DOCSLIB.ORG

United States Patent Office Patented Apr

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
United States Patent Office Patented Apr 3,378,337 United States Patent Office Patented Apr. 16, 1968 1. 2 and the hydrogen peroxide. This result is achieved without 3,378,337 contaminating the reaction mixture. The final solution PREPARATHON OF ODEC ACID AND DERVATIVES THEREOF contains substantially pure iodic acid, and can be evap Ricardo O. Bach, Gastonia, N.C., assignor to Lithium orated and dehydrated to obtain the iodic acid, or the Corporation of America, Inc., New York, N.Y., a cor anhydride thereof, or it can be used as a medium for the poration of Minnesota direct production of salts of iodic acid. No Drawing. Fied May 17, 1965, Ser. No. 456,561 In carrying out the method of the present invention, 12 Claims. (CI. 23-85) the iodic acid solution employed in forming the reaction mixture should contain sufficient iodic acid to provide a O hydrogen ion and iodate ion concentration in the reaction ABSTRACT OF THE DISCLOSURE mixture which will favor oxidation of iodine to its penta A method of preparing solutions of substantially pure valent state and impede decomposition of hydrogen iodic acid from which salts of the acid, the anhydride peroxide. Generally speaking, the quantity of iodic acid thereof and/or the crystalline form of the acid can be present in the starting solution should not be below about 5 0.5%, with especially good results being attained with directly obtained. The method involves reacting iodine from about 1% to about 10%, usually about 5%, of the with hydrogen peroxide in the presence of a relatively quantity of iodic acid to be produced. It is preferred to minor proportion of a solution of iodic acid. The hy work with aqueous iodic acid solutions wherein the acid drogen ions and iodate ions furnished by the iodic acid is present in a concentration, by weight, of about 5% to in solution are believed to catalyze or favor oxidation of about 35%. Especially satisfactory results are achieved the iodine to its pentavalent state thereby expediting the 20 with relatively strong aqueous iodic acid solutions of reaction between the iodine and the hydrogen peroxide. concentration of about 10% to 30%, particularly from about 15% to 25%, by weight. Stated differently, the Various methods heretofore have been proposed for starting aqueous iodic acid solutions in the concentrations preparing iodic acid. One of the more generally used prior 25 particularly preferred have a normality, or molarity, of art methods of preparing the acid involves oxidizing iodine from about 1 to about 2. In production, the desired con with concentrated or fuming nitric acid. Another known ditions of acidity and iodate ion concentration convenient method involves oxidizing iodine with hydrogen peroxide ly can be established in the reaction mixture by simply in the presence of nitric acid. The first mentioned method using a small portion, sometimes referred to as a "heel,” has significant economic disadvantages both from the 30 of the final iodic acid solution obtained in a previous run. standpoint of the quantities of concentrated or fuming The concentration of iodic acid in such solutions ranges nitric acid required to carry out the reaction, and the from about 25% to about 35%, by weight, with densities necessity for special handling and equipment dictated by ranging from about 1.2 to about 1.5 grams of iodic acid the corrosive character of the nitric acid. A further im per milliliter of solution. portant disadvantage of this prior art method, and one 35 The iodine utilized in the method of this invention which it shares with the second mentioned method, resides advantageously is in solid form. Especially satisfactory in the fact that the iodic acid always is obtained in solu results are achieved when the iodine is finely powdered. tion with other acidic constituents which first must be The increased reaction surface presented by the iodine in removed before the iodic acid can be recovered. In addi this form renders it more readily susceptible to oxidation tion, the unwanted acid constituents in the iodic acid solu 40 by the hydrogen peroxide and thus accelerates formation tions obtained in accordance with these known methods of the iodic acid. While the purity of the iodine used is not effectively prevent synthesis of salts such as iodates, for an overriding consideration in the preparation of iodic example, directly from the iodic acid solutions. It is only acid in accordance with the practice of this invention, it after the interfering acid constituents first have been is of marked importance when an anhydride of iodic acid, purged from the iodic acid solution that such salts rea 45 that is, iodine pentoxide, substantially conforming to ACS sonably can be prepared from the recovered iodic acid. specifications, is the desired end product to be obtained In accordance with the present invention, a method has from the final iodic acid solution. In such event, purified been discovered for preparing, in situ, substantially pure iodine should be used. iodic acid solutions from which iodic acid in crystalline The hydrogen peroxide component employed in the form, or in the form of its anhydride, can be obtained, 50 reaction may vary considerably in strength. Aqueous hy or from which salts of iodic acid can be directly pro drogen peroxide of strength of from about 3% to about duced. The solutions are free of interfering contaminants 98% can be used. However, since the strength of the aque characteristically present in iodic acid solutions obtained ous hydrogen peroxide used in carrying out a method of in accordance with heretofore used methods of preparing the present invention bears a direct relationship to the iodic acid. Substantially pure products can, therefore, be 55 volume of liquid comprising the final iodic acid solutions, obtained by the method of this invention simply by em and, therefore, the iodic acid concentration thereof, it is ploying conventional evaporation and dehydration tech especially desirable to use aqueous hydrogen peroxide of niques to remove the liquid phase of the solutions. strength of about 50% and higher, usually 60% to 90%, Briefly stated, the method of the present invention in preferably about 70%. There is a number of aqueous volves reacting iodine with hydrogen peroxide in the 60 solutions of hydrogen peroxide available commercially presence of a relatively minor proportion of a solution having utility for the purposes of this invention. Among of iodic acid. It has been discovered that the hydrogen these are the products sold under the trade designations ions and iodate ions furnished by the iodic acid in solution "Perone' and “Becco,” which products comprises aqueous catalyze or favor oxidation of the iodine to its pentavalent hydrogen peroxide solutions of strength ranging anywhere state thereby expediting the reaction between the iodine 65 from 25% to 98%, or higher. While standard commercial 3,378,337 3 4. grades of aqueous hydrogen peroxide can be used to ad Example 1 vantage in the preparation of the iodic acid solutions of To a solution comprising 29.4 grams of iodic acid in this invention, in utilizing the solutions to prepare an an 250 milliliters of water, 50 grams of iodine are added. hydride of iodic acid which substantially conforms to ACS While this mixture is being stirred, 10 milliliters of 70% specifications, it is desirable to use an "uninhibited' hy hydrogen peroxide are added every few minutes. The drogen peroxide solution. temperature of the reaction mixture rises. After the tem The proportions of the iodine and the hydrogen per perature reaches 65 C., further additions of the hydro oxide present in the aqueous reaction mixtures used in gen peroxide are regulated to maintain the temperature the practice of the method of this invention can be varied of the reaction mixture in the range of 65-75 C. As within appreciable limits. Ideally, the reaction between 10 the solution becomes clear, more iodine is added. After the iodine and the hydrogen peroxide proceeds in accord a total of 800 grams of iodine have been introduced the ance with the following equation: reaction mixture is filtered, and 100 milliliters of hydro gen peroxide are added to the filtrate to bring the total amount of hydrogen peroxide used to 1735 milliliters. This representation of the reaction would indicate that 5 The final solution is clear. The solution is evaporated approximately theoretical or stoichiometric proportions of to dryness, yielding 1050 grams of iodic acid. the iodine and the hydrogen peroxide, that is, an iodine to Example 2 hydrogen peroxide molar ratio of 1:5, can be employed. To a solution comprising 40 grams of iodic acid in However, in practice, due to catalytic decomposition of 20 250 milliliters of water, 100 grams of iodine are added. the hydrogen peroxide component in the reaction mixture, While the mixture is being stirred, 5 milliliters of 70% an excess of the hydrogen peroxide is used. Accordingly, hydrogen peroxide are added. After a few minutes an the generally optimum objectives of the invention are most additional 5 milliliters of hydrogen peroxide are added. advantageously attained with an iodine to hydrogen per This procedure is continued until the temperature of the oxide molar ratio of the order of approximately 1 of the 25 reaction mixture is in the range of 65-75 C. Iodine is iodine to about 10 of the hydrogen peroxide. added continuously to the mixture as the mixture be The temperature at which the method of the present comes clear. When approximately 1000 grams of iodine invention is carried out may range from about 60° C. have been added and the volume of the reaction mixture to about 80° C., more advantageously from 65 C. to is about 2 liters, the hydrogen peroxide is added at the 75° C., with about 70° C.
Load more

Recommended publications
  • Aqueous Equilibrium Constants
    BLB_APP_D_1062-1063hr.qxp 11/8/10 2:27 PM Page 1062 APPENDIX D AQUEOUS EQUILIBRIUM CONSTANTS TABLE D.1 • Dissociation Constants for Acids at 25 ˚C Name Formula Ka1 Ka2 Ka3 -5 Acetic acid CH3COOH (or HC2H3O2) 1.8 * 10 * -3 * -7 * -12 Arsenic acid H3AsO4 5.6 10 1.0 10 3.0 10 * -10 Arsenous acid H3AsO3 5.1 10 * -5 * -12 Ascorbic acid H2C6H6O6 8.0 10 1.6 10 * -5 Benzoic acid C6H5COOH (or HC7H5O2) 6.3 10 * -10 Boric acid H3BO3 5.8 10 * -5 Butanoic acid C3H7COOH (or HC4H7O2) 1.5 10 * -7 * -11 Carbonic acid H2CO3 4.3 10 5.6 10 * -3 Chloroacetic acid CH2ClCOOH (or HC2H2O2Cl) 1.4 10 * -2 Chlorous acid HClO2 1.1 10 * -4 * -5 -7 Citric acid HOOCC(OH) (CH2COOH)2 (or H3C6H5O7) 7.4 10 1.7 10 4.0 * 10 - Cyanic acid HCNO 3.5 * 10 4 * -4 Formic acid HCOOH (or HCHO2) 1.8 10 * -5 Hydroazoic acid HN3 1.9 10 - Hydrocyanic acid HCN 4.9 * 10 10 - Hydrofluoric acid HF 6.8 * 10 4 - -7 Hydrogen chromate ion HCrO4 3.0 * 10 * -12 Hydrogen peroxide H2O2 2.4 10 - -2 Hydrogen selenate ion HSeO4 2.2 * 10 * -8 * -19 Hydrogen sulfide H2S 9.5 10 1 10 - Hypobromous acid HBrO 2.5 * 10 9 - Hypochlorous acid HClO 3.0 * 10 8 - Hypoiodous acid HIO 2.3 * 10 11 * -1 Iodic acid HIO3 1.7 10 * -4 Lactic acid CH3CH(OH)COOH (or HC3H5O3) 1.4 10 * -3 * -6 Malonic acid CH2(COOH)2 (or H2C3H2O4) 1.5 10 2.0 10 * -4 Nitrous acid HNO2 4.5 10 * -2 * -5 Oxalic acid (COOH)2 (or H2C2O4) 5.9 10 6.4 10 * -2 * -9 Paraperiodic acid H5IO6 2.8 10 5.3 10 * -10 Phenol C6H5OH (or HC6H5O) 1.3 10 * -3 * -8 * -13 Phosphoric acid H3PO4 7.5 10 6.2 10 4.2 10 * -5 Propionic acid C2H5COOH (or HC3H5O2) 1.3 10 *
    [Show full text]
  • APPENDIX G Acid Dissociation Constants
    harxxxxx_App-G.qxd 3/8/10 1:34 PM Page AP11 APPENDIX G Acid Dissociation Constants §␮ ϭ 0.1 M 0 ؍ (Ionic strength (␮ † ‡ † Name Structure* pKa Ka pKa ϫ Ϫ5 Acetic acid CH3CO2H 4.756 1.75 10 4.56 (ethanoic acid) N ϩ H3 ϫ Ϫ3 Alanine CHCH3 2.344 (CO2H) 4.53 10 2.33 ϫ Ϫ10 9.868 (NH3) 1.36 10 9.71 CO2H ϩ Ϫ5 Aminobenzene NH3 4.601 2.51 ϫ 10 4.64 (aniline) ϪO SNϩ Ϫ4 4-Aminobenzenesulfonic acid 3 H3 3.232 5.86 ϫ 10 3.01 (sulfanilic acid) ϩ NH3 ϫ Ϫ3 2-Aminobenzoic acid 2.08 (CO2H) 8.3 10 2.01 ϫ Ϫ5 (anthranilic acid) 4.96 (NH3) 1.10 10 4.78 CO2H ϩ 2-Aminoethanethiol HSCH2CH2NH3 —— 8.21 (SH) (2-mercaptoethylamine) —— 10.73 (NH3) ϩ ϫ Ϫ10 2-Aminoethanol HOCH2CH2NH3 9.498 3.18 10 9.52 (ethanolamine) O H ϫ Ϫ5 4.70 (NH3) (20°) 2.0 10 4.74 2-Aminophenol Ϫ 9.97 (OH) (20°) 1.05 ϫ 10 10 9.87 ϩ NH3 ϩ ϫ Ϫ10 Ammonia NH4 9.245 5.69 10 9.26 N ϩ H3 N ϩ H2 ϫ Ϫ2 1.823 (CO2H) 1.50 10 2.03 CHCH CH CH NHC ϫ Ϫ9 Arginine 2 2 2 8.991 (NH3) 1.02 10 9.00 NH —— (NH2) —— (12.1) CO2H 2 O Ϫ 2.24 5.8 ϫ 10 3 2.15 Ϫ Arsenic acid HO As OH 6.96 1.10 ϫ 10 7 6.65 Ϫ (hydrogen arsenate) (11.50) 3.2 ϫ 10 12 (11.18) OH ϫ Ϫ10 Arsenious acid As(OH)3 9.29 5.1 10 9.14 (hydrogen arsenite) N ϩ O H3 Asparagine CHCH2CNH2 —— —— 2.16 (CO2H) —— —— 8.73 (NH3) CO2H *Each acid is written in its protonated form.
    [Show full text]
  • IODINE Its Properties and Technical Applications
    IODINE Its Properties and Technical Applications CHILEAN IODINE EDUCATIONAL BUREAU, INC. 120 Broadway, New York 5, New York IODINE Its Properties and Technical Applications ¡¡iiHiüíiüüiütitittüHiiUitítHiiiittiíU CHILEAN IODINE EDUCATIONAL BUREAU, INC. 120 Broadway, New York 5, New York 1951 Copyright, 1951, by Chilean Iodine Educational Bureau, Inc. Printed in U.S.A. Contents Page Foreword v I—Chemistry of Iodine and Its Compounds 1 A Short History of Iodine 1 The Occurrence and Production of Iodine ....... 3 The Properties of Iodine 4 Solid Iodine 4 Liquid Iodine 5 Iodine Vapor and Gas 6 Chemical Properties 6 Inorganic Compounds of Iodine 8 Compounds of Electropositive Iodine 8 Compounds with Other Halogens 8 The Polyhalides 9 Hydrogen Iodide 1,0 Inorganic Iodides 10 Physical Properties 10 Chemical Properties 12 Complex Iodides .13 The Oxides of Iodine . 14 Iodic Acid and the Iodates 15 Periodic Acid and the Periodates 15 Reactions of Iodine and Its Inorganic Compounds With Organic Compounds 17 Iodine . 17 Iodine Halides 18 Hydrogen Iodide 19 Inorganic Iodides 19 Periodic and Iodic Acids 21 The Organic Iodo Compounds 22 Organic Compounds of Polyvalent Iodine 25 The lodoso Compounds 25 The Iodoxy Compounds 26 The Iodyl Compounds 26 The Iodonium Salts 27 Heterocyclic Iodine Compounds 30 Bibliography 31 II—Applications of Iodine and Its Compounds 35 Iodine in Organic Chemistry 35 Iodine and Its Compounds at Catalysts 35 Exchange Catalysis 35 Halogenation 38 Isomerization 38 Dehydration 39 III Page Acylation 41 Carbón Monoxide (and Nitric Oxide) Additions ... 42 Reactions with Oxygen 42 Homogeneous Pyrolysis 43 Iodine as an Inhibitor 44 Other Applications 44 Iodine and Its Compounds as Process Reagents ...
    [Show full text]
  • Stencil Remover 285 Safety Data Sheet 01 June 2015
    Safety Data Sheet Section 1: Identification of the Substance/Mixture and of the Company/Undertaking 1.1 Product identifier Product Name • Stencil Remover 285 Product Description • Clear liquid. 1.2 Relevant identified uses of the substance or mixture and uses advised against Relevant identified use(s) • Liquid stencil remover concentrate 1.3 Details of the supplier of the safety data sheet Manufacturer • IKONICS Corporation 4832 Grand Ave. Duluth, MN 55807 United States www.ikonics.com [email protected] Telephone (General) • (218) 628-2217 Telephone (General) • (800) 328-4261 - Toll free 1.4 Emergency telephone number Chemtrec • 1-800-424-9300 - Within USA and Canada • +1 703-527-3887 - Outside USA and Canada (collect calls accepted) Section 2: Hazards Identification EU/EEC According to EU Directive 1272/2008 (CLP)/REACH 1907/2006 [amended by 453/2010] According to EU Directive 67/548/EEC (DSD) or 1999/45/EC (DPD) 2.1 Classification of the substance or mixture CLP • Oxidizing Liquids 2 - H272 Skin Corrosion 1 - H314 Serious Eye Damage 1 - H318 DSD/DPD • Corrosive (C) R35 2.2 Label Elements CLP DANGER Hazard statements • H272 - May intensify fire; oxidizer H314 - Causes severe skin burns and eye damage Stencil Remover 285 Safety Data Sheet Page 1 of 12 H318 - Causes serious eye damage Precautionary statements Prevention • P210 - Keep away from heat. P220 - Keep/Store away from clothing and other combustible materials. P221 - Take any precaution to avoid mixing with combustibles P260 - Do not breathe dusts or mists. P264 - Wash thoroughly after handling. P280 - Wear protective gloves/protective clothing/eye protection/face protection.
    [Show full text]
  • Common Acid and Base Storage Group Recommendations
    Recommended Storage Groups for Common Acids and Bases This list includes common acids and bases that are not classified as pyrophoric, water reactive or a flammable liquid under GHS. Chemicals are sorted by CAS#. A few substances that do not have a CAS# assigned appear at the end of the list. The CAS#, when assigned, should appear on the GHS container label. You may also search the list on the particular chemical/product name. Only acids and bases that are classified as corrosive to eyes and/or skin under GHS are included. The solvent for select acid or base solutions are given in parenthesis after the name. Organic acids [OA], inorganic acids [IA], and inorganic bases [IB] are assigned to designated storage groups. Many organic bases are assigned to the PW or FL storage groups. The remaining organic bases that do not fall into any other storage group are assigned the General Storage group [GS] in this list. For convenience these may be assigned to a designated Organic Base group, but this is not necessary for compatibility. The Comments column includes any special storage requirements. Where potential incompatibilities within a group exists the type of incompatible chemical is listed. Review SDS and product literature for additional storage information. Storage CAS # Name Synonyms Comments Group 10034-85-2 Hydriodic acid Hydriotic acid IA 2-8° C 10035-10-6 Hydrobromic acid Hydrogen Bromide IA 100-85-6 Benzyltrimethylammonium GS hydroxide solution (H2O) 10424-65-4 Tetramethylammonium GS hydroxide, pentahydrate 10450-60-9 Periodic acid
    [Show full text]
  • The Rate of The: Reaction Between Iodic and Hydriodic Acids
    THE RATE OF THE: REACTION BETWEEN IODIC AND HYDRIODIC ACIDS BY SAUL DUSHMAN In 1888 the rate of reaction between iodic and hydriodic acids was made the subject of a research by 0. Burchard,I who endeavored to discover a relation between the rate and the con- centrations of these two reagents. His results, however, were unsatisfactory, and the author concludes his paper with the words, ((Inspite of all attempts, I have not succeeded in represent- ing the rate of the reaction by a general differential equation ”. In light of the electrolytic dissociation theory introduced by Arrhenius just at the time of Burchard’s publication, it now seetns advisable to represent hydrogen iodide in solution as con- + - sisting almost entirely of hydrion (H) and iodion (I); simi- + larly a solution of iodic acid contains hydrion (H) and iodation - - (IO3), while brown “iodine ” solution contains tri-iodion (I3). Thus, in place of Burchard’s equation, 5HI f- HIO, = 31, + 3H,O, (1) it seems better to write + -- - 6H + 81 + IO, = 31, + 3H,O, (2) and in consequence, I have studied the effect of the concentra- T-- - tions of H, I, IO3 and I3 on the rate, instead of adopting the variables chosen by Burchard. In planning the experiments, I adopted a method which was originally employ-ed by Harcourt and Esson in their classi- cal research, “On the Observation of the Course of Chemical Change”, in 1866,‘ but which had, apparently been completely forgotten by 1888. The principle of the method is very sim- Zeit. phys. Chem. 2, 796 (1888). Jour.
    [Show full text]
  • Acid Nomenclature.Notebook February 02, 2017 Writing Acid Formulas/Naming Acids Formula Starts with "H" Name­Ends in "Acid"
    Acid nomenclature.notebook February 02, 2017 Writing Acid Formulas/Naming acids formula starts with "H" name­ends in "acid" Balance the overall charge to zero... (like ionic ­ criss cross) +1 ­3 All acids start with H+1 H PO4 H3PO4 Identify the acid: cation is always H+ use the anion to name it 3 ways to name: 1. binary acids ("bi" = "2") or non­oxy acid H+ and one other element anion ends in ­ide HCl Cl­1 chloride hydro­_____­ic acid HF F­1 fluoride hydro­_____­ic acid H2S S­2 sulfide hydro­_____­ic acid ­3 H3N N nitride hydro­_____­ic acid Binary rule: hydro­stem­ic acid use stem from anion 2. Oxyacid acids contain oxygen Again, look at the anion ­1 HNO3 NO3 nitrate _____ic acid ­2 _______ic acid H2SO4 SO4 sulfate ­3 _______ic acid H3PO4 PO4 phosphate oxyacid rule #1: Oxyacid rule #1: if anion ends in ­ate, use stem­ic acid I ate something ic­ky in the cafeteria ­1 HNO2 NO2 nitrite _____ous acid ­2 _______ous acid H2SO3 SO3 sulfite ­3 _______ous acid H3PO3 PO3 phosphite oxyacid rule #2: if anion ends in ­ite, use stem­ous acid 1 Acid nomenclature.notebook February 02, 2017 acid nomenclature: (review) Acids binary (non­oxy) oxy­acid ______­ide ______­ite ______­ate hydro______ic acid _______­ous acid _______­ic acid 2 Acid nomenclature.notebook February 02, 2017 Naming Acids Anion Ending Acid Name Binary @ ­ide hydro­(stem)­ic acid ­ate (stem) ­ic acid Oxyacid/ Ternary ­ite (stem) ­ous acid An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky” 3 Acid nomenclature.notebook February 02, 2017 Naming Acids
    [Show full text]
  • Measurement of Iodine Species and Sulfuric Acid Using Bromide
    https://doi.org/10.5194/amt-2020-494 Preprint. Discussion started: 18 December 2020 c Author(s) 2020. CC BY 4.0 License. 1 Measurement of iodine species and sulfuric acid using bromide 2 chemical ionization mass spectrometers 3 4 Mingyi Wang1,2*, Xu-Cheng He3*#, Henning Finkenzeller4, Siddharth Iyer3, Dexian Chen1,5, Jiali 5 Shen3, Mario Simon6, Victoria Hofbauer1,2, Jasper Kirkby6,7, Joachim Curtius6, Norbert Maier8, 6 Theo Kurtén3,8, Douglas R. Worsnop3,9, Markku Kulmala3,10,11,12, Matti Rissanen3,13, Rainer 7 Volkamer4, Yee Jun Tham3#, Neil M. Donahue1,2,5,14, and Mikko Sipilä3 8 9 1Center for Atmospheric Particle Studies, Carnegie Mellon University, Pittsburgh, PA, 15213, USA 10 2Department of Chemistry, Carnegie Mellon University, Pittsburgh, PA, 15213, USA 11 3Institute for Atmospheric and Earth System Research (INAR), University of Helsinki, 00014 Helsinki, Finland 12 4Department of Chemistry & CIRES, University of Colorado Boulder, Boulder, CO 80309, USA 13 5Department of Chemical Engineering, Carnegie Mellon University, Pittsburgh, PA, 15213, USA 14 6Institute for Atmospheric and Environmental Sciences, Goethe University Frankfurt, 60438 Frankfurt am Main, 15 Germany 16 7CERN, the European Organization for Nuclear Research, CH-1211 Geneve 23, Switzerland 17 8Department of Chemistry, University of Helsinki, 00014 Helsinki, Finland 18 9Aerodyne Research, Inc., Billerica, MA, 01821, USA 19 10Helsinki Institute of Physics, P.O. BoX 64 (Gustaf Hallstromin katu 2), FI-00014 University of Helsinki, Finland 20 11Joint International Research
    [Show full text]
  • Binary Acids, Oxyacids, Bases, Hydrates
    Working backwards: name to formula Naming Compounds • It’s possible to determine a formula from a name • E.g. What is the formula of sodium oxide? • To get the answer, first write the valences: 1 2 Na O → Na2O • What is the formula of copper(II) oxide? 2 2 Cu O → Cu2O2 → CuO • For covalent compounds, simply use the prefixes to tell you the number of each element: • What is the formula for dinitrogen trioxide? N2O3 • Give formulae for: lithium sulfide, dinitrogen Day 2 monoxide, lead(IV) sulfate Assignment Naming Bases 1. Name each according to IUPAC rules: • Bases contain an OH group •CH O does not have an OH group a) ZnS, b) FeCl3, c) CaCO3, d) P2O5, e) NaCN, 6 12 6 • If an OH group is present it will be clearly f) N2F2, g) MgHPO4, h) Cu(BrO3)2, i) K2O, j) BF3 2. Give the valence of a) Fe in FeO, b) Mn in MnO indicated: e.g. NaOH, Ca(OH)2 2 • Also notice that bases have a metal (or positive 3. Write formulas for: a) sodium oxide, ion such as NH + at their beginning) b) potassium iodide, c) plumbic sulfide, 4 • Bases are named like other ionic compounds: d) mercury(I) oxide, e) ferrous oxide, • +ve is named first, followed by the polyatomic ion f) iron(II) phosphate, g) copper(II) fluoride, h) dichlorine monoxide, i) silver sulfide, Ca(OH)2 j) magnesium nitride, k) aluminum hypochlorite, CuOH l) iodine pentafluoride, m) calcium chromate, aluminum hydroxide n) diphosphorus pentasulfide ammonium hydroxide Naming Acids: Binary acids Naming Acids: Oxyacids • Naming does not depend on the state (aq) • All acids start with H (e.g.
    [Show full text]
  • Selective Benzylic C–H Monooxygenation Mediated by Iodine Oxides
    Selective benzylic C–H monooxygenation mediated by iodine oxides Kelsey B. LaMartina1, Haley K. Kuck1, Linda S. Oglesbee1, Asma Al-Odaini1 and Nicholas C. Boaz*1,2,3 Full Research Paper Open Access Address: Beilstein J. Org. Chem. 2019, 15, 602–609. 1Department of Chemistry and Physics, North Central College, 30 N. doi:10.3762/bjoc.15.55 Brainard Street, Naperville, IL 60540 USA, 2Department of Chemistry, Frick Chemical Laboratory, Princeton University, Washington Road, Received: 13 December 2018 Princeton, NJ 08544 USA and 3Permanent address: Department of Accepted: 19 February 2019 Chemistry, North Central College, 30 N. Brainard Street, Naperville, IL Published: 05 March 2019 60540 USA; phone: +1-630-637-5187. Associate Editor: C. Stephenson Email: Nicholas C. Boaz* - [email protected] © 2019 LaMartina et al.; licensee Beilstein-Institut. License and terms: see end of document. * Corresponding author Keywords: acetoxylation; benzylic; iodate; NHPI; oxidation; radical Abstract A method for the selective monooxdiation of secondary benzylic C–H bonds is described using an N-oxyl catalyst and a hyperva- lent iodine species as a terminal oxidant. Combinations of ammonium iodate and catalytic N-hydroxyphthalimide (NHPI) were shown to be effective in the selective oxidation of n-butylbenzene directly to 1-phenylbutyl acetate in high yield (86%). This method shows moderate substrate tolerance in the oxygenation of substrates containing secondary benzylic C–H bonds, yielding the corresponding benzylic acetates in good to moderate yield. Tertiary benzylic C–H bonds were shown to be unreactive under similar conditions, despite the weaker C–H bond. A preliminary mechanistic analysis suggests that this NHPI-iodate system is functioning by a radical-based mechanism where iodine generated in situ captures formed benzylic radicals.
    [Show full text]
  • Dissociation Constants of Inorganic Acids and Bases
    DISSOCIATION CONSTANTS OF INORGANIC ACIDS AND BASES The data in this table are presented as values of pKa, defined as can be calculated from the equation the negative logarithm of the acid dissociation constant K for the a − + reaction OH NH4 = = KKb water/K a []NH BH B– + H+ 3 + where K = 1.01 10–14 at 25 °C. Note that pK + pK = pK . Thus pKa = –log Ka , and the hydrogen ion concentration [H ] can water × a b water be calculated from All values refer to dilute aqueous solutions at zero ionic strength at the temperature indicated. The table is arranged alphabetically + − HB by compound name. = K a [] BH Reference In the case of bases, the entry in the table is for the conjugate acid; – 1. Perrin, D. D., Ionization Constants of Inorganic Acids and Bases in e.g., ammonium ion for ammonia. The OH concentration in the Aqueous Solution, Second Edition, Pergamon, Oxford, 1982. system + – NH3 + H2O NH4 + OH Name Formula Step t/°C pKa Aluminum(III) ion Al+3 25 5.0 Ammonia NH3 25 9.25 Arsenic acid H3AsO4 1 25 2.26 2 25 6.76 3 25 11.29 Arsenious acid H2AsO3 25 9.29 Barium(II) ion Ba+2 25 13.4 Boric acid H3BO3 1 20 9.27 2 20 >14 Calcium(II) ion Ca+2 25 12.6 Carbonic acid H2CO3 1 25 6.35 2 25 10.33 Chlorous acid HClO2 25 1.94 Chromic acid H2CrO4 1 25 0.74 2 25 6.49 Cyanic acid HCNO 25 3.46 Germanic acid H2GeO3 1 25 9.01 2 25 12.3 Hydrazine N2H4 25 8.1 Hydrazoic acid HN3 25 4.6 Hydrocyanic acid HCN 25 9.21 Hydrofluoric acid HF 25 3.20 Hydrogen peroxide H2O2 25 11.62 Hydrogen selenide H2Se 1 25 3.89 2 25 11.0 Hydrogen sulfide H2S 1
    [Show full text]
  • Periodic Acid
    Periodic acid sc-215695 Material Safety Data Sheet Hazard Alert Code Key: EXTREME HIGH MODERATE LOW Section 1 - CHEMICAL PRODUCT AND COMPANY IDENTIFICATION PRODUCT NAME Periodic acid STATEMENT OF HAZARDOUS NATURE CONSIDERED A HAZARDOUS SUBSTANCE ACCORDING TO OSHA 29 CFR 1910.1200. NFPA FLAMMABILITY0 HEALTH3 HAZARD INSTABILITY2 OX SUPPLIER Company: Santa Cruz Biotechnology, Inc. Address: 2145 Delaware Ave Santa Cruz, CA 95060 Telephone: 800.457.3801 or 831.457.3800 Emergency Tel: CHEMWATCH: From within the US and Canada: 877-715-9305 Emergency Tel: From outside the US and Canada: +800 2436 2255 (1-800-CHEMCALL) or call +613 9573 3112 PRODUCT USE Oxidising agent, increasing wet strength of paper, photographic paper. SYNONYMS H5IO6, "per-iodic acid", "orthoperiodic acid", "o-periodic acid", "o-periodic acid" Section 2 - HAZARDS IDENTIFICATION CANADIAN WHMIS SYMBOLS EMERGENCY OVERVIEW RISK Contact with combustible material may cause fire. Causes burns. Risk of serious damage to eyes. POTENTIAL HEALTH EFFECTS 1 of 14 Periodic acid sc-215695 Material Safety Data Sheet Hazard Alert Code Key: EXTREME HIGH MODERATE LOW ACUTE HEALTH EFFECTS SWALLOWED ! The material can produce chemical burns within the oral cavity and gastrointestinal tract following ingestion. ! Accidental ingestion of the material may be damaging to the health of the individual. ! Ingestion of acidic corrosives may produce burns around and in the mouth. the throat and esophagus. Immediate pain and difficulties in swallowing and speaking may also be evident. Swelling of the epiglottis may make it difficult to breathe which may result in suffocation. More severe exposure may result in vomiting blood and thick mucus, shock, abnormally low blood pressure, fluctuating pulse, shallow respiration and clammy skin, inflammation of stomach wall, and rupture of esophageal tissue.
    [Show full text]