DOCSLIB.ORG

The Reaction of Barium Manganate with Acids and Their Precursors

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
The Reaction of Barium Manganate with Acids and Their Precursors Indian Journal of Chemistry Vol. 38A. September 1999, pp.966-968 The reaction of barium manganate with fraction data were collected on a Phillips PW 3710 acids and their precursors diffractometer, with a Cu monochromator. Synthesis oj barium manganate (VI) Liszlo Kotai, Agnes Keszler, Janos Pato. Sandor Holly Chemical Research Center, Institute of Chemistry. KMn04 (15.8 g) was dissolved in 300 ml of water, Hungarian Academy of Sciences then BaCI2.2Hp (24.9 g dissolved in 100 ml of water), H-1025, Budapest, Pusztaseri u. 59-67, Hungary KOH (56 g dissolved in 100 ml of water) and KI (2.0 g and dissolved in 20 ml of water) were added with vigorous Kalyan K Banerji ' Department of Chemistry, J N V University, stirring. The mixture was boiled for 15 min, cooled, Jodhpur 342 005, India filtered, and washed. The permanganate-free product was dried at 105° C for I h, then the traces of water were Received 30 November 1998; revised 4 Mal' 1999 removed by azeotropic distillation with benzene (yield - 100%). Analysis (found/calc. fo r BaMn0 ): Ba 53.69/ 4 A simple and easy preparative route to obtain permangani c ac id 53.59%; Mn 21.40121.44%. and permanganate salts from barium manganate and sulphuric acid is described. Sulphuric acid reacts with bari um manganate to pro­ duce sparingly soluble bariulll sulphate and well-soluble permanga­ Synthesis ojpermanganic acid nic ac id or bariulll permanganate, these in turn can be usee! to pre­ To barium manganate (2.56 g, 0 .0 I mol) suspended pare ot her metal permanganates. in 50 ml of di stilled water, sulphuric acid ( 100 ml , 0 . 1 mol) was added with stirring. The stirring was contin­ ued for I h. The reaction mixture was filtered and per­ Permanganates are widely used in organic syntheses as manganic acid was titrated with NaOH potentiometri­ selective oxidizing agentsl . Barium permanganate is su it­ cally using a glass e lectrode (PH 5.5). The product, so­ able for selective oxidation itsclf2-6 and can be used as dium permanganate trihydrate, was crystall ized and iden­ starting materi al for the synthesis of several other metal tified by IR spectroscopy; yield - 100%. 7 X permanganates als0 . • The reaction of permallganic acid with oxides, hydroxides or carbonate' yields a lot of cIe­ SYllthesis of barium permanganate ri vati ves') . Bariu m manganate (2.56 g, 0.01 mol) was suspended Synthesis of barium pennanganate starts from barium in 100 ml of di stilled water. Then sulphuric acid (55 ml , manganate which itself is obtained in pure form from 0. 1 mol) was added over I h with slow stirring and then potassium permanganate and water soluble barium salts. refluxed for 15 min. The reaction mixture was filte red Reported methods for the conversion of barium manga­ and concentrated while barium permanganate crystal­ nate to the corresponding permanganare are compl icated lized (yield: 0.7 g), analysis [found/calc. for Ba(Mn04)2]: procedures. In this note, the synthesis of permanganic Ba 36.57/36.61% ; Mn 29.30129 .28%. acid and barium permanganate and their use in the syn­ thesis of several other metal permanganates are reported. Reaction of barium l1Iangana fe with sodium hydrogen carbonate Experimental Barium manganate (2.56 g, 0.0 I mol) was suspended Analytical grade reagents (Aldrich) and double-dis­ in 100 ml distilled water and calculated amounts of tilled water were used throughout. The IR spectra were NaHC01 (Ba:Na = I :0.75, I: I, I: 1.34 mol) was added. obtained in nujolmull with NICOLET 205 FT-IR spec­ The mixture was slowly stirred for I h a nd then refluxed trometer and by diffuse reflectance technique in KBr with for 30 min . The reaction mixture was filtered and crys­ NICOLET 170SX spectrometer in the range of 400-4000 talli zed. According to TR spectroscopy and X-ray l cm· . rcp measurements were made with Atomscan 25 diffractometry, the products contai ned Ba(Mn04)2' (Thermo Jarral Ash) spectrometer. X-ray powder dif- NaMn04 and Na2CO, in different ratios. NOTES 967 Reaction ofbarium manganate with ammonium sulphate To barium manganate (2.56 g, 0.01 mol), suspended Table 1- Comparison of effecti ve charge values and acidity of some in 100 mol distilled water, was added ammonium sul­ inorganic oxoacids '4 phate (1.24 g, 0.0 I mol). The reaction mixture was stirred Oxoacid 8 8,,1 8 <jl for I h and then refluxed for I h. The mixture turned 11 8, / x dark violet and intense odor of ammonia was obtained. H S0 +0.38 -0.46 -0.36 +0.88 1.125 The reaction mixture was filtered, concentrated and crys­ l 4 HMn04 +0.37 -0.53 -0.46 +1 .56 1.114 tallized. According to IR spectroscopy the water-soluble HlMnO.j· +0.37 -0.52 -0.42 +1.42 1.106 product was ammonium permanganate. Even if 2/3 HlCO +0.39 -0.50 -0.42 +0.67 0.965 amount of ammonium sulphate used, the only product J formed, under similar conditions, was ammonium per­ • Our calculation manganate. sulphuric acid. The ionic character of the hydroxy Is Results and discussion (8i8o) are nearly similar in manganic and permanganic Synthesis of barium manganate in alkaline medium acids but the polarizing effect of the central atom is higher from potassium permanganate and barium chloride in in permanganic acid. Consequently manganic acid is the presence of an alkali iodide is a well-known reaction easily formed from barium manganate and sulphuric acid (I). It results in the fornlation of insoluble barium man­ due to the hi'gh acidity of sulphuric acid as well as the ganate, which can be obtained in dry form after insolubility of barium sulphate. Carbonic acid being azeotropic distillation of water with benzene. weaker than manganic acid, the main driving force of the reaction is the formation of insoluble barium car­ ~ 6 KMnO, + 6BaCI 2 + 6 KOH + KI BaMn04 + 12 KCI bonate. However, it is an equilibrium process and disso­ + KIO, + 3 Hp .. .. (1) lution of barium carbonate in manganic acid takes place. Manganic acid disproportionates to permanganic acid Unstable manganic acid is formed when barium manga­ and manganese dioxide (3). This reaction (log K = 58) nate is treated with sulphuric or carbonic acid (2). It takes place completely in acidic, neutral or slightly al­ disproportionates to permanganic acid and manganese kaline media". dioxide (3). Due to these facts permanganic acid is formed quickly from barium manganate and SUlphuric acid via dispro­ ... (2) portionation of manganic acid (5). Thus this method is where X = S04 or CO, suitable for the preparation of permanganic acid. 3 BaMn0 + 3 H S0 ~ 2 HMn04 + 3 BaS0 + Mn02 + 2 Hp .. (3) 4 2 4 4 .. (5) Dissociation constant of manganic acid has not been determined so far. In order to explain the mechanism of Permanganic acid being a relatively strong acid re·­ these reactions, the relative strengths of the acids mu st acts easily with metal oxides, hydroxides or carbonates. be known. To estimate them, a method published earlier This method can be used to synthesize any permangan­ has been used l4 . Effective charges of the atoms of man­ ate. ganic acid and <p constants which characterize the acid The analogous reaction between barium manganate, water and carbon dioxide yield only very small amount .. strength IS were calculated using relation (4) . of manganic acid as expected from the relative strength .. (4) of the acids. Consequently longer time is required to obtain a significant amount of permanganic acid. Barium where <p means the acid strength, 8H' 8 and 8 mean the carbonate is soluble in permanganic acid (latter being a 0 x relative charges of the H,O, and X(S,C or Mn) atoms stronger acid) and this reaction has been reported as a respectively. The results are presented in Table I. method of preparation of barium permanganatelO. 12 but The data showed that manganic acid is a stronger acid this method is less favourable than the new method re­ than carbonic acid but is weaker than permanganic or ported here. 968 INDIAN J CHEM, SEC. A , SEPTEMBER 1999 To understand the reaction of barium manganate with While NaHCO, is a source of carbonic acid at slightly carbonic acid (2), it was considered essential to study its alkaline pH, ammonium sulphate behaves as a slightly reaction with sodium hydrogencarbonate. NaHCO, gen­ acidic sulphuric acid precursor (8). erates carbonic acid in boiling solutions which can form barium permanganate as per reaction (2) .. (8) ... (6) The reaction of sulphuric acid and BaMn04 results in the formation of permanganic acid. The end product of Sodium carbonate can be detected by IR spectroscopy. the reaction of permanganic acid and ammonium hydrox­ The reaction of barium permanganate and sodium car­ ide is ammonium permanganate. bonate yields barium carbonate and sodium permangan­ Equivalent amounts of ammonium sulphate and ate trihydrate. When the molar ratio of the reactants is barium manganate yield 2/3 mol ammonium permanga­ I : I , the main product is barium permanganate and a small nate while ammonia is evolved. Using 2/3 mol of am­ amount of sodium permanganate trihydrate is formed. monium sulphate, the ex pected product is barium per­ Similar results are obtained when an excess of barium manganate (in analogy with sulphuric acid) but in prac­ manganate is used. However, an excess of NaHCn, ti ce ammonium permanganate was the product. Prob­ ( I: 1.34) enhances the reaction between barium perman­ ably, manganic acid reacts rapidly with ammonia before ganate and sodium hydrogencarbonate and the main anything else can happen.
Load more

Recommended publications
  • Transport of Dangerous Goods
    ST/SG/AC.10/1/Rev.16 (Vol.I) Recommendations on the TRANSPORT OF DANGEROUS GOODS Model Regulations Volume I Sixteenth revised edition UNITED NATIONS New York and Geneva, 2009 NOTE The designations employed and the presentation of the material in this publication do not imply the expression of any opinion whatsoever on the part of the Secretariat of the United Nations concerning the legal status of any country, territory, city or area, or of its authorities, or concerning the delimitation of its frontiers or boundaries. ST/SG/AC.10/1/Rev.16 (Vol.I) Copyright © United Nations, 2009 All rights reserved. No part of this publication may, for sales purposes, be reproduced, stored in a retrieval system or transmitted in any form or by any means, electronic, electrostatic, magnetic tape, mechanical, photocopying or otherwise, without prior permission in writing from the United Nations. UNITED NATIONS Sales No. E.09.VIII.2 ISBN 978-92-1-139136-7 (complete set of two volumes) ISSN 1014-5753 Volumes I and II not to be sold separately FOREWORD The Recommendations on the Transport of Dangerous Goods are addressed to governments and to the international organizations concerned with safety in the transport of dangerous goods. The first version, prepared by the United Nations Economic and Social Council's Committee of Experts on the Transport of Dangerous Goods, was published in 1956 (ST/ECA/43-E/CN.2/170). In response to developments in technology and the changing needs of users, they have been regularly amended and updated at succeeding sessions of the Committee of Experts pursuant to Resolution 645 G (XXIII) of 26 April 1957 of the Economic and Social Council and subsequent resolutions.
    [Show full text]
  • Carbonyl Compounds
    Carbonyl Compounds What are Carbonyl Compounds? Carbonyl compounds are compounds that contain the C=O (carbonyl) group. Preparation of Aldehydes: 1. Preparation from Acid Chloride (Rosenmund Reduction): This reaction was named after Karl Wilhelm Rosenmund, who first reported it in 1918. The reaction is a hydrogenation process in which an acyl chloride is selectively reduced to an aldehyde. The reaction, a hydrogenolysis, is catalysed by palladium on barium sulfate, which is sometimes called the Rosenmund catalyst. 2. Preparation from Nitriles: This reaction involves the preparation of aldehydes (R-CHO) from nitriles (R- CN) using SnCl2 and HCl and quenching the resulting iminium salt ([R- + − CH=NH2] Cl ) with water (H2O). During the synthesis, ammonium chloride is also produced. The reaction is known as Stephen Aldehyde synthesis. Dr. Sumi Ganguly Page 1 3. Preparation from Grignard Reagent: When Grignard Reagent is reacted with HCN followed by hydrolysis aldehyde is produced. Preparation of Ketones: 1. Preparation from Acid Chloride (Friedel-Crafts Acylation): Acid chlorides when reacted with benzene in presence of anhydrous AlCl3, aromatic ketone are produced. However, only aromatic ketones can be prepared by following this method. In order to prepare both aromatic and aliphatic ketones acid chlorides is reacted with lithium dialkylcuprate (Gilman Reagnt). Dr. Sumi Ganguly Page 2 The lithium dialkyl cuprate is produced by the reaction of two equivalents of the organolithium reagent with copper (I) iodide. Example: 3. Preparation from Nitriles and Grignard Reagents: When Grignard Reagent is reacted with RCN followed by hydrolysis aldehyde is produced. Dr. Sumi Ganguly Page 3 Physical Characteristic of Carbonyl Compounds: 1) The boiling point of carbonyl compounds is higher than the alkanes with similar Mr.
    [Show full text]
  • 1,45%,562 UNITED SATES P All.‘ Bl If" Til?
    Patented May 1, 1923. 1,45%,562 UNITED SATES P All.‘ bl if" til? . ROBERT E. WILSON, LEON ‘JV. PARSONS, AND STANLEY 1E. OHXSHOLIYI, OF WASHINGTON, DISTRICT OF COLUMBIA. PROCESS THE PRODUCTION OE‘ All‘HALLEAETELMLETAL PERTJIANGANATES. N0 Drawing". Application ?led September 27, 1918. Serial No. 255,975. To (all to]: am it may concern. .' manganate by oxidation or acidification, Be it known that we, Romain‘ E. lllinsou, metatheses into calcium pern'iangamite by LEON “7. Parsons, and STANLEY L. Unis treatment With calcium sulphate or milk at HoLM, citizens of the United States. and sta lime. tioned at ViTashington, District of Columbia, O'li' these four possible methods, (1.) is not 60 in the o?icc of the Director the Chemical a possible large scale method. on account l/Varfare Service, Research Division, have in of its use ot silver; (2) and are elec vented a Process for the ll’roduction oif Al trolytic methods Without a. great deal out kali-Earth-l\letal Permanpjanates, of which promise, and are to be considered elsewhere; ll) the ‘following is a speci?cation. (ll) the principal subject of this applica G3 in The present invention relates to the pro tion. duction oi? alkah» earth metal permangam Three distinct methods for preparing: ba~ nates and especially the permanganates of rium (or strontium) manganate have been calcium and magnesium as these have beenv here investigated. The ?rst of? these meth found to be very ellicient oxidizing agents ods involves heating together barium perox 70 for certain purposes, more e?icient even. than ide, hydroxide, or a salt, such as the nitrate the permanganates of the allmliearth metals.
    [Show full text]
  • Safety Practices in Chemistry Laboratories
    4/24/2012 Safety Practices in Chemistry Laboratory Sam Tung, HSE Specialist, CIH, RSO Health Safety and Environment Office, Hong Kong University of Science and Technology Contents 1. Introduction to Legislations related to Chemistry Laboratories 2. Introduction to Chemical Hazards 3. Criteria of Design for Laboratory Ventilation 4. Operations and Maintenance of Laboratory Fume hood 5. Case Studies of Laboratory Accidents 6. Handling of Chemical Spills 7. Emergency Response Equipment 1 4/24/2012 Importance of Health and Safety To protect your health and safety (and environment) To protect your colleagues’ and students’ health and safety Case Study: Laboratory Fire Kills UCLA Researcher A 23-year-old research assistant working at UCLA who was seriously burned in a lab fire in December 2008 recently died from her injuries. She was trying to transfer up to 2 ounces (~50ml) of t-butyl lithium (pyrophoric chemical), which was dissolved in pentane from one sealed container to another by a 50 ml syringe. The barrel of the syringe was either ejected or pulled out of the syringe, causing liquid to be released. A flash fire set her clothing ablaze and spread second- and third-degree burns over 43% of her body. 2 4/24/2012 Root Causes of the Accident Poor technique and improper method Use a 50ml syringe to transfer~50 ml pyrophoric chemical Should use a 100ml syringe Should use Cannula Method for transfer of pyrophoric chemical > 50 ml Lack of proper training No safety training record Lack of supervision No follow up actions had been
    [Show full text]
  • Manufacturing of Potassium Permanganate Kmno4  This Is the Most Important and Well Known Salt of Permanganic Acid
    Manufacturing of Potassium Permanganate KMnO4 This is the most important and well known salt of permanganic acid. It is prepared from the pyrolusite ore. It is prepared by fusing pyrolusite ore either with KOH or K2CO3 in presence of atmospheric oxygen or any other oxidising agent such as KNO3. The mass turns green with the formation of potassium manganate, K2MnO4. 2MnO2 + 4KOH + O2 →2K2MnO4 + 2H2O 2MnO2 + 2K2CO3 + O2 →2K2MnO4 + 2CO2 The fused mass is extracted with water. The solution is now treated with a current of chlorine or ozone or carbon dioxide to convert manganate into permanganate. 2K2MnO4 + Cl2 → 2KMnO4 + 2KCl 2K2MnO4 + H2O + O3 → 2KMnO4 + 2KOH + O2 3K2MnO4 + 2CO2 → 2KMnO4 + MnO2 + 2K2CO3 Now-a-days, the conversion is done electrolytically. It is electrolysed between iron cathode and nickel anode. Dilute alkali solution is taken in the cathodic compartment and potassium manganate solution is taken in the anodic compartment. Both the compartments are separated by a diaphragm. On passing current, the oxygen evolved at anode oxidises manganate into permanganate. At anode: 2K2MnO4 + H2O + O → 2KMnO4 + 2KOH 2- - - MnO4 → MnO4 + e + - At cathode: 2H + 2e → H2 Properties: It is purple coloured crystalline compound. It is fairly soluble in water. When heated alone or with an alkali, it decomposes evolving oxygen. 2KMnO4 → K2MnO4 + MnO2 + O2 4KMnO4 + 4KOH → 4K2MnO4 + 2H2O + O2 On treatment with conc. H2SO4, it forms manganese heptoxide via permanganyl sulphate which decomposes explosively on heating. 2KMnO4+3H2SO4 → 2KHSO4 + (MnO3)2SO4 + 2H2O (MnO3)2SO4 + H2O → Mn2O7 + H2SO4 Mn2O7 → 2MnO2 + 3/2O2 Potassium permanganate is a powerful oxidising agent. A mixture of sulphur, charcoal and KMnO4 forms an explosive powder.
    [Show full text]
  • Revision Guide
    Revision Guide Chemistry - Unit 3 Physical and Inorganic Chemistry GCE A Level WJEC These notes have been authored by experienced teachers and are provided as support to students revising for their GCE A level exams. Though the resources are comprehensive, they may not cover every aspect of the specification and do not represent the depth of knowledge required for each unit of work. 1 Content Page Section 2 3.1 – Redox and standard electrode potential 13 3.2 - Redox reactions 20 3.3 - Chemistry of the p-block 30 3.4 - Chemistry of the d-block transition metals 35 3.5 - Chemical kinetics 44 3.6 - Enthalpy changes for solids and solutions 50 3.7 - Entropy and feasibility of reactions 53 3.8 - Equilibrium constants 57 3.9 - Acid-base equilibria 66 Acknowledgements 2 3.1 – Redox and standard electrode potential Redox reactions In AS, we saw that in redox reactions, something is oxidised and something else is reduced (remember OILRIG – this deals with loss and gain of electrons). Another way that we can determine if a redox reaction has happened is by using oxidation states or numbers (see AS revision guide pages 2 and 44). You need to know that: - • oxidation is loss of electrons • reduction is gain of electrons • an oxidising agent is a species that accepts electrons, thereby helping oxidation. It becomes reduced itself in the process. • a reducing agent is a species that donates electrons, thereby helping reduction. It becomes oxidised itself in the process. You also should remember these rules for assigning oxidation numbers in a compound: - 1 All elements have an oxidation number of zero (including diatomic molecules like H2) 2 Hydrogen is 1 unless it’s with a Group 1 metal, then it’s -1 3 Oxygen is -2 (unless it’s a peroxide when it’s -1, or reacted with fluorine, when it’s +2).
    [Show full text]
  • Synthesis and Properties of Simple and Complex Salts Of
    PhD Theses SYNTHESIS AND PROPERTIES OF SIMPLE AND COMPLEX SALTS OF PERMANGANIC ACID Kótai László Institute of Materials and Environmental Chemistry Chemical Research Center, Hungarian Academy of Sciences 2006 1 1. INTRODUCTION AND AIMS Widespread applicapibility and the increased quality requirements of permanganate salts require development of new synthetic methods. The transition metal permanganates are precursors of numerous catalytically active metal-manganese oxide composites. Therefore, the exact kowledge of their structure, reactivity and the thermal decomposition characteristics of permanganate compounds is essenial to plan the properties of the decomposition products. The main target of this work was the development of new synthetic methods to prepare simple and complex salts of permanganic acid, including the preparation and the study of ammonium permanganate and some ammine-complex permanganates of transition metals such as Ag, Cu, Ni, Cd, Zn. 2. ANALYTICAL METHODS Classical inorganic analytical chemistry, IR and Raman spectroscopy, UV-VIS spectroscopy, ESR, XRD, GC-MS, single crystal X-ray and powder neutron diffractometry, TG-gas- titrimetry, TG-MS and DSC methods were used. 3. NEW RESULTS 3.1. SYNTHESES 3.1.1. Syntheses based on manganese heptoxide A method has been developed to prepare Ba, Mg, Ca, Ni, Zn, Cd, Cu(II), Al, Fe(III), Y, Ce(IV), Sm, Pr and Gd-permanganates by means of the reaction of KMnO4 with sulfuric acid monohydrate, followed by extraction of the Mn2O7 with CCl4 and the reaction of the Mn2O7 in CCl4 with catalytic amount of water and the oxide, hydroxide and carbonate of the appropriate metal. 3.1.2. Syntheses based on the metathesis reaction of KMnO4 Reaction of warm saturated solutions of NH4Cl and potassium permangnate provided Kx(NH4)1-xMnO4 (x=0.2-0.4) solid solutions instead of NH4MnO4 as it has been declared previously.
    [Show full text]
  • Prohibited and Restricted Chemical List
    School Emergency Response Plan and Management Guide Prohibited and Restricted Chemical List PROHIBITED AND RESTRICTED CHEMICAL LIST Introduction After incidents of laboratory chemical contamination at several schools, DCPS, The American Association for the Advancement of Science (AAAS) and DC Fire and Emergency Management Services developed an aggressive program for chemical control to eliminate student and staff exposure to potential hazardous chemicals. Based upon this program, all principals are required to conduct a complete yearly inventory of all chemicals located at each school building to identify for the removal and disposal of any prohibited/banned chemicals. Prohibited chemicals are those that pose an inherent, immediate, and potentially life- threatening risk, injury, or impairment due to toxicity or other chemical properties to students, staff, or other occupants of the school. These chemicals are prohibited from use and/or storage at the school, and the school is prohibited from purchasing or accepting donations of such chemicals. Restricted chemicals are chemicals that are restricted by use and/or quantities. If restricted chemicals are present at the school, each storage location must be addressed in the school's written emergency plan. Also, plan maps must clearly denote the storage locations of these chemicals. Restricted chemicals—demonstration use only are a subclass in the Restricted chemicals list that are limited to instructor demonstration. Students may not participate in handling or preparation of restricted chemicals as part of a demonstration. If Restricted chemicals—demonstration use only are present at the school, each storage location must be addressed in the school's written emergency plan. Section 7: Appendices – October 2009 37 School Emergency Response Plan and Management Guide Prohibited and Restricted Chemical List Following is a table of chemicals that are Prohibited—banned, Restricted—academic curriculum use, and Restricted—demonstration use only.
    [Show full text]
  • Basic Description for Ground and Air Hazardous
    BASIC DESCRIPTION FOR GROUND AND AIR GROUND AND AIR HAZARDOUS MATERIALS SHIPMENTS GROUND SHIPMENTS AIR SHIPMENTS SHIPMENTS HAZARD DOT DOT CLASS OR MAXIMUM EXEMPTION, GROUND EXEMPTION, HAZARDOUS MATERIALS DESCRIPTIONS DIVISION I.D. NUMBER LABEL(S) REQUIRED OR QUANTITY PER SPECIAL SERVICE TO LABEL(S) REQUIRED OR MAXIMUM NET CARGO SPECIAL NON-BULK AND PROPER SHIPPING NAME (Subsidiary if (ALSO MARK PACKING EXEMPTION, SPECIAL PERMIT INNER PERMIT CANADA EXEMPTION, SPECIAL PERMIT QUANTITY PER AIRCRAFT PERMIT SPECIAL EXCEPTIONS PACKAGING (ALSO MARK ON PACKAGE) applicable) ON PACKAGE) GROUP OR EXCEPTION RECEPTACLE OR 173.13 PERMITTED OR EXCEPTION PACKAGE** QUANTITY OR 173.13 PROVISIONS §173.*** §173.*** (1) (2) (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) (13) (14) (15) Accellerene, see p-Nitrosodimethylaniline Accumulators, electric, see Batteries, wet etc Accumulators, pressurized, pneumatic or hydraulic (containing non-flammable gas), see Articles pressurized, pneumatic or hydraulic (containing non-flammable gas) FLAMMABLE FLAMMABLE Acetal 3 UN1088 II LIQUID * YES LIQUID * 5 L 150 202 FLAMMABLE Acetaldehyde 3 UN1089 I LIQUID YES Forbidden None 201 May not be regulated when shipped via UPS Acetaldehyde ammonia 9 UN1841 III ground YES CLASS 9 * 30 kg 30 kg 155 204 FLAMMABLE FLAMMABLE Acetaldehyde oxime 3 UN2332 III LIQUID * YES LIQUID * 25 L 150 203 CORROSIVE, CORROSIVE, Acetic acid, glacial or Acetic acid solution, FLAMMABLE FLAMMABLE A3, A6, with more than 80 percent acid, by mass 8 (3) UN2789 II LIQUID * YES LIQUID * 1 L A7, A10 154 202 Acetic
    [Show full text]
  • A Manganate Ester Hydrolysis Mn(IV)
    LECTURE 7 (a) Dihydroxylation (X = Y = OH) Although dihydroxylation is formally the addition of hydrogen peroxide, in practice the addition of H2O2 to alkenes is almost impossible. Two reagents which work especially well for this overall addition are cold, neutral potassium permanganate, KMnO4, and osmium tetroxide, OsO4. They complement one another in that the first is used in aqueous solution whereas the latter is used in organic solvents. The mechanisms are very similar. Thus both proceed through a pericyclic mechanism: O O O O Mn(VII) Mn(V) +- K+-O O K O O a manganate ester hydrolysis O OH HO Mn(IV)O2 + KOH + 0.5 H2O2 Mn(V) + +- K O OH HO O O O O Os(VIII) Os(VI) O O O O an osmate ester, yellow black Because osmium tetroxide is expensive and very toxic it is rarely used in stoichiometric amounts. Rather a co-oxidant is added to oxidise the stable osmate ester back to OsO4. Since we want to hydrolyse the osmate ester as well, the co-oxidant is often aqueous hydrogen peroxide so the oxidation is two-phase. The alkene and the OsO4 remain in the organic phase, the H2O2 is in the aqueous phase and the osmate ester is at the interface between the two phases: H OH H OH H OsO4, + aq.H2O2, CH Cl H 2 2 OH H H OH (c) Epoxidation (X = Y = O) The reaction of alkenes with peroxy acids (RCO3H) leads to a cyclic ether, known as an epoxide, as follows: R R O O O H O H O O Although the reaction will work with peroxyacetic acid (R = Me) it works best with peroxy acids bearing electron-withdrawing groups e.g.
    [Show full text]
  • The True Formula
    ON THE TRUE FORMULA FOR PERMANGANATES. DISSERTATION PRESENTED TO THE FACULTY OF THE UNIVERSITT7 ' OF VIRGINIA. In application fir the Degree of Dadar of 'Pflilawplzj'. BY CHARLES M. B‘RADBURY, 0F VIRGINIA. THESIS —Permanga;zz}: acid is moiwéaszc, and the per-:V _ mangamztes are represented 6}! the generalfbmwla R (Mn 04 p. -' : . ; V To His Fat/tor, 31m ‘18. granary, (35511. 77:13 Paper is Inscribed IN TOKEN OF AFFECTION, BY film 9mm, Preface. The greater part of the following paper was written nearly a year ago. As it was nearing completion, I found, from an allusion in .an article by M. Raoult, of Paris, (see Bzzlleiz'n dc Soc. C/u'm. de Paris, XLVI, p. 805), that my conclusion as to the true formula for permanganates had been reached already by that eminent chemist, by means of a new method, origi- nated by himself, for determining molecular weights. Upon examining M. Raoult‘s original papem‘fHéWIz—Iifilc C/zz'm. ct dc Ply/5., (6), VIII, July, 1886, p. 3 30, however, it was found that nothing was given concerning permanganates, beyond the simple statement that they were shown by the method to be monobasic. T Dr. Victor Meyer and Dr. Auwers, of Gottingen, have recently extended and simplified the method of M. Raoult, (see Berk/zit a’n’ Dads. Chem. 656115., for February 27 and March 12, 1888), and I am therefore enabled to add materially to the evidence already collected in the dissertation, by a con- vincing application of this method. ‘ Had the detailed results of M.
    [Show full text]
  • Studies on the Behavior of Spontaneous Reductive Decomposition of Hydrogen Permanganate in Water for HP/CORD Process
    Studies on the Behavior of Spontaneous Reductive Decomposition of Hydrogen Permanganate in Water for HP/CORD Process Hyun-Kyu Lee*, June-Hyun Kim, Won-Zin Oh, and Sang-June Choi Kyungpook National University, 80 Daehakro, Bukgu, Daegu 41566, Republic of Korea *[email protected] 1. Introduction (Optima 2100DV, PerkinElmer Co., USA), respectively, for determining whether the cation + + The permanganic acid (HMnO4) as oxidizing agent exchange (K ˧H ) was completely conducted. is usually used to dissolve the NPP oxide layers containing Cr (III) in HP/CORD process [1]. 2.3 Apparatus and procedure However, little attention has been made for the spontaneous reductive decomposition of HMnO4, All experiments were carried out in 500 mL glass which is a competing reaction with the oxidation of reaction vessels equipped with reflux condenser, the chromium oxide by permanganate. The objective thermometer, mechanical stirrer, and electric heating of this study is to investigate the spontaneous mantle. Reaction volumes were nomally 200 mL and reductive decomposition behavior of HMnO4 for were stirred at 250 rpm. The temperature was HP/CORD process, depending on the variation of maintained at 90°C. Aliquots obtained from each initial concentration of HMnO4. experiment were quickly cooled, diluted, and placed in a dark bottle to avoid further reaction. The concentration of residual permanganate was 2. Materials and methods determined by UV-visible spectrophotometer (Agilent 8453, Agilent technologies, USA) after 2.1 Reagents filtration (0.2 um, Whatman, nylon membrane filters). All reagents were analytical grade and were used 3. Results and discussion without further purification. Deionized water (18.3 Mȍācm), which was prepared using a water 3.1 Effect of the initial concentration of HMnO purification system (Nex Power 1000, Human 4 corporation, Korea) was used to prepare all aqueous The change of concentration of residual solutions.
    [Show full text]