DOCSLIB.ORG

Kinetic Studies on Permanganate Oxidation of Acetophenones Under

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Kinetic Studies on Permanganate Oxidation of Acetophenones Under Indi an Journal of Chemistry Vol. 40A, June 2001, pp. 610-612 Kinetic studies on permanganate oxidation of The ketones were further purified by vacuum acetophenones under phase transfer catalysis distillation. The solvents employed were purified by standard methods and doubly distilled water was P S Sheeba & T D Radhakrishnan Nair* always used. The catalysts used were tricapryl­ Department of Chemistry, Calicut University methylammonium chloride (TCMAC) and tetrabutyl­ Calicut University P.O., Kerala 673 635. India ammonium bromide (TBAB). The former has Received 18 October 2000; revised 8 March 2001 relatively larger organic structure (C 10H21 )JN+CH 3Cr compared to the latter (C4 H9) 4N+B(. Kinetic studies on the permanganate oxidation of The solutions containing the permanganate ions in acetopheno_ne and some of its substituents in organic media using the organic solvents were prepared by shaking the techn1que of phase transfer catalysis are reported. aqueous potassium permanganate solution with the Tncaprylmethylammonium chloride and tetrabutylammonium bromide have been used as the phase transfer catalysts. The organic solvents contammg the phase transfer 4 reaction shows first order dependence each on [ketones] and the catalysts as reported elsewhere . The solutions of the [permanganate ions] respectively . The rate coefficients fit well oxidant thus prepared in the organic solvent and the with the Hammett equation and the p-value calculated aorees well substrate in the organic solvent were thermally with the reaction requirements. "' equilibrated (± 0.05°C) at the desired temperature for Potassium permanganate is a powerful oxidizing about half an hour before mixing. Kinetic runs were carried out under pseudo-first order conditions. The agent both for organic as well as inorganic oxidation reactions. It can be conveniently used as a selective progress of the reaction was followed by measuring oxidant for removing small quantities of organic the changes in the optical density of the reaction matter in water bodies and the reaction assumes mixture employing a Shimadzu 1601 UV spectro­ special significance when carried out under phase photometer at Amax 526 nm. transfer catalytic conditions, as water insoluble organic materials can be oxidized with ease. In the Results and discussion present study acetophenone and its p-nitro, p-bromo, The percentage extraction of the permanganate ions was found to be 97 to 100 with 0.02 mol dm-3 of the p -chloro, p-methyl, p-methoxy and m-nitro deriva­ catalysts employed. The transfer of the oxidant was ti ves have been subjected to oxidation reactions under more with TCMAC, as expected in accordance with phase transfer catalysis. Tricaprylmethylammonium 5 its greater organic structure . The extraction of Mn0 - chloride (Aliquat 336) and tetrabutylammonium 4 bromide were used as catalysts in various organic ions into benzene was 100% with TCMAC and 97% with TBAB in about 30 min for a catalyst solvents. 3 concentration of 0.02 mol dm- . The solutions Traditionally the organic oxidation reactions in remained stable for a fairly long duration of time. The aqueous medium were facilitated by the use of co­ loss in the concentration of Mn04 ions durina a solvents especially the dipolar aprotic ones. This • b penod of about 2 h was only about 2%. The could partially solve the situation through cation stoichiometry of the reaction was investigated by solvation. However, with the development of the equilibrating known amounts of acetoohenone with an phase transfer techniques it has become quite easy to excess of permanganate in the of the catalyst carry out oxidation reactions of organic compounds in presen~e and by estimating the unreacted permanganate. One organic media using permanganate, dichromate, 1 3 mole of Q+Mn04- consumed one mole of th e ketone to hypochlorite, etc - • Such oxidations have been carried produce the carboxylic acids. out in heterogeneous system of aqueous and organic media. Reports on the kinetics of oxidation of The kinetic rate data with various oxidant carbonyl compounds using phase-transferred oxidants concentrations and substrate concentrations are are scanty and hence the present work. presented in Table l. Under th e conditions when [Acph] >> [Mn04-], th e plots of log [Mn04-] versus Experimental time were found to be linear indicating first order Analar grade potassi um permanganate was used. dependence on Mn04- ions. This was further confirmed ----- NOTES 611 from the constancy of the specific rate values (kobs) for investigated. The solvents employed were benzene, various concentrations of Mn04- ions. This is given in toluene, carbon tetrachloride, chloroform and the set of k obs values in the first and second rows in dichloromethane. The specific rates with both the Table 1 for the two different catalysts. The observed catalysts showed similar trends and these values are in rate constants with different [substrate] and the same the decreasing order in the solvents as benzene> [oxidant] with both the catalysts (set of k obs values carbon tetrachloride> toluene> dichloromethane > given in the third and fourth rows of Table I) increase chloroform (Table 2). The observed decrease in rate linearly with increase in [substrate]. Plots of log k obs 0.6 .----------------, 0.-!0 versus log[acetophenone] was linear with a slope of unity showing that the reaction is first order with P'lC respect to the ketone also. This is further confirmed TBAB 0.3!1 from the reasonably constant values for the second ~ 0.5 order rate constant, k i.e kobsf[AcPh] obtained from 2 .... .... the values in Table l. It was also observed that the + + 0 .30 plots of log kobs versus log [PTC] (Fig. 1) for both the ~ ~ ~ -=. catalysts were linear with small fractional order 0 .9 0.4 .... dependence. The rate constants obtained also shows 0.:<!5 the influence of the structure of the quaternary ammonium cations on their catalytic efficiencies. TCMAC, [(C,oH21hN+CH3Cr] can be seen to be a o.s '-----=-o.'=s---o-:-~_...,..4 ___o,.....c::-o----:-'o.6°' 20 better catalyst than TBAB, [(C4H9)4N+BrT The effect of dielectric constants of the solvents loi[PTC] + 3 used, on the rate of these oxidations were also Fig. 1-Plot of log kobs versus log[PTC] Table ! -Effect of [subst rate], [oxidant] and [catalyst] on the rate of oxidation of acetophenone [Organic solvent : benzene; temp. : 303 K] 3 2 [Mn04' ] X 10 [AcPh] x 10 mol [TCMAC] x [TBAB] x 4 k obsX 10 s·l mol dm-3 dm-3 103 mol dm- 3 103 mol dm-3 0.50 1.00 2.00 2.694 1.00 1.00 2.00 2.755 1.50 1.00 2.00 2.663 2.00 1.00 2.00 2.740 0.50 1.00 2.00 1.846 1.00 1.00 2.00 1.850 1.50 1.00 2.00 1.896 2.00 1.00 2.00 1.811 1.00 1.00 2.00 2.755 1.00 1.50 2.00 4.133 1.00 2.00 2.00 5.323 1.00 2.50 2.00 5.964 1.00 1.00 2.00 1. 850 1.00 1.50 2.00 2.790 1.00 2.00 2.00 3.573 1.00 2.50 2.00 4.118 1.00 1.00 2.00 2.755 1.00 1.00 2.50 2.909 1.00 1.00 3.00 3. 101 1.00 1.00 3.50 3.216 1.00 1.00 2.00 1. 850 1.00 1.00 2.50 2.003 1.00 1.00 3.00 2.118 1.00 1.00 3.50 2.279 612 INDIAN 1 CHEM, SEC. A, JUNE 2001 2.1 Table 2-Effect of solvent polarity on the oxidation of 1.2 p acetophenone in organic solvents PTC ;r-p-NO, 3 3 2 3 1.0 {[Q•Mno4·]= LO x 10' mol dm- , [AcPh]== LOx 10· mol dm- , ,...NO, 1.8 'lBAB temp. -303 K} ~ 0.8 Organic solvent Intrinsic U5 dielectric TCMAC TBAB 0.1 + 0.6 "'+ constant .J.' .J.' ~ 1.2 ~ Benzene 2.27 2.755 L850 .s .s 0 .4 Toluene 2.40 2.406 1.731 Carbon tetrachloride 2.22 2.575 1.784 0 .9 Chloroform 4.70 1.992 1.539 0.2 Dichloromethane 8.90 2.203 1.638 • p-OCH, Table 3-Effect of substi tuents on the oxidation of 0 0.6 acetophenone in organi c solvents '~0.4 -0.1 0.2 0.~ 0.8 3 cr [Q+Mn04·] =LO X 10-J mol dm' ; organic solvent- benzene 2 3 Fig. 2-Hammett plot for the oxidation of acetophenone [substrate]= LOX 10' mol dm' ; temp=- 303 K Substituted acetophenone with maximum speed and the para- methoxy TCMAC TBAB derivative is the least reactive one. The linear free energy relationships as seen in the Hammett plots for p-N02 11.215 IL062 m-N02 10.432 9.181 both the catalysts gave positive p values indicating p-Cl 4.153 2.729 that electron deficiency at the seat of reaction favours p- Br 3.703 2.533 the reaction. The p values found are +0.8451 when Unsubstituted 2.755 L850 TCMAC was used as the catalyst and +0.9208 when p-CH3 1.400 0.6870 p-OCH3 Ll82 0.6060 TBAB was used as the catalyst. This observation supports the fact that the Mn04- attacks the polarisable carbonyl carbon atom of the of the oxidation in solvents of higher dielectric ketone and the speed of the reaction is enhanced more constant can be attributed to the larger stabilization by by the better electron-withdrawing para-nitro group solvation extended to the quaternary permanganate in the series of compounds chosen. ion pair by these solvents.
Load more

Recommended publications
  • Decolorization of Reactive Orange 16 Via Ferrate(VI) Oxidation Assisted by Sonication
    Turkish Journal of Chemistry Turk J Chem (2017) 41: 577 { 586 http://journals.tubitak.gov.tr/chem/ ⃝c TUB¨ ITAK_ Research Article doi:10.3906/kim-1701-8 Decolorization of reactive orange 16 via ferrate(VI) oxidation assisted by sonication Serkan S¸AHINKAYA_ ∗ Department of Environmental Engineering, Faculty of Engineering and Architecture, Nev¸sehirHacı Bekta¸sVeli University, Nev¸sehir,Turkey Received: 02.01.2017 • Accepted/Published Online: 24.03.2017 • Final Version: 05.09.2017 Abstract: The decolorization of azo dye C.I. reactive orange 16 (RO 16) via ferrate(VI) and sono-ferrate(VI) methods, which is the combination of the ferrate(VI) oxidation method with sonication, has been achieved in the present study. The influences of some important operating parameters, which are the initial pH, the concentration of potassium ferrate(VI) (K 2 FeO 4) and the RO 16 dye, and ultrasonic density (for only the sono-ferrate(VI) method), on the color removal have −1 been investigated. The optimum conditions have been determined as pH = 7 and [K 2 FeO 4 ] = 50 mg L for the −1 −1 individual ferrate(VI) oxidation method and pH = 7 and [K 2 FeO 4 ] = 50 mg L by direct sonication at 0.50 W mL ultrasonic density and 20 kHz fixed frequency for the sono-ferrate(VI) method. The color removal efficiencies were 85% by ferrate(VI) method and 91% by sono-ferrate(VI) method. Kinetic studies were also performed for the decolorization of RO 16 under the optimized conditions at room temperature. It was seen that the oxidative decolorization of RO 16 via the sono-ferrate(VI) method happened more rapidly because of the production of OH • radical through sonication compared to the individual ferrate(VI) method.
    [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]
  • Experiment: Determination of Manganese in Steel
    p.1 of 4 Chemistry 201 – Winter 2007 Experiment: Determination of Manganese in Steel Manganese (Mn) in steel may be determined upon dissolution as manganese (VII) after oxidation from the manganese oxidation state (II). This procedure calls for three oxidizing agents. Manganese (VII) may be determined spectrophotometrically. During dissolution of the sample with dilute nitric acid to form iron (II) and manganese (II), nitrogen oxide gases are formed. These must be removed, partially by boiling, and the rest with ammonium peroxydisulfate which also removes carbon or other organic matter present. The nitrogen oxides may react with periodic acid which is used to convert manganese to the (VII) oxidation state. Excess peroxydisulfate is decomposed by boiling. The equations are: - + 2+ 3 Mn + 2 NO3 + 8H ---> 3 Mn + 2 NO (g) + 4H2O 2- - 2- + 2 NO2 (g) + S2O8 + 2 H2O ---> 2 NO3 + 2 SO4 + 4 H 2- 2- + 2 S2O8 + 2 H2O + heat ---> 4 SO4 + O2 + 4 H 2+ - - + - 2 Mn + 5 IO4 + 3 H2O ---> 2 MnO4 + 6 H + 5 IO3 NO(colorless gas) + 1/2 O2 (g) <---> NO2 (brown gas) Note: Peroxydisulfate has the required oxidizing potential to change the oxidation state of manganese from (II) to (IV), but the reaction is too slow. Silver could be employed catalytically but the results are too erratic. Periodate oxidizes the manganese to the (VII) state quantitatively and rapidly at the boiling point, and it is advisable to add the sparingly soluble periodate salt in several portions to maintain an excess and to allow for some decomposition of the latter salt at the elevated temperatures.
    [Show full text]
  • Potassium Permanganate MSDS
    He a lt h 2 0 Fire 0 1 0 Re a c t iv it y 0 Pe rs o n a l Pro t e c t io n J Material Safety Data Sheet Potassium permanganate MSDS Section 1: Chemical Product and Company Identification Product Name: Potassium permanganate Contact Information: Catalog Codes: SLP4912, SLP3892, SLP1075 Sciencelab.com, Inc. 14025 Smith Rd. CAS#: 7722-64-7 Houston, Texas 77396 RTECS: SD6475000 US Sales: 1-800-901-7247 International Sales: 1-281-441-4400 TSCA: TSCA 8(b) inventory: Potassium permanganate Order Online: ScienceLab.com CI#: Not available. CHEMTREC (24HR Emergency Telephone), call: Synonym: Potassium Permanganate, Biotech Grade 1-800-424-9300 Chemical Name: Potassium Permanganate International CHEMTREC, call: 1-703-527-3887 Chemical Formula: KMnO4 For non-emergency assistance, call: 1-281-441-4400 Section 2: Composition and Information on Ingredients Composition: Name CAS # % by Weight Potassium permanganate 7722-64-7 100 Toxicological Data on Ingredients: Potassium permanganate, Biotech: ORAL (LD50): Acute: 1090 mg/kg [Rat]. 2157 mg/kg [Mouse]. Section 3: Hazards Identification Potential Acute Health Effects: Hazardous in case of skin contact (irritant), of eye contact (irritant), of ingestion, of inhalation. Slightly hazardous in case of skin contact (permeator). Possibly corrosive to eyes and skin. The amount of tissue damage depends on length of contact. Eye contact can result in corneal damage or blindness. Skin contact can produce inflammation and blistering. Inhalation of dust will produce irritation to gastro-intestinal or respiratory tract, characterized by burning, sneezing and coughing. Severe over-exposure can produce lung damage, choking, unconsciousness or death.
    [Show full text]
  • In Situ Chemical Oxidation of Creosote/Coal Tar Residuals: Experimental and Numerical Investigation
    In situ Chemical Oxidation of Creosote/Coal Tar Residuals: Experimental and Numerical Investigation by Steven Philip Forsey A thesis presented to the University of Waterloo in fulfillment of the thesis requirement of the degree of Doctor of Philosophy in Earth Sciences Waterloo, Ontario, Canada, 2004 ©Steven Philip Forsey 2004 I herby declare that I am the sole author of this thesis. This is a true copy of the thesis, including any required final version, as accepted by my examiners. I understand that my thesis may be made electronically available to the public Steven Forsey ii Abstract Coal tar, coal tar creosote and oily wastes are often present as subsurface contaminants that may migrate below the water table, leaving a widely distributed residual source of contaminants leaching to the ground water. In situ chemical oxidation is a potentially viable technology for the remediation of aquifers contaminated with creosote and coal tars. The oxidant of choice would be flushed through the contaminated area to oxidize aqueous contaminants and enhance the mass transfer of contaminants from the oil phase. A series of batch and column experiments were performed to assess the ability of a chemical oxidizing reagent to oxidize creosote compounds and to increase mass transfer rates. Results from the column experiments were then simulated using a reactive transport model that considered 12 different creosote compounds undergoing dissolution, oxidation and advective-dispersive transport. Three strong chemical oxidizing reagents, Fenton’s Reagent, potassium persulfate with ferrous ions, and potassium permanganate were tested with batch experiments to determine their reactivity towards creosote compounds. All three reagents successfully decomposed aqueous creosote compounds and were able to reduce the mass of the monitored creosote compounds within the oil phase.
    [Show full text]
  • Chemical Incompatibilities
    Chemical Incompatibilities Incompatibilities Chromic acid, nitric acid, hydroxyl compounds, ethylene glycol, Acetic acid perchloric acid, peroxides, permanganates Acetylene Chlorine, bromine, copper, fluorine, silver, mercury Acetone Concentrated nitric and sulfuric acid mixtures Alkali and alkaline earth metals (such as Water, carbon tetrachloride or other chlorinated hydrocarbons, powdered aluminum or magnesium, calcium, carbon dioxide, halogens lithium, sodium, potassium) Mercury (in manometers, for example), chlorine, calcium Ammonia (anhydrous) hypochlorite, iodine, bromine, hydrofluoric acid (anhydrous) Acids, powdered metals, flammable liquids, chlorates, nitrites, Ammonium nitrate sulfur, finely divided organic combustible materials Aniline Nitric acid, hydrogen peroxide Arsenical materials Any reducing agent Azides Acids Bromine See chlorine Calcium oxide Water Carbon (activated) Calcium hypochlorite, all oxidizing agents Carbon tetrachloride Sodium Ammonium salts, acids, powdered metals, sulfur, finely divided Chlorates organic or combustible materials Acetic acid, naphthalene, camphor, glycerol, alcohol, flammable Chromic acid and chromium liquids in general Ammonia, acetylene, butadiene, butane, methane, propane (or Chlorine other petroleum gases), hydrogen, sodium carbide, benzene, finely divided metals, turpentine Chlorine dioxide Ammonia, methane, phosphine, hydrogen sulfide Copper Acetylene, hydrogen peroxide Cumene hydroperoxide Acids (organic or inorganic) Cyanides Acids Ammonium nitrate, chromic acid, hydrogen peroxide,
    [Show full text]
  • Process Development for Permanganate Addition During Oxidative Leaching of Hanford Tank Sludge Simulants
    PNNL-16794 WTP-RPT-164, Rev 0 Process Development for Permanganate Addition During Oxidative Leaching of Hanford Tank Sludge Simulants B. M. Rapko G. J. Lumetta J. R. Deschane R. A. Peterson October 2007 Prepared for the U.S. Department of Energy under Contract DE-AC05-76RL01830 DISCLAIMER This report was prepared as an account of work sponsored by an agency of the United States Government. Neither the United States Government nor any agency thereof, nor Battelle Memorial Institute, nor any of their employees, makes any warranty, express or implied, or assumes any legal liability or responsibility for the accuracy, completeness, or usefulness of any information, apparatus, product, or process disclosed, or represents that its use would not infringe privately owned rights. Reference herein to any specific commercial product, process, or service by trade name, trademark, manufacturer, or otherwise does not necessarily constitute or imply its endorsement, recommendation, or favoring by the United States Government or any agency thereof, or Battelle Memorial Institute. The views and opinions of authors expressed herein do not necessarily state or reflect those of the United States Government or any agency thereof. PACIFIC NORTHWEST NATIONAL LABORATORY operated by BATTELLE for the UNITED STATES DEPARTMENT OF ENERGY under Contract DE-ACO5-76RL01830 PNNL-16794 WTP-RPT-164, Rev 0 Process Development for Permanganate Addition During Oxidative Leaching of Hanford Tank Sludge Simulants B. M. Rapko G. J. Lumetta J. R. Deschane R. A. Peterson October 2007 Test specification: 24590-PTF-TSP-RT-06-002, Rev. 0 Test Plan: TP-RPP-WTP-453, Rev. 0, and ICN-TP-RPP-WTP-453.1 Test exceptions: 24590-WTP-TEF-RT-07-00002 R&T focus area: Pretreatment Test scoping statement(s): None Pacific Northwest National Laboratory Richland, Washington 99352 Contents Acronyms....................................................................................................................................................
    [Show full text]
  • Sodium Chloride - Analytical Standard
    Sodium Chloride - Analytical Standard Determination of Nitrite Permanganate / Thiosulphate Titrimetric Method EUsalt/AS 001-2005 Former numbering: ECSS/CN 90-1973 & ESPA/CN-E-112-199 www.eusalt.com Determination of nitrite Permanganate/Thiosulphate Titrimetric Method EUsalt/AS 001-2005 1. SCOPE AND FIELD OF APPLICATION 3.5. Sodium thiosulphate, C(Na2S2O3) = 0.1 mol/l, standard volumetric solution The present EUsalt Analytical Standard describes a titrimetric method for the determination of 3.6. Starch solution, 2 g/l nitrites in nitrited sodium chloride. The method is Prepare this solution at the time of use from applicable to products of nitrite content soluble starch. (expressed as sodium nitrite) equal to or greater than 0.15 g per kilogram of salt. 4. APPARATUS Usual laboratory equipment. 2. PRINCIPLE Dissolution of the sample in water. 5. SAMPLING AND SAMPLES Oxidation of nitrite to nitrate with potassium A test sample of 500 g should be taken for permanganate. analysis, ensuring it is representative of the whole batch. Addition of potassium iodide and titration of the liberated free iodine corresponding to the excess 6. PROCEDURE of potassium permanganate with sodium 6.1. Test portion thiosulphate using starch as indicator. Weigh, to the nearest 0.1 g, about 50 g of the test 3. REAGENTS sample. Unless otherwise stated, use only reagents of 6.2. Test solution recognized analytical grade and only distilled Transfer the test portion (6.1.) and 300 ml of water or water of equivalent purity. water into a 500 ml volumetric flask, stir to dissolve, dilute to the mark and mix.
    [Show full text]
  • Permanganate Hazard Summary Identification
    Common Name: AMMONIUM PERMANGANATE CAS Number: 13446-10-1 RTK Substance number: 0110 DOT Number: UN 1482 Date: February 1988 Revision: August 2000 ----------------------------------------------------------------------- ----------------------------------------------------------------------- HAZARD SUMMARY WORKPLACE EXPOSURE LIMITS * Ammonium Permanganate can affect you when breathed No occupational exposure limits have been established for in. Ammonium Permanganate. This does not mean that this * Contact can irritate the skin and eyes. substance is not harmful. Safe work practices should always * Breathing Ammonium Permanganate can irritate the be followed. nose, throat and lungs. * Ammonium Permanganate is a HIGHLY REACTIVE WAYS OF REDUCING EXPOSURE CHEMICAL and a DANGEROUS EXPLOSION * Where possible, enclose operations and use local exhaust HAZARD. ventilation at the site of chemical release. If local exhaust ventilation or enclosure is not used, respirators should be IDENTIFICATION worn. Ammonium Permanganate is a violet-brown or dark purple, * Wear protective work clothing. crystalline (sand-like) solid. * Wash thoroughly immediately after exposure to Ammonium Permanganate and at the end of the REASON FOR CITATION workshift. * Ammonium Permanganate is on the Hazardous * Post hazard and warning information in the work area. In Substance List because it is cited by DOT and NFPA. addition, as part of an ongoing education and training * This chemical is on the Special Health Hazard Substance effort, communicate all information on the health and List because it is REACTIVE. safety hazards of Ammonium Permanganate to * Definitions are provided on page 5. potentially exposed workers. HOW TO DETERMINE IF YOU ARE BEING EXPOSED The New Jersey Right to Know Act requires most employers to label chemicals in the workplace and requires public employers to provide their employees with information and training concerning chemical hazards and controls.
    [Show full text]
  • Sodium Nitrite
    SODIUM NITRITE Prepared at the 44th JECFA (1995), published in FNP 52 Add 3 (1995) superseding specifications prepared at the 17th JECFA (1973), published in FNP 4 (1978) and in FNP 52 (1992). Metals and arsenic specifications revised at the 63rd JECFA (2004). An ADI of 0-0.06 mg/kg bw was established at 44th JECFA (1995). Nitrite should not be used for infants below 3 months SYNONYMS INS No. 250 DEFINITION Chemical names Sodium nitrite C.A.S. number 7632-00-0 Chemical formula NaNO2 Formula weight 69.00 Assay Not less than 97.0% on the dried basis DESCRIPTION White or slightly yellow, hygroscopic and deliquescent granules, powder, or opaque, fused masses of sticks FUNCTIONAL USES Antimicrobial preservative, colour fixative CHARACTERISTICS IDENTIFICATION Solubility (Vol. 4) Freely soluble in water, sparingly soluble in ethanol Test for sodium (Vol. 4) Passes test Test for nitrite (Vol. 4) Passes test PURITY Loss on drying (Vol. 4) Not more than 0.25% (over silica gel, 4 h) Lead (Vol. 4) Not more than 2 mg/kg Determine using an atomic absorption technique appropriate to the specified level. The selection of sample size and method of sample preparation may be based on the principles of the method described in Volume 4, “Instrumental Methods.” METHOD OF Weigh, to the nearest mg, 1 g of the dried sample. Transfer to a 100 ml ASSAY volumetric flask and dissolve in water diluting to the mark. Pipette 10.0 ml of this solution into a mixture of 50.0 ml of 0.1N potassium permanganate, 100 ml of water and 5 ml of sulfuric acid, keeping the tip of the pipette well below the surface of the liquid.
    [Show full text]
  • Chitosan Encapsulation of Ferratevi for Controlled Release to Water
    www.nature.com/scientificreports OPEN Chitosan Encapsulation of FerrateVI for Controlled Release to Water:Mechanistic Insights and Degradation of Organic Contaminant Bo-Yen Chen1, Hsuen-Wen Kuo1, Virender K. Sharma 2 & Walter Den3* VI 2− VI Tetraoxy-anion of iron in +6 oxidation state (Fe O4 , Fe ), commonly called ferrate, has shown tremendous potential as a green oxidative agent for decontaminating water and air. Encapsulation of solid potassium salt of ferrate (K2FeO4) circumvents the inherent drawbacks of the instability of ferrate under humid conditions. In the encapsulated strategy, controlled release without exposing the solid ferrate to the humid environment avoids self-decomposition of the oxidant by water in the air, and the ferrate is mostly used to decontaminate water efciently. This study demonstrated the formulation of oxidative microcapsules with natural materials present in chitosan, whose release rate of the core material can be controlled by the type of intermediate hydrocarbon layer and the pH-dependent swelling of chitosan shell. The pH played a pivotal role in swelling chitosan shell and releasing the core oxidant. In a strong acidic solution, chitosan tended to swell quickly and release FeVI at a faster rate than under neutral conditions. Additionally, among the several long-chain hydrocarbon compounds, oleic acid exhibited the strongest “locking” efect when applied as the intermediate layer, giving rise to the slow release of FeVI. Coconut oil and mineral oil, in comparison, allowed FeVI to penetrate the layer within shorter lengths of time and showed comparable degrees of degradation of target contaminant, methylene orange, under ambient temperature and near-neutral conditions.
    [Show full text]
  • (VI) Preoxidation in Enhancing the Coagulation of Surface Waters Jun Ma*, Wei Liu
    Water Research 36 (2002) 4959–4962 Effectiveness of ferrate (VI) preoxidation in enhancing the coagulation of surface waters Jun Ma*, Wei Liu School of Municipal and Environmental Engineering, Harbin Institute of Technology, P.O. Box 2627, Harbin 150090, People’s Republic of China Received 6 August 2001; received in revised form 18 April 2002; accepted 17 May 2002 Abstract Standard jar tests were conducted to evaluate the effectiveness of ferrate preoxidation in enhancing the coagulation of surface waters. A substantial reduction of residual turbidity after sedimentation and filtration was achieved by ferrate preoxidation in all cases of the investigation of various water qualities at low ferrate dosage (0.5–1.0 mg/l). The enhancement of the coagulation was more obvious when the organic content in the waters were relatively high. r 2002 Published by Elsevier Science Ltd. Keywords: Potassium ferrate; Preoxidation; Coagulation; Turbidity; Enhanced coagulation 1. Introduction pH range (ranging from –2.2 V in acid to –0.7 V in base) [4], has received more and more attention recently. Preoxidation has been one of the principle means for The results of initial studies, in which ferrate improving the coagulation process, which is generally preoxidation was applied in alum coagulation of the aimed at destroying the organic coating on the surface of surface waters, showed that ferrate preoxidation could particles. Traditionally, chlorine has been used to aid the decrease residual algae concentration [5–7], destroy coagulation of waters with a high organic content. phenol and coprecipitate heavy metal ions [8], and aid However, the negative effect of using chlorine, resulting the removal of turbidity [9,10].
    [Show full text]