[go: up one dir, main page]

WO2011108488A1 - Méthode de production d'arséniate de fer cristallin à partir d'une solution contenant de l'arsenic - Google Patents

Méthode de production d'arséniate de fer cristallin à partir d'une solution contenant de l'arsenic Download PDF

Info

Publication number
WO2011108488A1
WO2011108488A1 PCT/JP2011/054502 JP2011054502W WO2011108488A1 WO 2011108488 A1 WO2011108488 A1 WO 2011108488A1 JP 2011054502 W JP2011054502 W JP 2011054502W WO 2011108488 A1 WO2011108488 A1 WO 2011108488A1
Authority
WO
WIPO (PCT)
Prior art keywords
iron
arsenic
solution
reaction
arsenate
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Ceased
Application number
PCT/JP2011/054502
Other languages
English (en)
Japanese (ja)
Inventor
三雄 鐙屋
祐輔 佐藤
寛信 見上
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
Dowa Metals and Mining Co Ltd
Original Assignee
Dowa Metals and Mining Co Ltd
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Dowa Metals and Mining Co Ltd filed Critical Dowa Metals and Mining Co Ltd
Publication of WO2011108488A1 publication Critical patent/WO2011108488A1/fr
Anticipated expiration legal-status Critical
Ceased legal-status Critical Current

Links

Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G28/00—Compounds of arsenic
    • C01G28/02—Arsenates; Arsenites
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G49/00—Compounds of iron

Definitions

  • the present invention relates to a method for separating and recovering from a solution as crystalline iron arsenate (for example, scorodite crystal) as a compound.
  • Trivalent iron meaning “Fe 3+ ” in the present invention
  • pentavalent arsenic meaning “As 5+ ” in the present invention
  • the pH value of the solution was set under a condition exceeding 1 in order to improve the reaction rate.
  • the obtained iron arsenate becomes very fine, and further, it is easy to contain amorphous iron arsenate.
  • Patent Documents 1 and 2 have been proposed regarding a method for separating and recovering arsenic present in a solution from the solution as scorodite.
  • the proposal of Patent Document 1 is a method for producing iron arsenate from an acidic aqueous solution containing pentavalent arsenic and trivalent iron, wherein the molar ratio of trivalent iron to pentavalent arsenic contained in the acidic aqueous solution is determined. This is a method of generating scorodite after adjusting to 0.9 or more and 1.1 or less.
  • Patent Document 2 is a method for producing scorodite from an acidic aqueous solution containing pentavalent arsenic and trivalent iron, wherein the sodium concentration in the acidic aqueous solution exceeds 0 g / L and is 4 g / L or less.
  • a basic sodium compound is added to the acidic aqueous solution to generate scorodite.
  • the present inventors examined the production method of crystalline iron arsenate (scorodite) described in Patent Documents 1 and 2.
  • a large amount of seed crystals 50 g / L in the example
  • an acidic aqueous solution containing pentavalent arsenic and trivalent iron and heat treatment at a high temperature (in the example, (95 ° C., 24 hours) to generate scorodite.
  • a high temperature in the example, (95 ° C., 24 hours
  • Patent Document 2 requires a very long time of 24 hours for the generation time of scorodite.
  • Patent Document 1 also requires a very long time of 24 hours for the generation time of scorodite.
  • the production of iron arsenate having large crystal grains is not described in any of the conventional methods including Patent Documents 1 and 2.
  • the present invention has been made under the above circumstances, and the problem to be solved is that crystalline iron arsenate particles having a large particle diameter can be easily and quickly produced from a solution containing arsenic. And providing a method for obtaining crystalline iron arsenate.
  • the present inventors have conducted intensive research and obtained the following knowledge.
  • the pH of the acidic solution is higher than 1, preferably about 1.5, so that the production reaction Speed increases and arsenic processing efficiency increases.
  • the iron arsenate particles produced tend to be very fine.
  • the pH value of the acidic solution is 1 or less, crystalline iron arsenate is hardly produced unless seed crystals are present.
  • oxygen or air is blown into the acidic solution having a pH value of 1 or less as an oxidizing agent, for example, crystalline iron arsenate is hardly generated.
  • the present inventors have difficulty in easily producing crystalline iron arsenate particles having a large particle diameter in a short time from a solution containing arsenic in any region with a pH value of 1 as a boundary. Research was conducted to solve this situation. Then, in the acidic solution containing arsenic, trivalent iron and divalent iron (meaning “Fe 2+ ” in the present invention) are present and the pH value is adjusted to 1.0 or less, and then an oxidizing agent. The present invention has been completed by obtaining the epoch-making knowledge that crystalline iron arsenate particles having a large particle diameter can be easily and quickly produced from the solution by adding.
  • the first invention according to the present invention is: In this method, divalent iron is added to a solution containing pentavalent arsenic and trivalent iron, the pH value of the solution is adjusted to 1.0 or less, and an oxidizing agent is added to produce crystalline iron arsenate. And
  • the mole number of pentavalent arsenic is A mole
  • the mole number of trivalent iron is B mole
  • the mole number of divalent iron is C mole
  • B / A ⁇ 1.0 and A method for producing crystalline iron arsenate from a solution containing arsenic characterized in that C> 0 and B> 0.
  • the second invention is Furthermore, (B + C) ⁇ A is the method for producing crystalline iron arsenate from a solution containing arsenic according to the first aspect of the invention.
  • the third invention is The solution containing arsenic according to the first or second invention, wherein the oxidizing agent is at least one selected from oxygen gas, air, a gas containing oxygen, and an air dilution gas Is a method for producing crystalline iron arsenate.
  • the fourth invention is: In the production reaction of crystalline iron arsenate, the pH value of the solution is more than 1 and 2 or less after the time when the arsenic concentration in the solution becomes 30% or less of the arsenic concentration at the start of the reaction.
  • the fifth invention is: The arsenic according to any one of the first to fourth inventions, wherein the post-reaction solution after producing crystalline iron arsenate from a solution containing arsenic is reused as a divalent iron source Is a method for producing crystalline iron arsenate from a solution containing
  • crystalline iron arsenate particles having a large crystal grain size can be produced in a short time.
  • both trivalent iron and divalent iron are present in a solution containing arsenic, and the trivalent iron is prioritized over divalent iron under a pH value of 1 or less. It reacts to produce crystalline iron arsenate.
  • crystalline iron arsenate includes scorodite (FeAsO 4 .2H 2 O), kankit (FeAsO 4 .1.5H 2 O), zykaite (Fe 4 (AsO 4 ) 3 (SO 4 ) (OH 4 ) ) ⁇ 15H 2 O), bukovskyite (Fe 4 (AsO 4 ) 3 (SO 4 ) (OH) ⁇ 7H 2 O), saliente (Fe 4 (AsO 4 ) 3 (SO 4 ) (OH) ⁇ 7H 2 O) Etc.
  • the present invention relates to B /, which is a molar ratio of trivalent iron to arsenic in a solution having a pH value of 1 or less containing arsenic A mole, trivalent iron B mole, and divalent iron C mole.
  • An oxidizing agent is added as A ⁇ 1.0 (that is, A> B) to produce crystalline iron arsenate particles.
  • iron is a mixture of B moles of trivalent iron and C moles of divalent iron, A> B, and A ⁇ (B + C).
  • the arsenic is preferably pentavalent arsenic. This is because iron arsenate is a compound of trivalent iron and pentavalent arsenic.
  • the molar ratio of the trivalent iron B mole and the divalent iron C mole may be set according to the target amount of crystalline iron arsenate production and the situation, but the molar ratio (value of B / C) is Setting in the range of 0.1 to 2 is preferable from the viewpoint of productivity of crystalline iron arsenate.
  • the molar ratio may be changed before and during the reaction.
  • the present inventors set the pH value of the solution to 1 or less, B / A ⁇ 1 as described above, and divalent iron C mol.
  • the crystallization reaction of trivalent iron and pentavalent arsenic proceeds preferentially and quickly compared to the crystallization reaction of divalent iron and pentavalent arsenic, by adding an oxidizing agent. It has been found that crystalline iron arsenate particles having a large particle size are produced in a short time.
  • arsenic-containing material to which the present invention is applied trivalent iron source, divalent iron source, trivalent and divalent iron source addition method, oxidizing agent, solution pH value control, pH adjuster, reaction vessel Will be described in detail.
  • Arsenic-containing substances to which the present invention is applied include arsenate and arsenic acid. Specifically, waste water, smoke ash, and shrine generated from the smelting process. In order to safely treat these arsenic-containing materials generated in the smelting process, leaching or the like is performed to obtain an arsenic solution, which is the target solution of the present invention.
  • the present invention can also be applied to waste containing arsenic, and arsenic solutions generated with the purification of arsenic naturally contained in soil, rivers, and the like.
  • arsenic in the solution is preferably oxidized beforehand to pentavalent arsenic.
  • the present inventors coexisted arsenic, trivalent iron, and divalent iron (meaning “Fe 2+ ” in the present invention) in an acidic solution having a pH value of 1 or less, and a predetermined value.
  • an acidic solution having a pH value of 1 or less, and a predetermined value.
  • the crystalline iron arsenate production reaction proceeds rapidly and crystalline iron arsenate particles having a large particle size are produced. I found out.
  • the present inventors present both less than 1 mol (0.1 to 1.0 mol) of trivalent iron and divalent iron with respect to 1 mol of arsenic present in the solution.
  • the reaction conditions of adding an oxidizing agent (air, oxygen blowing, etc.) to the solution were conceived. Under the predetermined reaction conditions, the inventors have found a phenomenon in which the formation reaction of crystalline iron arsenate particles having a large particle diameter proceeds rapidly.
  • a trivalent iron source is a trivalent iron salt. Specifically, ferric sulfate, ferric chloride, ferric nitrate, etc., iron oxide, iron hydroxide, etc. are mentioned. Here, ferric sulfate is preferable from the viewpoint of corrosiveness to equipment and easy availability as a general-purpose drug.
  • the ferric sulfate is preferably dissolved in warm water and added as a solution of trivalent iron ions. However, from the viewpoint of suppressing the amount of liquid, it may be added directly to the solution to be treated in powder form.
  • divalent iron source As a divalent iron source, there is a divalent iron salt. Specifically, ferrous sulfate, ferrous chloride, ferrous nitrate, etc., iron oxide, iron hydroxide and the like can be mentioned. Here, ferrous sulfate is preferable from the viewpoint of corrosiveness to equipment and easy availability as a general-purpose drug. The ferrous sulfate may be dissolved in warm water and added as a solution of divalent iron ions. However, it is preferable to add the ferrous sulfate directly to the target solution in a powder form from the viewpoint of suppressing the amount of liquid.
  • the trivalent and divalent iron sources can be added to the solution to be treated at once, or they can be added in a plurality of divided portions as the crystalline iron arsenate formation reaction proceeds. However, according to the total addition all at once, the operation can be simplified and the working cost can be reduced. Further, the trivalent iron and pentavalent arsenic are scarcely contained in the post-reaction solution obtained after the crystalline iron arsenate is produced from the solution to be treated, while the divalent iron remains. Therefore, the post-reaction solution can be used again as a divalent iron source. This configuration is preferable because the drug cost can be reduced.
  • oxygen gas As the oxidizing agent, one or more selected from oxygen gas, air, gas containing oxygen, air dilution gas, ozone and the like can be used. The concentration may be adjusted using the partial pressure of these gases.
  • the oxygen-containing gas means a gas having an oxygen-containing composition of more than 21% (air-containing oxygen amount) and less than 100%, and the air-diluting gas is an inert gas such as nitrogen gas mixed with air.
  • the addition method if it is a gas body, it may be blown into the solution to be treated, and if it is liquid, it may be added to the solution.
  • the crystalline iron arsenate production reaction according to the present invention is a reaction that generates hydrogen ions. For this reason, as the crystalline iron arsenate production reaction proceeds, the pH value of the solution to be treated decreases. Here, if the pH value of the solution is allowed to go down and the pH value during the progress of the crystalline iron arsenate formation reaction is reduced from 0.70 to 0.79, the reaction rate is remarkably reduced, and after the reaction The knowledge that the concentration of arsenic remaining in the liquid was increased was obtained. On the other hand, in order to produce crystalline iron arsenate having a large particle size using trivalent iron in the crystalline iron arsenate production reaction, the inventors preferably have a solution having a pH value of 1 or less. I have obtained the knowledge.
  • the present inventors should neutralize the generated hydrogen ions and keep the pH value at the end of the reaction within a predetermined range during the progress of the crystalline iron arsenate production reaction.
  • the pH value of the solution is 0.8 or less
  • the pH value can be maintained at 0.8 or more and raised to pH 1.
  • the crystalline iron arsenate production reaction becomes slow at the late stage of the reaction when the arsenic concentration in the solution to be treated is 30% or less of the arsenic concentration at the start of the reaction. Therefore, in the latter stage of the reaction, it is also preferable to increase the pH value to around 1 to 2 to promote the crystalline iron arsenate production reaction.
  • the crystalline iron arsenate already produced is stable, and there is no problem because the crystalline iron arsenate does not re-dissolve due to an increase in pH value.
  • the pH value holding control width at a predetermined pH value is preferably as narrow as possible from the viewpoint of particle growth of crystalline iron arsenate.
  • the pH value control range when the predetermined pH value is held as 1.0 is controlled in a narrower range than the range where the pH value does not fall below 0.9 and does not exceed 1.0.
  • a pH adjusting agent to be described later is added to water, and added to the solution to be treated after forming a liquid with a high slurry concentration, thereby ensuring wetting of the solution. A method of facilitating diffusion into the solution is effective.
  • the pH adjuster is preferably an alkaline earth metal alkali such as Mg (OH) 2, Ca (OH) 2, MgO, CaO, or the like, or an alkali metal alkali such as NaOH or KOH. good. These single species or a mixture of a plurality of species may be used.
  • reaction vessel The container used for the production reaction of the crystalline iron arsenate may be an open type. Since the production reaction takes place under atmospheric pressure, the container does not require special pressure resistance.
  • Example 1 Test unit and test scale A 1 L beaker was used as a test container.
  • the stirrer installed in the test vessel was equipped with four baffle plates, a two-stage turbine blade, and a rotation speed of 600 rpm. At this time, the total amount of arsenic and iron mixed solution processed per batch was 650 mL. All examples are under atmospheric pressure (normal pressure).
  • pH adjuster a reagent manufactured by Kishida Chemical Co., Ltd., magnesium hydroxide Mg (OH) 2 (assay min 95%) was prepared as a pH adjuster.
  • Oxidizing agent In this example, air is used as the oxidizing agent in the stage from the start of the reaction until iron arsenate nuclei are generated in the solution, and thereafter, the crystalline iron arsenate particles grow. Then, oxygen gas was used as the oxidizing agent.
  • the pH value of the solution was raised to 1.5, and the pH value was controlled between 1.46 and 1.54.
  • the product was filtered to obtain a post-reaction solution and a product residue (scorodite). In this example, the filtration proceeded very smoothly and was completed in a few seconds, not 10 seconds.
  • Example 2 In “3) Preparation of Arsenic and Iron Mixed Solution” in Example 1 described above, 0.75 times equivalent (0.75 times mole) of pentavalent arsenic to 25 g / L of trivalent iron and the total amount of pentavalent arsenic of pentavalent arsenic.
  • divalent iron was a mixed solution of arsenic and iron in an amount equivalent to 0.75 times equivalent (0.75 times mole) of the total amount of pentavalent arsenic, and the air blowing time in the initial reaction was 60 minutes.
  • the product according to Example 2 was obtained. The product was filtered to obtain a solution and a product residue (scorodite). In this example as well, the filtration proceeded very smoothly and was completed in a few seconds, not 10 seconds.
  • Table 4 shows the particle size measurement results of the obtained scorodite after the filtrate at the end of the reaction was washed with pure water.
  • the pentavalent arsenic concentration, trivalent iron concentration, divalent iron concentration in the solution to be treated at the start of the reaction, 60 minutes after the start of the reaction, 120 minutes after the start of the reaction, and 240 minutes after the start of the reaction. was measured.
  • the measurement results are shown in Table 1.
  • the pentavalent arsenic concentration, trivalent iron concentration, and divalent iron concentration in the solution to be treated 240 minutes after the start of the reaction are very low, but the divalent iron concentration is high. Accordingly, it was found that the solution to be treated, which is a post-reaction solution 240 minutes after the start of the reaction, can be reused as a divalent iron source.
  • Example 3 In “3) Preparation of Arsenic and Iron Mixed Solution” in Example 1 described above, pentavalent arsenic is 25 g / L, and trivalent iron is 0.9 times equivalent (0.9 times mole) to the total molar amount of pentavalent arsenic.
  • the product according to Example 3 was obtained in the same manner as in Example 1 except that divalent iron was changed to 0.5 times equivalent (0.5 times mol) with respect to the total molar amount of pentavalent arsenic.
  • the product was filtered to obtain a solution and a product residue (scorodite). In this example as well, the filtration proceeded very smoothly and was completed in a few seconds, not 10 seconds.
  • Table 4 shows the particle size measurement results of the obtained scorodite after the filtrate at the end of the reaction was washed with pure water.
  • Example 4 In “3) Preparation of Arsenic and Iron Mixed Solution” in Example 1 described above, pentavalent arsenic is 25 g / L, and trivalent iron is 0.9 times equivalent (0.9 times mole) to the total molar amount of pentavalent arsenic.
  • a product according to Example 4 was obtained in the same manner as in Example 1 except that divalent iron was changed to 0.75 times equivalent (0.75 times mol) with respect to the total molar amount of pentavalent arsenic.
  • the product was filtered to obtain a solution and a product residue (scorodite). In this example as well, the filtration proceeded very smoothly and was completed in a few seconds, not 10 seconds.
  • Table 4 shows the particle size measurement results of the obtained scorodite after the filtrate at the end of the reaction was washed with pure water.
  • Comparative Example 1 1) Preparation of Arsenic / Iron Mixed Solution
  • the pentavalent arsenic was 25 g / L
  • the trivalent iron was adjusted to the total molar amount of pentavalent arsenic. Comparative Example 1 was carried out in the same manner as in Example 1 except that 0-fold equivalent (1.0-fold mole) and divalent iron were changed to 0.5-fold equivalent (0.5-fold mole) with respect to the total mole amount of pentavalent arsenic. This operation was performed.
  • the pentavalent arsenic concentration, trivalent iron concentration, and divalent iron concentration in the solution to be treated at the start of the reaction 60 minutes after the start of the reaction, 120 minutes after the start of the reaction, and 240 minutes after the start of the reaction. was measured.
  • the measurement results are shown in Table 2.
  • the scorodite obtained in Comparative Example 1 was produced by the reaction of pentavalent arsenic and trivalent iron under a solution pH value of 1.5, and the particle size of the produced scorodite was found to be as fine as 3.3 ⁇ m. In this reaction example, the same result was obtained when air was used as the oxidizing agent.
  • Comparative Example 2 1) Preparation of Arsenic / Iron Mixed Solution
  • the pentavalent arsenic was 25 g / L
  • the trivalent iron was adjusted to the total molar amount of pentavalent arsenic.
  • Comparative Example 2 was carried out in the same manner as in Example 1 except that 0-fold equivalent (1.0-fold mole) and divalent iron were changed to 1.5-fold equivalent (1.5-fold mole) with respect to the total mole amount of pentavalent arsenic. This operation was performed.
  • the pentavalent arsenic concentration, trivalent iron concentration, and divalent iron concentration in the solution to be treated at the start of the reaction 90 minutes after the start of the soot reaction, 180 minutes after the start of the reaction, and 240 minutes after the start of the soot reaction. was measured.
  • the measurement results are shown in Table 3.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Inorganic Chemistry (AREA)
  • Compounds Of Iron (AREA)

Abstract

La présente invention concerne une méthode de production simple et rapide de particules cristallines d'arséniate de fer de granulométrie importante à partir d'une solution contenant de l'arsenic. La méthode de production d'arséniate de fer cristallin à partir d'une solution contenant de l'arsenic implique l'ajout de fer divalent à une solution contenant de l'arsenic pentavalent et du fer trivalent, l'ajustement du pH de la solution à 1,0 ou moins, puis l'ajout d'un agent d'oxydation pour produire de l'arséniate de fer cristallin, où B/A < 1,0 et C > 0 et B > 0, A moles représentant le nombre de moles d'arsenic pentavalent, B moles le nombre de moles de fer trivalent, et C moles le nombre de moles de fer divalent dans la solution contenant de l'arsenic.
PCT/JP2011/054502 2010-03-01 2011-02-28 Méthode de production d'arséniate de fer cristallin à partir d'une solution contenant de l'arsenic Ceased WO2011108488A1 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
JP2010-044387 2010-03-01
JP2010044387A JP5662036B2 (ja) 2010-03-01 2010-03-01 ヒ素を含有する溶液からの結晶性ヒ酸鉄の生成方法

Publications (1)

Publication Number Publication Date
WO2011108488A1 true WO2011108488A1 (fr) 2011-09-09

Family

ID=44542140

Family Applications (1)

Application Number Title Priority Date Filing Date
PCT/JP2011/054502 Ceased WO2011108488A1 (fr) 2010-03-01 2011-02-28 Méthode de production d'arséniate de fer cristallin à partir d'une solution contenant de l'arsenic

Country Status (2)

Country Link
JP (1) JP5662036B2 (fr)
WO (1) WO2011108488A1 (fr)

Families Citing this family (1)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP6446229B2 (ja) * 2014-10-21 2018-12-26 Ｄｏｗａメタルマイン株式会社 ５価の砒素を含有する溶液からの結晶性砒酸鉄の製造方法

Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2008038401A1 (fr) * 2006-09-27 2008-04-03 Dowa Metals & Mining Co., Ltd. Procédé de fabrication d'un composé arséniure de fer presentant une bonne cristallinité
JP2008126104A (ja) * 2006-11-17 2008-06-05 Dowa Metals & Mining Co Ltd 砒素含有液の処理方法
JP2008540824A (ja) * 2005-05-03 2008-11-20 オウトテック オサケイティオ ユルキネン 溶液から有価金属および砒素を回収する方法
JP2009018291A (ja) * 2007-07-13 2009-01-29 Dowa Metals & Mining Co Ltd 種晶を添加する砒素の処理方法
JP2009079237A (ja) * 2007-09-25 2009-04-16 Nikko Kinzoku Kk スコロダイトの製造方法及びスコロダイト合成後液のリサイクル方法

Patent Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2008540824A (ja) * 2005-05-03 2008-11-20 オウトテック オサケイティオ ユルキネン 溶液から有価金属および砒素を回収する方法
WO2008038401A1 (fr) * 2006-09-27 2008-04-03 Dowa Metals & Mining Co., Ltd. Procédé de fabrication d'un composé arséniure de fer presentant une bonne cristallinité
JP2008126104A (ja) * 2006-11-17 2008-06-05 Dowa Metals & Mining Co Ltd 砒素含有液の処理方法
JP2009018291A (ja) * 2007-07-13 2009-01-29 Dowa Metals & Mining Co Ltd 種晶を添加する砒素の処理方法
JP2009079237A (ja) * 2007-09-25 2009-04-16 Nikko Kinzoku Kk スコロダイトの製造方法及びスコロダイト合成後液のリサイクル方法

Also Published As

Publication number Publication date
JP2011178602A (ja) 2011-09-15
JP5662036B2 (ja) 2015-01-28

Similar Documents

Publication Publication Date Title
US8092765B2 (en) Method of processing non-ferrous smelting intermediates containing arsenic
US8110162B2 (en) Method of processing copper arsenic compound
US8092764B2 (en) Method of processing non-ferrous smelting intermediate containing arsenic
JP5107637B2 (ja) 砒酸鉄粉末
JP4268196B2 (ja) スコロダイトの製造方法
CN105753218A (zh) 一种去除三价砷的方法
WO2010131686A1 (fr) Particules de compose a base de fer-arsenic de type scorodite, procede de production, et solide contenant de l&#39;arsenic
CN113184928A (zh) 硫酸镍溶液的制备方法
JP6286155B2 (ja) ５価の砒素を含有する溶液からの結晶性砒酸鉄の製造方法
JP2011177651A (ja) ヒ素含有溶液の処理方法
JP5662036B2 (ja) ヒ素を含有する溶液からの結晶性ヒ酸鉄の生成方法
CN107129018A (zh) 一种含砷废水中砷的浓缩方法
JP2010285322A (ja) 砒素を含有する溶液から結晶性スコロダイトを得る方法
JP4902450B2 (ja) 砒素の処理方法
JP5571517B2 (ja) 銅とヒ素とを含む非鉄製錬中間産物からの銅とヒ素との分離方法
JP6446229B2 (ja) ５価の砒素を含有する溶液からの結晶性砒酸鉄の製造方法
JP5156224B2 (ja) 鉄砒素化合物の製法
JP6102590B2 (ja) スコロダイトの製造方法
JP5966719B2 (ja) 四三酸化マンガンの製造方法
JP4985551B2 (ja) マグネシウム含有複合炭酸マンガンの製造方法
JP6480237B2 (ja) スコロダイトの製造方法
JP2003303590A (ja) アルカリ蓄電池用正極活物質の製造方法
JP2011168467A (ja) 結晶性スコロダイトの生成方法
JP6449706B2 (ja) スコロダイトの製造方法
JP7151916B2 (ja) 酸性スラリーの製造方法及び希土類元素の回収方法

Legal Events

Date Code Title Description
121 Ep: the epo has been informed by wipo that ep was designated in this application

Ref document number: 11750598

Country of ref document: EP

Kind code of ref document: A1

NENP Non-entry into the national phase

Ref country code: DE

122 Ep: pct application non-entry in european phase

Ref document number: 11750598

Country of ref document: EP

Kind code of ref document: A1