Science topic

Leaching - Science topic

Leaching is the process of extracting minerals from a solid by dissolving them in a liquid.
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Hi.
I have leaching solution with Ca ion. When I use NaOH, Ca(OH)2 is precipitated. Is there any way to make pH 1 to 7 without precipitate?
Thanks for read.
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you can deploy copilot To adjust the pH of a leaching solution containing calcium ions (Ca²⁺) from 1 to 7 without causing the precipitation of calcium hydroxide (Ca(OH)₂), you can consider the following approaches:
### 1. Use a Buffer Solution
Buffer solutions can help maintain a stable pH without causing precipitation. A suitable buffer system for your pH range could be a combination of a weak acid and its conjugate base, such as acetic acid (CH₃COOH) and sodium acetate (CH₃COONa). This buffer system can help control the pH without introducing hydroxide ions (OH⁻) that would precipitate Ca(OH)₂.
### 2. Gradual pH Adjustment
Instead of adding NaOH directly, you can gradually adjust the pH using a weaker base, such as sodium bicarbonate (NaHCO₃). Sodium bicarbonate will react with the acidic solution to form carbonic acid (H₂CO₃), which then decomposes into water (H₂O) and carbon dioxide (CO₂). This process helps to avoid the rapid increase in pH that causes Ca(OH)₂ precipitation.
### 3. Chelating Agents
Chelating agents, such as ethylenediaminetetraacetic acid (EDTA), can bind to calcium ions and prevent them from forming insoluble compounds. By adding a chelating agent to your solution, you can keep the calcium ions in solution while adjusting the pH.
### 4. Controlled Addition of Acid and Base
You can use a combination of a weak acid (e.g., acetic acid) and a weak base (e.g., ammonium hydroxide) to gradually adjust the pH. This method allows for more controlled pH adjustment without causing rapid changes that lead to precipitation.
### References
For more detailed information on preventing calcium hydroxide precipitation, you can refer to the following sources:
- [Calcination-free production of calcium hydroxide](https://pubs.rsc.org/en/content/articlehtml/2021/ra/d0ra08449b)
Good luck
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I got leached solution of rare earth metals (La, Ce, Sm, Nd, Pr) and other metals with calcium chloride in the leached solution after dissolution of Phosphogypsum. I want to selectively recover all the rare earth metals from its solution in high purity economically. Please suggest me a best method to recover it.
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A combination of precipitation and SX methods. Use a suitable precipitant to remove calcium first, followed by SX (D2EHPA or Cyanex 932).
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Hi,
I have a leach solution with Li present as LiOH. I did lime water leaching of material but also leached impurities such as Zn, Cr and Al with it. The pH of the solution is around 11. Now I want to remove the impurities and the literature suggests using ion exchange resins to remove them. The ion exchange resins would require pH adjustment to around 6-7 which might also alter the chemistry of dissolved LiOH, and I do not want that. So how should I proceed? Is there any other way I should explore to remove those impurities?
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Ph 6-7 will not affect LiOH. That is by definition.
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What is the method of measuring sulfur for minerals such as metal oxide or molybdenum oxide through Leco furnace (or similar furnaces) at different temperatures, times and weights after leaching and after cleaning by titration method (gravimetry)?
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X-ray fluorescence (XRF) and combustion methods for SO₂ detection are recommended for measuring sulfur in molybdenum oxide due to their efficiency and accuracy. The choice of method may depend on available equipment, detection limits, and sample characteristics.
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I want to know the sample preparation techniques for the leaching study.
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To conduct a leaching study for microwave plasma atomic emission spectroscopy (MP-AES), prepare samples by acid-washing containers, adding the sample and leaching solution, and heating in a microwave to extract analytes. After cooling, transfer the leachate, dilute it appropriately, and analyze it using MP-AES, ensuring proper calibration and blank corrections for accurate results.
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I'm trying to stain areas of dystrophic calcification in sections of FFPE perinatal brain tissue. Typical basophilic appearance on H&E but nothing with Alizarin Red (costochondral junction positive control works well). Tissue has been fixed in formalin with added glacial acetic acid. Is this likely to leach out the calcium resulting in a negative Alizarin Red, even though the material remains basophilic? I'm waiting for the von Kossa stain...and if the calcium IS leached out.. what's the basophilic material??
Thanks
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yes.it used for osteogenesis and live/dead cells
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Hello. I conducted batch leaching tests with samples of construction and demolition waste with adhered paints to assess the influence of the paint on the release of contaminants in the leachate. I observed that in all samples with water-based enamel paints, the pH of the leachate was significantly lower compared to the samples painted with acrylic paints. What could explain this decrease in pH?
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Water-Based Enamel Paints typically contain alkyd resins, which are modified with fatty acids and other organic components. During the leaching process, these components can hydrolyze and release organic acids into the leachate, thereby lowering the pH. Alkyd resins, when exposed to water, tend to break down into smaller organic acids such as acetic acid and formic acid, which are weak acids but sufficient to reduce the pH of the leachate....in other words: The fatty acids released during hydrolysis are weak acids, such as acetic acid (CH3COOH) and formic acid (HCOOH). These acids dissociate in water, releasing hydrogen ions (H+), which lower the pH of the leachate....
And the difference with Acrylic paints are... They are composed primarily of acrylic resins, which are more stable and less prone to hydrolysis compared to alkyd resins. Acrylic resins form a stable polymer network that does not readily degrade in water, leading to a less acidic leachate. The additives in acrylic paints, such as surfactants and coalescing agents, are typically neutral or slightly alkaline, which can help to maintain a higher pH.
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Unlike geopolymer cement, the AAM cement produced with sodium silicate/hydroxide will leach out the alkali Na+. Based on Davidovits' explanation, geopolymer cement will not leach out the sodium because Na+ was trapped inside the chain (the attached picture represents the K+ trapped inside the chain, the same thing with Na+).
Suppose the efflorescence can be tackled and no sodium leached. Can we classify the AAM cement was having a 3D structural model chemical that traps the Na+ or K+ and becomes the geopolymer cement?
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Idham Kholid Rahmatullah to answer quickly at your question…NO!
Professor Davidovits has explained the reasons of that reaction. Geopolymerization doesn’t happen casually or because has been found a trick to block the efflorescence, but following precise mix design, that is practically the same using all different types of precursors and reagents. Reagent isn’t an activator because what is already well reactive is the powder part, so the pH is user friendly (I can send you videos where I put my fingers inside without gloves with no issues or burning). Don’t try to put your finger inside an activator for AAM, take care.
It isn’t a question of description but GP and Alkali Activation follow different ways. The leaching happens because for AAM the real ”glue” that keeps all together is the strong pH obtained by corrosive liquids or by metasilicate plus water (the result is still a corrosive pH of 14 or even 14+ if activators are used in higher quantity). The alkaline ions are over saturated and don’t react with nothing a part the CO2 in the air so migration and carbonation are normal consequences. The issue in this case is that sodium or potassium carbonates are salts not minerals like the Calcium carbonate that grows on the surface of Portland based recipes…so their solubility in water is total while for calcium carbonate is still very low.
Geopolymers has very thin carbonation because the reaction, between precursor and reagent to create the final GP binder, is well balanced so there aren’t free alkali that can move to the surface to become carbonates.
Check on YouTube there are already the videos where Prof Davidovits explains these and much other aspects.
Best
Alex
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A lot of scientific papers state that BPA can "leach" from polycarbonate plastics, but what does that actually mean?
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BPA It is not a plasticizer, however when traces are present as free monomer in polycarbonates or epoxy resins, it can migrate (leaches) to the surface by dissolution in solvents or mobility due to high temperature. For example the degree to which BPA leaches from polycarbonate bottles into liquid may depend more on the temperature of the liquid or bottle, than the age of the container.
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In the pore water of a long-cultivated paddy soil with high CEC (smectitic clay dominance), high organic matter and a clay pan (physical constraint) below 15 cm depth, can the total anion equivalent be greater than the total cation equivalent? The soil has been fertilized with KCl (twice a year) and ZnSO4.7H2O (once every two years) for the last 33 years.
The dominant ions in the pore water of the given soil are Chloride>bicarbonate>sulphate>calcium>magnesium>other cations
and
the total anion equivalent>>total cation equivalent.
I am hypothesising that:
1. The clay pan is inhibiting the easily migrating chloride and sulphate ions from getting leached out of the surface soil.
2. The high CEC is causing negative adsorption of anions and, at the same time, keeping the cations from going to the soil solution to maintain charge balance.
Do my hypotheses make sense? Is there any study to substantiate my findings?
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Once you have extracted the pore water from the soil, the total equivalent of anions must be equal to total equivalent of cations in that extracted pore water, irrespective of the properties of the soil from which you have extracted it, period.
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I have followed a procedure to find out WHC of some sieved soil. I have also got the moisture % content of the soil. From this I have calculations that tell me exactly how much water to add to reach 60% WHC. However, after added this amount of water I can see the water leaching through the mesh bottom, suggesting that its beyond 60%
My question is, should 60% WHC happen instantly, or should I wait a certain period of time for the water to be absorbed?
As I need to weigh the wetted soil and maintain that weight. However, columns initially wetted weight more than the next day so I'm not sure which is the true WHC.
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Can you told me how to get 60%
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Imagine you have a field with excessive salt buildup. Assume the volumetric water content is 0.35 cm3 cm-3 and the root zone is 120 cm deep.
If the soil in the field is a clay loam soil with Ks= 5.5 cm per day, b = 5.2, and saturated water content (Theta)=0.5 cm3 cm-3, the hydraulic conductivity followed Campbell’s model, and the flow was under unit gradient conditions (i.e. negligible matric potential gradient), then how long would it take to leach out the salts?
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The leaching process duration can be estimated using the leaching requirement formula:
t = H/K
where:
- T is the leaching time,
- H is the leaching requirement (difference between initial and desired salt content), and
- K is the hydraulic conductivity.
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Adding lime in the process, apart from the formation of calcium sulfate compound in the neutralization stage with sulfuric acid,if have the negative effect on the precipitation process of metals from the leach solution?
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Dear Peyman Hassanpour Please do recommend my answer
Lime (calcium oxide, CaO) and caustic soda (sodium hydroxide, NaOH) are commonly used alkaline reagents in cyanide leaching operations, particularly in gold and silver mining. Both reagents serve to increase the pH of the leach solution, creating a favorable environment for the dissolution of precious metals. However, there are differences in their performance and considerations for their use:
### Lime (Calcium Oxide, CaO):
1. **Alkalinity Source:**
- Lime provides alkalinity to the leach solution by reacting with water to form hydroxide ions (OH⁻). This increase in pH facilitates the dissolution of gold and silver.
2. **Carbonate Formation:**
- Lime may contribute to the formation of carbonate ions (CO₃²⁻) in the leach solution, especially if carbon dioxide is present. Carbonate formation can affect the stability of the solution.
3. **Slaking Process:**
- Lime is typically added as a slurry (slaked lime or milk of lime), and the slaking process is essential to ensure proper dispersion and reactivity.
4. **Cost-Effective:**
- Lime is often considered more cost-effective than caustic soda, making it a preferred choice in many cyanide leaching operations.
5. **Precipitation of Impurities:**
- Lime can assist in the precipitation of certain impurities, such as heavy metals, which may be present in the ore or formed during leaching.
### Caustic Soda (Sodium Hydroxide, NaOH):
1. **Alkalinity Source:**
- Caustic soda provides alkalinity by dissociating into hydroxide ions (OH⁻) in solution. It directly contributes to the increase in pH.
2. **No Carbonate Formation:**
- Unlike lime, caustic soda does not contribute to carbonate formation, which can be advantageous for maintaining a stable leach solution.
3. **Ease of Handling:**
- Caustic soda is a liquid and is generally easier to handle and feed compared to lime, which is often delivered in the form of dry powder or slurry.
4. **pH Control:**
- Caustic soda allows for more precise control over pH due to its direct contribution of hydroxide ions without the complicating factor of carbonate formation.
5. **No Slaking Process:**
- Unlike lime, caustic soda does not require a slaking process, simplifying the handling and addition process.
### Considerations:
1. **Cost:**
- Lime is typically more cost-effective than caustic soda, which may influence the choice of reagent based on economic considerations.
2. **Solution Stability:**
- Caustic soda may offer better solution stability by avoiding carbonate formation, which can lead to precipitation and scale formation.
3. **Impurity Precipitation:**
- Lime may be preferred if impurity precipitation is desirable, but this needs to be balanced against potential carbonate-related challenges.
4. **Handling and Safety:**
- Caustic soda, being a liquid, may have advantages in terms of ease of handling and safety compared to lime dust.
Ultimately, the choice between lime and caustic soda depends on factors such as cost, solution stability, impurity precipitation requirements, and ease of handling based on the specific conditions and goals of the cyanide leaching operation. It is essential to consider the specific characteristics of the ore, the desired leaching conditions, and economic factors when selecting the alkaline reagent.
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We have leached ashes of some plant samples to determine the Ni concentration in the leachate using sulfuric acid. In our method, we have used two concentrations of sulfuric acid (1M and 5M) and three pulp densities (10g/L, 100 g/L and 200 g/L). However, I observed a white precipitate in the filtered samples of the with leachate 5M sulfuric acid, after few days. I tried adding few drops of conc. HCl to dissolve it, but it did not disappear.
What could have caused the formation of this precipitate? Is there any method to prevent it?
I really appreciate your valuable suggestions to improve this.
Thank you
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It could be a number of things depending on the type of plants the ash came from.
Some plants accumulate a significant amount of silicon which will precipitate as silica from sulphuric acid.
It could also be from calcium which precipitates as calcium sulphate. This is the more likely cause.
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If we have a leaching solution containing a mixture of heavy metals in a wide range of concentrations (for example, we have some heavy metals in solution in 10 - 100 mg/L concentration range while some others are in 100 - 1000 mg/L concentration range) what would be the best ICP standard concentration range to prepare for ICP-OES analysis of this solution?
Thanks in advance for sharing your experience.
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The range of ICP standards for ICP-OES analysis of a leaching solution depends on the specific elements being analyzed and their expected concentration levels. It is crucial to select ICP standards that cover the expected range to ensure accurate results. These standards should be sensitive enough to detect and quantify the target elements accurately, but they should not exceed the upper limit of the instrument's linear dynamic range to prevent signal saturation. The suitable concentration range for ICP standards can vary depending on the sample matrix and the elements being analyzed.
Major elements such as sodium, potassium, calcium, and magnesium typically require standards in the tens to hundreds of parts per million (ppm) range. On the other hand, trace elements like copper, lead, zinc, and arsenic may require lower concentration standards, often in the parts per billion (ppb) or even parts per trillion (ppt) levels.
To determine the appropriate range of ICP standards for your leaching solution, it is essential to have knowledge of the elements of interest and their expected concentration levels. This information can be obtained from previous characterization studies or existing literature on the leaching process. By considering the expected concentration range, you can select suitable ICP standards that cover low, medium, and high levels of the elements under investigation.
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the treatment carried out on ilmenite (from industry) where apart from the Fe2TiO3 content there is a lot of FeO content as an impurity material, what must be done to the ilmenite to separate it from the impurities before roasting and leaching so as not to interfere with the roasting and leaching process?
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If the iron in the raw material is in the form of magnetite, magnetic separation can be used for its preliminary separation.
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Hello everyone,
I am conducting an isotherm/kinetics experiment to measure the capacity of a concrete filter/pervious concrete (a filter made of concrete) to remove heavy metals.
My question is, how can I measure how the percentage of the heavy metals removed is due to chemical precipitation and how much is due to the adsorption of heavy metals to the concrete filter?
Please take a look at the picture attached to see the concrete filter.
Please consider the following conditions:
The filter leaches Ca and carbonate, so precipitation happens.
The pH is constant at 12, and I cannot change it.
The adsorbent is in a filter stape as attached and is not in powder form. So, a part of precipitated heavy metal ions are trapped inside of the filter.
The picture has been extracted from Holmes et al. 2017 (Enhancing the Ability of Pervious Concrete to Remove Heavy Metals from Stormwater).
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I should also add that the application of pervious concrete is in the pavement. however, the isotherm study is done in a small jar, and the concrete is submerged in the contaminated water for a specific period of time while the water is stirredcontinuously.
For more information, you can read the following article written by John T Kevern.
Title: Enhancing the Ability of Pervious Concrete to Remove Heavy Metals from Stormwater
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I did a leaching experiment to recover Lithium and Cobalt from wasted LIBs.
I need help in two parts I do not know what to do next.
(Element composition test) I dissolved 10 grams of my raw material (LiCoO2) in 200 ml aqua regia, then I dilluted it 1/100 in a volumetric flask. All this to find the element composition of my raw material (LiCoO2).
(Sample 1) I leached 1 gram of LiCoO2 in a mixtured of 3 grams acetic acid, 0.7 grams ascorbic acid, and 100 ml DI water. Then I dilluted the leachate solution in 1/100 volumetric flask.
Both solution I ran them in ICP-MS, I got the results but I do not know which data to use to calculate the element composition, and the leaching efficiency % of Li and Co of my sample 1.
Please I need all the possible help!
Can somebody explain to me how to calculate these things, and which value I need to use from the ICP-MS data.
Thank you!!
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Dear Marvin
To calculate the leaching efficiency, take a look at the following research paper. I Hope it will be useful for you.
""Reductive leaching of zinc, cobalt and manganese from zinc plant residue""
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I see a number of researchers investigate the bioleaching of WEEE and EV batteries usually citing it as an environmentally friendly option. What are the real advantages of bioleaching of WEEE? With ore, there are low-grade ores and crushed ore can be leached in heaps or dumps. As far as I know there are no classifications of low-grade WEEE. All studies that I have seen conduct experiments on powdered WEEE and of course the black mass from EV batteries is fine, hence heaps or dumps cannot be used. A number of those studies use, in my opinion, operational parameters that are not feasible such as S/L ratios of 1%, and extraction times of 6-40 days. If the material is not low grade or processed in heaps, the opex cannot be offset. Although current processes for EV batteries use acids like HCl and H2SO4, are there not methods to regenerate and re-use those acids hence reducing the environmental foot print?
Curious to read your thoughts.
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Bioleaching of WEE viability and sustainability depends on several factors: most importantly: the bioreagent that microbes produce, its concentration, pulp density and time of the process. generally, microbes are able to leach metals with much lower acid concentrations than similar chemical processes due to their fascinating live continuous factory which produces more than 200 chemical compounds, all of which can contribute to the dissolution of metals. What has been the challenge for decades for bioleaching is slow kinetic but recently researchers have found a solution that is using fast-growing bacteria that can produce organic acids, the good thing about these types of bacteria is that we already have developed biomanufacturing processes with these bacteria so adoption of technology for bioleaching will not be that hard, also the time of the process significantly reduces, LCA and TEA studies have shown that these type of bacteria that we call it heterotrophs can provide the lowest environmental impact and highest profit margin compared to all currently metal extraction methods,
here is a great reference:
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Describe the potential co-benefits and drawbacks of biochar application in agriculture, such as improved soil fertility, reduced nutrient leaching, and alterations in crop yields, using evidence from field research.
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Bonsoir!
Le biochar ou ce qui peut l’être améliore la dite production végétale.
  • On peut comprendre que tout cela dépend bien entendu de la fertilité des sols (substrats nourriciers),
  • A partir de cette donne il est utile de connaitre les éléments fertilisants principaux (Azote N, phosphore P et potasse K) et secondaires oligo-éléments (Magnésium Mg, Calcium Ca, Sulfates SO4 2(-), ...),
  • En agriculture cela est connu par une grande partie des agriculteurs, mais parfois les apports ne sont pas tout à fait respectés, ce qui entraîne des problèmes liés à la nutrition.
  • L'eau où sont dissous les éléments est à prendre en considération au niveau qualitatif (absence de salinité, d'éléments polluants, etc...).
  • Maintenant il s'agit de mieux apréhender on peut dire les expérimentations conduites en plein champ et au laboratoire afin de répondre ou tenter de répondre aux problématiques, quelle tache!
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I purified my protein of interest using Ni-NTA chromatography. The protein was eluted but it eluted with a yellowish brown color which I have experienced before. I believe it was due to excess DTT (buffer mismatch) which led to leaching of Ni with my eluted protein.
Any ideas as to how to remedy this and remove the color (and Ni) without compromising the integrity of the protein.
Thank you.
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1 mM dtt should be enough to reduce disulfide bonds (or prevent their formation). Higher concentrations will reduce the Ni ions. It is easier to decrease dtt conc before running imac. Moreover some Zn particles will start clogging the adsorbent pores.
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We can use EDX to measure the silver concentration before and after leaching test to know amount of silver leached. However, the concentration of leached silver from membrane is measured using ug/L or mg/L with the aid of ICP-MS. How to measure the silver concentration before leaching test of membrane using ug/L or mg/L unit?
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X-ray photoelectron spectroscopy (XPS) is a surface chemical analysis technique that can be used in the elemental analysis of silver.
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I did digestion of fly ash by HCl. Is it possible to evaporate HCl from filtrate? We don't have facility for evaporation of HCl by oven. Is there any chemical method?
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After acid leaching of fly ash using HCl, it is indeed possible to evaporate HCl from the filtrate. However, if you don't have access to an oven for evaporation, there are alternative chemical methods that can be employed. One common method is to use a chemical reaction to convert the HCl into a less volatile compound. For example, you can react the HCl with a base such as sodium hydroxide (NaOH) or calcium hydroxide (Ca(OH)2) to form a salt, such as sodium chloride (NaCl) or calcium chloride (CaCl2). This reaction will neutralize the acid and eliminate the need for evaporation. To carry out this method, you can add a stoichiometric amount of the base (NaOH or Ca(OH)2) to the filtrate containing HCl. The reaction will produce the corresponding salt and water. After the reaction is complete, you can separate the resulting salt from the solution by filtration or other appropriate methods. It is important to note that the specific details of the reaction, including the amount of base required, should be determined based on the concentration of HCl in the filtrate and the stoichiometry of the reaction. Additionally, proper safety precautions should be followed when working with corrosive substances such as HCl. If you require further guidance on the specific chemical method to employ in your situation, it is recommended to consult with a qualified chemist or chemical engineer who can provide more detailed advice tailored to your experimental setup.
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Increased costs as well as increased awareness of the impact of fertilizer leaching on the environment have increased interest in use of controlled release fertilizer to increase the nutrient uptake efficiency and reduced the nutrient leaching potential. The application cost of fertilizer also reduced considerably.
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CRFs can help improve N synchrony only under specific soil, crop, and climatic conditions and their high cost can prove a barrier to their widespread use. There is a need to explore combining CRFs with knowledge-based site-specific fertilizer management strategies to achieve high yields and high N use efficiency through improved N synchrony. Controlled-release coatings currently in use have been designed based on the predicted crop N demand. These are neither able to respond to the N needs of the crop plants in real-time nor take into account microbial interactions in the soil-plant systems. New economical CRFs are already being designed using enzyme inhibitors with modifiable chemical structures and biodegradable coatings that respond to plant rhizosphere signaling molecules.
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I am doing some leaching experiments now on metal-bearing wastes using citric acid as lixiviant. The metals of interest are REE, Co, Mo and V. Is there any specific method for each of them to be precipitated from organic (citrate) PLS? Or are the standard methods (e.g. precipitation of V using ammonia solutions) suitable for organic PLS?
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I am trying to see if my water filtration membrane is leaching during filtration
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Dear all, please have a look at the following free access paper. My Regards
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Three Central Northwest Coast wet sites have begun to highlight the significance of berries and nuts, particularly salal and acorns, to ancient subsistence practices (Figure 1). At the Ozette site (45CA24), located on the Olympic Peninsula of Washington, mudslide-encased houses and middens dating to 300-450 years ago produced flotation samples of 250,000 seeds of Salal (Gaultheria shallon; and/or its close look-alikes of genus Vaccinium). At the Sunken Village site (35MU4), located on Sauvie Island, Oregon, over 100 hemlock-lined acorn leaching pits dated to 150-700 years ago have been recorded. It is estimated that these leaching pits may represent processing of 2,500,000 acorns (Quercus garryana) in a season. Finally, at the QwuɁgwǝs site (45TN240), located at Mud Bay on Eld Inlet, Olympia, Washington, reanalysis of macrobotanical artifacts lead to the recognition that acorns were also abundant in the wet site midden. Acorn remains were seven times more common than hazelnut (Corylus cornuta) remains here, indicating that acorns might have been the most ubiquitous plant food at this south Salish Sea site. In this article it's argued that salal and acorn ecofacts from the Central Northwest Coast represent substantial ancient resources in the diets of this region.
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As a Northwest Coast wet sites archaeologist, I am always impressed how these sites open so many avenues of research. I should not be surprised since as much as 90% of the cultural materials, including plant ecofacts, are preserved in these wet sites. Hopefully, though I'm not a paleoethnobotanist, this essay properly covers what Northwest Coast wet sites are beginning to reveal. Please comment on any errors since may still be time to make corrections before the actual publication release. Thanks, Dale
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I want to prepare quantum dot material and add it to a hydrogel, has anyone faced the leaching problem or studied it?
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The stability and retention of quantum dots in hydrogels can be affected by various factors, including the size, surface chemistry, and concentration of the quantum dots, as well as the properties of the hydrogel itself. In some cases, quantum dots can leach out of the hydrogel, which may limit their effectiveness as a drug delivery system or other application.
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Can a particular type of stainless steel be recommended that will not leach magnesium?
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Any traces of magnesium or calcium at the surface of the steel would very likely leach quickly. You might be able to pre-treat it to leach them away beforehand but I'm not an expert in this area.
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none
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Dear Sameeha,
Using dried and preserved plant samples that are almost a year old for macronutrient analysis may not be ideal, as the nutrients in pieces may have degraded over time. Macronutrients, such as nitrogen, phosphorus, and potassium, are essential for plant growth and development. Their levels can change over time due to various factors, such as exposure to light, temperature, and humidity.
The preservation method used for the samples can also affect the nutrient content. Drying and grinding samples can help to preserve the pieces and maintain their nutrient content, but it is still possible that some nutrients may have leached out over time.
It's worth noting that the best practice for plant macronutrient analysis is to use fresh samples, which are collected and analyzed as quickly as possible. However, suppose dried-preserved samples are the only option. In that case, it's recommended to consult with the lab to check their capabilities on the analysis of old samples and also to compare the results with fresh samples.
I hope this explanation was helpful,
Edgar M Cambaza
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I have some flyash and want to leach out Al2O3 and SiO2 using NaOH. IS there any additive which can help me to improve rate of leaching or dissolution .
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Under some circumstances there are a few organic acid ions such as oxalate, glycolate that marginally assist in silicate leaching but I am not sure if they would work in your case. However, if you find nothing else, they might be worth investigating.
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Does this soil will suffer from potassium deficiency soon or it will still be rich in K for much longer? It's clay soil so will the K be leached into the soil because it's high in the solution.
Should we recommend further k application even if it will be small amount or should not.
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Rainwater will leach away the soluble K over time, maybe in a single season or two. Soluble K was around 10% of the total K content. So even after the depletion of soluble K, around 4000 ml/Kg will remain in the soil. Now the further application of K will depend on the techno-economic feasibility of the process being applied to extract K from the source.
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Subject suggestion PhD Thesis
In the field of extracting new and updated manganese dioxide nanoparticles
Innovation in the leaching stage
instantaneous
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The question of leaching comes when the NPs are employed in the surface coating. Perhaps they can be coated on mild steel to prevent corrosion by mixing with a polymeric material such as polyuretane.
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Greetings,
I am an undergraduate BS chemistry student who is working on a slow-release nano fertilizer, how should I treat my leached samples for each time interval; that is do I employ the Kjeldahl method for each leached sample?
Thank you
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Thank you Sir.
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Rock in chemical solution will appear chemical damage, this damage is a kind of water-rock interaction, so we can expect rock mechanical properties cracking, what else can we pay attention to?
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Thank you for your reply. In fact, I once studied the dissolution process of rock minerals in the process of acid leaching, and observed the rock morphology after the acid leaching process by scanning electron microscope. I'm actually curious about the formation of rock cracks https://www.researchgate.net/profile/Blessing-Taiwo-5during acid leaching.@
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we have an aerated heap with sensing temperature. Shockingly, the part with aeration pipes records very lower temperatures (21-34 C) in comparison with the parts with no aeration pipes (56 C).
What are the probable reasons from operational and scientific viewpoints?
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Presumably (you didnt say) the aeration pipes are at the bottom of the heap. Hot air rises and usually the bilogical activity creates heat, therefore the air rising through the heap gets hotter. The oxygen from the air is required for the bugs to be active to create the heat in the heap so there is some practical limitations, but the air flow is also required to cool the highly active zones as the bugs like a temperature window and die if too hot and go dormant or slow down if too cold.
If the air ingress into the heap is not forced (by a fan or compressor) then the temperature of the inlet air will be the atmospheric temperature at the inlet and the air will reach equilibrium in the heap.
If mechanically forced into the heap, there will be some heat gain from the mechanical fan or compressor and then inside the heap it will attain equilibrium, again by heating or cooling the surroundings.
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Hello All,
I am currently working on the research topic, "Metals recovery from Jarosite and Jarofix". The study will entail performing experiments using the acid and water leaching approach for the recovery of metals. I intend to focus on just Zn and Cu. I have reviewed some literature however I have not found a clear algorithm for the process and necessary parameters like temperature etc to be used in the process. I would appreciate if anyone with insight on this could explain it to me or render any form of help.
Thank you.
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hello All, Please I am currently working on the material and methods of the recovery Of Jarosite. i am suppose to use the acid leaching and water leaching technique. during my risk assessment, inwas told the temperatures needed are too high and this has made my risk assessmen to continue to get disapproved. i really need some help with the methodology for this work. I have limited time and the reviews I have read through all use high temperatures are some point. either for roasting or pretreatment. i was told that HCL even tho mixed with the sample is hazardous to heat up and will evaporate. it will also produce flammable gases. Can anyone suggest journalsnor technique that will give me better understanding of the techniques I need to use. The heating equipments mentioned Include the Bunsen heater,microwave and hot plate. The hot plate can only heat to 100oC and I need a higher temperature at some point. this is urgent please .
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knowing that the acid concentration and the temperature are optimal.
Increasing the reaction temperature from ambient to 80°C increased the leaching yield
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Dear Fatima
Stirring speed is a key parameter which affects nearly all chemical or electrochemical leaching reactions. It is worth noting that depending on the leaching material and other parameters, increasing the stirring rate can affect the leaching kinetics in different ways. For instance, in some cases increasing the stirring rate can decrease the thickness of boundary layer and consequently, it promotes the diffusion and increases the reaction rate. On other other hand, when a certain reaction is to be considered as chemically reaction-controlled, an increase in the stirring speed will not change the reaction rate. For more details, our recent review paper is highly recommended.
"Kinetics of leaching: a review", 2020.
Best of luck
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After IMAC1, the protein in the elution has some Ni leached out from the Ni column. The elution fraction seem to be brown in colour.
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Reduce pH of your solution or coat your Ni column with a Teflon
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I need to know the complete calculation how much mol percentage of palladium is left after recycling my catalyst do that I can understand how much metal has leached from the prepared catslyst
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ICP AES gives the concent of Pd in the catalyst, which is a absolute content value. (0.658-0.358)/0.658*100% of Pd was leaching.
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Jadeite itself is an anhydrous mineral. However, the secondary action it undergoes, the leaching of limonite will change the appearance of jadeite, can the infrared spectrum be used to indicate its water content? If so, which wavelength data can be used to characterize it?
Thanks for your answers
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I'm not expert of this materials, but if you have the chance to acquire more than one spectra before and after a specific treatment (e.g. limonite leaching), you can check the region between 1700-1600 cm-1 (around 1630 cm-1) which is related to the bending mode of water (check the presence of some cut-off in that region) and run a mathematical difference of spectra. If the peak/band around 1630 cm-1 increses than water content is increasing. You can also check the OH region beyond 3000 cm-1. To be sure about the presence of water you could perform some experiment using D2O but it would be more complicated).
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Gender representation in numerous school textbooks across diverse societies has been studied and discussed since the 1970s. A substantial number of these studies stated that gender bias in textbooks (GBIT) is quite stubborn and practically a barrier in the way of gender inequality (Ullah & Haque, 2016). In particular, in textbooks of Social Studies, the construction of gender is solely stereotypical (Jabeen, Choudry, Omar, 2014). Hameed (2012) in his study on gendered based English textbooks found that in shaping up ideas of the children and for encouraging optimist gender roles in children, textbooks play a decisive role and can be a valuable tool. Further, Jabeen and Illyas (2012) emphasize that characters in (learning resources (textbooks) play a significant part in children. Characters influence children's choices concerning to what type of being they want to become (Jabeen & Illyas, 2012).
Unterhalter and North (2010) therefore argue that to achieve gender equality through education, the concerns of men and women would be considered as integral parts monitoring, designing, evaluating policies programs in all social, political, and socio-economical domains to provide equal benefit for men and women and to not perpetuate inequality. Emphasizing on efficiency approach of Gender and Development (GAD), Cornwall (2000) also mentioned that men as oppressors and women as a victim of gender inequalities is a simplification of reality. So, there is a need to view gender, not as a unilateral issue of women but it should also be considered in terms of power relations and powerlessness where men and women may be dis-empowered and vulnerable (as cited in Gender analysis framework of Leach, 2003, pp.10-11).
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There is need to relook at the true meaning of gender-neutral laws on sexual harassment which should aim at protecting both men and women against sexual harassment in work settings. An enabling environment for prompt reporting and quick redressal with an unbiased investigation and a well laid out counselling system to ensure safety, as well as emotional and mental support to the victims, are important preventive strategies. These measures may help address the problem of hesitancy &/or other reasons for non-reporting. It is also pertinent to offer the accused a fair opportunity to defend, as there may be instances of false allegations
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Noted. Thank You everyone
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I do agree with Matthew F. Gladfelter.
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A student is installing a field trial that we expect to largely impact soil moisture and temperature, and we simultaneously want to measure the secondary impacts on N-mineralization in the field. What are the best methods for doing this. I've seen methods of installing closed bags of soil, but that will only react to temperature, not the soil moisture. We could measure total and inorganic N at the start and after the experiment, but there could potentially be differences in leaching losses that are not accounted for. Suggestions would be most welcome!
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Nitrogen (N) is among the vital elements needed for the survival of living things. It being an abundant common element on earth, it forms approximately 78% in the earth's atmosphere. Nitrogen is chemically reacted with other compounds such as ammonia, nitric acid, organic nitrates and cyanides to form unique compounds with totally different chemical and physical properties. Since plants cannot use or take nitrogen directly from the atmosphere, uptake is through nitrogen forms that include ammonium and nitrate.
Majorly N-mineralization in field experiments can be measured by adopting the three different methods:
In situ cylinder incubation: In this method Galvanized iron tubes (13 cm diameter, 65 cm long) were set up on each site in the middle of the inter row a few days after sowing the crop. At harvest, soil samples were collected from the 0–20 cm, 20–40 cm and 40–60 cm layers of each tube for inorganic N determination. The amounts of N mineralized from soil organic matter were estimated.
Incubation tests: In this method Soil samples of about 30 kg were collected for the incubation tests. They were taken from the 0–20 cm layer at four places on the different sites each year before the beginning of the field experiment and kept at 5 °C until laboratory incubation and then we estimated mineralized N in the sample. Incubation tests are divided into two types:
i. Incubation test at 20 °C: 1.2 kg of the fresh soil sample, previously homogenized by hand, was put in a PVC jar (11.2 cm diameter, 13.0 cm length). In order to maintain soil moisture at 90% of water content at 0.1 MPa matrix suction, the jars were weighed regularly and the lost water was made up. The soil water content remained above 80% of the moisture at 0.1 MPa matrix suction during the experiment. After approximately 25, 120 and 200 days of incubation, the soil in one jar was removed for NO3 –-N and NH4 +-N determination;
ii. Outdoor incubation test: In this method Three kilograms of fresh soil were homogenized by hand and placed in 30 cm long PVC jars installed upright in the soil. The soil moisture was maintained between 80 and 90% of the water content at 0.1 MPa matrix suction by weighing the jars every week and then we estimated mineralized-N in sample.
Analytical procedures: NO3 –-N and NH4 +-N in soil was extracted with 1.0 mol·L-1 KCl (soil/extracting ratio: 1/2) and determined by colorimetric using a technic on an autoanalyzer. Soil and plant total N was measured by the Kjeldahl method followed by colorimetric NH4 + N analysis. 15N excess of total N was measured at the Laon Agronomy Station using a mass spectrometer (VG SIRA 9) linked to a CN analyzer (NA 1500 Fisons Instruments). The 15N excess of inorganic soil N was determined on NH4+ collected in 0.05 mol·L-1 H2SO4 after reduction and steam distillation of the KCl extract.
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Hi, I found that when I use MgO or Mg(OH)2 for catalysis in water, the leaching of Mg is serve. Is there any method to suppress the Mg leaching, like change the reaction solvent etc? Thank you!
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MgO will ultimately form Brucite (Mg(OH)2) in water. It starts as a magnesia MgO particle, which forms a hydroxide shell. The shell eventually goes to a more crystalline, less reactive state. Normally, in the hydrometallurgical use of MgO, that's the last thing you want! But if you're happy with synthetic brucite and are using it in alkaline or near-alkaline water, then soaking the MgO in fresh water for (say) 6 hours (keep it in suspension if you want to retain the particulate nature) then you should have something like it. You will get minor Mg solubility, but maybe it will be OK for your application. Good luck! Mike
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Many research has been done on the use of Chitosan as an adsorbent material. When I was studying the material, I noticed that it was leaching organics when I did a leaching test. Are there any recommendations to prevent organic leaching from chitosan beads?
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Nayim Sepay Thank you very much sir for your suggestion. I will try characterizing and identify the organics of the material I have.
Madhukar Baburao Deshmukh Thank you sir for the comments. I will try and see the modification method to see where the issue is.
Thank you very much Professor Frank T. Edelmann . The mentioned articles were very useful to get an idea on what aspects I should proceed. I will do a thorough literature check again and see.
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I am observing a high UV260 absorbance plateau during the cleaning in place of my HIC column using 1 M NaOH. This is giving me confounding results in regards to mass balance. The HIC column uses a butyl ligand. Could this suggest that the integrity of the ligand is poor or could it be leaching out because of the high concentration of NaOH? The UV260 peak appears with or without loading sample.
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Dear Jomar Difuntorum sorry to see that your interesting technical question has not yet received any expert answers. Unfortunately I'm not an expert either because we work in synthetic inorganic chemistry. However, I just found out that a closely related technical question has been asked several years ago on RG. Perhaps it might be helpful reading the answers given to that question:
Does anyone know why my 1N NaOH solutions have a high absorbance at 280nm during chromatography runs?
(7 answers)
Also please check the following ppotentially useful link:
Sodium hydroxide sanitization of AxiChrom™ columns packed with chromatography resin
I hope this helps. Good luck with your work and best wishes!
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I run a model on an aquifer with 3 layers. the contaminant is leaching on the upper layer. At the point of entry, the contaminant concentration is constant at 0.1 mg/m³.
I am having a hard time selecting the appropriate option in Sink/Source Concentration under MT3DMS/SEAWAT model as the options available are Constant head cells, well, river, and time-variant specified concentration.
Also, no recharge is applied to this model.
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In soils normally the erosion losses of soil phosphate -P are considerable and they are monitored.The leaching losses are presumed to be  negligible. Under what soil crop  conditions the leaching losses of phosphate are considerable and need monitoring? 
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According to the literature review and due to the nature of structure and function of phosphorous cycle in soil in various ecosystems and when the vital activities of some organisms is endangered due to its fluctuations, it should be considered a series suitable management decisions to prevent diminish of that. In fact, the balancing/equilibrium building of this macro element/ion as a conventional approach is proposed in soil science. Among that, the pH of soil is decisive role that should be considered.
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I have done hot filtration test for the catalyst to show leaching and I found no reaction after filtration. So, is it still necessary to perform ICP analysis of the catalyst??
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Dear Loveneesh Kumar thanks for sharing this very interesting technical question with the RG community. According to the relevant literature reference cited below, a "hot filtration test alone cannot prove that the reaction occurs heterogeneously":
Synthesis, catalytic activity, and leaching studies of a heterogeneous Pd-catalyst including an immobilized bis(oxazoline) ligand
Fortunately this article has been posted by the authors as public full text on RG, so that you can freely download it as pdf file.
It might also be worth a try to check the answers given to the following closely related questions which have been asked earlier on RG:
How might I measure the leaching of heterogeneous catalyst using simple techniques?
(4 answers)
and
What is the best technique to test the heterogeneity of a reaction in catalysis?
(58 answers)
Good luck with your work and please stay safe and healthy!
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According to the available references, PbCO3 and PbO are easily soluble in HBF4 and it is sometimes mentioned that adding H2O2 will improve the efficiency of the leaching by preventing the production of PbO2.
In my experiments, a white substance forms as soon as PbO or PbCO3 is added to HBF4 and dissolution does not occur at all. I also have done some 24 hours tests and even the temperature raised to 80 ° C in these tests, but no progress is observed in the process of leaching of this materials.
It would be really appreciated if anyone can help me through this leaching process of PbO or PbCO3 in HBF4!
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Dear Hadi Sharifidarabad many thanks for sharing this very interesting technical question with the RG community. In principle, both PbO and PbCO3 should be soluble in tetrafluoroboric acid (HBF4). Of course it is difficult to judge from the distance what perhaps went wrong in your case. My suggestion would be to make sure that your samples are finely ground in a mortar prior to the leaching experiments. For some general information you might want to have a look at the following potentially useful article:
Optimization and kinetics studies of lead concentrate leaching using
fluoroboric acid
This paper is freely available on the internet as public full text (please see attached pdf file).
Good luck with your work and please stay safe and healthy! With best wishes, Frank Edelmann
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Hello,
I have a question about the interaction of the glass surface (soda-lime glass) with moisture and white paper. I would like to find some sources of information (articles, publications, studies, etc.). I have not yet found anything specific in the available libraries.
I have found experimentally that when wrapping glass in white paper (to store it), there is a problem with leaching of ions from the glass. This changes the adhesion properties of the glass.
I know that white paper is not generally recommended for packing and storing glass. Bleached paper reacts with Na ions from the glass. The low concentration of sodium ions on the glass surface results in further leaching of ions from the glass to the surface. And also deacidified paper has a so-called alkaline reserve. Glass is less resistant to alkaline environments, especially in connection with humidity.
I would like to know more. Please do you have experience with this phenomenon? Alternatively, can you send me links to publications that deal with this?
Thank you.
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Joseph Cukjati Thank you very much for your reply and information provided. Your explanation is clear. In addition to carbonates, sulphates (mostly sodium sulphate) were also present on the glass surface.
I will read the recommended literature and resources. Thank you for them.
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Good day, dear colleagues!
One of the critical point in the glass industry is a glass surface leaching.
Many factors may lead to this problem. Some of them is critical visible on the surface even vefore heat treatment (bending, tempering etc).
But I wanna talk about nonvisible (via human eyes) leaching.
Can You advice any method without destroing glass for identeficate glass surface nonvisible leaching?
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If the leaching involve some differences in the height it would be possible to use a optical profilometer which is non-destructive method however do have some limitations in terms of size of sample.
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What are the most effective and sustainable measures to prevent leaching from glass (precursor)-based geopolymer? Please recommend your suggestions and publications. Thanks.
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Dear Alesha,
My research evidenced that silica gel, the main reaction product from waste glass dissolution, can be significantly stabilized by its interaction with polymerized C-S-H. Moreover, silica gel can be also modified with Ca from CaCO3 , which also enhances the hydrolysis resistance. We believe that modified silica gel can be a new promising hydraulic cementitious phase, but I need to do more research in this regard.
I agree with Alex, achieving geopoymerization with waste glass as precursor is quite complicated. Because of the low Al content, the polymerization process of silica gel can take several weeks. In a recent submitted paper, we tried to promote polymerization through constant curing at 60°C, with pastes developing more than 100 MPa at 28 days. However, the pastes had drastic strength losses afterwards, result of drying and polymeric shrinkage.
On the other hand, the formation of a hydraulic alkali-activated cement (AAC) with good mechanical properties is feasible (1-year mortars up to 29 MPa).
Cheers,
Luis Menchaca
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I am doing an experiment to leach polonium-210 from my plant samples. I am having trouble getting decent recoveries. I am not able to use any heating methods because of the volatility of polonium. Does anyone have any recommendations to improve my leaching procedures? currently I am soaking the grinded plant samples overnight in HCl in a shaker.
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The autoclave allows you to use pressure to control the vapor pressure of the process, generally the vapor pressure of gases and liquids increase with temperature at a constant pressure, if you raise the pressure you generally depress the equilibrium vapor pressure allowing a higher temperature to be used.
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I was going though this paper "Extraction of vanadium from high calcium vanadium slag using direct roasting and soda leaching" but finally how could they extract from the leached solution I didn;t get.
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Generally, metals recovery from a solid waste includes two stages. First, the metal has to be liberated from the solid complex through acidification or alkalinization. Then, the solution condition should be altered in a way (usually by pH adjustment) that the desired metal selectively precipitates in the form of metal oxide. Thereafter, the precipitate can be collected using filter paper. Other ways to recover the solubilized metal from the solution are electrowinning, solvent extraction, and ion exchange.
You can refer to the below paper for more info
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I'm working on a manganese processing project. Unfortunately, in the manganese ore high amounts of divalent iron are present and it remain in solution after acidic leaching and increasing pH to 5.
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Hi
Mr nasser
I think you use ore of manganese ore.
For remove completly of ferros ion you must rise ph of solution by cao to ph =7 . Then stirr the solution 1h at 80c.
Then filter it.
Almost of ferrous ion will be remove.
I have question
What is your reduction agent ?
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Chemicals added to swimming pools leach into the air above the surface of the water, with the result that regular lap swimmers must be inhaling them to a significantly greater degree than casual pool users. Have there been any studies on the long term health effects?
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Studies have revealed that pool chemicals and their by-products (some chemicals combine to form new chemicals) cause burning eyes, skin irritation, allergies, asthma and higher rates of cancer.
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The EDS analysis reported the decreasing amount of Nickel on catalyst surface after hydrogenation reaction. I thought there is leaching of Nickel during reaction and easier than leaching copper. But why and what is the properties of Nickel that can explain this result, the leaching of Nickel on catalyst.
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Dear Thanakorn Lowasri I'm not an expert in heterogeneous catalysis, but to my knowledge the encapsulation of metal catalysts in SBA mesoporous silica materials in done particularly in order to prevent leaching of the metals. For more information about this please have a look at the following very useful review article:
Current advances in the utility of functionalized SBA mesoporous silica for developing encapsulated nanocatalysts: state of the art
This is an Open Access article which is freely available on the internet (see attached pdf file). Several cases of metal leaching are discussed in this review. I actually do not know why in your case nickel is leached to a larger extent than copper.
Good luck with your research!
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I am using a Ni, Co, Ru activated carbon catalyst (simple impregnation method) for hydrogenation. But I am facing the metal leaching problem during recyclability. Please suggest to me some synthesis modifications, which will be beneficial to stop metal leaching and will not affect catalyst activity.
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Dear Adarsh Kumar you should change your synthesis method to achieve your purpose. You can use two methods:
1) You can graft linker on the surface inside the pores then when you using impregnation technique the linker help the metal salt to diffuse into the pores and stabilized there then use a reducing agent like NaBH4 to form particles inside the pores.
2) You can use the activated carbon substrate as a sieve to filter the particles. First you should synthesis the particles by hydrothermal treatment or some method that has low aggregation. Then you must add the substrate to the suspension and keep it on stirring and evaporate the solvent (this step take too much time and should done slowly about one week). Then you can do the calcination step.
Read these articles for more information about the synthesis methods:
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I need to prepare yttrium nitrate by dissolving its oxide into 6M nitric acid.
I would like to know any experimental considerations in this process to get best results.
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Dear Mohammad Jazirehpour many thanks for posting this interesting technical question. The preparation of Y(NO3)3􏰀x6H2O powder has been reported in the article cited below. It was obtained by dissolving yttrium oxide in 6 M nitric acid:
Size dependence of the upconverted luminescence of NaYF4:Er,Yb microspheres for use in ratiometric thermometry
From our own experinence I would suggest the following procedure: Place the nitric acid in a beaker and heat it to ca. 50-80 °C. With stirring, add a little more than the calculated amount of Y2O3 and let the mixture stir until most of the oxide has dissolved. A small excess of oxide is useful to completely consume the acid. Then filter the mixture and evaporate the clear filtrate until crystals begin to form. Pour the hot solution into a crystallization dish and let it stand at room temperature over night so that the remaining water evaporates. Then collect the product.
Good luck and best wishes, Frank Edelmann
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  • I have a very complex XRD spectrum (fly ash leaching residue) and couldn't match all the peaks with JADE. Do you know any free or paid software which may has strong database and can do search and match of complexes? In JADE you have to guess which is inside your sample and then compare with your peaks but when you are not sure about the formed minerals, this method is not helpful. Thank you!
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Theoretically:
From XRD patterns as follows:
Variations in the height of the specimen in its holder, whether increasing or decreasing, cause XRD peaks to change from their original location.
Important and useful pathways are connected to the XRD Curve:
Scherrer’s equation:
Particle Size, D = (0.9 x λ)/ (d cosθ)
λ = 1.54060 Å (in the case of CuKa1) so, 0.9 x λ = 1.38654
Θ = 2θ/2 (in the example = 20/2)
d = the full width at half maximum intensity of the peak (in Rad) – you can calculate it using Origin software.
To convert from angle to rad
Rad = (22 x angle) / (7 x 180) = angle x 0.01746
Example: if d = 0.5 angle (θ)
= (22 x 0.5)/ (7x 180) = 0.00873 rad
Then
Delta=1/D^2
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A daily leaching column Nitrogen was conducted to investigate the rate of soil leaching. Now I search for a simple model of equation to represent scientifically the results.
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Leaching of heavy metal can be a concern as heavy metal contaminated sludge is introduced to the finished products. It should be confirmed that leaching of heavy metal from bricks does not exceed the maximum permissible limit even under extreme conditions. The leaching efficiency was defined as the ratios of concentration of the heavy metal in the original sample and leachate of the sample
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Hazardous Wastes (Management, Handling and Transboundary Movement) Rules, 2008
IS 9806 (2001): Methods of Test for and Permissible Limits of Toxic Materials Released from Ceramicware, Vitreous Enamelware, Glassware and Glass-cerami
TCLP regulatory limits given by United States Environment Protection Agency (USEPA) and Germany Leachate Quality Standards.
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I'm planning the calcium leaching experiment. Thereby, the cement paste specimens were immersed in the 6M ammonium nitrate(NH4NO3) solution. If the specimens were removed at a specific immersion age, what method should be used to maintain the condition at that time? (For example, can it be maintained when the specimens were immersed in acetone and then dried?)
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Hello,I am pleased to answer your question.I think you can put the cement paste specimen into the constant temperature and humidity curing box to ensure its condition. If you follow your method, making the specimens were immersed in acetone and then dried, the moisture content of the specimen will change with the drying time. I hope my answer will help you.
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Hello everyone, my research is about leaching of gold from end-of-life printed circuit board by using Fe2(SO4)3 solution and the leachability was approximately 30-40%. Hence, i have some questions to ask.
1. Could these reactions be spontaneous in my solution?
Au + Fe3+ --> Au+ + Fe2+
2Au + SO42- + 2Fe3+ --> Au2SO4 + 2Fe2+
2. If not, in your opinion, what reactions might occur in my solution for gold leaching?
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Dear Natrawee Khetwunchai thank you for your very interesting technical question. Please find cited below some research articles in which the mechanism of gold leaching using Fe2(SO4)3 has been investigated:
1. Recovery of Gold from the Refractory Gold Concentrate Using Microwave Assisted Leaching
(see attached pdf file)
2. Bacterially generated Fe2(SO4)3 from pyrite, as a leaching agent for heavy metals from lignite ash
This article is freely available as public full text on ResearchGate.
3. Leaching kinetics of gold bearing pyrite in H2SO4−Fe2(SO4)3 system
(see attached pdf file)
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Hello everyone. My research is about kaolin bioleaching which reduced Fe3+ to Fe2+. I am required to filter out leaching solutions so I can dry the kaolin to powder form for ICPOES analysis to detect Fe3+ ions.
Since the leaching solution contains glucose, bacteria cells and reduced Fe2+ ions, may I know is cellulose nitrate or cellulose acetate membrane can be used for this filtration?
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We are trying to add nanoparticle power waste material in sustainable concrete, so we want to see any leaching effect of this material. Need suggestions and discussion from experts.
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Many Thanks Prof. Nehdi
I will go through the suggested article for more information
Thanks
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The commercial graphite is purchased from the market. And the recycled graphite is simply and mechanically recycled from the copper foil of a spent lithium-ion battery. There is no leaching or any other purity removal process on it. Does anyone could help to analyze these two spectra?
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Hi Zhao Hua, the intensity ratio of D band (ca. 1350 cm-1) to G dand (ca. 1560 cm-1) for the recycled graphite powder is increased compared to the commercial graphite powder, which indicates that the defect degree of graphite powder is increased after cycling. In addition, the intensity of 2D band (ca. 2700 cm-1) for the recycled graphite powder is decreased compared to the commercial graphite powder, suggesting the partial destruction of the hexagonal ring structure.
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We want to couple proteins to Fe3O4 particles via their primary amine or SH groups. We can generate large amounts of these particles. We are currently trying coupling via epoxide group in which particles have been coated with a silane compound but are not having much luck. The coupling needs to be covalent and resistant to pH 3-13 so that there is low leaching of proteins. Please let me know if you can provide this expertise.
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For how many metric tons?
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In zinc production plant, in leaching step, there are 20 g/l zinc and 0.6 g/l chloride. Is there any practical approach to remove chloride to less than 300 mg/l?
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There are two common methods to produce a solution with lower Cl, one is to precipitate the zinc (and other metals) with caustic or carbonate, use a filter to recover the precipitate and then re-dissolve the zinc with acid solution with low
Cl water, typically demineralised water. The second option is to extract the zinc using ion exchange or solvent extraction and strip the zinc from the organic extractant or resin into a a low chloride solution.
Both options mean that a base is required to neutralise the acid associated with the metal ion, you don't need to do this for all of the zinc solution but only enough to meet your Cl target.
It is preferable to limit the chloride ingress into the leach solution, this could be by washing the ore/concentrate prior to leaching in a low chloride solution, or evaluating water quality used in the leaching process, especially if leach solution is recycled then chloride levels will increase to an equilibrium level, a bleed stream may be a good way to manage the chloride levels...
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I had prepared 50ml of 0.5M Sulphuric acid and to that I added 20ml of 0.5M sulphuric acid containing 9 drops of 2M sodium hydroxide. I then leached the mixture for 15 minutes using a magnetic stirrer. In the same standard procedure I continued to increase the pH by adding more drops of sodium hydroxide that is from 9 to 34 and 50 drops. 
thank you
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I need to know the particle size for the test, concentration of acid, amount of sample to be tested and the apparatus to be used as well as how to analyze the solution.
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some one please suggest me software for analysis of leaching pollutant in soil.I have the physio-chemical result of the soil.
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The U.S. EPA's model for pesticide leaching to groundwater (PWC) is located here:
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Examples of articles of trivial scientific values:
1. Meswak extract did not have much effect on f