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EC number: 246-140-8 | CAS number: 24304-00-5
- 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)
- Endpoint:
- adsorption / desorption: screening
- Data waiving:
- study technically not feasible
- Justification for data waiving:
- other:
- Reason / purpose for cross-reference:
- data waiving: supporting information
- Endpoint:
- adsorption / desorption: screening
- Type of information:
- experimental study
- Adequacy of study:
- key study
- Study period:
- No data
- Reliability:
- 2 (reliable with restrictions)
- Rationale for reliability incl. deficiencies:
- study well documented, meets generally accepted scientific principles, acceptable for assessment
- Qualifier:
- equivalent or similar to guideline
- Guideline:
- OECD Guideline 106 (Adsorption - Desorption Using a Batch Equilibrium Method)
- GLP compliance:
- not specified
- Remarks:
- No data available, publication.
- Type of method:
- batch equilibrium method
- Media:
- soil
- Radiolabelling:
- no
- Test temperature:
- 25 °C
- Analytical monitoring:
- yes
- Details on sampling:
- No details reported
- Matrix no.:
- #1
- Matrix type:
- other: Clay, kaolonite
- CEC:
- 8.03 other: mmol/100 g
- Matrix no.:
- #2
- Matrix type:
- other: Clay, vermiculite
- CEC:
- 119.07 other: mmol/100 g
- Matrix no.:
- #3
- Matrix type:
- other: Clay, calcium montmorillonite
- CEC:
- 106.83 other: mmol/100 g
- Matrix no.:
- #4
- Matrix type:
- other: Clay, palygorskite
- CEC:
- 21.23 other: mmol/100 g
- Matrix no.:
- #5
- Matrix type:
- other: Clay, sepiolite
- CEC:
- 18.9 other: mmol/100 g
- Matrix no.:
- #6
- Matrix type:
- other: Clayl, halloysite
- CEC:
- 6.1 other: mmol/100 g
- Details on matrix:
- COLLECTION AND STORAGE
- Geographic location: All natural clay minerals were collected from China, namely:
* kaolinite (Kaol) sample from Maoming, Guangdong province,
* vermiculite (Ver) sample from Lingshou, Hebei province,
* calcium montmorillonite (Mt) sample from Chifeng, Inner Mongolia,
* palygorskite (Pla) sample from Mingguang, Anhui Province,
* sepiolite (Sep) sample from Baoding, Hebei province, and
* halloysite (Hal) sample from Linfen, Shanxi province
- Collection procedures: not reported
- Sampling depth (cm): not reported
- Storage conditions: not reported
- Storage length: not reported
- Soil preparation: clay samples were pulverized and passed through a 74 μm sieve, and subsequently washed with distilled water to remove soluble matter and oven-dried at 100 °C for 24 h - Details on test conditions:
- 1. Batch adsorption experiments
- 1000 mg/L NH4Cl stock solution was further diluted with distilled water to get the desired experimental working solutions.
- Experiments were carried out using stopper test tube (50 mL) in a thermostatic shaker with clay mineral/liquid ratio of 0.3 g/25 mL.
- Dtermination of NH4+ concentration in solution by means of the Nessler's method with anm UV–vis spectrophotometer at 420 nm (UV-759S, Jinghua, China).
- Quality control testing included experiments with blanks and duplicates.
1.1 Adsorption kinetics experiments
- The optimum time required for the NH4+ adsorption to attain equilibrium was determined as a function of contact time in the range of 5–120 min
- NH4+ concentration: 10 mg/L
- pH: 7
- T: 25 °C
1.2 Adsorption isotherm experiments
- To investigate the effect of initial NH4+ concentration on the removal capacity of NH4+ in the batch adsorption experiment
- Concentration range: 10–1500 mg/L
- Duration: 2 h
1.3 Effect of solution pH on NH4+ adsorption
- pH range: of 2–10 pH
- NH4+ concentration: 30 mg NH4+/L
- Duration: 2 h.
- The initial pH was adjusted by 1 M HCl or NaOH solution.
1.4.Effect of clay dosage on NH4+ adsorption
- Clay amount: 0.1–0.5 g
- Initial NH4+ concentration: 30 mg/L
- Duration: 2 h
- Calculation of the removal efficiency (%) for the six clays and the equilibrium adsorption capacity (qe) were calculated, respectively by using the following equations:
Removal efficiency (%) = ((Co - Ce)/ Co) x 100
qe = (C0-Ce) V/ M
where Co = initial ammonium concentration (mg/L), Ce = equilibrium ammonium concentration (mg/L), qe = adsorption capacity (mg/g), V = volume of the ammonium solution (L), and M = mass of natural clay mineral (g). - Sample No.:
- #1
- Duration:
- 30 min
- Initial conc. measured:
- >= 10 - <= 1 500 other: mg NH4+/L
- pH:
- 7
- Temp.:
- 25 °C
- Sample No.:
- #2
- Duration:
- 30 min
- Initial conc. measured:
- >= 10 - <= 1 500 other: mg NH4+/L
- pH:
- 7
- Temp.:
- 25 °C
- Sample No.:
- #3
- Duration:
- 30 min
- Initial conc. measured:
- >= 10 - <= 1 500 other: mg NH4+/L
- pH:
- 7
- Temp.:
- 25 °C
- Sample No.:
- #4
- Duration:
- 30 min
- Initial conc. measured:
- >= 10 - <= 1 500 other: mg NH4+/L
- pH:
- 7
- Temp.:
- 25 °C
- Sample No.:
- #5
- Duration:
- 30 min
- Initial conc. measured:
- >= 10 - <= 1 500 other: mg NH4+/L
- pH:
- 7
- Temp.:
- 25 °C
- Sample No.:
- #6
- Duration:
- 30 min
- Initial conc. measured:
- >= 10 - <= 1 500 other: mg NH4+/L
- pH:
- 7
- Temp.:
- 25 °C
- Sample No.:
- #1
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.092 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Kaolinite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #2
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.301 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Vermiculite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #3
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.227 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Calcium montmorillinite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #4
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.223 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Palygorskite
- % Org. carbon:
- > 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #5
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.156 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Sepiolite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #6
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.092 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Halloysite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Transformation products:
- no
- Validity criteria fulfilled:
- not applicable
- Conclusions:
- NH4+ from aqueous solution strongly adsorbs to clay. The main driver of the adsorption is the cation exchange capacity (CEC) of the clay.
- Executive summary:
Six different clay types (kaolinite, halloysite, montmorillonite, vermiculite, palygorskite, and sepiolite) were used in this study to investigate the adsorption of ammonium (NH4+) from aqueous solution. Experiments were conducted at 0.3 g clay/25 mL NH4+solution at pH 7.
NH4+ solutions were applied to clay samples at concentrations ranging between 10 and 1,500 mg/L.
Adsorption equilibrium was quickly achieved after 30 minutes of exposure. Adsorption was measured by quantifying the remaining NH4+ in aqueous solution by means of UV-vis spectrometry after the equilibrium was reached.
Adsorption kinetics showed that the adsorption behaviour followed the pseudo-second-order kinetic model. The adsorption isotherms fitted by the Langmuir model illustrated that among all the clay types studied, vermiculite (50.06 mg/g) and montmorillonite (40.84 mg/g) showed the highest ammonium adsorption capacities. The main parameter driving NH4+ adsorption in soil is the cation exchange capacity (CEC).
- Endpoint:
- adsorption / desorption: screening
- Type of information:
- read-across from supporting substance (structural analogue or surrogate)
- Adequacy of study:
- key study
- Study period:
- No data
- Reliability:
- 2 (reliable with restrictions)
- Rationale for reliability incl. deficiencies:
- study well documented, meets generally accepted scientific principles, acceptable for assessment
- Justification for type of information:
- Aluminium nitride (AlN) as such is not soluble in water. However, aluminium nitride undergoes hydrolytic transformation in contact with water, predominantly forming insoluble aluminium salts like bayerite, Al(OH)3, and polymeric aluminium hydroxide species. In addition to aluminium, ammonia is formed as an important product of hydrolysis upon contact of aluminium nitride with water (e.g. soil pore water). Thus, read-across to the transformation products is applied to fulfil the endpoint requirements for adsorption/desorption screening.
For further details and justification of read-across please refer to the report attached in section 13 of IUCLID which provides information on the hypothesis for the analogue approach, information on purity and impurities of source and target chemical(s), the analogue approach justification as well as the data matrix. - Reason / purpose for cross-reference:
- read-across source
- Radiolabelling:
- no
- Sample No.:
- #1
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.092 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Kaolinite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #2
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.301 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Vermiculite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #3
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.227 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Calcium montmorillinite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #4
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.223 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Palygorskite
- % Org. carbon:
- > 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #5
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.156 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Sepiolite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Sample No.:
- #6
- Type:
- Kd
- Remarks:
- Langmuir constant
- Value:
- 0.092 other: L/mg
- pH:
- 7
- Temp.:
- 25 °C
- Matrix:
- Halloysite
- % Org. carbon:
- >= 1 - <= 2
- Remarks on result:
- other: Organic carbon (OC) was not reported in the present study. According to information from OECD guideline 106, the OC content in clay is typically between 1 and 2 %.
- Transformation products:
- no
- Validity criteria fulfilled:
- not applicable
- Conclusions:
- NH4+ from aqueous solution strongly adsorbs to clay. The main driver of the adsorption is the cation exchange capacity (CEC) of the clay.
- Executive summary:
Six different clay types (kaolinite, halloysite, montmorillonite, vermiculite, palygorskite, and sepiolite) were used in this study to investigate the adsorption of ammonium (NH4+) from aqueous solution. Experiments were conducted at 0.3 g clay/25 mL NH4+ solution at pH 7.
NH4+ solutions were applied to clay samples at concentrations ranging between 10 and 1,500 mg/L.
Adsorption equilibrium was quickly achieved after 30 minutes of exposure. Adsorption was measured by quantifying the remaining NH4+ in aqueous solution by means of UV-vis spectrometry after the equilibrium was reached.
Adsorption kinetics showed that the adsorption behaviour followed the pseudo-second-order kinetic model. The adsorption isotherms fitted by the Langmuir model illustrated that among all the clay types studied, vermiculite (50.06 mg/g) and montmorillonite (40.84 mg/g) showed the highest ammonium adsorption capacities. The main parameter driving NH4+ adsorption in soil is the cation exchange capacity (CEC).
This information is used in a read-across approach in the assessment of the target substance. For justification of read-across please refer to the attached read-across report (see IUCLID section 13).
Referenceopen allclose all
Adsorption characteristics of NH4+ onto natural clay minerals
1. Adsorption kinetics
- Removal efficiency of NH4+: increases with the increasing reaction time and reaches equilibrium in 30 min.
- To further investigate the adsorption behavior, pseudo-first order and pseudo-second-order kinetics models were used to analyze the obtained data and can be summarized as follows.
- The linear equations of pseudo-first, pseudo-second order models for boundary conditions of qe = 0 at t = 0 and qt = qe at t = te are as follows:
* The pseudo-first order: ln(qe − qt) = lnqe − k1t
* Pseudo-second order: t/qt = 1/(k2qe²) + (1/qe)t ; h = k2qe²
where qt = adsorption capacity at time t (mg/g),
k1and k2: adsorption constants (1/min) and (g/mg min), respectively, and
h = rate of adsorption (mg/g min).
- Results indicate that the adsorption kinetics of NH4+ is of pseudo-second-order
2. Effect of solution pH
- The removal efficiency of NH4+ increases with increasing pH from 2.0 to 7.0. With further increasing pH (up to pH 10) , it decreases steadily:
* pH < 7: negative charge on the clay mineral surface declines due to the excess protons in solution and competition for adsorption/exchange sites onto clay particles
* pH > 7: the removal efficiency of NH4+ decreases as NH4+ is transformed to aqueous NH3
--> Further experiments were performed at pH 7.
3. Effect of clay dosage
- The removal efficiency of NH4+ ions by increases with increasing adsorbent dosage from 0.1 g to 0.5 g.
- Basis fro effect: increasing number of active surface sites for NH4+ adsorption
--> 0.3 g was selected as the optimal dosage for all clays and used in the subsequent experiments.
4. Asorption isotherms
- Increase in the adsorption capacities for all clays with an increase of initial ammonium concentration from 10 to 1,000 mg NH4+/ L. At even higher concentrations, no remarkable change in adsorption capacities were noted.
- Vermiculite has the highest adsorption capacity followed by calcium montmorilinite. The adsorption capacity as such is presumably related to the high amount of exchangeable cations (such as Ca2+ and Na+) present in both clay types.
- The two main isotherm models, Langmuir model (LM) and Freundlich model (FM) were used to describe the experimental results of NH4+ as follow:
* LM adsorption isotherm: Ce/qe = 1/Kqmax + (1/qmax)Ce
where
K = Langmuir constant (L/mg)
qmax = max. adsorption capacity (mg/g).
* Freundlich model: log qe = log kF + 1/n log Ce
where
kF = Freundlich adsorbent capacity (mg/g (L/mg)1/n)
n = reciprocal of reaction order
- Results idicate the Langmuir model has a better fit for NH4+ adsorption on clay (R² > 0.92) than Freundlich model, indicating that the adsorption process of NH4+ by clay is a monolayer adsorption.
Adsorption characteristics of NH4+ onto natural clay minerals
1. Adsorption kinetics
- Removal efficiency of NH4+: increases with the increasing reaction time and reaches equilibrium in 30 min.
- To further investigate the adsorption behavior, pseudo-first order and pseudo-second-order kinetics models were used to analyze the obtained data and can be summarized as follows.
- The linear equations of pseudo-first, pseudo-second order models for boundary conditions of qe = 0 at t = 0 and qt = qe at t = te are as follows:
* The pseudo-first order: ln(qe − qt) = lnqe − k1t
* Pseudo-second order: t/qt = 1/(k2qe²) + (1/qe)t ; h = k2qe²
where qt = adsorption capacity at time t (mg/g),
k1and k2: adsorption constants (1/min) and (g/mg min), respectively, and
h = rate of adsorption (mg/g min).
- Results indicate that the adsorption kinetics of NH4+ is of pseudo-second-order
2. Effect of solution pH
- The removal efficiency of NH4+ increases with increasing pH from 2.0 to 7.0. With further increasing pH (up to pH 10) , it decreases steadily:
* pH < 7: negative charge on the clay mineral surface declines due to the excess protons in solution and competition for adsorption/exchange sites onto clay particles
* pH > 7: the removal efficiency of NH4+ decreases as NH4+ is transformed to aqueous NH3
--> Further experiments were performed at pH 7.
3. Effect of clay dosage
- The removal efficiency of NH4+ ions by increases with increasing adsorbent dosage from 0.1 g to 0.5 g.
- Basis fro effect: increasing number of active surface sites for NH4+ adsorption
--> 0.3 g was selected as the optimal dosage for all clays and used in the subsequent experiments.
4. Asorption isotherms
- Increase in the adsorption capacities for all clays with an increase of initial ammonium concentration from 10 to 1,000 mg NH4+/ L. At even higher concentrations, no remarkable change in adsorption capacities were noted.
- Vermiculite has the highest adsorption capacity followed by calcium montmorilinite. The adsorption capacity as such is presumably related to the high amount of exchangeable cations (such as Ca2+ and Na+) present in both clay types.
- The two main isotherm models, Langmuir model (LM) and Freundlich model (FM) were used to describe the experimental results of NH4+ as follow:
* LM adsorption isotherm: Ce/qe = 1/Kqmax + (1/qmax)Ce
where
K = Langmuir constant (L/mg)
qmax = max. adsorption capacity (mg/g).
* Freundlich model: log qe = log kF + 1/n log Ce
where
kF = Freundlich adsorbent capacity (mg/g (L/mg)1/n)
n = reciprocal of reaction order
- Results idicate the Langmuir model has a better fit for NH4+ adsorption on clay (R² > 0.92) than Freundlich model, indicating that the adsorption process of NH4+ by clay is a monolayer adsorption.
Description of key information
Adsorption/desorption is not relevant for aluminium nitride.
Key value for chemical safety assessment
Additional information
In accordance with REACH Annex XI, section 2, “testing for a specific endpoint may be omitted, if it is technically not possible to conduct the study as a consequence of the properties of the substance”.
Aluminium nitride (AlN) as such is not soluble in water. Since adsorption/desorption testing requires the test substance to be dissolved in aqueous medium, testing of the adsorption/desorption behaviour of AlN as such is technically not feasible. However, aluminium nitride undergoes hydrolytic transformation in contact with water, predominantly forming insoluble aluminium salts like bayerite, Al(OH)3, and polymeric aluminium hydroxide species. Free Al3+ ions are also released in low amounts, at maximum ca. 1 mg/L, positively related to the loading rate (see section 5.1.2 of this IUCLID dossier). Therefore, aluminium nitride as such cannot be tested for adsorptive properties.
The adsorption/desorption from the soluble fraction of Al3+ generated in contact with water is influenced and at the same time also superimposed by other effects occuring in soil, rendering it impossible to measure only the adsorption behaviour of soluble Al3+ deliberately added to soil matrix in an experimental setup. In view of the high abundance of aluminium in soil, aluminium deliberately added to the soluble fraction in laboratory experiments is indistinguishable from soil-originated aluminium, preventing quantification of the test material; accordingly, differentiation of adsorption and desorption processes is technically not feasible.
In addition to aluminium, ammonia is formed as an important product of hydrolysis upon contact of aluminium nitride with water (e.g. soil pore water). Ammonium has a strong tendency to adsorb to soil. Adsoption is driven by the cation exchange capacity (CEC) of the soil.
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.