Magnesium and Magnesia from Brines
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
Alkalinity Management in Soilless Substrates and Landscape Architecture Roberto G
Purdue extension HO-242-W Commercial Greenhouse and Nursery Production Purdue Department of Horticulture Alkalinity Management in Soilless Substrates and Landscape Architecture Roberto G. Lopez and Michael V. Mickelbart, Purdue Horticulture and Landscape Architecture www.hort.purdue.edu Ohio State University Horticulture Claudio Pasian, Ohio State University Horticulture and Crop Science and Crop Science www.hcs.osu.edu Purdue Floriculture Greenhouse and nursery growers often assume yellow and pale leaves are signs of nutritional flowers.hort.purdue.edu deficiencies. Sometimes, however, the problem may be due to a lack of specific nutrients in the substrate — in other cases, the nutrients may be present but high substrate pH makes them unavailable to the plant. Growers commonly add sulfuric or other acids to irrigation water to help lower substrate pH or apply iron chelates to quickly “green up” their crops before shipping. Unfortunately, growers often do not have a clear understanding of the underlying causes behind increased substrate pH — water alkalinity, rather than water pH, is typically the source of the problem. The purpose of this publication is to help growers differentiate between high pH and high alkalinity and how to manage alkalinity in soilless substrates. What Is pH? The pH scale measures the concentration of hydrogen ions (H+) in a solution. Examples of solutions are tap water and the water in the substrate inside a pot. The pH scale ranges from 0 to 14. A value of 7.0, which is pure water, is neutral. Values less than 7.0 are called acidic, and values greater than 7 are called basic or alkaline. -
Summary Statistics for Selected Common Ions, Including Dissolved
Common Ions Precambrian Aquifers Summary statistics for selected common ions, Generally, water from the Precambrian aquifers including dissolved solids, calcium, magnesium, is fresh (less than 1,000 mg/L dissolved solids concen- sodium, percent sodium, sodium-adsorption ratio tration). Calcium and bicarbonate generally are dominant among the common ions. Water from the (SAR), potassium, bicarbonate, carbonate, sulfate, Precambrian aquifers has the highest median chloride chloride, fluoride, bromide, iodide, and silica, are concentration, lowest mean and median concentrations presented in table 4. The significance of the various of calcium, magnesium, and bicarbonate, and the common ions is described in table 1. Boxplots are pre- lowest median sulfate (equal to the Deadwood aquifer) sented in figure 16 for each of the common ions, except of the major aquifers. for carbonate. The water type for the various aquifers The water type of the Precambrian aquifers also is discussed in this section. Trilinear diagrams generally is a calcium bicarbonate or a calcium magne- (fig. 17) are presented for each of the aquifers. sium bicarbonate type but also can be a mixed type Changes in water type as ground water flows down- (fig. 17). The original rock mineralogy, degree of gradient are discussed for the Madison, Minnelusa, and metamorphism, and degree of weathering all can Inyan Kara aquifers. contribute to the variations in water type. Two of 56 samples from Precambrian aquifers Specific conductance can be used to estimate the exceed the SMCL of 500 mg/L for dissolved solids. concentration of dissolved solids using the equations Two of 112 samples exceed the SMCL of 250 mg/L for presented in table 5. -
( 12 ) United States Patent
US010682325B2 (12 ) United States Patent ( 10 ) Patent No.: US 10,682,325 B2 Comb et al. (45 ) Date of Patent : * Jun . 16 , 2020 (54 ) COMPOSITIONS AND METHODS FOR THE 3,988,466 A 10/1976 Takagi et al. TREATMENT OF LIVER DISEASES AND 4,496,703 A 1/1985 Steinmetzer 4,871,550 A 10/1989 Millman DISORDERS ASSOCIATED WITH ONE OR 4,898,879 A 2/1990 Madsen et al . BOTH OF HYPERAMMONEMIA OR 4,908,214 A 3/1990 Bobee et al. MUSCLE WASTING 5,028,622 A 7/1991 Plaitakis 5,034,377 A 7/1991 Adibi et al. 5,106,836 A 4/1992 Clemens et al . ( 71) Applicant: AXCELLA HEALTH INC . , 5,229,136 A 7/1993 Mark et al. Cambridge , MA (US ) 5,276,018 A 1/1994 Wilmore 5,348,979 A 9/1994 Nissen et al . (72 ) Inventors : William Comb , Melrose , MA (US ); 5,356,873 A 10/1994 Mark et al . Sean Carroll, Cambridge, MA (US ) ; 5,405,835 A 4/1995 Mendy Raffi Afeyan , Boston , MA (US ) ; 5,438,042 A 8/1995 Schmidl et al. 5,504,072 A 4/1996 Schmidl et al. Michael Hamill, Wellesley , MA (US ) 5,520,948 A 5/1996 Kvamme 5,571,783 A 11/1996 Montagne et al. (73 ) Assignee : AXCELLA HEALTH INC . , 5,576,351 A 11/1996 Yoshimura et al . Cambridge, MA (US ) 5,712,309 A 1/1998 Finnin et al . 5,719,133 A 2/1998 Schmidl et al. Subject to any disclaimer, the term of this 5,719,134 A 2/1998 Schmidl et al. -
Magnesium Recycling in the United States in 1998
FLOW STUDIES FOR RECYCLING METAL COMMODITIES IN THE UNITED STATES Magnesium Recycling in the United States in 1998 By Deborah A. Kramer Abstract......................................................................................................................................................................................................3 Introduction................................................................................................................................................................................................3 Global geologic occurrence of magnesium.........................................................................................................................................3 Production technology ........................................................................................................................................................................3 Uses.....................................................................................................................................................................................................4 Prices...................................................................................................................................................................................................6 Sources of magnesium scrap......................................................................................................................................................................6 Disposition of magnesium scrap ................................................................................................................................................................7 -
Distribution of Impurities in Magnesium Via Silicothermic Reduction
Distribution of impurities in magnesium production via silicothermic reduction Distribution of impurities in magnesium via silicothermic reduction Winny Wulandari1, M. Akbar Rhamdhani1, Geoffrey Brooks1, and Brian J. Monaghan2 1Faculty of Engineering and Industrial Sciences, Swinburne University of Technology John St, Hawthorn, Melbourne VIC, 3122, Australia 2Faculty of Engineering, University of Wollongong Northfield Ave, Wollongong NSW, 2522, Australia Abstract The desire for light weight materials, particularly in the automotive field, is fuelling greater magne- sium production. The Pidgeon process is currently the most widely used process for the production of magnesium. This batch process involves reduction of dolomite by ferro-silicon, carried out at temperature between 1100-1200oC under vacuum in a retort, producing magnesium vapour which is then cooled and collected as a condensate. The major attractions of the process are its simplicity and low capital cost; however, the process is also labour and energy intensive. The Magnetherm process is also a vacuum batch process based on similar chemistry but operates at higher tempera- tures with magnesia dissolved in a slag. Various operational issues relating to the batch and vacuum nature of the process have limited its development. Higher temperatures will improve the kinetics of the silicothermic reduction but will also promote greater impurities into the vapour. Thermody- namic analysis of the distribution of impurities during condensation of magnesium vapour has been carried using FactSage thermodynamic package. The results from the multi-stage equilibrium model show that at equilibrium it should be possible to condense solid impurities before the major- ity of the magnesium vapour is condensed below 750oC, depending on the operating pressure of the system and the particular chemistry of the process. -
The Solubility of Magnesium Carbonate in Aqueous Solutions of Certain
c THE SOLUBILITY OF MAGNESIUM CARBONATE IN AQUEOUS SOLUTIONS OF CERTAIN ELECTROLYTES I BY F. K. CAMERON AND A. SEIDEIJ, P The work herein described was done in connection with and for the most part antedated that upon the solubility of cal- cium carbonate in solutions of other salts, which has already been described.z The solubility of magnesium carbonate is obviously depen- dent upon the partial pressure of the carbon dioxide in the at- mosphere or gas phase in contact with the solution. This has led to the development of this investigation in three parts : I, When the solutions were in contact with ordinary atnios- pheric air containing a small and practically constant percent- age of carbon dioxide. 2. When the atmosphere in contact with the solutions con- tained practically nothing but carbon dioxide and water. 3. When the solutions were in contact with an atmosphere practically free from carbon dioxide. Under these several conditions the ratio of normal carbon- ate to hydrogen carbonate or bicarbonate for any given concen- tration of solution might be expected to vary greatly. Moreover, it was found, in the case of solutions of mag- nesium carbonate, that temperature changes frequently prodiiced relatively large changes in the solubility, and it was therefore necessary to take precautions to prevent variations in this re- spect during the progress of the work. Unless otherwise stated the work described here was done at 23' C. As is well known, solution studies of magnesium carbonate, when other salts are present, have always given great difficulty Published by the permission of the Secretary of Agriculture. -
US3099524.Pdf
3,099,524 United States Patent 0 Patented July 30, 1963 1 2 aluminium and magnesium with a mixture of sodium 3,099,524 hydroxide and sodium canbonate in appropriate amounts. ANTAClD CGMPOSITIONS The aluminium and magnesium salts are preferably the Frederick Grossmith, Pinner, England, assignor to chlorides. Beecham Research Laboratories Limited, Breutford, A further method for preparing the compounds of the Middlesex, England present invention is to suspend a magnesium hydroxo Filed June 28, 1960, Ser. No. 39,245 Claims priority, application Great Britain July 2, 1959 aluminate of the type disclosed in by said co?pending 6 Claims. (Cl. 23—l4) application Serial No. 842,042, ?led September 24, 1959, in a liquor containing bicarbonate ions. A suitable This invention relates to improvements in antacid 10 liquor is a dilute solution of magnesium bicarbonate. compositions and is particularly concerned with new A still further method for preparing the magnesium chemical compounds which have been found to have bicarbonate hydroxoaluminates, which method minimises desirable antacid properties being eminently suitable for the formation of a basic magnesium carbonate impurity, medicinal use for the treatment of gastric hyperacidity. is to react a solution containing aluminium and mag In my co-pending application Serial No. 842,042, ?led 15 nesium salts in appropriate amounts with sodium hy September 24, 1959, now abandoned, I have disclosed droxide at a suitable rate of delivery. An addition of certain novel compounds which are formed by reacting ‘sodium bicarbonate is made at an appropriate stage and aluminium and magnesium salts with caustic allcalis, in a ?nal addition of mixed sodium hydroxide and sodium which the magnesium content, expressed as Mg(OI-I)2, bicarbonate is made to precipitate all the magnesium lies between the approximate limits 2.5% to 75% by 20 without allowing the pH to rise too high. -
Mineral Carbonation and Industrial Uses of Carbon Dioxide 319 7
Chapter 7: Mineral carbonation and industrial uses of carbon dioxide 319 7 Mineral carbonation and industrial uses of carbon dioxide Coordinating Lead Author Marco Mazzotti (Italy and Switzerland) Lead Authors Juan Carlos Abanades (Spain), Rodney Allam (United Kingdom), Klaus S. Lackner (United States), Francis Meunier (France), Edward Rubin (United States), Juan Carlos Sanchez (Venezuela), Katsunori Yogo (Japan), Ron Zevenhoven (Netherlands and Finland) Review Editors Baldur Eliasson (Switzerland), R.T.M. Sutamihardja (Indonesia) 320 IPCC Special Report on Carbon dioxide Capture and Storage Contents EXECUTIVE SUMMARY 321 7.3 Industrial uses of carbon dioxide and its emission reduction potential 330 7.1 Introduction 322 7.3.1 Introduction 330 7.3.2 Present industrial uses of carbon dioxide 332 7.2 Mineral carbonation 322 7.3.3 New processes for CO2 abatement 332 7.2.1 Definitions, system boundaries and motivation 322 7.3.4 Assessment of the mitigation potential of CO2 7.2.2 Chemistry of mineral carbonation 323 utilization 333 7.2.3 Sources of metal oxides 324 7.3.5 Future scope 334 7.2.4 Processing 324 7.2.5 Product handling and disposal 328 References 335 7.2.6 Environmental impact 328 7.2.7 Life Cycle Assessment and costs 329 7.2.8 Future scope 330 Chapter 7: Mineral carbonation and industrial uses of carbon dioxide 321 EXECUTIVE SUMMARY This Chapter describes two rather different options for carbon and recycled using external energy sources. The resulting dioxide (CO2) storage: (i) the fixation of CO2 in the form of carbonated solids must be stored at an environmentally suitable inorganic carbonates, also known as ‘mineral carbonation’ or location. -
Effect of Some Deacidification Agents on Copper-Catalyzed Degrardation
Preservation Research and Testing Series No. 9501 Effect of Some Deacidification Agents on Copper-Catalyzed Degradation of Paper C. J. Shahani and F. H. Hengemihle Preservation Research and Testing office Preservation Directorate Library of Congress Washington, DC November 1995 Effect of Some Deacidifying Agents on Copper-Catalyzed Degradation of Paper Preservation Research and Testing Series No. 9501 November 1995 Page 1 of 12 Library of Congress ♦ Preservation Directorate www.loc.gov/preservation/ Effect of Some Deacidification Agents on Copper-Catalyzed Degradation of Paper Conservation of Historic and Artistic Works on Paper Organized by the Canadian Conservation Institute Ottawa, Canada, October 3-7, 1988 Introduction Paper conservators are all too familiar with artifacts in which iron gall ink or copper in verdigris pigment has caused severe deterioration of the paper base. But even trace concentrations of these metals, which are generally present in paper, contribute significantly to its aging by catalyzing oxidation reactions.1,2,3 Copper and iron contaminants can also cause foxing in paper.4,5 Williams and his co-workers observed that paper samples containing copper acetate, which degraded rapidly when aged at 90˚C and 50˚C relative humidity (RH), were stabilized appreciably after deacidification treatment with magnesium bicarbonate.3 However, deacidification by a Barrow two-step treatment with calcium hydroxide and calcium bicarbonate solutions did not stabilize against the degradative effect of copper acetate to a comparable -
Indcor Limited
INDCOR LIMITED TECHNICAL OVERVIEW OF THE PRODUCTION OF MAGNESIUM METAL BY THE CARBOTHERMERIC ROUTE AND A PRELIMINARY ASSESSMENT OF THE MTL TECHNOLOGY CONFIDENTIAL AUGUST 2003 PREPARED BY PROCESS TECHNOLOGIES AUSTRALIA PTY LTD ABN 82 315 791 707 PO Box 210, Deloraine, Tasmania 7304, Australia Tel: (03) 63 623 202 Fax: (03) 63 623 437 Mob: 0419 553 256 [email protected] DISCLAIMER This document has been prepared for Indcor Limited (Indcor) by Process Technologies Australia Pty Ltd (PTA) based on information supplied by Indcor, information supplied by Magnesium Technologies Limited (MTL), and additional information that is in the public domain in the form of technical papers, reports, patents and patent applications. PTA is not in a position to, and does not, verify the accuracy of, or adopt as its own, the information and data supplied by or sourced from others. PTA does not accept any legal responsibility to any person, organisation or company for any loss or damage suffered resulting from reliance on this report however caused, and whether by breach of contract, negligence or otherwise. CONTENTS DISCLAIMER EXECUTIVE SUMMARY 1 INTRODUCTION 2 SCOPE OF WORK 3 INFORMATION SOURCES 4 THERMAL REDUCTION OF MAGNESIUM OXIDE 4.1 Basic Principles 4.2 Current Status of the Carbothermic Route 5 THE MTL TECHNOLOGY 5.1 Background 5.2 Process Proving at the Laboratory Scale 5.3 Process Proving at the Demonstration Scale 5.4 Independent Review of Testwork Data and Proposed Development Strategy 5.5 MTL Propriety Know-How 5.6 Comparison with Alternative -
Magsonic™ Carbothermal Technology Compared with the Electrolytic and Pidgeon Processes
Magnesium Technology 2012 Edited by: Suveen N. Mathaudhu, Wim H. Sillekens, Neale ft Neelameggham, and Norbert Hort TMS (The Minerals, Metals Λ Materlab Society), 2012 MAGSONIC™ CARBOTHERMAL TECHNOLOGY COMPARED WITH THE ELECTROLYTIC AND PIDGEON PROCESSES Leon H. Prentice1; Nawshad Haque1 'CSIRO Process Science and Engineering; Box 312; Clayton South, VIC, 3169, Australia Keywords: Carbothermal Magnesium, Carbothermic Reduction, Pidgeon Process, Silicothermic Magnesium, Electrolysis, Technology Comparison, Techno-Economic Evaluation, Environmental Impact, Life Cycle Analysis Abstract Magnesium Production Technologies A broad technology comparison of carbothermal magnesium production with present technologies has not been previously Electrolytic Production presented. In this paper a comparative analysis of CSlRO"s MagSonic™ process is made with the electrolytic and Pidgeon Historically, the electrolytic process was dominant from the start processes. The comparison covers energy intensity (GJ/tonne of commercial production up until the 1990s. Significant Mg), labor intensity (person-hours/tonne Mg), capital intensity production facilities were constructed around the world, the (USD/tonne annual Mg installed capacity), and Global Warming largest of which was Dow's plant at Freeport, TX. Presently, Potential (GWP, tonnes C02-equivalent/tonne Mg). Carbothermal magnesium is produced using the electrolytic process in the technology is advantageous on all measures except capital United States, Russia, Ukraine, and Israel, with potential start-up intensity (where it is roughly twice the capital cost of a similarly- in China. sized Pidgeon plant). Carbothermal and electrolytic production can have comparatively low environmental impacts, with typical While there are a number of variations of the electrolytic process, emissions one-sixth those of the Pidgeon process. Despite recent all now electrolyze anhydrous magnesium chloride or carnallite. -
For Production of Magnesium Via the Pidgeon Process
Mineral Processing & Extractive Metall. Rev., 33: 316–326, 2012 Copyright # Taylor & Francis Group, LLC ISSN: 0882-7508 print=1547-7401 online DOI: 10.1080/08827508.2011.601478 EVALUATION OF ZEFREH DOLOMITE (CENTRAL IRAN) FOR PRODUCTION OF MAGNESIUM VIA THE PIDGEON PROCESS Behzad Mehrabi1, Masud Abdellatif2, and Fariborz Masoudi3 1Geology Department, Tehran Tarbiat Moallem University, Tehran, Iran 2Mintek Corporate, Randburg, South Africa 3Faculty of Earth Sciences, Shahid Beheshti University, Tehran, Iran This study evaluates the production of magnesium metal from the Zefreh dolomite ore of Central Iran using the Pidgeon process. The investigation consisted of mineralogical and chemical characterization of the dolomite ore, calcining, chemical characterization, LOI (loss on ignition) determination, reduction tests on the calcined dolomite (dolime), using Iranian (Semnan) ferrosilicon and mineralogical, and chemical characterization of the reactants and products. Calcining of dolomite samples was carried out at approximately 1400 C in order to remove CO2, moisture, and other easily volatilized impurities. The dolime was then milled, along with ferrosilicon, thoroughly mixed, and briquetted. The briquettes were heated at 1125C–1150C and 500 Pa in a tube reactor for 10–12 hours to extract the magnesium. The ferrosilicon to dolime ratio was determined based on the chemical analyses of the two reactants, using as a guide, and Mintek’s Pyrosim software package. Magnesium extraction varied with ferrosilicon addition and with the dolime used,