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EC number: 233-135-0 | CAS number: 10043-01-3
- 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
Adsorption / desorption
Administrative data
Link to relevant study record(s)
Description of key information
Adsorption of aluminium occurs only under pH conditions where it hydrolyzes to give various hydrolysis products. Progressive hydrolysis leads to the formation of colloidal aluminium hydroxide.
Aluminium sulphate has a propensity to leach through soil if water is applied, i.e. it does have mobility through soil, and providing sufficient water is present. As it moves downwards into layers where the water content is low, the leaching will stop.
On this basis, it does not have a high potential for adsorption to soil if water is not present andonly part of the aluminium sulphate in the solid phase is adsorbed.
On the other basis if water is present aluminium sulphate as aluminium hydroxide precipitate (Al(OH)3) have a high potential for adsorption to soil.
The estimated Soil Adsorption Coefficient was 75.41 L/kg measured by calculation from EPI SuiteTM v4.0..This is Exposure Assessment Tools and Models made from EPA (Environmental Protection Agency).
Koc Estimate from MCI:
---------------------
First Order Molecular Connectivity Index ........... : 7.431
Non-Corrected Log Koc (0.5213 MCI + 0.60) .......... : 4.4734
Fragment Correction(s):
2 Miscellaneous S(=O) group .......... : -2.5960
Corrected Log Koc .................................. : 1.8774
Estimated Koc: 75.41 L/kg <===========
Key value for chemical safety assessment
- Koc at 20 °C:
- 75.41
Additional information
Adsorption of aluminium occurs only under pH conditions where it hydrolyzes togive various hydrolysis products.Progressive hydrolysis leads to the formation of colloidalaluminium hydroxide.
The rate at which soluble aluminium sulphate are gradually leached away is dependent upon the water supply. In humid regions, the upper layers of soil and rock are kept thoroughly leached, and as fast as they are formed the soluble products are removed in the drainage water. In semi-arid regions, the soils are not fully leached and soluble substances tend to accumulate.
When dissolved in a large amount of neutral or slightly-alkaline water, aluminium sulfate hydrolyzes to form the aluminium hydroxide precipitate(Al(OH)3) and a dilute sulfuric acid solutionandreduce the pH of soil.
The anhydrous form occurs naturally as a rare mineral millosevichite, found e.g. in volcanic environments and on burning coal-mining waste dumps. Aluminium sulfate is rarely, if ever, encountered as the anhydrous salt. It forms a number of different hydrates, of which the hexadecahydrate Al2(SO4)3•16H2O and octadecahydrate Al2(SO4)3•18H2O are the most common. The heptadecahydrate, whose formula can be written as [Al(H2O)6]2(SO4)3•5H2O, occurs naturally as the mineral alunogen.
The above information indicates that aluminium sulphate has a propensity to leach through soil if water is applied, i.e. it does have mobility through soil, and providing sufficient water is present. As it moves downwards into layers where the water content is low, the leaching will stop.
On this basis, it does not have a high potential for adsorption to soil if water is not present andonly part of thealuminium sulphatein the solid phase is adsorbed.
On the other basis if water is present aluminium sulphate asaluminium hydroxide precipitate(Al(OH)3) have a high potential for adsorption to soil.
- soil, the colloidal surface can adsorb large quantities ofaluminium
Selectivity of cation adsorption
The affinity of most cations for an adsorbing surface is greater for divalent than for monovalent ions, and for large cations than for small ones of the same charge because the larger the cation the less hydrated it is. The usual affinity is:
Al3+> Ba2+>Sr2 +>Ca2+>Mg2+= Cs+>Rb+>K+= NH4+>Na+
The soil cations that are readily adsorbed onto soil colloids can be divided ino two groups. Firstly there are the base catoins,which include the important plant nutrients Ca2+, Mg2+ ,K+and Na+. Secondly there are acid cations,which include Al3+and H+. Related to this distinction in cations is the term base saturation, which is defined as the proportion of exchange sites occupied by base cations. A soil with a high base saturation (greater than 35%) is more fertile than a soil with a low base saturation.
Al3+, Ca2+and H+are the commonly adsorbed cations in humid regions. This reflects the long-term leaching loss of basic cations and their replacement by acidic cations. In contrast, Ca2+,Mg2+, K+and Na+are the commonly adsorbed cations in arid regions.
Aluminium influences of soil acidity
As clay minerals weather and break down, the aluminium in the octahedral layer is released into the soil solution, where it either reacts with water or is adsorbed onto the exchange sites of negatively charged clay minerals. Al3+ions are adsorbed in preference to all the other major cations. The influence that aluminium has on soil acidy is itself dependant on the acidity of the soil. At Ph less 5, aluminium is soluble and exists as Al3+. When Al3+enters the soil solution it reacts with water (it is hydrolysed) to produce H+ions:
Al3++ H2O <===> AlOH2++ H+
Thus the acidity of the soil increases (pH falls). In soils with a pH of between 5 and 6.5, aluminium also contributes H+oins to the soil solution but by different mechanisms, as aluminium can no longer exist as Al3+ions but is converted to aluminium hydroxyl ions:
Al3++ OH-<===> AlOH2+
AlOH2++H-<===> Al(OH)2+
ALUMINIUM HYDROXY IONS
These hydroxyl aluminium ions act as exchangeable cations just like Al3+, and are adsorbed by the clay minerals. They are in equilibrium with hydroxyl aluminium ions in the soil solution, where they produce H+ions by the following reactions:
AlOH2++H20 <===> Al(OH)2+ + H+
Al(OH)2 ++H20 <===> Al(OH)3+ + H+
In soils where the pH is above 7 Ca2+and Mg2+dominated the exchange sites and most of the hydroxyl aluminium ions have been converted to gibbsite (Al(OH)3), is insoluble and cannot be by the negative clay minerals as no charge. In a neutral soil the exchangeable cations that dominate the cation exchange sites are the base cations, whereas in an acidics soils aluminium and hydrogen ions dominate the exchange sites.
On this basis if water is present aluminium sulphate as aluminium hydroxide precipitate (Al(OH)3) have a high potential for adsorption to soil.
If released into water, aluminium sulphate is not expected to adsorb to suspended solids and sediment based upon the Koc. The Koc of aluminium sulphate can be estimated to be 75.41. This estimated Koc value suggests that Aluminium sulphate is expected to have very high mobility in soil.
These results suggest that Aluminium sulphate has high soil mobility and does not have a high potential for adsorption to soil.
The estimated Soil Adsorption Coefficient was 75.41 L/kg measured by calculation from EPI SuiteTM v4.0..This is Exposure Assessment Tools and Models made from EPA (Environmental Protection Agency).
Koc Estimate from MCI:
---------------------
First Order Molecular Connectivity Index ........... : 7.431
Non-Corrected Log Koc (0.5213 MCI + 0.60) .......... : 4.4734
Fragment Correction(s):
2 Miscellaneous S(=O) group .......... : -2.5960
Corrected Log Koc .................................. : 1.8774
Estimated Koc: 75.41 L/kg <===========
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