DOCSLIB.ORG

(12) Patent Application Publication (10) Pub. No.: US 2011/0251399 A1 Dingerdissen Et Al

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
(12) Patent Application Publication (10) Pub. No.: US 2011/0251399 A1 Dingerdissen Et Al US 2011 O251399A1 (19) United States (12) Patent Application Publication (10) Pub. No.: US 2011/0251399 A1 Dingerdissen et al. (43) Pub. Date: Oct. 13, 2011 (54) METHOD FOR PRODUCING ALDEHYDES (86). PCT No.: PCT/EP10/50772 AND KETONES FROM PRIMARY AND SECONDARY ALCOHOLS S371 (c)(1), (2), (4) Date: Jun. 20, 2011 (75) Inventors: Uwe Dingerdissen, Seeheim (DE); (30) Foreign Application Priority Data Jan Pfeffer, Essen (DE); Thomas Tacke, Alzenau (DE); Thomas Feb. 6, 2009 (DE) ....................... 10 2009 OOO662.1 Haas, Muenster (DE); Harald Publication Classification Schmidt, Muelheim an der Ruhr (51) Int. Cl. (DE); Florian Klasovsky, Haltern C07D 40/04 (2006.01) am See (DE); Roger Sheldon, C07C 45/78 (2006.01) Hoog-Kappel (NL); Michiel C07D 307/68 (2006.01) Janssen, Den Haag (NL); Michael CD7C 45/82 (2006.01) Volland, Duelmen (DE); Michael CD7C 45/38 (2006.01) Rimbach, Herne (DE); Stefanie CD7C 45/6 (2006.01) Rinker, Huenxe (DE) CD7C 45/8 (2006.01) (52) U.S. Cl. ...................... 546/276.4:568/354:568/397; (73) Assignee: EVONIK DEGUSSA GMBH, 568/471; 549/498 ESSEN (DE) (57) ABSTRACT The invention relates to a method for producing aldehydes (21) Appl. No.: and ketones from easily accessible primary and secondary 13/140,921 alcohols by oxidation with atmospheric oxygen or pure oxy gen using a catalyst system which consists of a derivative of (22) PCT Filed: Jan. 25, 2010 a free nitroxyl radical. Patent Application Publication Oct. 13, 2011 Sheet 2 of 10 US 2011/0251399 A1 Fig. 2: Oxidation of isomannitol with with AA-Tempo/nitrite/nitrate Oxygen eeJW Xee 000,000|- 000’00!.-- 000'00/— | 000'009-- 000006, 000'009–-------------------------------------+---- |---- 000'008+/ 000'009–—————————Á----- 000'007-7—~~~ ~~~~---- O-------~~~~4%…• 00?.080907 Š C. O O If u Oeulueouoso Patent Application Publication Oct. 13, 2011 Sheet 3 of 10 US 2011/0251399 A1 Fig. 3 --e-Diketa-e-looketo--sosorbide - - - - --Cyfy. - -- keto -g-konsketc. --S&Soft).ds -- (oft, C 4. 9. 8 gtra 3003) - - - s 5G 2000 t 2 O 2 OQ ... O 10 9. 8 arx 70 60 50 it 208 30an 38 || 58 {{ 2 13 O 30 SO SO 2 EC 80 2G Time (min) Patent Application Publication Oct. 13, 2011 Sheet 4 of 10 US 2011/0251399 A1 Figure 4: Oxidation of 2-propanol with AA-TEMPO/nitric acid/oxygen -e-2-Propanol -a-Acetone.--Isopropyl acetate 100 80 60 40 20 O Timeh) Patent Application Publication Oct. 13, 2011 Sheet 5 of 10 US 2011/0251399 A1 Figure 5: Oxidation of 1-propanol with AA-TEMPO/nitric acid/oxygen -o-1-Propanol -- Propanal -- Propy acetate 100 Timeh Patent Application Publication Oct. 13, 2011 Sheet 6 of 10 US 2011/0251399 A1 Figure 6. Oxidation of cyclohexanol with AA-TEMPO/nitric acid/oxygen |-o- Cyclohexanol -A - Cyclohexanone -- Cyclohexyl acetate 80 60 40 20 O Time (h) Patent Application Publication Oct. 13, 2011 Sheet 7 of 10 US 2011/0251399 A1 Figure 7. Oxidation of furfuryl alcohol with AA-TEMPO/nitric acid/oxygen -o- Furfury alcohol -- Furtural --Furfural acetate 100 80 SS: 60 40 20 O Patent Application Publication Oct. 13, 2011 Sheet 8 of 10 US 2011/0251399 A1 Figure 8. Oxidation of 1,3-dihydroxycyclohexane with AA-TEMPO/nitric acid/oxygen -o- 1 3-Dihydroxycyclohexane -A-3-hydroxycyclohexanone -- 2-Cyclohexenone 100 SS 80 : 60 40 20 O O 1 2 3 Patent Application Publication Oct. 13, 2011 Sheet 9 of 10 US 2011/0251399 A1 Figure 9. Oxidation of nicotinyl alcohol with AA-TEMPO/nitric acid/oxygen -e-Nicotinyl alcohol -- Nicotinaldehyde |-- Nicotinyl acetate 1 OU 80 60 40 20 O Timeh) Patent Application Publication Oct. 13, 2011 Sheet 10 of 10 US 2011/0251399 A1 Figure 10: Oxidation of borneol with AA-TEMPO/nitric acid/oxygen -e-Borneol -d- Menthol -- Bornyl acetate 100 :O O Time (h) US 2011/025 1399 A1 Oct. 13, 2011 METHOD FOR PRODUCING ALDEHYDES wherein nitric acid is used as a further reagent. However, the AND KETONES FROM PRIMARY AND ketone yields reported are below 90% and conversions were SECONDARY ALCOHOLS only between 24 and 72% in the case of the aldehydes. This method is more useful for synthesizing carboxylic acids (U.S. Pat. No. 5,239,116). It is only when nitric acid is used as a 0001. The present invention describes a process for pro Stoichiometric reagent, i.e., when oxygen is omitted as an ducing aldehydes and ketones from inexpensively available inexpensive oxidant (U.S. Pat. No. 5,155,279), conversions primary and secondary alcohols by oxidation with atmo of 42-84% are reported at selectivities of 69-81%. spheric oxygen or pure oxygen using a catalyst system con 0009. The prior art processes have the disadvantage that sisting of a free nitroxyl radical derivative. they are frequently unsuitable for large scale industrial pro 0002 Stable nitroxyl radical derivatives were first duction of aldehydes and ketones owing to the low yields and described by Hoffmann (A. K. Hoffmann, A.T. Henderson, J. many process steps or the Stoichiometric use of costly, cor Am. Chem. Soc. 83 (1961) 4671) and Lebeder (O. L. Leb rosive and poisonous reagents. Particularly the addition of eder, S.N. Kazarnovski, Zh. Obshch. Khim. 30 (1960) 1631; halogen Sources which is needed in the nitroxyl radical-cata O. L. Lebeder, S. N. Kazarnovski, C A 55 (1961) 1473a.). lyzed reaction of alcohols, in conjunction with carboxylic They were first used as radical Scavengers. Their usefulness acids, but also in organic solvents, is an extremely corrosive as catalysts for the oxidation of alcohols was only discovered system which makes implementation on an industrial scale recently (e.g., J. M. Bobbitt, C. L. Flores, Heterocycles 27 difficult. Alternatively, poisonous and difficult-to-remove (1988) 509 or A. E. J. de Nooy, A. C. Besemer, H. van transition metals are frequently used as catalyst constituent. Bekkum, Synthesis (1996) 1153). 0010. It is an object of the present invention to provide a 0003. One disadvantage with this type of catalysis is that process for producing aldehydes and ketones which allows the oxygen required for oxidation frequently is generated the use of primary or secondary alcohols as a starting material from expensive sources of oxygen. The use of hypochlorite, and which is such that the addition of halogen sources, more chloroperbenzoic acid, peroxomonosulfuric acid, periodic particularly bromine sources and the use of transition metals acid or trichloroisocyanuric acid for example has been can be dispensed with. reported (e.g. L. Anelli, C. Biffi, F. Montanari, S. Quici, J. 0011 We have found that this object is achieved, surpris Org. Chem. 52 (1987) 2559; J. A. Cella, J. A. Kelley, E. F. ingly, by a process for producing aldehydes and ketones Kenehan, J. Org. Chem. 40 (1975) 1850; S. D. Rychovsky, R. which allows the use of primary and secondary alcohols as a Vaidyanathan, J. Org. Chem. 64 (1999) 310: Bolm, Carsten; starting material and which overcomes precisely the above Magnus, Angelika S.; Hildebrand, Jens P. Organic Letters mentioned disadvantages of the prior art. (2000), 208), 1173-1175: S. S. Kim, K. Nehru, Synletter 0012. The present invention accordingly provides a pro (2002) 616; De Luca, Lidia; Giacomelli, Giampaolo; cess for producing aldehydes and ketones comprising the Porcheddu, Andrea. Organic Letters (2001), 3(19), 3041 oxidation of primary or secondary alcohols with an oxygen 3043). In addition, many of the reagents mentioned contain containing gas in the presence of a catalyst composition com halogens (chlorine, bromine and iodine in particular) which, prising at least one nitroxyl radical, one or more NO sources under the reaction conditions, can have a corrosive effect and and at least one or more carboxylic acids oranhydrides and/or often lead to undesired secondary reactions. mineral acids or anhydrides, optionally in the presence of one 0004. The oxidation of alcohols with oxygen by using or more solvents, characterized in that the primary and sec nitroxyl radical derivatives is accomplished through addition ondary alcohols used have a value of less than 2 for the of transition metals, for example cobalt, copper, tungsten, decadic logarithm of the n-octanol-water partition coefficient ruthenium, manganese and iron (e.g., Sheldon Roger A.; (log P), and in that the aldehydes and ketones are preferably Arends, Isabel W. C. E. Journal of Molecular Catalysis A: obtained in a yield of more than 92%, based on the alcohol Chemical (2006), 251(1-2), 200-214; Minisci, Francesco; used. Punta, Carlo: Recupero, Francesco. Journal of Molecular 0013 The process of the present invention has the advan Catalysis A: Chemical (2006), 251(1-2), 129-149). One dis tage that the alcohol is oxidized using a mild method in the advantage with this method is the frequently difficult removal presence of nitroxyl radicals in a single process step. This of the transition metal salts and their toxic properties. mild method Surprisingly makes it possible to oxidize even 0005 Augustine (U.S. Pat. No. 7,030,279) describes in sterically hindered alcohols which are not available using general the oxidation of primary or secondary alcohols with other methods. This oxidation frequently provides almost oxygen as oxidant to the corresponding aldehydes and quantitative conversions and selectivities, i.e., the high yields ketones using a catalyst system consisting of a free nitroxyl testify to the high efficiency of the process according to the radical derivative, a nitrate Source, a bromine source and a present invention. This high efficiency is completely Surpris carboxylic acid, which is acetic acid in all cases. ing on the basis of the prior art. 0006 Xinquan Hu et al. describe in J. AM. CHEM. SOC. 0014 More particularly, corrosive sources of halogen are 2004, 126, 4112-41 13 the alcohol oxidation using nitroxyl avoided as is the use of transition metals, and the Substrate radical derivative and oxygen, wherein the nitrate source was which constitutes the NO source is adjusted to the particular replaced by a nitrite source.
Load more

Recommended publications
  • Cyanide Remediation: Current and Past Technologies C.A
    CYANIDE REMEDIATION: CURRENT AND PAST TECHNOLOGIES C.A. Young§ and T.S. Jordan, Department of Metallurgical Engineering, Montana Tech, Butte, MT 59701 ABSTRACT Cyanide (CN-) is a toxic species that is found predominantly in industrial effluents generated by metallurgical operations. Cyanide's strong affinity for metals makes it favorable as an agent for metal finishing and treatment and as a lixivant for metal leaching, particularly gold. These technologies are environmentally sound but require safeguards to prevent accidental spills from contaminating soils as well as surface and ground waters. Various methods of cyanide remediation by separation and oxidation are therefore reviewed. Reaction mechanisms are given throughout. The methods are compared in regard to their effectiveness in treating various cyanide species: free cyanide, thiocyanate, weak-acid dissociables and strong-acid dissociables. KEY WORDS cyanide, metal-cyanide complex, thiocyanate, oxidation, separation INTRODUCTION ent on the transport of these heavy metals through their tissues, cyanide is very toxic. Waste waters from industrial operations The mean lethal dose to the human adult is transport many chemicals that have ad- between 50 and 200 mg [2]. U.S. EPA verse effects on the environment. Various standards for drinking and aquatic-biota chemicals leach heavy metals which would waters regarding total cyanide are 200 and otherwise remain immobile. The chemicals 50 ppb, respectively, where total cyanide and heavy metals may be toxic and thus refers to free and metal-complexed cya- cause aquatic and land biota to sicken or nides [3]. According to RCRA, all cyanide species are considered to be acute haz- die. Most waste-water processing tech- ardous materials and have therefore been nologies that are currently available or are designated as P-Class hazardous wastes being developed emphasize the removal of when being disposed of.
    [Show full text]
  • Acids and Bases
    Name Date Class CHAPTER 14 REVIEW Acids and Bases SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Name the following compounds as acids: sulfuric acid a. H2SO4 sulfurous acid b. H2SO3 hydrosulfuric acid c. H2S perchloric acid d. HClO4 hydrocyanic acid e. hydrogen cyanide 2. H2S Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas for the following acids: HNO2 a. nitrous acid HBr b. hydrobromic acid H3PO4 c. phosphoric acid CH3COOH d. acetic acid HClO e. hypochlorous acid 4. Calcium selenate has the formula CaSeO4. H2SeO4 a. What is the formula for selenic acid? H2SeO3 b. What is the formula for selenous acid? 5. Use an activity series to identify two metals that will not generate hydrogen gas when treated with an acid. Choose from Cu, Ag, Au, Pt, Pd, or Hg. 6. Write balanced chemical equations for the following reactions of acids and bases: a. aluminum metal with dilute nitric acid ϩ → ϩ 2Al(s) 6HNO3(aq) 2Al(NO3)3(aq) 3H2(g) b. calcium hydroxide solution with acetic acid ϩ → ϩ Ca(OH)2(aq) 2CH3COOH(aq) Ca(CH3COO)2(aq) 2H2O(l ) MODERN CHEMISTRY ACIDS AND BASES 117 Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class SECTION 1 continued 7. Write net ionic equations that represent the following reactions: a. the ionization of HClO3 in water ϩ → ϩ ϩ Ϫ HClO3(aq) H2O(l ) H3O (aq) ClO3 (aq) b. NH3 functioning as an Arrhenius base ϩ → ϩ ϩ Ϫ NH3(aq) H2O(l ) ← NH4 (aq) OH (aq) 8.
    [Show full text]
  • Combining Sodium Bicarbonate and Lidocaine Injection
    Combining Sodium Bicarbonate and Lidocaine injection Tom Simpleman Consultant Pharmacist the FAWKS company http://dailymed.nlm.nih.gov/dailymed/lookup.cfm?setid=f9c826a7‐8f19‐4857‐b5be‐11dcafcfc7a9 Referenced information from National Institutes of Health DESCRIPTION: Sodium Bicarbonate Inj., 8.4% USP Neutralizing Additive Solution is a sterile, nonpyrogenic, solution of sodium bicarbonate (NaHCO3) in Water for Injection. It is added to an appropriate local anesthetic as a neutralizing agent immediately prior to administration. The solution contains no bacteriostat, antimicrobial agent or added buffer and is intended only for single-use. pH is adjusted with carbon dioxide. Per the USP monograph for Sodium Bicarbonate Inj., pH is between 7.0 and 8.5. Osmolar concentration is 2 mOsmol/mL (calc.). Sodium bicarbonate, 84 mg is equal to one milliequivalent each of Na+ and HCO3-. Sodium Bicarbonate, USP is chemically designated as NaHC03, a white crystalline powder soluble in water. Sodium bicarbonate in water dissociates to provide sodium (Na+) and bicarbonate (HCO3-) ions. Sodium (Na+) is the principal cation of the extracellular fluid and plays a large part in the therapy of fluid and electrolyte disturbances. Bicarbonate (HCO3-) is a normal constituent of body fluids and the normal plasma level ranges from 24 to 31 mEq/liter. Bicarbonate anion is considered “labile” since at a proper concentration of hydrogen ion (H+) it may be converted to carbonic acid (H2CO3) and thence to its volatile form, carbon dioxide (CO2) excreted by the lung. Normally a ratio of 1:20 (carbonic acid; bicarbonate) is present in the extracellular fluid. In a healthy adult with normal kidney function, practically all the glomerular filtered bicarbonate ion is reabsorbed; less than 1% is excreted in the urine.
    [Show full text]
  • Important Prescribing Information
    Important Prescribing Information Subject: Temporary importation of 8.4% Sodium Bicarbonate Injection to address drug shortage issues June 14, 2019 Dear Healthcare Professional, Due to the current critical shortage of Sodium Bicarbonate Injection, USP in the United States (US) market, Athenex Pharmaceutical Division, LLC (Athenex) is coordinating with the U.S. Food and Drug Administration (FDA) to increase the availability of Sodium Bicarbonate Injection. Athenex has initiated temporary importation of another manufacturer’s 8.4% Sodium Bicarbonate Injection (1 mEq/mL) into the U.S. market. This product is manufactured and marketed in Australia by Phebra Pty Ltd (Phebra). At this time, no other entity except Athenex Pharmaceutical Division, LLC is authorized by the FDA to import or distribute Phebra’s 8.4% Sodium Bicarbonate Injection, (1 mEq/mL), 10 mL vials, in the United States. FDA has not approved Phebra’s 8.4% Sodium Bicarbonate Injection but does not object to its importation into the United States. Effective immediately, and during this temporary period, Athenex will offer the following presentation of Sodium Bicarbonate Injection: Sodium Bicarbonate Injection, 8.4% (1mEq/mL), 10mL per vial, 10 vials per carton Ingredients: sodium bicarbonate, water for injection, disodium edetate and sodium hydroxide (pH adjustment) Marketing Authorization Number in Australia is: 131067 Phebra’s Sodium Bicarbonate Injection contains the same active ingredient, Sodium Bicarbonate, in the same strength and concentration, 8.4% (1 mEq/mL) as the U.S. registered Sodium Bicarbonate Injection, USP by Pfizer’s subsidiary, Hospira. However, it is important to note that Phebra’s Sodium Bicarbonate Injection (1 mEq/mL), is provided only in a Single Use 10 mL vials, whereas Hospira’s product is provided in 50 mL single-dose vials and syringes.
    [Show full text]
  • UNITED STATES PATENT OFFICE. ">Co
    UNITED STATES PATENT OFFICE. LEONHARD LEDERER, OF MUNICH, GERMANY. PROCESS OF PRE PARNG HAO D DERVATIVES OF ACET ONE. SPECIFICATION forming part of Letters Patent No. 643,144, dated February 13, 1900. Application filed August 10, 1897, Serial No. 647,759. (No specimens.) To all livhon, it nay conce77: iodacetone. Also if not kept dry it some Beit known that I, LEONHARDLEDERER, a times undergoes decomposition at an ordi citizen of the Kingdom of Bavaria, residing nary temperature, thereby evolving so much SO at Munich, Bavaria, Germany, have invented heat that vapor of iodin is set free. Alco a new and useful Process of Preparing the hol, ether, and most of the organic solvents IIalogen Derivatives of Acetone, of which the set free iodin from per-iod-acetone. With following is a specification. dilute soda-lye it forms iodoform in the cold. 55 It is well known that the halogens act read The action of iodin on acetone-dicarbonic. ily upon acetonedicarbonic acid. For in acid can be so regulated by definite diminu stance, bromin added to an aqueous solution tions of the quantity of iodin added as to re of acetonedicarbonic acid is immediately sult in lower stages of iodin combination with taken up. An aqueous solution of acetonedi acetone. With regard to its behavior toward carbonic acid decomposed with an alcoholic alcohol and ether the penta-iod derivative is iodin solution takes up quickly the color of in close relation with the periodacetone. On the latter without visible reaction. If, how the addition of dilute soda-lye it is trans ever, this mixture be gently Warmed, reac formed into iodoform even in the cold, but tion takes place, evolving carbonic acid gas; not with the soda solution.
    [Show full text]
  • Structure and Functioning of the Acid–Base System in the Baltic Sea
    Earth Syst. Dynam., 8, 1107–1120, 2017 https://doi.org/10.5194/esd-8-1107-2017 © Author(s) 2017. This work is distributed under the Creative Commons Attribution 3.0 License. Structure and functioning of the acid–base system in the Baltic Sea Karol Kulinski´ 1, Bernd Schneider2, Beata Szymczycha1, and Marcin Stokowski1 1Institute of Oceanology, Polish Academy of Sciences, IO PAN, ul. Powstanców´ Warszawy 55, 81-712 Sopot, Poland 2Leibniz Institute for Baltic Sea Research Warnemünde, IOW, Seestrasse 15, 18119 Rostock, Germany Correspondence: Karol Kulinski´ ([email protected]) Received: 6 April 2017 – Discussion started: 12 April 2017 Revised: 21 October 2017 – Accepted: 6 November 2017 – Published: 11 December 2017 Abstract. The marine acid–base system is relatively well understood for oceanic waters. Its structure and func- tioning is less obvious for the coastal and shelf seas due to a number of regionally specific anomalies. In this review article we collect and integrate existing knowledge of the acid–base system in the Baltic Sea. Hydro- graphical and biogeochemical characteristics of the Baltic Sea, as manifested in horizontal and vertical salinity gradients, permanent stratification of the water column, eutrophication, high organic-matter concentrations and high anthropogenic pressure, make the acid–base system complex. In this study, we summarize the general knowledge of the marine acid–base system as well as describe the peculiarities identified and reported for the Baltic Sea specifically. In this context we discuss issues such as dissociation constants in brackish water, differ- ent chemical alkalinity models including contributions by organic acid–base systems, long-term changes in total alkalinity, anomalies of borate alkalinity, and the acid–base effects of biomass production and mineralization.
    [Show full text]
  • Alternative Solvents for Catalysis and Organic Reactions
    ALTERNATIVE SOLVENTS FOR CATALYSIS AND ORGANIC REACTIONS A Thesis Presented to The Academic Faculty By Vittoria Madonna Blasucci In Partial Fulfillment of the Requirements for the Degree Doctor of Philosophy in Chemical & Biomolecular Engineering Georgia Institute of Technology December 2009 ALTERNATIVE SOLVENTS FOR CATALYSIS AND ORGANIC REACTIONS Dr. Charles A. Eckert, Advisor School of Chemical & Biomolecular Engineering Georgia Institute of Technology Dr. Charles L. Liotta, Co-Advisor School of Chemistry & Biochemistry Georgia Institute of Technology Dr. William Koros School of Chemical & Biomolecular Engineering Georgia Institute of Technology Dr. Christopher Jones School of Chemical & Biomolecular Engineering Georgia Institute of Technology Dr. Amyn Teja School of Chemical & Biomolecular Engineering Georgia Institute of Technology Date Approved: September 30th 2009 For my Mom and Dad- Without them I would have never made it through ACKNOWLEDGEMENTS First, I would like to acknowledge my advisor, Prof. Charles Eckert. Under his guidance, I was given the freedom to take my research into the areas that interest me the most. Not only is he a valuable information source, but he is also an excellent mentor. In addition, I thank my co-advisor, Prof. Charles Liotta. It has been my pleasure to work with someone who truly loves what they do and refreshing to see somebody who enjoys science so much. Due to these two professors, my time at Georgia Tech has been excellent. I greatly appreciate the time and advice of my committee members: Professors Amyn Teja, Bill Koros, and Chris Jones. Thank you for reading through and editing this document! I would also like to acknowledge Dr.
    [Show full text]
  • Ph Buffers in the Blood
    pH Buffers in the Blood Authors: Rachel Casiday and Regina Frey Department of Chemistry, Washington University St. Louis, MO 63130 For information or comments on this tutorial, please contact R. Frey at [email protected]. Please click here for a pdf version of this tutorial. Key Concepts: Exercise and how it affects the body Acid-base equilibria and equilibrium constants How buffering works Quantitative: Equilibrium Constants Qualitative: Le Châtelier's Principle Le Châtelier's Principle Direction of Equilibrium Shifts Application to Blood pH How Does Exercise Affect the Body? Many people today are interested in exercise as a way of improving their health and physical abilities. But there is also concern that too much exercise, or exercise that is not appropriate for certain individuals, may actually do more harm than good. Exercise has many short-term (acute) and long-term effects that the body must be capable of handling for the exercise to be beneficial. Some of the major acute effects of exercising are shown in Figure 1. When we exercise, our heart rate, systolic blood pressure, and cardiac output (the amount of blood pumped per heart beat) all increase. Blood flow to the heart, the muscles, and the skin increase. The body's metabolism becomes more active, producing CO and H+ in the muscles. We breathe faster and deeper to supply the oxygen 2 required by this increased metabolism. Eventually, with strenuous exercise, our body's metabolism exceeds the oxygen supply and begins to use alternate biochemical processes that do not require oxygen. These processes generate lactic acid, which enters the blood stream.
    [Show full text]
  • Carbon Species of the Lithosphere and Hydrosphere: the Carbonic Acid System1
    Experiment 18B SC151 10/07/10 CARBON SPECIES OF THE LITHOSPHERE AND HYDROSPHERE: 1 THE CARBONIC ACID SYSTEM MATERIALS: pH meter (2); magnetic stirrer and stirbar (2); standardization buffers (pH=4, 7 and 10); 50 mL buret (2); 400 mL beaker (3); 100 mL beaker (2); 100 mL graduated cylinder; filter funnel and filter paper; anhydrous Na2CO3; saturated solution of MgCO3; 0.036 M H2SO4; 0.0072 M H2SO4. PURPOSE: The purpose of this experiment is to introduce the use of the pH meter and to identify important features in the titration curves of weak acids and bases. LEARNING OBJECTIVES: By the end of this experiment, the student should be able to demonstrate the following proficiencies: 1. Standardize and use a pH meter. 2. Perform a pH titration. 3. Identify the dominant chemical species at various points in a titration curve. 4. Obtain values of pKa for weak acids from pH titration data. DISCUSSION Every carbon atom in your body has been used in countless other molecules since the beginning of time, as CO2 in the air you breathe, as carbohydrates in the food you eat, as bicarbonate “fixed” by sea life, or as carbonate salts in the rocks and soil you walk on. The Carbon Cycle is a complex series of processes which describes how carbon atoms circulate among these realms of atmosphere, biosphere, hydrosphere and lithosphere. By far, the greatest store of carbon atoms on earth can be found in marine sediments and sedimentary rocks (~8 x 1016 metric tons), with the ocean providing a distant second store (~4x1013 metric tons).
    [Show full text]
  • 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.
    [Show full text]
  • Ph Regulation During Exercise Acid-Base Equilibria Experiment
    Blood, Sweat, and Buffers: pH Regulation During Exercise Acid-Base Equilibria Experiment Authors: Rachel Casiday and Regina Frey Revised by: C. Markham, A. Manglik, K. Castillo, K. Mao, and R. Frey Department of Chemistry, Washington University St. Louis, MO 63130 For information or comments on this tutorial, please contact Kit Mao at [email protected]. Key Concepts: • Exercise and how it affects the body • Acid-base equilibria and equilibrium constants • How buffering works Equilibrium Constants Henderson-Hasselbalch Equation Direction of Equilibrium Shifts Application to Blood pH Related Tutorials: • Hemoglobin and the Heme Group: Metal Complexes in the Blood for Oxygen Transport • Iron Use and Storage in the Body: Ferritin and Molecular Representations • Maintaining the Body’s Chemistry: Dialysis in the Kidneys How Does Exercise Affect the Body? Many people today are interested in exercise as a way of improving their health and physical abilities. When we exercise, our heart rate, systolic blood pressure, and cardiac output (the amount of blood pumped per heart beat) all increase. Blood flow to the heart, the muscles, and the skin + increase. The body's metabolism becomes more active, producing CO2 and H in the muscles. We breathe faster and deeper to supply the oxygen required by this increased metabolism. With strenuous exercise, our body's metabolism exceeds the oxygen supply and begins to use alternate biochemical processes that do not require oxygen. These processes generate lactic acid, which enters the blood stream. As we develop a long-term habit of exercise, our cardiac output and lung capacity increase, even when we are at rest, so that we can exercise longer and harder than before.
    [Show full text]
  • Ph – Carbonate Equilibrium and Applications to Manufacture of Still Water
    Carbonate Chemistry Applied to the Beverage Production of Still Water By Phillip L. Hayden, Ph.D., P.E. True North Thinking, LLC 591 Congress Park Drive Dayton, OH 45459 The chemistry of the carbonate equilibrium, including carbon dioxide (CO2), directly affects the beverage production of still water, which has strict pH and alkalinity standards. CO2 (g) will pass through a Reverse Osmosis (RO) membrane, which is commonly used in still water production, and end up in the final water. Unless the CO2 is removed, adjusting the final pH to specifications will result in high alkalinity concentrations in excess of the specifications. The purpose of this paper is to define the carbonate chemistry, present various treatment options and the impact of CO2 (gas) on final still water quality. 1.0 REVIEW Most ground waters have high levels of hardness consisting of calcium and magnesium ions and alkalinity, which are the carbonate ions. These waters, when removed from the ground, increase in temperature and become oversaturated with respect to precipitation of calcium carbonate. As a result, calcium carbonate scale forms on pipes, valves, heating coils and process equipment. High levels of calcium and magnesium also impact the sensory qualities of carbonated soft drink products (CSD). In groundwater’s originating from limestone aquifers, the hardness ions calcium and magnesium are normally accompanied with carbonate alkalinity. The carbonate equilibrium, which includes free CO2 or carbonic acid, bicarbonate ions and carbonate ions, is highly pH dependent. The CO2 – bicarbonate equilibrium exists in the pH range of 4.3 to 8.3 and the bicarbonate – carbonate equilibrium dominating at pH 8.3 – 12.3.
    [Show full text]