831–836.  
  10. ^ Yip, T.C.M.; Tsang, D.C.W.; Ng, K.T.W.; Lo, I.M.C. (2009). "Empirical modeling of heavy metal extraction by EDDS from single-metal and multi-metal contaminated soils". Chemosphere 74 (2): 301–307.  
  11. ^ Tsang, D.C.W.; Yip, T.C.M.; Lo, I.M.C. (2009). "Kinetic interactions of EDDS with soils. 2. Metal-EDDS complexes in uncontaminated and metal-contaminated soils". Environ. Sci. Technol. 43 (3): 837–842.  


  • Sigma Aldrich page on EDDS, containing a link to a MSDS

External links

[11] On the other hand, during soil remediation which involves continuous flushing, metal extraction is often limited by the amount of EDDS. Under EDDS deficiency, initial unselective extraction of heavy metals was observed, followed by heavy metal exchange and re-adsorption of heavy metals that have lower stability constant with EDDS.[10] When EDDS is applied in chemical-enhanced soil remediation in excessive case (e.g., when applied for ex-situ soil washing), higher extraction efficiency for heavy metals can be achieved and the amount of extraction is less independent with the EDDS dosage;[9][8] (S,S)-EDDS is a biodegradable chelating agent that offers an alternative to EDTA, of which 80 million kilograms are produced annually. Under natural conditions, EDTA has been found to convert to ethylenediaminetriacetic acid and then cyclize to the


Another comparison that can be made between (S,S)-EDDS and EDTA is the structure of the chelated complex. EDTA’s six donor sites form five five-membered chelate rings around the metal ion, four NC2OFe rings and one C2N2Fe ring. The C2N2Fe ring and two of NC2OFe rings define a plane, and two NC2OFe rings are perpendicular to the plane that contains the C2-symmetry axis. The five-membered rings are slightly strained. EDDS’s six donor sites form both five- and six-membered chelate rings around the metal ion: two NC2OFe rings, two NC3OFe rings, and one C2N2Fe ring. Studies of the crystal structure of the Fe[(S,S)-EDDS]- complex show that the two five-membered NC3OFe rings project out of the plane of the complex, reducing the equatorial ring strain that exists in the Fe[EDTA]- complex.[7] The complex also has C2 symmetry.

Because of the lower stability for [Fe(S,S)-EDDS]-, the useful range being roughly 3<pH(S,S)-EDDS<9 and 2EDTA<11. However, this range is sufficient for most applications.[6]

Formation Reaction Formation Constant
[Fe(H2O)6]3+ + (S,S)-EDDS4- → Fe[(S,S)-EDDS]- + 6 H2O KEDDS = 1020.6
[Fe(H2O)6]3+ + EDTA4- → Fe(EDTA)- + 6 H2O KEDTA = 1025.1

In comparing the effectiveness of (S,S)-EDDS versus EDTA as chelating agents for iron(III):

In its octahedral complexes, edds poses the six-membered chelate rings in the equatorial positions.

Coordination chemistry

(S,S)-EDDS is produced stereospecifically by the alkylation of an ethylenedibromide with L-aspartic acid. Racemic EDDS is produced by the reaction of ethylenediamine with fumaric acid or maleic acid.

From aspartic acid


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