Industrial Hygiene Hexavalent Chromium www.saif.com INDUSTRIAL HYGIENE Hexavalent Chromium Introduction Hexavalent chromium‚ Cr(VI)‚ has many uses in industrial processes. Some major industrial sources of hexavalent chromium are: Chromate pigments in dyes‚ paints‚ inks‚ and plastics. Chromates added as anti-corrosive agents to paints‚ primers and other surface coatings. Chrome plating by depositing chromium metal onto an item’s surface using a solution of chromic acid. Particles released
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TEXT BOOK OF BIOCHEMISTRY For 2nd year Medical Laboratory Technician Course (INTERMEDIATE VOCATIONAL) Author : S. Srinivasa Rao‚ B.Pharmacy‚ Jr. Lecturer in M.L.T.‚ Alluri Sri Rama Raju Govt. Junior College‚ Shanthi Nagar‚ Khammam. Editor : S. Kamalakar Rao‚ M. Pharmacy Senior Lecturer in Pharmacy‚ Department of Biotechnology‚ Govt. institute for post diploma courses in engineering and technology‚ Ramanthapur‚Hyderabad. INDEX Chapter I. Page No. Instrumental methods of Biochemical
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mass) of the following: (a) iron (III) oxide (Fe = 70.0%‚ O = 30.0%) (b) barium phosphate (Ba = 68.4%‚ P = 10.3%‚ O= 21.3%) 2. What is the percentage of sodium (by mass) in sodium phosphate? (42.1%) 3. For the hydrate sodium sulfate decahydrate‚ calculate the following: (a) the percent of sodium (by mass) in the hydrate (14.3%) (b) percent of TOTAL oxygen (by mass) in the hydrated compound. (69.6%) (c) Percent of water (by mass) in the hydrate (55.9%)
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concentration of the chloride ions would increase and some sodium ions would be formed. Because of this‚ the concentration of reactants increases which causes the equilibrium system to move to the right (products) side. Therefore‚ the solution turns purple. 6) Cr2O72- + 2OH- ↔ 2CrO42- + H2O 9) In step 7‚ there was HCL added prior to the addition of barium nitrate and this caused the reaction to shift right causing the production of additional dichromate. This meant there was a
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BeBr2 27) Na2O 28) CaF2 29) BP 30) Al2O3 1) magnesium sulfide 2) potassium bromide 3) barium nitride 4) aluminum oxide 5) sodium iodide 6) strontium fluoride 7) lithium sulfide 8) radium chloride 9) calcium oxide 10) aluminum phosphide 11) potassium sulfide 12) lithium bromide 13) strontium phosphide 14) barium chloride 15) sodium bromide 16) magnesium fluoride 17) sodium oxide 18) strontium sulfide 19) boron nitride 20) aluminum nitride 21) cesium oxide 22) rubidium iodide 23) magnesium oxide
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useful solution can be prepared by dissolving 0.10 gram in 100 mL of water. The Eo’ value for this indicator is 0.53V. (n = 2) What is the useful voltage range of this indicator? (B) Starch indicators are useful when iodine titrations (organic oxidations) are performed. Why is it considered an advantage in these titrations to have iodine as the titrant instead of the analyte? 3. An environmental chemist is going to field test the chemical oxygen demand factor for a stream in Yellowstone Park
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oxidizing agents. Some products that contain oxidizing agents are bleaches‚ hair coloring agents‚ scouring powders‚ and toilet bowl cleaners. The most common oxidizing agent in bleaches is sodium hypochlorite‚ NaClO (sometimes written NaOCl). Commercial bleaches are created by bubbling chlorine gas into a sodium hydroxide solution (remember this from your “funky redox rxns”?). Some of the chlorine is oxidized to the hypochlorite ion‚ ClO- and some is reduced to the chloride ion‚ Cl- (a disproportionation
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permanganate c) H2SO4 ____sulphuric acid______ d) H2O ______hydrogen oxide____ e) AgNO3 ____silver nitrate______ f) Sodium bicarbonate ______Na2CO3____ g) Nitric acid _________HNO3________ h) Hydrochloric acid _________HCl_______ i) Potassium dichromate _______K2CrO4____ j) Sodium hydroxide __________NaOH____ 6. Complete the following conversion factors or problems: a) 1 cm3. = __1___ mL. 1 kg. = _1000___ g
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Analysis of Commercial Bleach Lab I. Purpose In this experiment‚ the amount of sodium hypochlorite in a commercial bleach will be determined by reacting it with sodium thiosulfate in the presence of iodide ions and starch. A solution of sodium thiosulfate of known concentration will be added to the bleach using a buret in a titration procedure. The disappearance of the dark blue color of the starch-iodine complex will signal the end point. II. Procedures Pre-Lab Questions 1. What is
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! ! To review oxidation-reduction reactions and their stoichiometry. To learn the concept and technique of redox titration. To determine the percent (m/v) of an active ingredient‚ sodium hypochlorite (NaOCl)‚ in a commercial bleaching agent. B. Theoretical Background Whereas acid-base reactions involve the transfer of a proton‚ oxidation-reduction or redox reactions involve the transfer of electrons from one substance to another‚ resulting in changes in oxidation numbers of two or more
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