Registration Dossier
Registration Dossier
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EC number: 932-833-9 | CAS number: -
Hydrolysis
Administrative data
Link to relevant study record(s)
Description of key information
The speciation of iron citrate in aqueous solution is complicated and a variety of coordination compounds may be formed. However, this is not a hydrolytic degradation reaction. Ammonium iron (III) citrate and ammonium sulfate are both expected to dissociate under environmentally relevant conditions (see Section 1.3 of the CSR).
Key value for chemical safety assessment
Additional information
The requirement to test the substance for hydrolysis was waived as the chemical structure of the substance is not suggestive of a hydrolytic degradation mechanism.
The speciation of iron citrate in aqueous solution is complicated and a variety of coordination compounds may be formed. However, this is not a hydrolytic degradation reaction. Ammonium iron (III) citrate and ammonium sulfate are both expected to dissociate under environmentally relevant conditions (see Section 1.3 of the CSR). Therefore, the hydrolytic stability of the components is discussed below.
Iron
The behaviour of ions of iron (Fe2+and Fe3+) in solution is dependent on the different conditions. Key conditions that influence iron behaviours are:
- Oxygen content
- pH
- Presence of potential ligand anions with which the cationic iron might associate.
Iron (III) reacts with hydroxide ions to give insoluble iron oxides (Cotton F.A. and Wilkinson G.,1972), with the reaction being favoured by higher pH. Ferric hydroxide (Fe(OH)3) is highly insoluble with solubility product Ksp= 1 x 10-36(CRC Handbook). Formation of ferric hydroxide at pH levels above 5.0 limits the presence of iron in aqueous systems.
Citrate
Citrate is readily biodegradable and, therefore, a hydrolysis study is not required according to Column 2 of REACH Annex VIII. The substance contains no chemical groups that are hydrolytically unstable.
Ammonia/Ammonium sulphate
Neither ammonia/ammonium or sulphate contain any groups that are hydrolytically unstable.
In aqueous solution, ammonium sulfate is completely dissociated into the ammonium ion (NH4+) and the sulfate anion (SO42-). Ammonia (NH3) exists in equilibrium with the ammonium ion (NH4+), with the position of the equilibrium depending on the pH:
NH4+ + H2O <-> NH3 + H3O+.
In general, as pH increases, the fraction of the total ammonia which is un-ionized increases.
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