Table 4. Water-Quality Criteria, Standards, Or Recommended Limits for Selected Properties and Constituents [All Standards Are from U.S
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Oregon Department of Human Services HEALTH EFFECTS INFORMATION
Oregon Department of Human Services Office of Environmental Public Health (503) 731-4030 Emergency 800 NE Oregon Street #604 (971) 673-0405 Portland, OR 97232-2162 (971) 673-0457 FAX (971) 673-0372 TTY-Nonvoice TECHNICAL BULLETIN HEALTH EFFECTS INFORMATION Prepared by: Department of Human Services ENVIRONMENTAL TOXICOLOGY SECTION Office of Environmental Public Health OCTOBER, 1998 CALCIUM CARBONATE "lime, limewater” For More Information Contact: Environmental Toxicology Section (971) 673-0440 Drinking Water Section (971) 673-0405 Technical Bulletin - Health Effects Information CALCIUM CARBONATE, "lime, limewater@ Page 2 SYNONYMS: Lime, ground limestone, dolomite, sugar lime, oyster shell, coral shell, marble dust, calcite, whiting, marl dust, putty dust CHEMICAL AND PHYSICAL PROPERTIES: - Molecular Formula: CaCO3 - White solid, crystals or powder, may draw moisture from the air and become damp on exposure - Odorless, chalky, flat, sweetish flavor (Do not confuse with "anhydrous lime" which is a special form of calcium hydroxide, an extremely caustic, dangerous product. Direct contact with it is immediately injurious to skin, eyes, intestinal tract and respiratory system.) WHERE DOES CALCIUM CARBONATE COME FROM? Calcium carbonate can be mined from the earth in solid form or it may be extracted from seawater or other brines by industrial processes. Natural shells, bones and chalk are composed predominantly of calcium carbonate. WHAT ARE THE PRINCIPLE USES OF CALCIUM CARBONATE? Calcium carbonate is an important ingredient of many household products. It is used as a whitening agent in paints, soaps, art products, paper, polishes, putty products and cement. It is used as a filler and whitener in many cosmetic products including mouth washes, creams, pastes, powders and lotions. -
Ocean Acidification and Oceanic Carbon Cycling 13
Ocean Acidification and Oceanic Carbon Cycling 13 Dieter A. Wolf-Gladrow and Bjo¨rn Rost Contents Atmospheric CO2 ............................................................................... 104 Air-Sea CO2 Exchange and Ocean Carbonate Chemistry ..................................... 104 Rate of Surface Ocean Acidification and Regional Differences .. ........................... 104 The Physical Carbon Pump and Climate Change .............................................. 105 Impact of Ocean Acidification on Marine Organisms and Ecosystems ....................... 106 The Biological Carbon Pump and Climate Change ............................................ 107 Take-Home Message ............................................................................ 108 References ....................................................................................... 109 Abstract The concentration of atmospheric CO2 is increasing due to emissions from burning of fossil fuels and changes in land use. Part of this “anthropogenic CO2” invades the oceans causing a decrease of seawater pH; this process is called “ocean acidification.” The lowered pH, but also the concomitant changes in other properties of the carbonate system, affects marine life and the cycling of carbon in the ocean. Keywords Anthropogenic CO2 • Seawater acidity • Saturation state • Climate change • Physical carbon pump • Global warming • Biological carbon pumps • Phyto- plankton • Primary production • Calcification D.A. Wolf-Gladrow (*) • B. Rost Alfred Wegener Institute, Helmholtz Centre -
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. -
Interaction of Calcium Supplementation and Nonsteroidal Anti-Inflammatory Drugs and the Risk of Colorectal Adenomas
2353 Interaction of Calcium Supplementation and Nonsteroidal Anti-inflammatory Drugs and the Risk of Colorectal Adenomas Maria V. Grau,1 John A. Baron,1,2 Elizabeth L. Barry,1 Robert S. Sandler,3 Robert W. Haile,4 Jack S. Mandel,5 and Bernard F. Cole1 Departments of 1Community and Family Medicine and 2Medicine, Dartmouth Medical School, Lebanon, New Hamsphire; 3Department of Medicine, University of North Carolina, Chapel Hill, North Carolina; 4Department of Preventive Medicine, University of Southern California, Los Angeles, California; and 5Department of Epidemiology, Rollins School of Public Health, Emory University, Atlanta, Georgia Abstract Background: Calcium and aspirin have both been found to be Results: In the Calcium Trial, subjects randomized to calcium chemopreventive against colorectal neoplasia. However, the who also were frequent users of NSAIDs had a reduction joint effect of the two agents has not been well investigated. of risk for advanced adenomas of 65% [adjusted risk ratio Methods: To explore the separate and joint effects of calcium (RR), 0.35; 95% confidence interval (95% CI), 0.13-0.96], and and aspirin/nonsteroidal anti-inflammatory drugs (NSAID), there was a highly significant statistical interaction between we used data from two large randomized clinical trials calcium treatment and frequent NSAID use (Pinteraction = among patients with a recent history of colorectal adenomas. 0.01). Similarly, in the Aspirin Trial, 81 mg aspirin and In the Calcium Polyp Prevention Study, 930 eligible subjects calcium supplement use together conferred a risk reduction were randomized to receive placebo or 1,200 mg of elemental of 80% for advanced adenomas (adjusted RR, 0.20; 95% CI, calcium daily for 4 years. -
Some Drugs Are Excluded from Medicare Part D, but Are Covered by Your Medicaid Benefits Under the Healthpartners® MSHO Plan (HMO)
Some drugs are excluded from Medicare Part D, but are covered by your Medicaid benefits under the HealthPartners® MSHO Plan (HMO). These drugs include some over‐the‐counter (OTC) items, vitamins, and cough and cold medicines. If covered, these drugs will have no copay and will not count toward your total drug cost. For questions, please call Member Services at 952‐967‐7029 or 1‐888‐820‐4285. TTY members should call 952‐883‐6060 or 1‐800‐443‐0156. From October 1 through February 14, we take calls from 8 a.m. to 8 p.m., seven days a week. You’ll speak with a representative. From February 15 to September 30, call us 8 a.m. to 8 p.m. Monday through Friday to speak with a representative. On Saturdays, Sundays and holidays, you can leave a message and we’ll get back to you within one business day. Drug Description Strength 3 DAY VAGINAL 4% 5‐HYDROXYTRYPTOPHAN 50 MG ABSORBASE ACETAMINOPHEN 500 MG ACETAMINOPHEN 120MG ACETAMINOPHEN 325 MG ACETAMINOPHEN 650MG ACETAMINOPHEN 80 MG ACETAMINOPHEN 650 MG ACETAMINOPHEN 160 MG/5ML ACETAMINOPHEN 500 MG/5ML ACETAMINOPHEN 160 MG/5ML ACETAMINOPHEN 500MG/15ML ACETAMINOPHEN 100 MG/ML ACETAMINOPHEN 500 MG ACETAMINOPHEN 325 MG ACETAMINOPHEN 500 MG ACETAMINOPHEN 80 MG ACETAMINOPHEN 100.00% ACETAMINOPHEN 80 MG ACETAMINOPHEN 160 MG ACETAMINOPHEN 80MG/0.8ML ACETAMINOPHEN‐BUTALBITAL 50MG‐325MG ACNE CLEANSING PADS 2% ACNE TREATMENT,EXTRA STRENGTH 10% ACT ANTI‐CAVITY MOUTH RINSE 0.05% Updated 12/01/2012 ACTICAL ACTIDOSE‐AQUA 50G/240ML ACTIDOSE‐AQUA 15G/72ML ACTIDOSE‐AQUA 25G/120ML ACTIVATED CHARCOAL 25 G ADEKS 7.5 MG -
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. -
Product Safety Summary
Product Safety Summary Calcium Carbonate CAS No. 497-34-1 This Product Safety Summary is intended to provide a general overview of the chemical substance. The information on the summary is basic information and is not intended to provide emergency response information, medical information or treatment information. The summary should not be used to provide in-depth safety and health information. In-depth safety and health information can be found on the Safety Data Sheet (SDS) for the chemical substance. Names Calcium carbonate Chalk Product Overview Solvay Fluorides, LLC does not sell calcium carbonate directly to consumers. Consumers may be exposed to calcium carbonate in many consumer product applications where the calcium carbonate is not transformed or reacted and is present in powder or granule form. Calcium carbonate is a white, granular or powdered solid. It is used primarily in construction, to make glass, production of polymer compounds as well as for acid gas treatment and pH adjustment. It is also used in the manufacture of other chemicals and pharmaceuticals. Exposure to calcium carbonate, especially powder, can cause irritation to the skin, eyes, and respiratory tract. Manufacture of Product Solvay Fluorides, LLC imports the calcium carbonate it sells from a Solvay affiliate in Europe. Solvay manufactures calcium carbonate by calcining (removing carbon dioxide) quarried marble to form lime (calcium oxide). Water is added to make calcium hydroxide and carbon dioxide (CO2) is passed through the solution to reform a purified calcium carbonate, which is then precipitated (crystallized) into its final form. Page 1 of 4 Copyright 2011-2013, Solvay America, Inc. -
The Investigation of Acetylsalicylic Acid, Sodium Bicarbonate, and Calcium Carbonate
CALIFORNIA STATE SCIENCE FAIR 2010 PROJECT SUMMARY Name(s) Project Number Irfan S. Habib J2113 Project Title The Investigation of Acetylsalicylic Acid, Sodium Bicarbonate, and Calcium Carbonate Abstract Objectives/Goals Does the amount of acetylsalicylic acid in various brands of aspirin tablets depend on the price of the aspirin tablet? Are CaCO3 (calcium carbonate) antacids or NaHCO3 (sodium bicarbonate) antacids more efficient in neutralizing stomach acidity? Does the strength of the base within an antacid depend on the price of the antacid? Methods/Materials A: Titration of Ammonia and Vinegar to obtain basic understanding of titration. B: Titration of aspirin and ammonia was performed to determine the normality (which is the concentration of H+ per 1 L of solution) of each aspirin brand. C: Titration of antacid tablets and vinegar was performed to determine the normality (which is the concentration of OH- per 1L of solution) of each antacid brand. D: Added antacid to 0.5M HCl 1g at a time and recorded pH after each gram was added in order to determine which antacid brand increased the pH of solution at a faster rate. Results A: Normality of Ammonia= 1.06 Normality of Vinegar = 0.83 B: St. Joseph#s was the most expensive aspirin and the Rite Aid brand was the least expensive; however, Ecotrin was the 3rd most expensive and it had the greatest H+ content. The Rite Aid brand had the least amount of H+ content. C: Alka-seltzer was most expensive antacid and Equaline was the least expensive. The Alka-seltzer and Rite Aid brand of antacids had greatest amount of OH- content (both had NaHCO3)and the Equaline (contained CaCO3)had least amount of OH-. -
Calcium Carbonate Dissolution and Precipitation in Water: Factors Affecting the Carbonate Saturometer Method
Utah State University DigitalCommons@USU All Graduate Theses and Dissertations Graduate Studies 5-1971 Calcium Carbonate Dissolution and Precipitation in Water: Factors Affecting the Carbonate Saturometer Method Lyle M. Dabb Utah State University Follow this and additional works at: https://digitalcommons.usu.edu/etd Part of the Chemistry Commons, and the Soil Science Commons Recommended Citation Dabb, Lyle M., "Calcium Carbonate Dissolution and Precipitation in Water: Factors Affecting the Carbonate Saturometer Method" (1971). All Graduate Theses and Dissertations. 2991. https://digitalcommons.usu.edu/etd/2991 This Thesis is brought to you for free and open access by the Graduate Studies at DigitalCommons@USU. It has been accepted for inclusion in All Graduate Theses and Dissertations by an authorized administrator of DigitalCommons@USU. For more information, please contact [email protected]. ACKNOWLEDGMENTS I would like to thank Dr. Jerome J . Jurinak for his patience and guidance during my classwork and lab experiments. I would also like t o thank Dr . R. L . Smith and Dr. H. B. Petersen for serving as committee members. I thank Robert A. Griffin and Dr. Sung-Ho Lai for their friendship, help, and encouragement. I thank Dr. John J. Hassett for his help when I started this research. Pa rtial support of this study by the Federal Water Quality Admin- istration is gr atefully acknowledged. I thank my wife, Sandy, for keeping our horne affairs running so smoothly and for her understanding and patience. ¥ m fJJt- Lyle M. Dabb TABLE OF CONTENTS Page INTRODUCTION 1 REVIEW OF LITERATURE 3 METHODS AND MATERIALS RESULTS AND DISCUSSION 10 EIGHT NATURAL WATERS FROM VERNAL, UTAH 31 SUMMARY AND CONCLUSIONS . -
Amorphous Calcium–Magnesium Carbonate (ACMC)
Amorphous Calcium–Magnesium Carbonate (ACMC) Accelerates Dolomitization at Room Temperature under Abiotic Conditions German Montes-Hernandez, François Renard, Anne-Line Auzende, Nathaniel Findling To cite this version: German Montes-Hernandez, François Renard, Anne-Line Auzende, Nathaniel Findling. Amorphous Calcium–Magnesium Carbonate (ACMC) Accelerates Dolomitization at Room Temperature under Abiotic Conditions. Crystal Growth & Design, American Chemical Society, 2020, 20 (3), pp.1434- 1441. 10.1021/acs.cgd.9b01005. hal-02896885 HAL Id: hal-02896885 https://hal.archives-ouvertes.fr/hal-02896885 Submitted on 5 Nov 2020 HAL is a multi-disciplinary open access L’archive ouverte pluridisciplinaire HAL, est archive for the deposit and dissemination of sci- destinée au dépôt et à la diffusion de documents entific research documents, whether they are pub- scientifiques de niveau recherche, publiés ou non, lished or not. The documents may come from émanant des établissements d’enseignement et de teaching and research institutions in France or recherche français ou étrangers, des laboratoires abroad, or from public or private research centers. publics ou privés. 1 Amorphous calcium-magnesium carbonate (ACMC) accelerates 2 dolomitization at room temperature under abiotic conditions 3 4 German Montes-Hernandeza *, François Renarda, b, Anne-Line Auzendea, Nathaniel Findlinga 5 6 a Univ. Grenoble Alpes, Univ. Savoie Mont Blanc, CNRS, IRD, IFSTTAR, ISTerre, 38000 7 Grenoble, France 8 b The Njord Centre, Department of Geosciences, University of Oslo, box 1048 Blindern, 0316 Oslo, 9 Norway 10 11 12 13 *Corresponding author: Dr. German Montes-Hernandez 14 E-mail address: [email protected] 15 1 16 Abstract 17 The challenge to produce dolomite CaMg(CO3)2 at low temperature (20-35°C) over laboratory time 18 scales remains so far unsuccessful, which has led to long-lasting scientific debates in the last two 19 centuries. -
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.