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EC number: 237-415-3 | CAS number: 13776-88-0
- Life Cycle description
- Uses advised against
- Endpoint summary
- Appearance / physical state / colour
- Melting point / freezing point
- Boiling point
- Density
- Particle size distribution (Granulometry)
- Vapour pressure
- Partition coefficient
- Water solubility
- Solubility in organic solvents / fat solubility
- Surface tension
- Flash point
- Auto flammability
- Flammability
- Explosiveness
- Oxidising properties
- Oxidation reduction potential
- Stability in organic solvents and identity of relevant degradation products
- Storage stability and reactivity towards container material
- Stability: thermal, sunlight, metals
- pH
- Dissociation constant
- Viscosity
- Additional physico-chemical information
- Additional physico-chemical properties of nanomaterials
- Nanomaterial agglomeration / aggregation
- Nanomaterial crystalline phase
- Nanomaterial crystallite and grain size
- Nanomaterial aspect ratio / shape
- Nanomaterial specific surface area
- Nanomaterial Zeta potential
- Nanomaterial surface chemistry
- Nanomaterial dustiness
- Nanomaterial porosity
- Nanomaterial pour density
- Nanomaterial photocatalytic activity
- Nanomaterial radical formation potential
- Nanomaterial catalytic activity
- Endpoint summary
- Stability
- Biodegradation
- Bioaccumulation
- Transport and distribution
- Environmental data
- Additional information on environmental fate and behaviour
- Ecotoxicological Summary
- Aquatic toxicity
- Endpoint summary
- Short-term toxicity to fish
- Long-term toxicity to fish
- Short-term toxicity to aquatic invertebrates
- Long-term toxicity to aquatic invertebrates
- Toxicity to aquatic algae and cyanobacteria
- Toxicity to aquatic plants other than algae
- Toxicity to microorganisms
- Endocrine disrupter testing in aquatic vertebrates – in vivo
- Toxicity to other aquatic organisms
- Sediment toxicity
- Terrestrial toxicity
- Biological effects monitoring
- Biotransformation and kinetics
- Additional ecotoxological information
- Toxicological Summary
- Toxicokinetics, metabolism and distribution
- Acute Toxicity
- Irritation / corrosion
- Sensitisation
- Repeated dose toxicity
- Genetic toxicity
- Carcinogenicity
- Toxicity to reproduction
- Specific investigations
- Exposure related observations in humans
- Toxic effects on livestock and pets
- Additional toxicological data
Hydrolysis
Administrative data
Link to relevant study record(s)
- Endpoint:
- hydrolysis
- Type of information:
- experimental study
- Adequacy of study:
- supporting study
- Reliability:
- 2 (reliable with restrictions)
- Rationale for reliability incl. deficiencies:
- guideline study with acceptable restrictions
- Remarks:
- Summary report with acceptable restrictions
- Qualifier:
- according to guideline
- Guideline:
- OECD Guideline 111 (Hydrolysis as a Function of pH)
- Principles of method if other than guideline:
- Summary report for three chemical classes about biotic degradation, hydrolysis as a function of pH for phosphates, pyrophosphates and triphosphates.
- GLP compliance:
- no
- Analytical monitoring:
- yes
- Transformation products:
- not measured
- Remarks on result:
- not measured/tested
- Remarks on result:
- not measured/tested
- Endpoint:
- hydrolysis
- Type of information:
- migrated information: read-across from supporting substance (structural analogue or surrogate)
- Adequacy of study:
- supporting study
- Reliability:
- 2 (reliable with restrictions)
- Rationale for reliability incl. deficiencies:
- study well documented, meets generally accepted scientific principles, acceptable for assessment
- Principles of method if other than guideline:
- The change of water activity due to the variation of the aluminium content of alkaline aluminate solutions was determined.
- GLP compliance:
- no
- Analytical monitoring:
- yes
- Details on sampling:
- Sodium aluminate solutions with concentrations of 4.5, 5.8, 7.2 and 9 mole/dm³ were prepared
- Transformation products:
- not measured
- Remarks on result:
- not measured/tested
- Remarks on result:
- not measured/tested
- Endpoint:
- hydrolysis
- Type of information:
- migrated information: read-across based on grouping of substances (category approach)
- Adequacy of study:
- supporting study
- Reliability:
- 2 (reliable with restrictions)
- Rationale for reliability incl. deficiencies:
- study well documented, meets generally accepted scientific principles, acceptable for assessment
- Principles of method if other than guideline:
- The effect of pH on aluminium chloride hydrolysis was determined.
- GLP compliance:
- no
- Details on sampling:
- A test substance concentration of 1.5E-4 mol/L was prepared. The pH of the solution was adjusted to 4.0, 4.8, 5.0, 5.2, 5.8, and 6.4 respectively
- Buffers:
- - pH: 4.01 and 7.00
- Type of buffer: Tetramethylammmonium hydroxide pentahydrate and HCL solution - Transformation products:
- not measured
- Remarks on result:
- not measured/tested
- Remarks on result:
- not measured/tested
Referenceopen allclose all
Chemical Class |
Substance Used for Experimental Determination |
Anticipated Half-Life at 25°C |
References |
Phosphates Orthophosphates |
Not applicable, no possible mechanism for hydrolysis |
pH 4 > 1 year pH 7 > 1 year pH 9 > 1 year |
N/A |
Pyrophosphates Diphosphates |
Tetrapotassium Pyrophosphate CAS No. 7320-34-5 |
pH 4 > 1 year pH 7 > 1 year pH 9 > 1 year |
1 |
Triphosphates Tripolyphosphates |
Pentapotassium Triphosphate CAS No. 13845-36-8 |
pH 4 = 14.5 days pH 7 > 1 year pH 9 > 1 year
|
2 |
The hydrolytic half-life anticipated for the anions of specified phosphates, pyrophosphates and triphosphates has been addressed by read across from a single example for each chemical class, where applicable. The ionic substances were assumed to undergo dissociation in aqueous solution and the resulting cation to have negligible influence on the hydrolysis rate of the anion within the buffer solutions used as instructed by Method 111 of the DECD Guidelines for Testing of Chemicals, 13 April
2004.
Such a phenomenon may be replicated at environmentally relevant concentrations and on dissolution into complex environmental matrices. Although the cation composition of the final matrix may retain some minor influence on the hydrolytic rate, such a relationship is considered beyond the scope of the standard test method and would not have been addressed or identified by testing in accordance with OECD Method 111. The reported data was generated using buffer solutions with sodium salt
compositions.
References:
1. Tetrapotassium pyrophosphate: Determination of water solubility and abiotic
degradation, hydrolysis as a function of pH. Harlan Laboratories Ltd, Shardlow, UK, final
report for project number292010047.
2. Pentapotassium triphosphate: Determination of water solubility and abiotic
degradation, hydrolysis as a function of pH. Harlan Laboratories Ltd, Shardlow, UK, final
report for project number292010053.
3. Watanabe, Matsuura and Yamada (1981) The Mechanism of the Hydrolysis of
Polyphosphates. V. The Effect of Cations on the Hydrolysis of Pyro- and Triphophates.
Bull. Chem. Soc. Jpn,54, 738-741.
4. Watanabe (1982) The Mechanism of the Hydrolysis of Polyphosphates. V. The Effect
of Cations on the Hydrolysis of cyclo-Tri- and cyclo-Tetraphosphate.Bull. Chem. Soc.
Jpn,55,3766-3769.
The water activity increased with increasing aluminium concentration. The increase was attributed to the coordination of hydroxide ion to aluminium and/or dimerization connected with the dehydration of the monomeric species.
On the basis of the GIBBS-DUHEM equation the water activity data gave an indication of the concentration ranges in which the sodium aluminate solution exists mainly as I) NaOH + monomeric Al(OH)4-and II) NaOH + dimeric Al2O(OH)62-ions.
In systems of the same total alkali concentration an increase of the aluminium content leads to a general increase in the water activity of the solution.The water activity at low aluminium concentrations showed a smaller, almost linear, increase. In case smaller mole ratios (greater aluminium concentrations) a greater increase of water activity occurred leading to a steeper straight line. The change in water activity can be described - depending on the total electrolyte concentration - by assuming the presence of Al(OH)4- and NaOH in the solution of smaller aluminium concentrations (1 -4 M/dm3) and NaOH and dimer Al2O(OH)62- complex aluminate ions in systems of higher aluminium concentrations (2 -7 M/dm3) under alkaline conditions.
When AlCl3 was diluted to a concentration of 1.5*E-4 mol/L hydrolysis occurred immediately At pH 4 mono- and dimeric aluminium species were detected as main products. With increasing pH the hydrolysis and polymerisation increased. Monomeric and dimeric aluminium species hydrolysed and polymerised into small polymeric aluminium species at pH 4.8. At pH 5 the small polymeric aluminium species polymerised into median polymeric species. At pH 5.8 metastable median and large polymers decomposed into small aluminium species and disaggregated into dimeric species. At pH 6.4 the majority of aluminium species formed Al(OH)3 amorphous flocks.
Description of key information
Key value for chemical safety assessment
Additional information
According to the column II of Annex VIII, an experimental study on hydrolysis as a function of pH is not required for aluminium metaphosphate (CAS 13776-88-0) as the substance is poorly soluble.
Basically aluminium metaphosphate is subject to hydrolysis when the substance is released to water. During hydrolysis, triphosphate decomposes into orthophosphate ion and pyrophosphate ion in a parallel step. The pyrophosphate ion undergoes further hydrolysis and is converted into orthophosphate ions. Thus the hydrolysis reaction leads directly to the formation of orthophosphate.
The kinetic of hydrolysis of cyclic sodium trimetaphosphate (P3O92-) was investigated at acidic and alkaline solution, and at temperatures between 50 and 70 °C, by Healy & Kilpatrick (1955). The hydrolysis was rapid in acid solution, less rapid in alkaline solution, but negligible at pH9. The kinetic data showed that although H3P3O9 has been classified as a strong tribasic acid, it is necessary to take into account that the reaction solution reactivity increases with increase in (positive) charge of species involved and hydrolysis will speed up in present of metal ions, such Ca. Mg, Ba and Al. The experimental data were in good agreement with the following mechanism and gave a pseudo first-order reaction law and the hydrolysis may be written as:
P3O92- + H2O → P3O105- → PO43- + P2O74- + 2H
P2O74- + H2O →2 O43- + 2H+
The kinetics of hydrolysis of triphosphate and pyrophosphate were also studied in sterile lake water and sterile algal culture media and in non-sterile media at 25 °C by Clesceri and Lee (1965a, 1965b),and compared to published results obtained in distilled water. The results showed that triphosphate and pyrophosphate were hydrolysed in orthophosphate in a period of several days. Addition of glucose increased the rate of hydrolysis, indicating that microbial activity was one of the primary mechanisms of hydrolysis.
The hydrolytic half-life anticipated for the anions of specified phosphates, pyrophosphates and triphosphates has been addressed by read across from a single example for each chemical class, where applicable. The ionic substances were assumed to undergo dissociation in aqueous solution and the resulting cation to have negligible influence on the hydrolysis rate of the anion within the buffer solutions used as instructed by Method 111 of the OECD Guidelines (Harlan, 2011).
The available data demonstrate that triphosphates and triphosphates are hydrolytically stable under environmental conditions with a half-life > 1 year.
Chemical Class |
Substance Used for Experimental Determination |
Anticipated Half-Life at 25°C
|
|
Phosphates Orthophosphates |
Not applicable, no possible mechanism for hydrolysis |
N/A |
|
Pyrophosphates Diphosphates |
Tetrapotassium Pyrophosphate CAS 7320-34-5 |
pH4 > 1 year pH 7 > 1 year |
|
Triphosphates Tripolyphosphates |
Pentapotassium Triphosphate CAS 13845-36-8 |
pH 9: > 1 year |
|
pH4 - pH 7: 14.5 days > 1 year |
|||
pH 9: > 1 year |
The presence of multivalent metal ions, such as aluminium ion, catalyses hydrolysis reactions and increases hydrolysis rate, as hydrolysis of aluminium itself forms insoluble hydrolytic precipitantes, such as aluminium hydroxide or oxide. Orthophosphate can be incorporated into either biological solids (e.g. microorganisms) or chemical precipitates and removed from water,
The hydrolysis of aluminium strongly depends on pH and on the aluminium concentration. The pH dependency of aluminium hydrolysis was investigated by Zhao et al. (2009). The hydrolysis of aluminium chloride was tested at pH values ranging from 4 to 6.4. When AlCl3 was diluted to a concentration of 1.5*E-4 mol/L hydrolysis occurred immediately. At pH 4 mono- and dimeric aluminium species were detected as main products. With increasing pH the hydrolysis and polymerisation increased. Monomeric and dimeric aluminium species hydrolysed and polymerised into small polymeric aluminium species at pH 4.8. At pH 5 the small polymeric aluminium species polymerised into median polymeric species. At pH 5.8 metastable median and large polymers decomposed into small aluminium species and disaggregated into dimeric species. At pH 6.4 the majority of aluminium species formed Al(OH)3 amorphous flocks. Szabo et al. (1978) determined the change of water activity due to the variation of the aluminium content of alkaline aluminate solutions. In systems of the same total alkali concentration an increase of the aluminium content leads to a general increase in the water activity of the solution. The water activity at low aluminium concentrations showed a smaller, almost linear, increase. In case smaller mole ratios (greater aluminium concentrations) a greater increase of water activity was determined leading to a steeper straight line.
References:
Clesceri N.L. and Lee G.F. (1965a) Hydrolysis of Condensed Phosphates – II : Sterile Environment, Int. J. Air Wat. Poll. 9, 743-751.
Clesceri N.L. and Lee G.F. (1965b) Hydrolysis of Condensed Phosphates – I : Non-Sterile
Healy R.M., Kilpatrick M.L., (1955) A Kinetic Study of the Hydrolysis of Trimetaphosphates, J. Am. Chem. Soc., 1955, 77 (20), pp 5258–5264
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