WO2004043862A1 - Procede de lixiviation d'elements de valeur de beryllium au moyen d'acide fluorhydrique - Google Patents

Procede de lixiviation d'elements de valeur de beryllium au moyen d'acide fluorhydrique Download PDF

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Publication number
WO2004043862A1
WO2004043862A1 PCT/IL2003/000954 IL0300954W WO2004043862A1 WO 2004043862 A1 WO2004043862 A1 WO 2004043862A1 IL 0300954 W IL0300954 W IL 0300954W WO 2004043862 A1 WO2004043862 A1 WO 2004043862A1
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Prior art keywords
beryllium
reacting
fluorine
process according
containing compound
Prior art date
Application number
PCT/IL2003/000954
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English (en)
Inventor
Simcha Harel
Lev Shapira
Eli Barnea
Tuvia Zisner
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Mti - Metal Technologies Israel 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
Priority claimed from IL15280202A external-priority patent/IL152802A0/xx
Priority claimed from IL15776403A external-priority patent/IL157764A0/xx
Application filed by Mti - Metal Technologies Israel Ltd. filed Critical Mti - Metal Technologies Israel Ltd.
Priority to AU2003282349A priority Critical patent/AU2003282349A1/en
Publication of WO2004043862A1 publication Critical patent/WO2004043862A1/fr

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Classifications

    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B35/00—Obtaining beryllium
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F3/00—Compounds of beryllium
    • C01F3/02—Oxides; Hydroxides
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B3/00—Extraction of metal compounds from ores or concentrates by wet processes
    • C22B3/04—Extraction of metal compounds from ores or concentrates by wet processes by leaching
    • C22B3/06—Extraction of metal compounds from ores or concentrates by wet processes by leaching in inorganic acid solutions, e.g. with acids generated in situ; in inorganic salt solutions other than ammonium salt solutions
    • C22B3/10—Hydrochloric acid, other halogenated acids or salts thereof
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P10/00—Technologies related to metal processing
    • Y02P10/20—Recycling

Definitions

  • the present invention relates to a method of leaching beryllium values from beryllium-containing ores using a fluorine-containing compound in an acidic aqueous medium.
  • Beryllium (Be) is one of the lightest of all metals and has one of the highest melting points of any light metal.
  • Beryllium metal and its alloys are used principally in aerospace and defense applications because of its stiffness, low specific gravity, and dimensional stability over a wide temperature range.
  • Beryllium metal is stiffer than 1010 steel, and is also highly conductive.
  • Beryllium and alloys thereof are often the preferred materials for electronic equipment.
  • Beryllium-copper alloys are used in a variety of applications because of their electrical and thermal conductivity, high strength and hardness, good corrosion resistance and fatigue resistance, and nonmagnetic properties.
  • Beryllium oxide is an excellent heat conductor, with high strength and hardness, and acts as an electrical insulator in some applications.
  • beryllium is extracted from mineral ores, primarily from beryl, bertrandite and phenakite.
  • the composition of beryl is 3BeO-Al 2 ⁇ 3 -6Si0 2 .
  • Commercial Beryl contains about 12% BeO, which is close to the theoretical composition of beryl (14% BeO).
  • the composition of bertrandite is 4BeO-2Si0 2 ⁇ ?0, which, according to the theoretical chemical composition, contains 42% BeO.
  • Commercially-available bertrandite contains only about 0.6%-0.9% BeO.
  • the commercially-available beryl is almost a pure mineral
  • the commercially-available bertrandite contains only 1.0-1.5% of the pure bertrandite, admixed with additional minerals such as aluminum and iron oxides, calcium and alkali oxides or silicates and quartz.
  • boiling sulfuric acid is used to dissolve the bertrandite, along with various oxide impurities (e.g., aluminum, iron) typically present in the commercial ore.
  • oxide impurities e.g., aluminum, iron
  • the solution is filtered to remove any insoluble silica from the solution.
  • bertrandite as a feed material is that commercially- available bertrandite contains less than 1 % BeO, i.e., only 5-8% of the BeO content of commercially-available beryl.
  • alkali treatment finely ground beryl is heated until fusion or sintered- below the melting point with a sufficient quantity of alkaline flux.
  • Suitable alkali compounds include hydroxides or carbonates of sodium, potassium and calcium; mixtures of these carbonates; calcium oxide; borax; lead chloride; and sodium sulfate and charcoal.
  • the ratio of flux to beryl depends on the operating conditions, especially the temperature: the higher the temperature the less flux.
  • gas-heated or oil-heated rotary furnaces or blast furnaces are suitable.
  • Rotary kilns, muffle furnaces, or tunnel kilns are used for sintering.
  • the beryl In the heat treatment, the beryl is melted, without additives, at a temperature exceeding 1650°C. and then quenched in water. After this treatment, about 50-60% of the beryl has an enhanced solubility in sulfuric acid. The rest of the beryllium oxide forms a solid solution with silicon dioxide that is not attacked by sulfuric acid. At 900°C this solid solution separates into beryllium oxide and silicon dioxide components, hence, a second heat treatment at this high temperature produces a free beryllium oxide that is soluble in sulfuric acid.
  • the obtained powder After cooling and grinding to 200 mesh, the obtained powder is heated to 250°C to 300°C in concentrated sulfuric acid, reacting so as to convert the beryllium, aluminum, and any iron, to soluble sulfates.
  • the silica fraction largely remains in the dehydrated, water insoluble form. This two-stage heat treatment typically renders soluble a total of about 90% of the beryl.
  • the heat-treated beryl is extracted with hot concentrated sulfuric acid, whereas alkali-treated beryl is extracted with cold sulfuric acid. While in the alkali process, there are relatively low heating costs, the total consumption of acid is considerably greater because of the alkali added.
  • the insoluble silicon dioxide is separated by filtration.
  • the filtrate contains not only beryllium and aluminum sulfate but also considerable quantities of iron sulfate and smaller amounts of other impurities, all of which must be removed before the precipitation of beryllium hydroxide.
  • Many separation processes are known, including alum separation, ammonium carbonate separation, and chelate separation.
  • beryl is melted or sintered with sodium hexafluorosilicate at approximately 700°C, according to the stoichiometry of the following equation: 2 (3BeO-Al 2 O 3 -6SiO 2 ) + 6Na 2 SiF 6 ⁇ 6Na 2 BeF 4 + 2Al 2 O 3 -+ 15SiO 2 + 3SiF (1)
  • A4, p.18 are hydrogen fluoride gas at 630°C, molten fluorides, other fluorosilicates, or silicon tetrafluoride.
  • Rotary kilns are used for reaction with the gases (hydrogen fluoride, silicon tetrafluoride); the solid mixtures (molten fluorides, other fluorosilicates) are briquetted and sintered in muffle furnaces or tunnel kilns. All of these processes are gas-phase or molten-phase processes conducted at extremely high temperatures and requiring expensive equipment.
  • U.S. Patent No. 3,375.060 to Olson, et al. discloses a method of solubilizing beryllium values in a mineral by reacting the mineral with fl ⁇ orite (CaF 2 ) and sulfuric acid. The reaction takes place at a temperature of 200°C - 300°C and atmospheric pressure. The products of the reaction are gaseous hydrogen fluoride and a salt cake containing water soluble beryllium sulfate along with calcium sulfate, aluminum sulfate, iron sulfate and various impurities. Separation of beryllium values from the solid calcium sulfate is subsequently performed by leaching with water.
  • U.S. Patent No. 3,375,060 to Zimmermann teaches a method of decomposing beryl and beryl-containing minerals by reacting- powdered beryl with gaseous hydrogen fluoride at 100°C - 900°C. Preferably, the reaction is performed at 500°C - 600°C.
  • the products of the reaction are SiF 4 vapor (which is condensed with water to produce Si0 2 ) and a cake containing water-soluble beryllium fluoride along with aluminum fluoride, iron fluoride and various impurities. Separation of beryllium values from the cake is subsequently performed by leaching with hot water.
  • the main disadvantages in the above-described process relate to the use of hydrogen fluoride in the vapor phase. Operation at elevated temperatures of 100°C - 900°C, and preferably, at 500°C - 600°C, requires extremely high pressures, tremendous superheating, or both. In the case of superheating, an extremely large reaction volume is required. Operation at elevated pressures requires special equipment. In particular, operation above about 200°C requires exotic materials of construction that render the process impractical.
  • the present invention is a production process for treating a beryllium feed material, such as beryl, by reacting the beryllium feed material with a fluorine- containing compound in an acidic aqueous medium.
  • a production process for dissolving beryllium in a beryllium feed source by means of a fluorine-containing compound in an aqueous medium including the steps of: (a) providing the beryllium feed source; (b) reacting the beryllium feed source with the fluorine-containing compound in a reaction stage to produce dissolved beryllium values in the aqueous medium, and (c) processing the dissolved beryllium values to produce a refined beryllium-containing product.
  • the fluorine-containing compound is an active fluorine-containing compound.
  • the fluorine-containing compound is a major component.
  • the fluorine-containing compound includes hydrofluoric acid. According to still further features in the described preferred embodiments, the fluorine-containing compound includes hydrofluoric acid. According to still further features in the described preferred embodiments, the reacting is performed at a pressure exceeding a pressure of one atmosphere absolute ( 1 ata).
  • the reacting is performed at a pressure exceeding a pressure of 1.5 atmospheres absolute (1.5 ata).
  • the reacting is performed at a pressure exceeding a pressure of two atmospheres absolute (2 ata). According to still further features in the described preferred embodiments, the reacting is performed at a pressure exceeding a pressure of three atmospheres absolute (3 ata).
  • the fluorine-containing compound includes silicon tetrafluoride.
  • the aqueous medium is an acidic aqueous medium.
  • the reaction stage yields a solid residue along with the aqueous medium
  • the process further including the step of: (d) separating at least a portion of the aqueous medium from the solid residue.
  • the beryllium feed source includes beryl.
  • the beryl is directly introduced to the reaction stage.
  • the reacting is performed at a temperature below 250°C.
  • the reacting is performed at a temperature below 220°C.
  • the reacting is performed at a temperature below 180°C. According to still further features in the described preferred embodiments, the reacting is performed at a temperature below 150°C.
  • the process further includes the step of: (d) introducing a second beryllium source, prior to step (c). so as to dissolve additional beryllium values and to consume at least a portion of any excess acid from step (b).
  • the second beryllium source includes a readily soluble beryllium feed source.
  • the second beryllium source is a readily soluble beryllium feed source.
  • the reacting is performed in a vessel that is fl ⁇ idly sealed from an outside environment.
  • reaction stage is performed at a temperature above 120°C and below 350°C.
  • Figure 1 is a block diagram of the inventive method for processing a beryllium feed source in an aqueous medium by means of a fluorine-containing acid such as hydrofluoric acid. DESCRIPTION OF THE PREFERRED EMBODIMENTS
  • the present invention is a method of treating a beryllium feed material, such as beryl, by reacting the beryllium feed material with a fluorine-containing compound in an acidic aqueous medium.
  • the beryllium feed source 6 largely or completely dissolves, leaving the highly soluble beryllium values (largely) in the liquid phase. Most of the other species are also dissolved in the liquid phase. If necessary, the reaction product mixture 18 produced in reaction stage 10 is subsequently subjected to a solid/liquid separation 20, to produce a residue 14 and a beryllium-rich solution 16. Residue 14 may be processed for further retrieval of beryllium values, or may be discarded. It must be emphasized that the production process of the present invention is appropriate for both batch and continuous modes of operation.
  • beryllium feed source 6 is a commercially-available ore containing beryl (3BeO-Al 2 ⁇ 3 -6Si0 2 ). bertrandite (4BeO-2SiO?-H 2 0), and/or phenakite (Be 2 Si0 4 ). Often, such commercially-available ores include additional minerals containing aluminum and iron oxides, calcium and alkali oxides or silicates and quartz. In reaction stage 10, various aluminum, silica, and iron-based minerals from beryllium feed source 6 tend to dissolve.
  • beryl is known to be the most difficult to dissolve.
  • beryllium feed source 6 will refer specifically to beryl.
  • sulfuric acid 12 may be added to reaction stage 10 to promote the dissolution of beryllium feed source 6, the addition of sulfuric acid 12 has been found to be unnecessary, as the dissolution proceeds essentially to completion at atmospheric or near-atmospheric pressures and at a temperature of about 100°C.
  • the temperature in the reaction stage is at least S0°C. and more preferably. above about 100°C.
  • hydrofluoric acid reacts with SiO? values to produce fluosilicic acid (H 2 SiF 6 ) and water according to the following stoichiometry:
  • Reaction stage 10 can be operated such that vapor stream 13, which may contain hydrofluoric acid, silicon tetrafluoride and water, is removed from reaction stage 10. Alternatively, vapor stream 13 can be refluxed back to the reaction mixture in reflux stream 15.
  • the dissolution of beryllium feed source 6, and more specifically, beryl is performed in a sealed vessel, autoclave, or the like (reaction stage 10), which is hermetically sealed from the environment (i.e., there is no vapor stream 13 being discharged from reaction stage 10).
  • reaction stage 10 a sealed vessel, autoclave, or the like
  • substantially all of the reaction volume is filled with the reaction mixture.
  • Substantially complete dissolution of the beryl can be effected using hydrofluoric acid 8. added in excess. Under such conditions, no addition of sulfuric acid 12 is needed. With increasing temperature, and for a fixed residence time, the fraction of dissolved beryllium increases. 5
  • reaction stage 10 Upon completion of reaction stage 10, a mixture of (excess) hydrofluoric acid and fluosilicic acid, together with the products of dissolution, is typically obtained. This mixture can be separated, and all the acids recovered, according to various processes known in the art.
  • reaction stage 10 26 is introduced to a second reaction stage 30 along with reaction product mixture 18 so as to dissolve beryllium values present in second beryllium source 26 as well as to allow additional beryllium values to be leached from any residue remaining from reaction stage 10. This is particularly advantageous in that at least a portion, and preferably substantially all of the excess acid from reaction stage 10 can be consumed,
  • Second beryllium source 26 preferably includes bertrandite, which has been found by the inventors to dissolve readily (substantially 100%) in the presence of these acids at moderate temperatures as low as 60°C - 110°C.
  • Other beryllium feed 0 sources that dissolve more readily than beryl may also be used in second beryllium source 26.
  • beryllium feed source' refers to a raw material, or combination of raw materials, containing beryllium.
  • Beryllium feed source specifically includes, but is 5 not limited to, materials containing beryl, bertrandite, and/or phenakite.
  • readily soluble beryllium feed source refers to a beryllium feed source that includes, but is not limited to, bertrandite, and/or phenakite.
  • readily soluble beryllium feed source is meant to specifically exclude beryl. .
  • the term "directly introduced to the reaction stage” and the like, used in conjunction with “beryllium feed source” refers to a beryllium feed source that is reacted with hydrofluoric acid, without first undergoing melting or other high-temperature treatments, and particularly, without undergoing high-temperature treatment at temperatures exceeding 600°C.
  • the particular operating conditions of the process of the present invention will understandably vary according to the composition of beryllium feed source 6, local process conditions, etc.
  • the high toxicity of beryllium introduces various safety and ecology issues into the production process.
  • the inhalation of beryllium particles or fumes can trigger acute or chronic lung disease of a serious nature.
  • the inventive process obviates the need for the high-temperature, multiple-stage thermal treatment, significantly reducing thereby the health risk to plant personnel and/or reducing the costs associated with maintaining the requisite high standard of air quality for beryllium production facilities.
  • the amount of beryllium dissolved is typically around 90%. In the inventive process, the amount of beryllium dissolved is typically up to 100%. under relatively mild conditions and reasonable residence times.
  • the finely-ground beryl used in Examples 1-5 contained: 13.08% BeO, 17.25% A1 2 0 3 , 63.91% Si0 2 , 0.91 % Fe 2 0 3. 0.19% MgO, 0.7% Na 2 0, 1.4% ZrO, 0.35% PbO.
  • the evaporate was completely refluxed (see stream 15 of
  • EXAMPLE 6 The beryl used in Example 6 contained 13.08% BeO, 17.25% A1 2 0 3: and 0.91 % Fe 2 0 3. To a Teflon® (polytetrafluoroethylene)-lined capsule having a reaction volume of 60 ml were added 12.2 grams of beryl and 58 ml of hydrofluoric acid (38% HF), such that the entire volume o ⁇ the capsule was filled with the reaction mixture. The non-agitated capsule was hermetically sealed and placed in an oven that was heated to 125°C for 20 hours ' . The capsule was then cooled and opened. The content of the capsule was filtered, and the solid residue was washed, dried and weighed.
  • Teflon® polytetrafluoroethylene
  • the beryl used in Example 7 contained 12.25% BeO. and 17.5% AI9O 3.
  • Example 7 The results of Example 7 are provided in Table 2.
  • Example 7 the only difference being that 20.0 grams of beryl were added to the capsule.
  • the results of Example 8 are provided in Table 2.
  • Example 9 The beryl used in Example 9 contained 12.25% BeO, 17.5 % A1 2 0 3 , and 1.0%? Fe 2 0 3 _ The beryl particles were ground to a size of -325 mesh (44 microns). To a stirred and heated reaction vessel were added 17.5 grams of beryl and 140ml of hydro fluoric acid (507o HF). The evaporate from the reaction vessel was completely refluxed (see stream 15 of Figure 1) to the reaction mixture. After three hours, the reaction mixture - which contained a small quantity of solids - was filtered. The solid residue was washed with distilled water, dried and weighed. From the results, solute material balances were calculated, wet residue weight: 1.64g dry residue weight: 1.06g filtrate and washing liquor weight: 263.7 g filtrate and washing liquor specific gravity: 1.163
  • the liquor was then boiled in an Erlenmeyer flask fluidly connected to a condenser. Solids precipitated in the reaction mixture. Fine solids (silica) were also deposited on the walls of the condenser. After 30 minutes, the reaction mixture was filtered. The wet solid residue, weighing 13.59 g, was dried. The dry residue, which largely consisted of A1F 3 -3H 2 0, weighed 9.33 g.
  • the concentration of Be in the solution was 15.41 g/1. From the solute material balances, it is evident that all the beryllium values remained in the aqueous phase.
  • the liquor remaining after sampling weighed 62.22 g.
  • the concentration of Be in the solution was 14.2 g/1, corresponding to a substantially
  • the solution produced can then be further processed [e.g., using processes known in the art, as outlined in Ullmann's Encyclopedia of Industrial Chemistry, Vol. 4a, Wiley-VCH Verlag GmbH & Co. (1985)] to produce various refined beryllium products, including, but not limited to, beryllium hydroxide and beryllium metal.
  • active used with respect to "fluorine-containing compound” and the like, is meant to include any material containing fluorine that is effective by itself, or in combination with another material (e.g., a concentrated acid), in the dissolution of a beryllium-containing mineral such as beryl, bertrandite. and/or phenakite.
  • active fluorine-containing compounds include hydrogen fluoride, silicon tetrafluoride (typically in concentrated acidic media), and fl ⁇ orosilicic acid.
  • major component used with respect to "fluorine-containing compound” and the like, refers to a fluorine-containing compound containing at least 3 wt.-% fluorine and/or resulting in a fluorine concentration in the reaction mixture of at least 2 wt.-% fluorine.
  • the fluorine-containing compound contains at least 10 wt.-% fluorine, more preferably, at least 15 wt.-% fluorine, and most preferably, at least 20 wt.-7o fluorine.

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  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Organic Chemistry (AREA)
  • Materials Engineering (AREA)
  • Geology (AREA)
  • Manufacturing & Machinery (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Mechanical Engineering (AREA)
  • Metallurgy (AREA)
  • Inorganic Chemistry (AREA)
  • General Life Sciences & Earth Sciences (AREA)
  • Geochemistry & Mineralogy (AREA)
  • Environmental & Geological Engineering (AREA)
  • Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)

Abstract

L'invention concerne un procédé de production pour la dissolution de béryllium dans une source d'alimentation en béryllium au moyen d'un composé contenant du fluor tel que l'acide fluorhydrique dans un milieu aqueux, comprenant les étapes consistant : (a) à fournir la source d'alimentation en béryllium ; (b) à faire réagir la source d'alimentation en béryllium avec le composé contenant du fluor dans une phase de réaction pour produire des éléments de valeur de béryllium dissous dans le milieu aqueux, et (c) à traiter les éléments de valeur de béryllium dissous pour produire un produit contenant du béryllium raffiné.
PCT/IL2003/000954 2002-11-12 2003-11-12 Procede de lixiviation d'elements de valeur de beryllium au moyen d'acide fluorhydrique WO2004043862A1 (fr)

Priority Applications (1)

Application Number Priority Date Filing Date Title
AU2003282349A AU2003282349A1 (en) 2002-11-12 2003-11-12 Method of leaching beryllium values using hydrofluoric acid

Applications Claiming Priority (4)

Application Number Priority Date Filing Date Title
IL15280202A IL152802A0 (en) 2002-11-12 2002-11-12 A method for leaching beryllium oxide from its ores
IL152802 2002-11-12
IL157764 2003-09-04
IL15776403A IL157764A0 (en) 2003-09-04 2003-09-04 Method of leaching beryllium values using hydrofluoric acid

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WO2004043862A1 true WO2004043862A1 (fr) 2004-05-27

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Cited By (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
RU2494964C1 (ru) * 2012-05-03 2013-10-10 Российская Федерация, от имени которой выступает Государственная корпорация по атомной энергии "Росатом" Способ получения фторида бериллия
RU2546945C1 (ru) * 2013-12-03 2015-04-10 Федеральное государственное автономное образовательное учреждение высшего профессионального образования "Уральский федеральный университет имени первого Президента России Б.Н. Ельцина Способ переработки смеси бериллиевых концентратов
RU2547060C1 (ru) * 2013-12-11 2015-04-10 Федеральное государственное автономное образовательное учреждение высшего профессионального образования "Уральский федеральный университет имени первого Президента России Б.Н. Ельцина Способ совместной переработки бериллиевых концентратов
CN106676285A (zh) * 2016-12-23 2017-05-17 江西合纵锂业科技有限公司 一种用于锂云母分解的混合酸及其浸出方法

Citations (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3879520A (en) * 1963-01-31 1975-04-22 Atomic Energy Commission Method for dissolving ceramic beryllia
US4729881A (en) * 1986-12-16 1988-03-08 Fmc Corporation Hydrometallurgical process for the production of beryllium

Patent Citations (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3879520A (en) * 1963-01-31 1975-04-22 Atomic Energy Commission Method for dissolving ceramic beryllia
US4729881A (en) * 1986-12-16 1988-03-08 Fmc Corporation Hydrometallurgical process for the production of beryllium

Cited By (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
RU2494964C1 (ru) * 2012-05-03 2013-10-10 Российская Федерация, от имени которой выступает Государственная корпорация по атомной энергии "Росатом" Способ получения фторида бериллия
RU2546945C1 (ru) * 2013-12-03 2015-04-10 Федеральное государственное автономное образовательное учреждение высшего профессионального образования "Уральский федеральный университет имени первого Президента России Б.Н. Ельцина Способ переработки смеси бериллиевых концентратов
RU2547060C1 (ru) * 2013-12-11 2015-04-10 Федеральное государственное автономное образовательное учреждение высшего профессионального образования "Уральский федеральный университет имени первого Президента России Б.Н. Ельцина Способ совместной переработки бериллиевых концентратов
CN106676285A (zh) * 2016-12-23 2017-05-17 江西合纵锂业科技有限公司 一种用于锂云母分解的混合酸及其浸出方法

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