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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
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Endpoint summary
Administrative data
Description of key information
Additional information
Transport and distribution
Distribution modelling are not applicable sincealuminium sulfateis an inorganic substance whichwhen is 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 solution and reduce the pH of soil.
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.
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 as aluminium 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 anadsorbingsurface 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 thebase catoins,which include the important plant nutrients Ca2+, Mg2+ ,K+and Na+. Secondly there areacid 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 commonlyadsorbedcations 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.
The estimated Soil Adsorption Coefficient was31.82L/kg measured by calculation from EPI SuiteTM v4.0..This is Exposure Assessment Tools and Models made from EPA (Environmental Protection Agency).
Inorganic compounds are outside the estimation domain.
For Soil Adsorption Comparison Purposes:
Koc Estimate from MCI:
---------------------
First Order Molecular Connectivity Index ........... : 1.732
Non-Corrected Log Koc (0.5213 MCI + 0.60) .......... : 1.5027
Fragment Correction(s) --> NONE : ---
Corrected Log Koc .................................. : 1.5027
Estimated Koc: 31.82 L/kg <===========
Distribution modelling is not applicable since aluminium sulphate is an inorganic substance and it is designed for organic chemicals.
The estimated Fugacity model is applied to estimate the distribution of this substance in the environment.
The estimated STP Fugacity Model and Volatilization From Waterwere measured by calculation from EPI SuiteTM v4.0 Program. This is Exposure Assessment Tools and Models made from EPA (Environmental Protection Agency) .
STP Fugacity Model: Predicted Fate in a Wastewater Treatment Facility
======================================================================
(using 10000 hr Bio P,A,S)
PROPERTIES OF: Aluminium sulphate
-------------
Molecular weight (g/mol) 346.17
Aqueous solubility (mg/l) 1E+006
Vapour pressure (Pa) 1.49321E-021
(atm) 1.47368E-026
(mm Hg) 1.12E-023
Henry 's law constant (Atm-m3/mol) 5.10144E-030
Air-water partition coefficient 2.08634E-028
Octanol-water partition coefficient (Kow) 1.51356E-008
Log Kow -7.82
Biomass to water partition coefficient 0.8
Temperature [deg C] 25
Biodeg rate constants (h^-1),half life in biomass (h) and in 2000 mg/L MLSS (h):
-Primary tank 0.04 15.97 10000.00
-Aeration tank 0.04 15.97 10000.00
-Settling tank 0.04 15.97 10000.00
STP Overall Chemical Mass Balance:
---------------------------------
g/h mol/h percent
Influent 1.00E+001 2.9E-002 100.00
Primary sludge 2.50E-002 7.2E-005 0.25
Waste sludge 1.50E-001 4.3E-004 1.50
Primary volatilization 2.78E-027 8.0E-030 0.00
Settling volatilization 7.58E-027 2.2E-029 0.00
Aeration off gas 1.87E-026 5.4E-029 0.00
Primary biodegradation 1.76E-003 5.1E-006 0.02
Settling biodegradation 5.27E-004 1.5E-006 0.01
Aeration biodegradation 6.93E-003 2.0E-005 0.07
Final water effluent 9.82E+000 2.8E-002 98.15
Total removal 1.85E-001 5.3E-004 1.85
Total biodegradation 9.22E-003 2.7E-005 0.09
Level III Fugacity Model (Full-Output):
=======================================
Chem Name : Aluminium sulphate
Molecular Wt : 346.17
Henry's LC : 5.1e-030 atm-m3/mole (calc VP/Wsol)
Vapor Press : 1.12e-023 mm Hg (Mpbpwin program)
Liquid VP : 1.83e-020 mm Hg (super-cooled)
Melting Pt : 350 deg C (Mpbpwin program)
Log Kow : -7.82 (Kowwin program)
Soil Koc : 86.4 (KOCWIN MCI method)
Mass Amount Half-Life Emissions
(percent) (hr) (kg/hr)
Air 2.17e-009 1.83e+003 1000
Water 18 900 1000
Soil 81.9 1.8e+003 1000
Sediment 0.109 8.1e+003 0
Fugacity Reaction Advection Reaction Advection
(atm) (kg/hr) (kg/hr) (percent) (percent)
Air 1.47e-033 3.89e-008 1.03e-006 1.3e-009 3.43e-008
Water 6.28e-035 656 852 21.9 28.4
Soil 1.34e-033 1.49e+003 0 49.7 0
Sediment 6.18e-035 0.441 0.103 0.0147 0.00344
Persistence Time: 1.58e+003 hr
Reaction Time: 2.2e+003 hr
Advection Time: 5.55e+003 hr
Percent Reacted: 71.6
Percent Advected: 28.4
Half-Lives (hr), (based upon Biowin (Ultimate) and Aopwin):
Air: 1834
Water: 900
Soil: 1800
Sediment: 8100
Biowin estimate: 2.434 (weeks-months)
Advection Times (hr):
Air: 100
Water: 1000
Sediment: 5e+004
Volatilization From Water
=========================
Chemical Name: Aluminium sulphate
Molecular Weight : 346.17 g/mole
Water Solubility : 1E+006 ppm
Vapor Pressure : 1.12E-023 mm Hg
Henry's Law Constant: 5.1E-030 atm-m3/mole (calculated from VP/WS)
RIVER LAKE
--------- ---------
Water Depth (meters): 1 1
Wind Velocity (m/sec): 5 0.5
Current Velocity (m/sec): 1 0.05
HALF-LIFE (hours) : 2.135E+026 2.329E+027
HALF-LIFE (days ) : 8.897E+024 9.706E+025
HALF-LIFE (years) : 2.436E+022 2.657E+023
Aluminum (Al) and water
Aluminum and water: reaction mechanisms, environmental impact and health effects
The amount of aluminum in seawater varies between approximately 0.013 and 5 ppb. The Atlantic Ocean is known to contain more aluminum than the Pacific Ocean. Riverwater generallycontains about 400 ppb of aluminum.
Aluminum mainly occurs as Al3+ (aq) under acidic conditions, and as Al(OH)4- (aq) under neutral to alkalic conditions. Other forms include AlOH2+ (aq) en Al(OH)3 (aq).
Aluminum reaction with water
Aluminum metal rapidly develops a thin layer of aluminum oxide of a few millimeters that prevents the metal from reacting with water.
When this layer is corroded a reaction develops, releasing highly
flammable hydrogen gas.
Aluminum chloride hydrolyses in water, and forms a mist when it comes in
contact with air, because hydrochloric acid drops form when it reacts
with water vapor.
Aluminum ions in other compounds also hydrolyze, and this continues
until the cationic charge has run out, ending the reaction by hydroxide
formation. The beginning of the hydrolysis reaction is as follows:
Al3+(aq) + 6H2O(l) <-> [Al(H2O)6]3+ (aq)
Solubility of aluminum and aluminum compounds
The most abundant aluminum compounds are aluminum oxide and aluminum hydroxide, and these are water insoluble.
Aluminum oxide may be present in water both in alkalic form (2Al2O3 (s)
+ 6H+ (aq) -> Al3+ (aq) + 3H2O (l)) and in acidic form (2Al2O3 (s) +
2OH- (aq) -> AlO2- (aq) + H2O (l)).
An example of a water soluble aluminum compound is aluminum sulphate with
a water solubility of 370 g/L.
Aluminum present in water
Aluminum forms during mineral weathering of feldspars, such as and orthoclase, anorthite, albite, micas and bauxite, and subsequently ends up in clay minerals. A number of gemstones contain aluminum, examples are ruby and sapphire.
Currently, only iron and steel are produced in larger amounts than
aluminum. Additionally, aluminum is largely recycled because this is
very distinctly possible. It is applied in for example frames, door
knobs, car bodies, plane parts (the weight/ strength relation is very
favourable), engines, cables and cans. Aluminum is a good reflector and
is therefore applied in solar mirrors and heat reflecting blankets.
Aluminum is processed to cans, wiring and alloys.
Aluminum salts are often added to water to start precipitation reactions
for phosphate removal.
Consequently, sewage sludge in water purification with a pH value between 6.8 and 7.3 is present as hydroxides.Alums are applied as fertilizer in tea plantations. Other aluminum compounds are applied in paper production. Alloys such as duraluminum are applied because these are stronger than aluminum itself. Aluminum foam is applied in tunnels as soundproofing material.
Other examples of aluminum application include aluminum chloride use in
cracking processes, aluminum oxide as an abrasive or for production of
inflammable objects, aluminum sulphate use as a basic material in paper
glue, tanners, mordants and synthetic rubber, and aluminum hydrogen as a
reduction and hydration agent.
Aluminum occurs as an aerosol in oceanic surface layers and in waters.
This is because aluminum dust end up in water. Particles end up in water
through surface run-off or atmospheric transport.Generally, aluminum
concentrations increase with increasing water depth
Environmental effects of aluminum in water
Aluminum may negatively affect terrestrial and aquatic life in different
ways. Regular aluminum concentrations in groundwater are about 0.4 ppm,
because it is present in soils as water insoluble hydroxide. At pH
values below 4.5 solubility rapidly increases, causing aluminum
concentrations to rise above 5 ppm. This may also occur at very high pH
values.
Dissolved Al3+-ions are toxic to plants; these affect roots and decrease
phosphate intake. As was mentioned above, when pH values increase
aluminum dissolves. This explains the correlation between acid rains and
soil aluminum concentrations. At increasing nitrate deposition the
aluminum amount increases, whereas it decreases under large heather and
agricultural surfaces. In forest soils it increases.
Aluminum is not a dietary requirement for plants, but it may positively influence growth in some species. It is taken up by all plants because of its wide distribution in soils. Grass species may accumulate aluminum concentrations of above 1% dry mass.
Acid rain dissolves minerals in soils, and transports these to water sources. This may cause aluminum concentrations in rivers and lakes to rise.
Aluminum naturally occurs in waters in very low concentrations. Higher
concentrations derived from mining waste may negatively affect aquatic
biocoenosis. Aluminum is toxic to fish in acidic, unbuffered waters
starting at a concentration of 0.1 mg/L. Simultaneous electrolyte
shortages influence gull permeability, and damage surface gull cells.
Aluminum is mainly toxic to fish at pH values 5.0-5.5. Aluminum ions
accumulate on the gulls and clog these with a slimy layer, which limits
breathing. When pH values decrease, aluminum ions influence gull
permeability regulation by calcium. This increases sodium losses.
Calcium and aluminum are antagonistic, but adding calcium cannot limit
electrolyte loss. This mainly concerns young animals. An aluminum
concentration of 1.5 mg/L turned out to be fatal to trout. The element
also influences growth of freshwater bony fish.
Phytoplankton contains approximately 40-400 ppm aluminum (dry mass),
which leads to a bioconcentration factor of 104-105 compared to seawater.
Terrestrial organisms also contain some aluminum. Examples: mosquito larvae 7-33 ppm, springtails 36-424 ppm (dry mass). Together, pH values and aluminum concentrations determine larvae mortality.
A number of LD50 values for rats are known for aluminum. For oral intake this is 420 mg/kg for aluminum chloride, and 3671 mg/kg for aluminum nonahydrate. The mechanism of toxicity is mainly based on enzyme inhibition.
Only one non-radioactive aluminum isotope occurs naturally. There are eight instable isotopes.
Health effects of aluminum in water
The total aluminum concentration in the human body is approximately 9
ppm (dry mass). In some organs, specifically the spleen, kidneys and
lung, concentrations up to 100 ppm (dry mass) may be present. Daily
aluminum intake is approximately 5 mg, of which only a small fraction is
absorbed. This leads to relatively low acute toxicity. Absorption is
about 10 μg per day. These amounts are considered harmless to humans.
Silicon may decrease aluminum uptake. However, once the element is taken
up in the body it is not easily removed.
Large aluminum intake may negatively influence health. This was
connected with nerve damage. Particularly people with kidney damage are
susceptible to aluminum toxicity. There is a risk of allergies. Aluminum
is probably mutagenic and carcinogenic. A correlation between aluminum
uptake and an increased number of Alzheimer cases is suspected. However,
this is uncertain because aluminum concentrations always increase with
age. Increased aluminum intake may also cause osteomalacia (vitamin D
and calcium deficits).
Aluminum intake mainly occurs through food and drinking water. The most
recent standards were between 50 and 200 μg/L. Aluminum particles may
cause functional lung disorder.
No known diseases are linked to aluminum shortages.Aluminum chloride may
corrode the skin, irritate the mucous membranes in the eyes, and cause
perspiration, shortness of breath and coughing. Alum increases blood
clotting.
Water purification technologies applied to remove
aluminum from water
Aluminum may be removed from water by means of ion exchange or coagulation/ flocculation. Aluminum salts are applied in water treatment for precipitation reactions. Adding aluminum sulphate and lime to water causes aluminum hydroxide formation, which leads to settling of pollutants. Hydroxide is water insoluble, therefore only 0.05 ppm dissolved aluminum remains. This is below the legal limit for drinking water of the World Health Organization (WHO), of 0.2 ppm aluminum.
Information on Registered Substances comes from registration dossiers which have been assigned a registration number. The assignment of a registration number does however not guarantee that the information in the dossier is correct or that the dossier is compliant with Regulation (EC) No 1907/2006 (the REACH Regulation). This information has not been reviewed or verified by the Agency or any other authority. The content is subject to change without prior notice.
Reproduction or further distribution of this information may be subject to copyright protection. Use of the information without obtaining the permission from the owner(s) of the respective information might violate the rights of the owner.
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