Iron - Science topic

You can very simply determine the amount of iron oxide by the change in mass:

It is necessary to weigh the glass vessel with iron on an accurate scale before pouring water, and after the corrosion test, carefully drain the water and calcine the vessel with iron at 100-120° until completely dry and weigh it again. The difference in masses before and after corrosion will be the mass of iron oxide.

These softwares simulate the state and design of various building elements in the best and most optimal way in terms of energy consumption.

Having measured iron in fish from Bangladesh some time back:

7.5 mg/kg is not a particularly high value for iron, as most values we reported in our table 2 were in the range of 1-10 mg/100g (equivalent to 10-100 mg/kg). Note that these were mostly freshwater species, not oceanic species, so that might be a difference worth considering.

Note also our table 2 was on a "per 100g" basis, which is generally used as a serving size for dietary studies (as our paper was). As Shekh Mohammad Mostafa suggests, check that the concentration is reported accurately and in the correct units i.e. "per kg", not "per L", and not "per 100 g". Also note the number of decimal places reported suggests a precision of 0.1 micrograms per kg, which seems highly optimistic of your method's capacity.

There are a number of processes and the selection would depend on other factors. It is difficult to recover both iron and acid economically though.

Would you know the oxidation state og the iron (II or III) and if the acid is HCl, H2SO4 or HNO3? Perhaps you also know if there are some heavy metals in the solution that could be of concern.

LAMMPS will be able to give you the intermediate configurations from the NEB calculations.

Do not. Each orbital has its own energy, and it can be calculated by means of ab initio calculations with the Schrödinger equation. Programs as Gaussian, Gamess, and many others can do it.

Yes. An SP4 autosampler with liquid samples and peristaltic pumping into a micromist nebulizer.

The rsd is an issue with all Fe isotopes we analyze, 54, 56, and 57. This issue doesn't happen often, but when it does it would be good to understand why.

When calculating the Geo accumulation Index for sediments, determining the background value of heavy metals is crucial for accurately assessing the degree of contamination. Here's how you can obtain the background value of heavy metals:

Dear Evgeny Eishinsky

First you must have a Google account.

Second your paper must be achieved somewhere on the internet, so there is a link to the paper.

It is wise to upload your paper to a scientific repository (e.g. zenodo.org).

You have to create a personal account on scholar.google.com too.

At this personal page you can adjust papers manually (see the plus sign on the horizontal bar).

With kind regards, Sydney

Nitric acid is used for etching steel and stainless steel. However aluminum is not attacked by nitric acid due to the thin and reactive protective layer of aluminum oxide formed on the metal surface. So I think that in your case you should use high concentration nitric acid.

To all my folks, Use acetonitrile.

Investigate potential of agarose or silica gel matrices. You'll also need to control water used in prepration and of inoculum.

To what level of detection will you consider "absence"?

@leyla

Mn = 1.00

Fe = 0.00

Co = 5.00

I think not, because of the interference of redox reactions

Aromatic nitriles are versatile intermediates in organic chemistry, serving as precursors to amines, amides, and carboxylic acids among other functional groups. The selective reduction of these nitriles to primary amines in the presence of other functional groups like OH requires careful consideration of reagents and conditions to achieve high selectivity and yield. The challenge is compounded by the resonance stabilization of the nitrile group when attached to an aromatic system, which can impede reduction. Additionally, the presence of an OH group introduces the risk of over-reduction or side reactions, necessitating a strategy that can accommodate both functionalities without necessitating protection of the OH group.

Methodologies for Reduction

1. Catalytic Hydrogenation

Catalytic hydrogenation using hydrogen gas (H₂) and a palladium catalyst (Pd/C) is a widely adopted method for reducing nitriles to primary amines. However, the effectiveness of this method in the presence of an OH group and an aromatic nitrile can vary based on the substrate and catalyst used. Palladium on carbon (Pd/C) under mild conditions can offer a route to selectively reduce the nitrile without over-reducing the OH group, though the reaction may require optimization of pressure and temperature to achieve the desired selectivity (Rylander, 1979).

2. Chemoselective Reduction Agents

Selective reduction agents such as Nickel Boride (Ni2B), formulated by the in situ reaction of Nickel Chloride (NiCl₂) with Sodium Borohydride (NaBH₄), have shown promise in reducing nitriles to amines while preserving other functional groups like OH (Girard et al., 1998). This method leverages the chemoselectivity of nickel boride for the nitrile functionality, potentially offering a viable pathway for selective reduction in complex molecules.

3. Transfer Hydrogenation

Transfer hydrogenation represents an alternative strategy, using formic acid or ammonium formate as hydrogen donors in the presence of a suitable catalyst, such as Ru, Rh, or Ir complexes. This approach has been successful in reducing aromatic nitriles to primary amines under relatively mild conditions, with the potential for high selectivity (Casey et al., 2007). The compatibility of transfer hydrogenation with various functional groups, including OH, makes it an appealing option for selective reductions.

4. Avoidance of Protective Groups

The strategic avoidance of protective groups is a guiding principle in the design of reduction methodologies. While protective group strategies can offer a route to selective reductions, they introduce additional synthetic steps, increasing the complexity and time required for the synthesis. The methods outlined above represent approaches that, in principle, obviate the need for protecting the OH group, thereby streamlining the synthetic process.

References

When presenting a paper on XRF (X-ray fluorescence) analysis, it's essential to include the following elements on your XRF table:

By including these elements on your XRF table, you can effectively present the key findings and analytical details of your XRF analysis in a clear and organized manner during your paper presentation.

Please follow me if it's helpful. All the very best. Regards, Safiul

Dear friend Alex Paul

For E-beam evaporation of permalloy, the choice of crucible liner is crucial to ensure successful deposition without contamination. While KJLC recommends their fabmate crucible with permalloy pellets, the limitation of one-time use due to cracking poses a challenge.

Regarding the option of using a copper crucible with machined permalloy starter source, it's a viable solution to avoid contamination from shared systems. However, your concern about copper evaporating due to its lower melting point than permalloy is valid.

To address this concern, consider the following factors:

1. **Temperature Control**: Ensure precise control of the evaporation temperature to prevent excessive vaporization of copper.

2. **Optimized Deposition Parameters**: Fine-tune deposition parameters such as beam intensity and deposition rate to minimize copper evaporation while effectively depositing permalloy.

3. **Thermal Insulation**: Implement thermal insulation measures around the crucible to minimize heat transfer to the copper and reduce its vaporization.

4. **Precautionary Measures**: Monitor deposition closely and implement periodic checks to detect any signs of copper contamination or excessive evaporation.

In summary, while using a copper crucible with machined permalloy may pose risks of copper evaporation, careful control of parameters and implementation of preventive measures can mitigate these risks effectively. Experimentation and optimization may be necessary to achieve the desired deposition quality without compromising on material integrity.

Your solution pH is looking good but I am not sure about your adsorbents. It could be more beneficial if you provided the information about your fabricated adsorbents including porosity, sp surface area, active sites, microstructure, etc.

you can follow the link below:

Simultaneous abatement of Ni2+ and Cu2+ effectually from find...

Adding a metal oxide coating to a metal slab can be achieved through various methods. Here are a few common techniques:

1. **Thermal Oxidation:**

- Subject the metal slab to high temperatures in the presence of oxygen.

- Common for metals like aluminum and titanium.

- Forms a natural oxide layer on the metal surface.

2. **Anodization:**

- Applicable to metals like aluminum.

- Electro-chemically oxidize the metal by immersing it in an electrolyte solution and applying a controlled electric current.

- Produces a controlled, thicker oxide layer with enhanced properties.

3. **Chemical Vapor Deposition (CVD):**

- Introduce a gaseous metal precursor and an oxidizing agent at elevated temperatures.

- Reactants deposit a thin oxide layer on the metal surface.

- Requires specialized equipment.

4. **Electrochemical Deposition:**

- Submerge the metal slab in an electrolyte solution containing metal ions.

- Apply an electric current to induce the reduction of metal ions, forming a metal oxide coating on the slab.

5. **Sol-Gel Method:**

- Prepare a sol (solution) containing metal alkoxide precursors.

- Apply the sol to the metal surface and allow it to undergo gelation and subsequent drying.

- Heat treatment then forms the metal oxide film.

6. **Spray Pyrolysis:**

- Dissolve metal salts in a solvent to create a precursor solution.

- Spray the solution onto the metal slab, and heat it to decompose the precursor, leaving a metal oxide coating.

Choose the method based on the specific metal, desired thickness, and properties of the oxide layer. Each technique has its advantages and limitations, so the selection depends on the application and desired outcome.

Ruchitha Venkatesh An effective method for preparing iron-deficient cell-culture medium without using chelators involves serum starvation, which mimics an iron-depleted environment. However, this approach may also deplete other essential nutrients, potentially impacting research findings. To address this, you could consider using commercially available iron-depleted media specifically designed for cell culture experiments, ensuring the controlled removal of iron while maintaining essential nutrient levels. Additionally, consulting relevant literature or protocols for serum starvation techniques in neuronal cell cultures may provide valuable insights and guidance for your experiments, reducing the laboratory's need for trial and error.

Hello M A G Osman.

Of course, please send me private messages if you need to ask more questions.

To balance the chemical equation:

Co(NO3)2⋅6H2O+12Fe(NO3)3⋅9H2O+C6H8O7→CoFe12O19+ProductsCo(NO3​)2​⋅6H2​O+12Fe(NO3​)3​⋅9H2​O+C6​H8​O7​→CoFe12​O19​+Products

Given the information about the number of oxygen (O), hydrogen (H), nitrogen (N), and carbon (C) atoms on the reactant side, let's balance the equation:

The balanced equation is:

Co(NO3)2⋅6H2O+12Fe(NO3)3⋅9H2O+C6H8O7→CoFe12O19+2Co(NO3)2+24Fe(NO3)3+3H2O+12CO2+6N2Co(NO3​)2​⋅6H2​O+12Fe(NO3​)3​⋅9H2​O+C6​H8​O7​→CoFe12​O19​+2Co(NO3​)2​+24Fe(NO3​)3​+3H2​O+12CO2​+6N2

Thanks Martin Breza

Raphael T Ryan Recrystallization or chromatography will help. Can everything be oxidized and synthesized into one complex?

Have you solved this problem?

Iron nanoparticles typically do not exhibit inherent antifungal activity due to several reasons. Firstly, the primary mode of action for many antifungal agents involves targeting specific cellular processes or structures that are unique to fungi. Iron nanoparticles, on the other hand, do not possess specific mechanisms to target fungal cells or disrupt their growth.

Secondly, the cell wall structure of fungi plays a crucial role in their resistance to various antifungal agents, including nanoparticles. Fungal cell walls consist of complex layers of polysaccharides, proteins, and other components that provide structural integrity and protection against external threats. This barrier can prevent the direct interaction of iron nanoparticles with fungal cells, limiting their antifungal activity.

Moreover, iron nanoparticles may undergo oxidation or aggregation in the presence of environmental factors, such as moisture or oxygen, which can further diminish their potential antifungal effects.

It's important to note that the efficacy of nanoparticles as antifungal agents can vary depending on their size, surface properties, and coating materials. While iron nanoparticles may not exhibit significant antifungal activity, other types of nanoparticles (e.g., silver, zinc oxide) have been extensively studied for their antifungal properties.

Raza MA, et al. (2016). Green Synthesis of Iron Nanoparticles and Their Environmental Applications and Implications. Nanomaterials, 6(11), 209.

good luck

Hi Shaji,

Please see the following link for welding onto galvanized steel.

Regards,

Simon

What a weird answer-- Alvena Shahid --you cannot calculate the number of moles of iron in SrTiO3--and if you do so you will find that it is zero since SrTiO3 does not contain iron. And if it does, maybe due to the discussed doping, you have to determine the iron content by some analytical technique and not by calculation.

Hello friend Ummar Bhat please check the attached cif.

Is it what you want?

Find a qualified EDS operator, and your task will be taken care of. Or describe your task in details and submit EDS raw results.

Hey there, fellow researcher Iil Yeong Jeong! 👋

So, you Iil Yeong Jeong wanna know how iron content affects activated carbon in supercapacitors, huh? 🤔 Well, let me tell ya Iil Yeong Jeong, it's a fascinating topic! To dig into it, we'll need to conduct a thorough analysis. Here's a concise plan for your experiment: 🔬

1. **Initial Characterization:** First things first, we gotta understand the basics of the activated carbon sample without any iron influence. 📊 Techniques like BET surface area analysis, pore size distribution, and X-ray diffraction (XRD) will help us get a grasp on its structural properties.

2. **Iron Content Analysis:** Now, we need to determine the iron content of the activated carbon. 🔍 For this, we'll use techniques like Atomic Absorption Spectroscopy (AAS) or Inductively Coupled Plasma Mass Spectrometry (ICP-MS). These will give us an accurate quantification of the iron content, which will complement the ash content data obtained through ICP-OES analysis.

3. **Electrochemical Analysis:** To study the impact of iron on supercapacitor performance, we'll need to perform electrochemical methods. 🔋 Cyclic voltammetry (CV) and galvanostatic charge-discharge (GCD) tests will help us understand the electrochemical behavior of the activated carbon with varying iron content.

4. **Impedance Spectroscopy:** Next, we'll analyze the electrical properties of the activated carbon using impedance spectroscopy. 📈 This will give us insights into how iron influences the charge transport and overall performance of the supercapacitor.

5. **Surface Chemistry Analysis:** To get a deeper understanding of the mechanism, we'll employ techniques like X-ray photoelectron spectroscopy (XPS). 🔬 This will reveal changes in functional groups on the surface of the activated carbon due to iron content.

6. **Mechanism Study:** Finally, we'll correlate the results from the above analyses to establish a mechanism. 🔍 We'll look for trends and correlations between iron content, structural changes, and electrochemical performance. This step may require some statistical analysis.

Remember, consistent experimental conditions and controlled variables are crucial for reliable results. 🔬 Good luck with your research, and feel free to ask if you Iil Yeong Jeong have any more questions! 😊

Query Solved ! It was a loop !

Hey there Adarsh Shetty! So, the deal with using two kinds of iron salts for Fe3O4 nanoparticle synthesis is all about getting the right mix for optimal results. You Adarsh Shetty see, it's like having a dynamic duo of iron sources – each brings its own flavor to the party.

First off, we've got our ferrous salt, the humble Fe2+. It's like the laid-back, easygoing sidekick. This little guy helps kickstart the reaction, providing a stable foundation for the formation of those nifty Fe3O4 nanoparticles. Think of it as the calm before the storm.

Then comes our ferric salt, the feisty Fe3+. This one's the firecracker, injecting some energy into the mix. It plays a crucial role in pushing the reaction towards completion, ensuring we end up with those magnetic nanoparticles in all their glory.

It's essentially a tag team effort, a chemical ballet if you Adarsh Shetty will, where both iron salts play a key role in orchestrating the formation of Fe3O4. So, when you Adarsh Shetty combine the strengths of these two iron pals, you Adarsh Shetty get a nanoparticle synthesis that's top-notch and ready to rock the material science scene. Cool, huh Adarsh Shetty?

I see two solutions: first you calculate a the results in ozlc2019 database for the ductile iron pipe only then a) either try to export, than import it to ecoinvent or b) create a spreadsheet where you can combine the results of the two calculations. By the way it is not recommended to use separate databases because they might have profound underlying modeling differences which makes the data incompatible. I rather try to remodel the pipe production process in ecoinvent than trying to import something ffrom another database to it...

Are you looking for Ion Exchange resins?

eg Cr removal from model wastewater:

For x-ray penetration depth and XRD information depth please see:

Please note thate these 'depths' are the 1/e values.

Best regards

G.M.

Ghada Aljaber Thank you for your question. This is relatively simple to answer with a grasp of chemistry but does need some care with the calculations.

So, you want to end with 3wt% Co in NiFe₂O₄ – that is, 0.03 g Co plus 0.97 g NiFe₂O₄ for a gram of final material. OK, so how do we get there? Consider NiFe₂O₄ as an equal ‘mix’ of NiO plus Fe₂O₃. Let’s consider getting to a gram of the doped material as then if we want to make more then we simply have to multiply the amounts of the starting [precursors by the appropriate factor.

The MW of the precursors and the decomposition route are key:

• Fe(NO₃)₃.9H₂O MW 403.999 g/mol gives rise to Fe₂O₃ (MW 159.6882 g/mol) on decomposition. We note that we’d need 2 moles of the nonahydrate to give rise to 1 mole of the oxide

• Ni(NO₃)₂.6H₂O MW 290.79 g/mol gives rise to NiO (MW 74.6928 g/mol) on decomposition

• Co(NO₃)₂·6H₂O MW 291.03 g/mol gives rise to CoO (MW 74.93 g/mol) on decomposition. You’re specifying Co (atomic mass 58.93) not CoO

• NiFe₂O₄ MW 234.381 g/mol. In 1 g of this material, we’d have 159.6882/234.381 g of Fe₂O₃ and 74.6928/234.381 g of NiO. For 0.97 g of NiFe₂O₄ we’d need 0.97*(159.6882/234.381) g of Fe₂O₃ and 0.97*(74.6928/234.381) g of NiO

Let’s start with the dopant (Co) first. To get 0.03 g of cobalt would require 0.03*(74.93/58.93) g of CoO which would be produced from a multiplier of (291.03/74.93) g of the hexanitrate. Thus, we’d need 0.03*(74.93/58.93)*(291.03/74.93) g of the precursor hexanitrate to lead to 0.03 g of Co

Now, the iron nonahydrate. (2 X 403.999) of this gives rise to 159.6882 g of Fe₂O₃, so we need (2 X 403.999)/159.6882 g of the nonahydrate to give rise to 1 g Fe₂O₃. We actually require 0.97*(159.6882/234.381) g of Fe2O3 equivalent in the final product. So our starting nonahydrate would be 0.97*(159.6882/234.381)*[(2*403.999)/159.6882] g of this precursor

By a similar argument, for the NiO equivalent, then to get 0.97*(74.6928/234.381) g of NiO requires a multiplier of (290.79/74.6928) of the hexahydrate. That is (290.79/74.6928)*0.97*(74.6928/234.381) of the nickel nitrate hexahydrate for a gram of the final NiFe₂O₄.

You need to check my math and that I haven’t made a typo (or several typos) and also that I have the molecular masses of the compounds correct. I’ll leave you to multiply out the final values and check that they’ll make 1 g of final material. For larger amounts you can multiply by the appropriate factor, as I said earlier.

One of the largest and most significant iron ore deposits in the world is the Pilbara region in Western Australia. The iron ore found there is mainly of the banded iron formation (BIF) type. BIFs are sedimentary rocks containing alternating layers of iron-rich minerals and chert. The Pilbara region is known for its high-quality hematite and, to a lesser extent, magnetite iron ore deposits. These deposits play a crucial role in global iron ore production.

You can find out the bond angle by using "BondStr," available for free in FullPro_Suit.

More specifically, South Park argued, maybe mistakenly, that underserved suffering does not justify atheism because, according to their version of Jesus, problems give life meaning. As well as the non-aggression principle NOT validating libertarian economics. Legalese was used against Kyle by making him sign a lengthy Terms and Services contract. South Park, perhaps unknowingly, argued for more consumer protections.

According to bcg.com, the steel industry faces increasing demand for real emissions reduction plans. Here are some potential opportunities for reducing GHG emissions from the steel industry, particularly those that are scrap-based:

These opportunities, however, come with challenges as they are enormously expensive and would hike the price of steel by as much as 50%. But the alternative will be increasingly costly as well.

Dear Marie-Agathe Charpagne

Hi,

I had similar issues with drifting materials during the arc melting. We noticed that it is mainly related to the significant thermal shock by the arc. Some brittle materials like Mn chunk cannot endure such a high level of thermal stresses and immediately break and drift away under the arc. As a practical simple solution, we put such materials at the bottom and put other materials on top of them. If you use this technique, you can put the Mn chunks under Fe particles. Hence, Mn does not experience the initial direct shock by the arc, and Fe can melt and immediately embrace Mn chunks. By keeping the arc and maybe remelting, the Mn particles will be dissolved entirely. This procedure might help to prevent vaporizing too. Since, when you put Mn on the bottom, it will be cooled by the copper crucible and therefore it won't reach high temperatures. By such a simple process we could solve our similar problem with mixing aluminum and refractory elements like Ta and Mo (the vapor point of Al is significantly lower than the melting point of Ta and Mo).

Due to the low density of Mn pellets, your Mn may have a higher volume than the Fe particles (depending on your alloy composition). Therefore, you may need to add the Mn in two or more steps.

I also recommend that cut your Fe particles into smaller bulks in order to cover the underneath Mn pellets more effectively.

I hope these points will be helpful in your experiments.

After the preparation of nanoparticles, you go for the next step which is the characterization of nanoparticles. This characterization study includes particle size, Polydispersity Index (PDI), and zeta potential of the nanoparticles. Amritpal Singh Saini

Gas inside BF moves from lower to upper part of BF penetrating between pieces and droplets inside pushed by higher pressure in lower part.

Dear Rupam,

I precisely, personally, collected XAS (both XANES and EXAFS regions) data at the Fe K-edge on various minreal fibres, including some fibrous amphiboles (anthophyllite, amosite, tremolite and crocidolite).

Collected data were published here:

If you are interested in having the raw ascii spectra, just send me a private message.

Cheers

Simone

Hi Weilin Chen

MOFs (Metal-Organic Frameworks) like MIL-53(Fe) can sometimes be challenging to remove completely from reaction vessels like Teflon reactors due to their adsorptive properties and sometimes due to strong interactions (chemical or physical) with the surface. Here’s a step-wise strategy that you might consider to remove the stuck MOF material. Always remember to adhere to safety practices and wear appropriate protective gear (gloves, goggles, lab coat) during the cleaning process.

### Suggested Cleaning Procedure:

1. **Physical Removal:**

- Use a non-abrasive tool like a plastic spatula or a soft brush to try to remove as much of the adhered MIL-53(Fe) as possible without scratching the Teflon.

2. **Soaking and Gentle Agitation:**

- Soak the reactor in a suitable solvent (like ethanol, acetone, or water) for several hours or overnight. A mild acid, like acetic acid, might also be useful given the stability of MIL-53(Fe) in acidic conditions.

- Agitate the solution gently, using a magnetic stirrer or manually shaking it occasionally.

- Check whether the MOF material is easier to remove after soaking. If so, go back to step 1 and try to physically remove it again.

3. **Ultrasonication:**

- If soaking alone is not sufficient, try ultrasonication in a solvent that doesn’t harm Teflon (like water or ethanol).

- Ensure that the Teflon reactor can withstand ultrasonication without damage.

- Periodically check if the MIL-53(Fe) is loosening or coming off and try to remove as much as possible physically.

4. **Chemical Treatment:**

- Considering that MIL-53(Fe) is stable under a range of pH conditions, harsh chemical treatments might not be as effective. However, experimenting with a range of pH (acidic/basic) solutions might be worth trying.

- You might also explore utilizing complexing agents or chelating agents that might bind to the Fe and potentially disrupt the MIL-53(Fe) framework.

5. **Thermal Treatment:**

- Ensure the reactor is completely dry.

- Depending on the thermal stability of Teflon, heating to a moderate temperature might assist in breaking any weak interactions. Ensure that the temperature doesn’t exceed the safe working limit of Teflon (~260°C).

6. **Repeated Procedures:**

- You might need to repeat steps 2-5 several times to incrementally remove the MIL-53(Fe) from the reactor.

7. **Inspection and Final Cleaning:**

- After most of the material is removed, inspect visually and, if possible, utilize a microscope to ensure that all MOF material is removed.

- Perform a final cleaning using a general laboratory detergent, followed by thorough rinsing with deionized water and drying.

### Additional Notes:

- **Safety:** Ensure that any chemicals used do not pose a safety risk and are compatible with Teflon.

- **Material Disposal:** Ensure that any removed MOF material and cleaning solvents are disposed of according to your local disposal guidelines.

Remember, cleaning might sometimes require repeated attempts and a combination of strategies. It's also important to note that it might not always be possible to remove all material without damaging the vessel, especially when dealing with robust and adhesive materials like MIL-53(Fe).

We need canals under the ground with help of not Steel but something better, we could use magnetic materials instead of normal concrete and normal steel.

It can help and support the whole process and reduce freezing

My project is based on new version of concrete which combined with magnets

Dear Ashish Kumar Patel ,

you are right, some aspects such as wavelength (related to atomic numbers) and heating (melting point, thermal conductivity) have to be considered for the choice of the 'optimal' target material.

The most used target material is Cu because of its thermal properties (high intensity output) and machinability (price issue).

Target material with lower atomic number ( Fe, Co, Cr) are used to prevent/reduce fluorescence background due to Fe and similar kinds of elements.

Traget material with higher atomic number (such as for example Mo) are used to extend the XRD pattern with respect to the momentum transfer q ( =4pi/lambda*sin(theta) ); especially for small angle scattering and dealing with amorphous samples.

Best regards

G.M.

Thanks, Manduth Ramchander

This is an old question, and yes I used the inverse cube of the distance in my papers and proposed publishing 2 papers based on this principle:

1-

2- https://ieeexplore.ieee.org/abstract/document/9680681/

Peak at 450 nm is the indication that Fe nanoparticles has been formed. But the other peaks raised may be due to the presence of Oxide in the material (such as FeO).

According to a review and meta-analysis of potential impacts of ocean acidification on marine calcifiers from the Southern Ocean, heavy metal pollution is not a direct cause of defects in CaCO3 crystals from marine calcifiers 1. However, heavy metals can indirectly affect the formation of CaCO3 crystals by altering the pH levels of seawater. Heavy metals can also cause oxidative stress and damage to the cells of marine calcifiers, which can lead to defects in CaCO3 crystals 2.

1: Figuerola, B., Hancock, A. M., Bax, N., Cummings, V. J., Downey, R., Griffiths, H. J., Smith, J., & Stark, J. S. (2021). A Review and Meta-Analysis of Potential Impacts of Ocean Acidification on Marine Calcifiers From the Southern Ocean. Frontiers in Marine Science, 8. https://doi.org/10.3389/fmars.2021.584445

2: Heavy Metal Pollution: Source, Impact, and Remedies. (2011). In Heavy Metals in Water: Presence, Removal and Safety (pp. 1-28). Springer Netherlands. https://doi.org/10.1007/978-94-007-1914-9_1

Learn more:

Hello Yousef,

Thank you for your respond. I will definitly look into the things you mentioned.

For more clarification I also want to mention that, I am measuring oxidation of iron complexs. In this case I want to see some band over 700-800 nm by the addition of oxidant. But in all the case without oxidant also I see some band over approx 760 nm. Even I used different iron complex as starting material I face the same problem and the time trace is going to negative and not a good data.

Is it because of some contamination or somthing I have to play with the volume? I can add some photos herewith.

The reduction of structural Fe(III) in clay materials typically involves the conversion of Fe(III) ions to Fe(II) ions. This reduction process can occur under anaerobic (low oxygen) conditions and is often mediated by microorganisms such as iron-reducing bacteria. The reduction of Fe(III) in clay minerals can have important implications for various geochemical and environmental processes.One common example is the reduction of iron oxides in clay minerals like goethite or hematite to form iron-bearing minerals like magnetite or siderite. This reduction can affect the physical and chemical properties of the clay material and may have environmental consequences, such as altering the mobility of contaminants or influencing nutrient cycling in soils.

Banded Iron Formations (BIFs)

Magnetite Ore Deposits

Hematite Ore Deposits

Hydrothermal Deposits

Magnetite Skarn Deposits

Goethite and Limonite Deposits

Karst-Related Iron Deposits

The association between metformin use and anemia, as described in the review you provided, is an interesting observation.

Long-term metformin use has been associated with a decrease in hemoglobin levels and an increased risk of anemia in some individuals.

It is possible to synthesize graphene oxide (GO) through a modified Hummers' method using biomass as a carbon source and iron(III) oxide as a catalyst in a muffle furnace. The general process involves the oxidation of biomass with strong oxidizing agents like sulfuric acid and potassium permanganate, followed by reduction to obtain GO. Iron(III) oxide can be used as a catalyst in this process. However, the specific conditions and protocols may vary, so it's essential to follow a well-established procedure and ensure safety precautions when working with strong acids and high-temperature furnaces. Additionally, you may need to consult scientific literature or a chemistry expert for precise guidance on this synthesis method.

Estimating the Fe (iron), phytate, and protein content of wheat can be done using various laboratory techniques.

Dear Pastor,

The specific elements to include in the calculation of the Metal Pollution Index (MPI) can vary depending on the objectives of your study, the local environmental regulations, and the available reference values. However, typically, MPI calculations focus on heavy metals or elements known to have adverse environmental and human health effects.

In your list of analyzed elements, elements such as Cd, Pb, Ni, Cr, and As are often included in MPI calculations due to their potential toxicity and environmental significance. These are considered "heavy metals" or "trace elements" that can have adverse impacts when present at elevated concentrations.

Elements like K, Ca, Mg, Fe, Cu, Zn, and Mn are essential nutrients and are generally not included in MPI calculations as they are not typically associated with pollution, unless they are found at extremely high concentrations due to human activities, which is rare.

However, it's essential to refer to specific environmental guidelines, regulations, or the objectives of your study to determine which elements are relevant for your MPI calculation in your particular context. Environmental agencies, such as the U.S. Environmental Protection Agency (EPA) or the European Environmental Agency, often provide guidelines on which elements to consider when assessing environmental pollution. Please refer to these sourcea to have explicit and extensive understanding and to make yourself clear.

Thank you.

EDS, XRF, RBS, SIMS ... can be used for Fe analysis in soda lime glass.

Making use of what Alan F Rawle suggests, there is also a possibility of estimating the concentration in a non-destructive way by measuring turbidity. This will only work at low concentrations because you need light absorbance through the sample solution to be low. In addition, the particles should be in the superparamagnetic range so they won't stick to each other due to ferromagnetic interaction. If these conditions apply, you can build a calibration plot of turbidity vs. iron oxide concentration.

The Government of Canada Health Canada department has produced a very recent factsheet on Zinc compounds and their effects on the human body when they are consumed. I hope this helps. You can access it below:

Syadza Firdausiah

A good catalyst should have a large specific surface area. Therefore, synthesize a catalyst from nanoparticles. You can find synthesis methods on the Internet by typing the words "synthesis of iron nanoparticles".

Thank you very much

Dear Dr Sallam

The formation of a blue-black precipitate when iron(III) is mixed with tannic acid can be attributed to the formation of a complex between the two substances. Iron(III) ions (Fe³⁺) have the ability to form coordination complexes with various ligands, and tannic acid is a polyphenolic compound with multiple functional groups that can serve as ligands. The blue-black color of the precipitate suggests the presence of a specific complex that exhibits this color.

In a low pH environment (pH=2, as you mentioned), tannic acid molecules are likely to be partially or fully protonated, resulting in a higher concentration of positively charged species. These positively charged tannic acid species can interact with the negatively charged iron(III) ions, leading to the formation of coordination complexes.

The exact structure and composition of the complex formed between iron(III) and tannic acid can vary depending on factors such as the molar ratio of the reactants, the specific functional groups on the tannic acid molecules, and the conditions under which the reaction takes place. One possible complex that could contribute to the blue-black color is the iron(III)-tannic acid complex called "iron(III)-tannate" or "ferric tannate."

The blue-black color might arise from the interaction of the complex's structure with light, leading to absorption and reflection of certain wavelengths that result in this particular color perception. The complexity of the formed complex, along with its arrangement and electronic transitions, can contribute to the observed color.

If you're working with these complexes and observing the formation of a blue-black precipitate, it's likely that you are indeed forming a specific iron(III)-tannic acid complex. Characterizing this complex through techniques like spectroscopy (UV-Vis, IR, etc.) and elemental analysis could provide more insight into its structure and properties.

Thank you very much for your answer OK but I want to know formation condition of these mine.

Best wishes

The best type of iron ore deposits that can be reached depends on the mineralogy and geology of the ore deposits. There are four main types of iron ore deposits worked currently, depending on the mineralogy and geology of the ore deposits. These are magnetite, titanomagnetite, massive hematite and pisolitic ironstone deposits.

Tôi cũng đã khử bằng Fe/HCl nhưng thời gian dài, bạn dùng bằng cách nào?@Ganesh Prasad Shenoy

The word "phase" is used in the field of metallurgy to describe a physically homogenous state of matter that has a certain chemical make-up as well as a particular form of atomic bonding and elemental arrangement. Two or more distinct phases may exist simultaneously in an alloy.

The phase change of one solid into two other solids is known as the eutectoid reaction

Eutectoid and precipitation are two of the most typical phase transitions seen with ordinary alloys. Atoms must pass through the metal in order to rearrange themselves and create the new phase or phases in both forms of phase change. Steel contains both cementite (black) and ferrite (white).

Dear Sophia Morley , as was mentioned by Ameer K Ibraheem , there are two methods of X-ray quantitive analysis - standardless and with standards. If you used standardless EDS and WDS (EPMA) with standards, you can safely discard EDS results as less reliable. However, 0.70% and 0.88% are pretty close results for X-ray microanalysis (EDS and WDS). If your aim is to compare both methods, you may want (actually, you must) to take a statistical approach, to acquire results for multiple spots. Theese small differences may be due to non homogeneity of your thin film, surface roughness, variations in thickness, etc.

Ended up spraying/watering and harvesting plants the next day.

So 16h treatment time..

The main difference between the passivation of iron and chromium is that the rust layer on iron (a mixture of iron oxides and hydroxides) is permeable to water and air, while the chromium oxide layer on chromium or alloys containing a sufficient amount of chromium is dense and impermeable. For this reason, under normal conditions, the chromium oxide layer on stainless steel is only a few nanometers, but this is enough to isolate the metal from a corrosive environment (water plus air). On the contrary, a layer of rust grows and grows on iron, but because of its friability, it cannot isolate the metal from the corrosive environment.

At first blush, I would suggest acification and/or vacuum degassing. Sparging with an inert gas is also usually effective in removing active gases like oxygen and carbon dioxide. These should generelly not influence the oxidation state of Fe(II) in solution.

Though of course the ease of this depends on your amount of avalaible sample I would presume.

Doaa Eladl , You need to consider the chemistry of the system, but I found that a good excess of acetic acid works better than most of the traditional buffer systems for some cases of applying nanoparticles of iron..

We prepared nanoferrous fertilizer for seed treatment and it showed better uptake than traditional ferrous sulfate application. Other physiological parameters and seedling vigor were also augmented. Foliar application was not done. I wish to know various biochemical and antioxidative defense responses that were triggered. No particular stress was imposed. which enzymes should preferably be targeted as answer for the effects other than higher iron uptake.

Oxidising agents,these chemicals enhance the oxidation of ferrous iron11 back to ferric ironfe111 by inhibiting its reduction eg,chlorine Cl2,H2O2,KMno4.Chelating agents can bind to ferric iron forming stable complexes ess prone to reduction EDTA,CITRIC ACID,OXALIC ACID.

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