DOCSLIB.ORG

SUMMARY of the INVENTION of a Salt of an Oxy Acid of Sulfur Wherein

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
SUMMARY of the INVENTION of a Salt of an Oxy Acid of Sulfur Wherein 3,597,456 thirds water. Such a mixture is preferred as higher con 3,597,456 METHOD FOR PREPARNG STERILE LECTHEN centrations of lecithin tend to be difficult to handle, while Charles Rifkin, Highland Park, and Rudolfo Cilento, lower concentrations require excessively large vessels North Brunswick, N.J., assignors to E. R. Squibb & and involve heating excessive amounts of water. It is Sons, Inc., New York, N.Y. 5 to be understood, however, that the foregoing considera No Drawing. Filed May 20, 1969, Ser. No. 826,258 tions are primarily economic, not chemical, and it is em Int, CI. A237/00; C07f 9/02 phasized that the present invention is applicable to any U.S. C. 260-403 9 (Claims aqueous mixture of lecithin and water. The sterilizing conditions comprise elevated tempera tures and pressures. The temperatures are suitably above ABSTRACT OF THE DISCLOSURE 10 100 C. and the pressures are at least atmospheric and The presence of from 0.1 to 5% by weight of a salt of Suitably superatmospheric. The upper limit of the steri an oxy acid of sulfur wherein the apparent oxidation state lizing conditions is the decomposition point of the lecithin. of the sulfur is not greater than -- 4 prevents color In practice, there is little or no advantage in temperatures degradation during the sterilization of lecithin. above about 130° C. or pressures above a few atmos ls pheres. The lecithin is generally treated at these elevated temperatures and pressures for upwards of fifteen min BACKGROUND OF THE INVENTION utes,minutes. typically from about thirty minutes to about sixty The present invention relates to the sterilization of According to the present invention the sterilizing treat lecithin, and more particularly, to a method of sterilizing ment is carried out in the presence of a small amount lecithin whereby color degradation is prevented. of a salt of an oxy acid of sulfur wherein the apparent Lecithin is an organic chemical compound, phospho oxidation state of sulfur is not greater than --4. The lipid in nature, which is used in pharmaceutical practice oxy acids of Sulfur wherein the sulfur has an apparent as a dispersant and surface active agent. In view of the oxidation state not greater than +4 are Sulfoxylic acid "natural' character of lecithin, it has for many years been 25 (H2SO2), dithionous acid (H2SO4), sulfurous acid used as a dispersant in sterile aqueous suspensions of pro (HSOs), and pyrosulfurous acid (HSO). In deter caine penicillin. Modern medical practice dictates that mining the apparent oxidation state of sulfur in the OXy very large doses of procaine pencillin be injected in order acid, hydrogen is assigned its normal valence of --1 and to achieve a good therapeutic response. When 50% mi 30 oxygen its normal valence of -2. In this way the appar cronized penicillin solids are formulated into an aqueous ent oxidation state of sulfur can be computed to be 2 suspension, the resultant mixture is so thick that it will in sulfoxylic acid, --3 in dithionous acid, and --4 in not flow out of a syringe. The addition of relatively small both sulfurous acid and pyrosulfurous acid. By way of quantities of sterile lecithin fluidizes this mixture, and contrast, Sulfur has an apparent valence of -6 insul permits the injection of high doses. furic acid. Lecithin is commercially available as a light yellow or 35 The Salts of the oxy acids wherein the apparent oxida light tan granular solid, or in various liquid forms. The tion state of Sulfur is not greater than --4 include inor preparation of sterile lecithin has always been a problem ganic salts and organic salts. Among the inorganic salts in the pharmaceutical industry, particularly while trying are the alkali metal salts and ammonium salts. The or to retain its original light color. Lecithin is susceptible to 40 ganic Salts include the formyl derivatives of sulfoxylic auto-oxidation and decomposition, resulting in an un acid, that is, organic sulfones, and formyl and acetonyl desirable darkening of the color. Various methods are derivatives of sulfurous acid. used in commercial practice, none of which are entirely Some examples of inorganic salts are lithium sulfite, satisfactory. Commercial lecithin can be sterilized by dis Sodium Sulfite, potassium sulfite, ammonium sulfite, persing it in water and autoclaving the mixture at about 45 lithium sodium sulfite, lithium potassium sulfite, lithium 121 C. and at about 15 lbs. steam pressure, for from ammonium sulfite, sodium potassium sulfite, sodium am about 30 to about 60 minutes. In the normal course of monium sulfite, potassium ammonium Sulfite, lithium bi events this procedure will yield sterile lecithin. The prod sulfite, Sodium bisulfite, potassium bisulfite, ammonium uct, however, is extremely discolored and dark. bisulfite, lithium metabisulfite, sodium metabisulfite, po It is, accordingly, an object of the present invention to 50 tassium metabisulfite, ammonium metabisulfite, lithium provide an improved process for sterilizing lecithin while Sodium metabisulfite, lithium potassium metabisulfite, at the same time avoiding color degradation. A further lithium ammonium metabisulfite, sodium potassium meta object is to prepare light colored sterile lecithin. These and bisulfite, Sodium ammonium metabisulfite, potassium am other objects of the present invention will be apparent monium metabisulfite, lithium hydrogen metabisulfite, from the following description. 55 Sodium hydrogen metabisulfite, potassium hydrogen meta bisulfite, ammonium hydrogen metabisulfite, lithium hy SUMMARY OF THE INVENTION drosulfite, sodium hydrosulfite, potassium hydrosulfite, ammonium hydrosulfite, lithium sodium hydrosulfite, It has now been found that color degradation is avoided lithium potassium hydrosulfite, lithium ammonium hy by contacting aqueous lecithin under sterilizing condi 60 drosulfite, sodium potassium hydrosulfite, sodium am tions with a small amount of a salt of an oxy acid of sulfur monium hydrosulfite, potassium ammonium hydrosulfite, wherein the apparent oxidation state of sulfur is not lithium hydrogen hydrosulfite, sodium hydrogen hydro greater than --4. Sulfite, potassium hydrogen hydrosulfite and ammonium DETALED DESCRIPTION hydrogen hydrosulfite. 65 The organic salts may be, for example, sodium for Aqueous lecithin is a mixture of lecithin and water. maldehyde sulfoxylate (formosul), sodium formaldehyde The mixture may be in the form of a dispersion, suspen bisulfite, acetone sodium bisulfite, and the corresponding sion or emulsion. The process of the present invention is lithium, potassium and ammonium salts. applicable to any mixture of lecithin and water, regard The quantity of the salt of the oxy acid of sulfur may less of the lecithin concentration. A preferred aqueous 70 vary from about 0.1% to about 5% by weight of the lecithin mixture consists of one-third lecithin and two lecithin. 3,597,456 3 4. The sterile lecithin obtained by subjecting lecithin to EXAMPLE 5 a sterilizing treatment in the presence of a Salt of an The procedure of Example 1 was repeated except that oxy acid of sulfur according to the present invention may when the bottle was removed from the autoclave it was be used directly in solution or dispersion such as in the allowed to cool somewhat, but while still warm, was preparation of procaine pencillin aqueous Suspension, or poured into a sterile stainless steel tray, covered and the dispersion of sterile lecithin can be frozen and lyo frozen. The tray was subsequently freeze-dried at a philized so that sterile dry lecithin can be obtained and vacuum of 50 microns of mercury to yield a porous sterile used for various purposes in the dry state. The quantity mass which had a very light acceptable color. of lecithin which can be treated in this manner is limited only by the equipment size. O EXAMPLE 6 The following examples illustrate the present invention The lecithin dispersion of Example 3 was poured into without, however, limiting the same thereto. trays and freeze-dried as in Example 5 to yield a porous EXAMPLE 1. sterile mass similar in appearance to that of Example 5. What is claimed is: 500 g. of lecithin and 1 1. of water in which 10 g. of 1. A process for preparing sterile lecithin wherein sodium formaldehyde sulfoxylate had been predissolved aqueous lecithin is contacted under sterilizing conditions were added to a 4 1. Pyrex bottle. The bottle was sealed with a salt of an oxy acid of sulfur wherein the apparent and autoclaved at 121 for one hour. It was then removed oxidation state of sulfur is not greater than --4, the from the autoclave and the dispersion of lecithin allowed amount of the reducing agent being effective to prevent to cool. The lecithin dispersion was very light in color 20 discoloration of the lecithin. and acceptable for the preparation of aqueous Suspen 2. A process according to claim 1 wherein the salt sions of procaine penicillin. On testing for sterility, it of the oxy acid of sulfur is present in an amount of from was found to be sterile. Aqueous suspensions of procaine about 0.1% to about 5% by weight of the lecithin. penicillin made from this lecithin were tested for muscle 3. A process according to claim 1 wherein the oxy irritation and toxicity. There was no significant difference 25 acid of sulfur is sulfoxylic acid, dithionous acid, sulfurous between these preparations and controls. acid or pyrosulfurous acid. EXAMPLE 2 4. A process according to claim 3 wherein the cation of the salt of the oxy acid of sulfur is an alkali metal or The foregoing procedure was repeated except that no ammonium salt. sodium formaldehyde sulfoxylate was present. The re 30 5. A process according to claim 3 wherein the anion sulting lecithin dispersion was sterile but much darker in of the salt of the oxy acid of sulfur is a sulfite, bisulfite, color and unacceptable for the preparation of aqueous metabisulfite or hydrosulfite.
Load more

Recommended publications
  • Recent Developments on the Origin and Nature of Reductive Sulfurous Off-Odours in Wine
    fermentation Review Recent Developments on the Origin and Nature of Reductive Sulfurous Off-Odours in Wine Nikolaus Müller 1,* and Doris Rauhut 2 1 Silvanerweg 9, 55595 Wallhausen, Germany 2 Department of Microbiology and Biochemistry, Hochschule Geisenheim University, Von-Lade-Straße 1, 65366 Geisenheim, Germany; [email protected] * Correspondence: [email protected]; Tel.: +49-6706-913103 Received: 9 July 2018; Accepted: 3 August 2018; Published: 8 August 2018 Abstract: Reductive sulfurous off-odors are still one of the main reasons for rejecting wines by consumers. In 2008 at the International Wine Challenge in London, approximately 6% of the more than 10,000 wines presented were described as faulty. Twenty-eight percent were described as faulty because they presented “reduced characters” similar to those presented by “cork taint” and in nearly the same portion. Reductive off-odors are caused by low volatile sulfurous compounds. Their origin may be traced back to the metabolism of the microorganisms (yeasts and lactic acid bacteria) involved in the fermentation steps during wine making, often followed by chemical conversions. The main source of volatile sulfur compounds (VSCs) are precursors from the sulfate assimilation pathway (SAP, sometimes named as the “sulfate reduction pathway” SRP), used by yeast to assimilate sulfur from the environment and incorporate it into the essential sulfur-containing amino acids methionine and cysteine. Reductive off-odors became of increasing interest within the last few years, and the method to remove them by treatment with copper (II) salts (sulfate or citrate) is more and more questioned: The effectiveness is doubted, and after prolonged bottle storage, they reappear quite often.
    [Show full text]
  • Thiosulfate Degradation During Gold Leaching In
    THIOSULFATE DEGRADATION DURING GOLD LEACHING IN AMMONIACAL THIOSULFATE SOLUTIONS : A FOCUS ON TRITHIONATE By NOELENE AHERN B.Sc, University of Natal, 1994 B.Sc. (Hons), University of Natal, 1995 M.A.Sc, University of Cape Town, 1997 A thesis submitted in partial fulfillment of the requirements for the degree of Doctor of Philosophy in the Faculty of Graduate Studies (Materials Engineering) The University of British Columbia October 2005 © Noelene Ahern, 2005 ABSTRACT Thiosulfate has shown considerable promise as an alternative to cyanide for gold leaching. However, one of the main limitations of the thiosulfate system is the high consumption of thiosulfate. Besides increasing the cost of the process, the degradation products of thiosulfate have been claimed to passivate gold surfaces and the polythionates often produced are loaded onto resins proposed for gold recovery. The thiosulfate degradation process is not completely understood. Of the degradation products, trithionate is a concern in the resin recovery of gold and is persistent in gold leach solutions. Very little is known about the expected behaviour of trithionate, both with respect to its formation and its interaction with other solution species. The focus of this work was therefore to further the understanding of the behaviour of trithionate in gold leach solutions. Experimental work was carried out to determine the kinetics of trithionate degradation in systems resembling gold leaching solutions, and a kinetic model was derived for trithionate degradation. The rate of degradation of trithionate in aqueous ammoniacal solutions was expressed by Equation 1. 2 + 2 -d[S306 -]/dt = (k3[NH4 ] + k2[NH3] + k,[OHl + k0)[S3O6 T [1] 1 1 1 1 1 where k0 = 0.012 h"\ = 0.74 IvV.h;, k2 = 0.0049 M" .h' , k3 = 0.01 M" .^ .
    [Show full text]
  • Hydrogen from Hydrogen Sulfide Ryan J. Gillis
    Theory and Applications for Sulfur Chemistry: Hydrogen from Hydrogen Sulfide by Ryan J. Gillis B.S., Brigham Young University (2015) Submitted to the Department of Chemical Engineering in partial fulfillment of the requirements for the degree of Doctor of Philosophy in Chemical Engineering at the MASSACHUSETTS INSTITUTE OF TECHNOLOGY September 2020 ○c Massachusetts Institute of Technology 2020. All rights reserved. Author................................................................ Department of Chemical Engineering July 30, 2020 Certified by. William H. Green Professor Thesis Supervisor Accepted by . Patrick S. Doyle Graduate Officer, Department of Chemical Engineering 2 Theory and Applications for Sulfur Chemistry: Hydrogen from Hydrogen Sulfide by Ryan J. Gillis Submitted to the Department of Chemical Engineering on July 30, 2020, in partial fulfillment of the requirements for the degree of Doctor of Philosophy in Chemical Engineering Abstract In this thesis, I explore the chemistry of reacting sulfur species computationally and experimentally. The computational work centers around creating the capability to automatically predict the thermochemical properties of arbitrary sulfur molecules and the kinetic parameters of reactions between these species. A demonstration of this enhanced capability is shown in the automatic creation of detailed chemical mech- anism describing the partial oxidation of dimethyl sulfide. The experimental work focuses on a hydrogen generating chemical cycle that uses a hydrogen sulfide feed- stock. Initially exploring the reactivity of hydrogen sulfide, water, and iodine mixtures to form hydroiodic acid, two competing pathways were discovered. The more inter- esting pathway involved the reaction of hydrogen sulfide with iodine and water to form hydroiodic acid and sulfur dioxide. A bench-top prototype was created demon- strating the creation of hydrogen gas from hydrogen sulfide through this pathway.
    [Show full text]
  • ABSTRACT FEI, XIUZHU. Decolorization of Dyed Polyester
    ABSTRACT FEI, XIUZHU. Decolorization of Dyed Polyester Fabrics using Sodium Formaldehyde Sulfoxylate. (Under the direction of Dr. David Hinks and Dr. Harold S. Freeman). Polyethylene terephthalate (PET) fiber is now the largest single fiber type within global textile production, taking over from cotton. In view of environmental stewardship, an effective approach to recycling colored PET fabrics has drawn wide attention. A key step in the recycling process is dye removal. Disperse dyes are used to dye PET fibers and designed to be durable inside the fiber. In addition, disperse dyes are hydrophobic and will not be substantially extracted with water as the only solvent. In this work, the organic solvent, acetone, was used in combination with water to remove disperse dyes from the PET, and sodium formaldehyde sulfoxylate (SFS) was employed to decolorize the dye. This agent was found effective for decolorizing Disperse Yellow 42, Yellow 86, Blue 56 and Blue 60 in acetone/water solutions and the process was extended to decolorization of dyed PET. An optimized combination of treatment time (30 min), water to acetone ratio (1:2), SFS concentration (10g/L), temperature (100 ˚C), and liquor ratio (1:50) was found to give sufficient color removal for a broad range of disperse dyes. Reuse of the water/acetone medium for five times was achieved for decolorization of Disperse Yellow 42 but could not be achieved for Disperse Blue 56. Fabric strength assessments were also investigated. It was found that SFS decolorization has no adverse influence on PET strength, as judged by viscosity measurements. © Copyright 2015 Xiuzhu Fei All Rights Reserved Decolorization of Dyed Polyester Fabrics using Sodium Formaldehyde Sulfoxylate by Xiuzhu Fei A thesis submitted to the Graduate Faculty of North Carolina State University in partial fulfillment of the requirements for the degree of Master of Science Textile Chemistry Raleigh, North Carolina 2015 APPROVED BY: _______________________________ _______________________________ Dr.
    [Show full text]
  • Sodium Dithionite Cas N°: 7775-14-6
    OECD SIDS SODIUM DITHIONITE FOREWORD INTRODUCTION SODIUM DITHIONITE CAS N°: 7775-14-6 OECD SIDS SODIUM DITHIONITE SIDS Initial Assessment Report For SIAM 19 Berlin, Germany, 19-22 October 2004 1. Chemical Name: Sodium dithionite 2. CAS Number: 7775-14-6 3. Sponsor Country: Germany Contact Point: BMU (Bundesministerium für Umwelt, Naturschutz und Reaktorsicherheit) Contact person: Prof. Dr. Ulrich Schlottmann Postfach 12 06 29 D- 53048 Bonn 4. Shared Partnership with: 5. Roles/Responsibilities of BASF AG = lead company the Partners: • Name of industry sponsor BASF AG, Germany /consortium Contact person: Dr. Hubert Lendle GUP/CL – Z 570 D-67056 Ludwigshafen • Process used The BUA Peer Review Process : see next page 6. Sponsorship History • How was the chemical or by ICCA-Initiative category brought into the OECD HPV Chemicals Programme? 7. Review Process Prior to last literature search (update): the SIAM: 14 February 2003 (Human Health): databases medline, toxline; search profile CAS-No. and special search terms 5 February 2004 (Ecotoxicology): databases CA, biosis; search profile CAS-No. and special search terms OECD/ICCA 8. Quality check process: As basis for the SIDS-Dossier the IUCLID was used. All data have been checked and validated by BUA. A final evaluation of the human health part has been performed by the Federal Institute for Risk Assessment (BfR) and of the ecotoxicological part by the Federal Environment Agency (UBA). 9. Date of Submission: Deadline for circulation: 23 July 2004 10. Date of last Update: 11. Comments: OECD SIDS SODIUM DITHIONITE OECD/ICCA - The BUA* Peer Review Process Qualified BUA personnel (toxicologists, ecotoxicologists) perform a quality control on the full SIDS dossier submitted by industry.
    [Show full text]
  • IUPAC Provisional Recommendations] 2 ] 2 2 2 +D O 2 − − 3 Osi(O) ] ]
    1 Table IR-8.1 Acceptable common names and fully systematic (additive) names for oxoacid and related structures. (March 2004) This Table includes compounds containing oxygen and hydrogen and at least one other element and with at least one OH group; certain isomers; and examples of corresponding partially and fully dehydronated anions. Formulae are given in the classical oxoacid format with the 'acid' (oxygen-bound) hydrogens listed first, followed by the central atom(s), then the hydrogen atoms bound directly to the central atom, and then the oxygen atoms (e.g. HBH2O, H2P2H2O5), except for chain compounds such as e.g. HOCN. In most cases formulae are also written as for coordination entities, assembled according to the principles of Chapter IR-7 (e.g. the Table gives 'HBH2O = [BH2(OH)]' and 'H2SO4 = [SO2(OH)2]'). More names of oxoanions are given in Table IX. Note that Section P-42 of Ref. 1 lists a great many inorganic oxoacid structures for use as parent structures in the naming of organic derivatives, cf. the discussion in Section IR-8.1. Most of those structures, but not all, are included here; a number of di- and polynuclear acids are not explicitly included. Formula Common name Fully systematic additive name(s) (unless otherwise stated) a H3BO3 = [B(OH)3] boric acid trihydroxidoboron − − H2BO3 = [BO(OH)2] dihydrogenborate dihydroxidooxidoborate(1−) − 2− HBO32 = [BO2(OH)] hydrogenborate hydroxidodioxidoborate(2−) 3− − [BO3] borate trioxidoborate(3 ) (HBO2)n = (B(OH)O)n metaboric acid catena-poly[hydroxidoboron-µ-oxido] − n− (BO2
    [Show full text]
  • Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005)
    International Union of Pure and Applied Chemistry Nomenclature of Inorganic Chemistry IUPAC RECOMMENDATIONS 2005 Issued by the Division of Chemical Nomenclature and Structure Representation in collaboration with the Division of Inorganic Chemistry Prepared for publication by Neil G. Connelly Ture Damhus University of Bristol, UK Novozymes A/S, Denmark Richard M. Hartshorn Alan T. Hutton University of Canterbury, NewZealand University of Cape Town, South Africa IR-9.3 COORDINATION COMPOUNDS IR-9.3.2.2 Choosing between closely related geometries For real molecules or ions, the stereochemical descriptor should be based on the nearest idealizedgeometry. However, someidealized geometries are closely related [ e.g. square planar ( SP-4), four-coordinate square pyramidal ( SPY- 4), see-saw ( SS-4), and tetrahedral ( T-4);T-shaped ( TS- 3), trigonalplanar ( TP-3), and trigonalpyramidal ( TPY-3)] and care may therefore be requiredinmaking the choice. The following approach is useful in determining the polyhedralsymbol for four- coordinate structures. The key is to consider the locations of the central atom and the coordinating atoms in relation to each other. If all five atoms are in (or are close to beingin) the same plane, then the molecule should be treated as square planar. If the four coordinating atoms are in aplane, but the central atom is significantly displaced from the plane, then the squarepyramidal geometry is appropriate.Ifthe four coordinating atoms do not lie in (or close to) aplane, then apolyhedron can be defined by joiningall four coordinating atoms togetherwith lines. If the central atom lies inside this polyhedronthe molecule shouldberegarded as tetrahedral, otherwise, it should be regarded as having a see-saw structure.
    [Show full text]
  • The Institute of Paper Chemistry
    The Institute of Paper Chemistry Appleton, Wisconsin Doctor's Dissertation Effects of pH and Oxidizing Agents on the Rate of Absorption of Hydrogen Sulfide into Aqueous Media C. Neal Carter January, 1966 I EFFECTS OF pH AND OXIDIZING AGENTS ON THE RATE OF ABSORPTION OF HYDROGEN SULFIDE INTO AQUEOUS MEDIA A thesis submitted by C. Neal Carter B.S. 1961, North Carolina State University M.S. 1963, Lawrence College in partial fulfillment of the requirements of The Institute of Paper Chemistry, for the degree of Doctor of Philosophy from Lawrence University, Appleton, Wisconsin Publication Rights Reserved by The Institute of Paper Chemistry January, 1966 TABLE OF CONTENTS Page SUMMARY 1 INTRODUCTION 3 BACKGROUND OF THE THESIS PROBLEM 5 Tne Aqueous Hydrogen Sulfide System 5 Thermodynamic Considerations 5 Physical Equilibrium 5 Chemical Equilibrium 10 Reaction Considerations 10 Hypochlorite Oxidation 11 Kinetic Considerations 17 Rate of Dissociation 17 Rate of Reaction with Hydroxyl Ion 18 Rate of Oxidation 18 The Penetration Theory of Gas Absorption 19 The Mathematical Model 19 Physical Absorption 20 Absorption with Chemical Reaction 21 Penetration Theory as Applied to Hydrogen Sulfide Absorption 24 Previous Work 24 Information from Gas Absorption Measurements 24 APPARATUS AND PROCEDURES 25 The Secondary Experiments 25 Physical Properties of Absorbents 25 Solubility Measurements 25 Static Method 25 Dynamic Method 26 iii Diffusivity Measurements 26 Free Boundary Techniques 27 Electrophoresis-Diffusion Apparatus Procedure 27 Ultracentrifuge Apparatus
    [Show full text]
  • ABSTRACT FEI, XIUZHU. Towards Closed Loop
    ABSTRACT FEI, XIUZHU. Towards Closed Loop Recycling of Polyester Fabric. (Under the direction of Dr. Harold S. Freeman and Dr. David Hinks). Polyethylene terephthalate (PET) is extensively used in various types of apparel, home textiles, and outdoor products that are regularly placed in landfills after use. But unlike natural fibers, PET is not readily biodegradable. In view of sustainability, research regarding the recycling of textiles derived from PET fibers is of interest, and effective color removal has been recognized as a crucial step towards recycling of colored PET fabrics. To this end, a decolorization process was developed using sodium formaldehyde sulfoxylate (SFS) as the reducing agent. Disperse dye decolorization studies were conducted in water and acetone media, and an optimized combination of treatment time (30 min), water to acetone ratio (1:2), SFS concentration (10g/L), temperature (100oC), and liquor ratio (1:50) was found effective for decolorizing various commercial disperse dyes as well as basic dyes. Results in terms of intrinsic viscosity of decolorized PET showed that the optimized SFS decolorization method has no significant effect on fiber strength. The goal of this work was to study the recyclability of bath and fabric after decolorization, investigate the ecotoxicity of the decolorization process, study the life cycle assessment of the closed-loop recycling process, characterize dyes from commercial fabrics and study their decolorization properties. Fabric decolorization using the optimized SFS method followed by re-dyeing using Disperse Yellow 42, Disperse Orange 30, Disperse Red 60, and Disperse Blue 79 was conducted on cationic dyeable PET. It was found that fabrics containing nitro and anthraquinone dyes, Disperse Yellow 42 and Disperse Red 60, respectively, have better decolorization efficiency than those containing azo Disperse Orange 30 and Disperse Blue 79 dyed fabrics.
    [Show full text]
  • (12) United States Patent (10) Patent No.: US 6,552,141 B1 Chmelir Et Al
    USOO65521.41B1 (12) United States Patent (10) Patent No.: US 6,552,141 B1 Chmelir et al. (45) Date of Patent: Apr. 22, 2003 (54) METHOD FOR PRODUCING SYNTHETIC (56) References Cited POLYMERIZATES WITH VERY LOW RESIDUAL MONOMER CONTENT U.S. PATENT DOCUMENTS 4,766,173 A * 8/1988 Bailey et al. ............... 524/819 (75) Inventors: Miroslav Chmelir, Krefeld (DE); Kurt Dahmen, Moenchengladbach (DE) 4,929,717 A * 5/1990 Chmelir ...................... 528/490 4,954,562 A 9/1990 Anderson ................... 524/430 4,985,518 A 1/1991 Alexander et al. .......... 526/240 (73) Assignee: Stockhausen GmbH & Co. KG, 5,264,471. A 11/1993 Chmelir ....................... 524/35 Krefeld (DE) 5,684,106 A 11/1997 Johnson et al. ............. 526/295 (*) Notice: Subject to any disclaimer, the term of this patent is extended or adjusted under 35 FOREIGN PATENT DOCUMENTS U.S.C. 154(b) by 0 days. DE 19529348 A 2/1997 (21) Appl. No.: 09/554,098 EP OSO5163 A 9/1992 (22) PCT Filed: Nov. 13, 1998 * cited by examiner (86) PCT No.: PCT/EP98/07289 Primary Examiner J. Zalukaeva S371 (c)(1), (74) Attorney, Agent, or Firm-Oblon, Spivak, McClelland, (2), (4) Date: Jun. 14, 2000 Maier & Neustadt, P.C. (87) PCT Pub. No.: WO99/26987 (57) ABSTRACT PCT Pub. Date:Jun. 3, 1999 The invention relates to a method for producing water (30) Foreign Application Priority Data soluble or water-swellable polymerizates with a low residual monomer content from acrylic acid and/or acrylic acid Nov. 25, 1997 (DE) ......................................... 197 52 127 derivatives. The method is characterized by the addition of (51) Int.
    [Show full text]
  • Synthetic Utility of Beta-Keto Sulfoxides Gerard Joseph Mikol Iowa State University
    Iowa State University Capstones, Theses and Retrospective Theses and Dissertations Dissertations 1966 Synthetic utility of beta-keto sulfoxides Gerard Joseph Mikol Iowa State University Follow this and additional works at: https://lib.dr.iastate.edu/rtd Part of the Organic Chemistry Commons Recommended Citation Mikol, Gerard Joseph, "Synthetic utility of beta-keto sulfoxides " (1966). Retrospective Theses and Dissertations. 2908. https://lib.dr.iastate.edu/rtd/2908 This Dissertation is brought to you for free and open access by the Iowa State University Capstones, Theses and Dissertations at Iowa State University Digital Repository. It has been accepted for inclusion in Retrospective Theses and Dissertations by an authorized administrator of Iowa State University Digital Repository. For more information, please contact [email protected]. This dissertation has been microfihned exactly as received 6 6—10,431 MIKOL, Gerard Joseph, 1940— SYNTHETIC UTILITY OF BETA-KETO SULFOXIDES. Iowa State University of Science and Technology Ph.D., 1966 Chemistry, organic University Microfilms, Inc., Ann Arbor, Michigan SYNTHETIC UTILITY OP BSTA-KETO SULFOXIDES oy Gerard Joseph Mikol / A Dissertation Submitted, to the Graduate Faculty in Partial'Fulfillment of The Requirements for the Degree of DOCTOR OF PHILOSOPHY Major Subject: Organic Chemistry Approved; Signature was redacted for privacy. In Charge of Major Work Signature was redacted for privacy. Head of Major ^Department Signature was redacted for privacy. Defan of . Graduate Colle.ee Iowa State University Of Science and Technology Ames, Iowa 1966 11 TABLE OP CONTENTS Page INTRODUCTION' 1 LITEBATUEE REVIEW 4 The Kethylsulfinylcarbanlon: Generation and Properties 4 Beta-keto Sulfoxides 10 Asymmetry of the Sulfoxide Group 12 Chemical .Reduction of Sulfoxides l4 Pummerer Rearrangement 21 Dimethyl Sulfoxide as an Oxidizing Agent 31 EXPERIMENTAL ^ 40 Preparation of Methylsulfinylmethyl Aryl Ketones, I; Reaction of Aromatic Esters with Dimethyl Sulfoxide and.
    [Show full text]
  • Characterization of the Metal Sulfide Sulfur-Dioxide Reaction in Aqueous
    INFORMATION TO USERS This material was produced from a microfilm copy of the original document. While the most advanced technological means to photograph and reproduce this document have been used, the quality is heavily dependent upon the quality of the original submitted. The following explanation of techniques is provided to help you understand markings or patterns which may appear on this reproduction. 1. The sign or "target" for pages apparently lacking from the document photographed is "Missing Page(s)". If it was possible to obtain the missing page(s) or section, they are spliced into the film along with adjacent pages. This may have necessitated cutting thru an image and duplicating adjacent pages to insure you complete continuity. 2. When an image on the film is obliterated with a large round black mark, it is an indication that the photoyapher suspected that the copy may have moved during exposure and thus cause a blurred image. You will find ja good image o f the page in the adjacent frame. 3. When a map, drawing or chart, etc., was part of the material being photographed the photographer followed a definite method in "sectioning" the material. It is customary to begin photoing at the upper left hand corner of a large sheet and to continue photoing from left to right in equal sections with a small overlap. If necessary, sectioning is continued again — beginning below the first row and continuing on until complete. 4. The majority of users indicate that the textual content is of greatest value, however, a somewhat higher quality reproduction could be made from "photographs" if essential to the understanding of the dissertation.
    [Show full text]