DOCSLIB.ORG

Solid-Liquid Phase Equilibria and Crystallization of Disubstituted Benzene Derivatives

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text

Load more

Royal Institute of Technology School of Chemical Science and Engineering Department of Chemical Engineering and Technology Division of Transport Phenomena Solid-Liquid Phase Equilibria and Crystallization of Disubstituted Benzene Derivatives Fredrik Nordström Doctoral Thesis Akademisk avhandling som med tillstånd av Kungliga Tekniska Högskolan i Stockholm framlägges till offentlig granskning för avläggande av teknologie doktorsexamen den 30:e Maj 2008, kl. 10:00 i sal D3, Lindstedtsvägen 5, Stockholm. Avhandlingen försvaras på engelska. i Cover picture: Crystals of o-hydroxybenzoic acid (salicylic acid) obtained through evaporation crystallization in solutions of ethyl acetate at around room temperature. Solid-Liquid Phase Equilibria and Crystallization of Disubstituted Benzene Derivatives Doctoral Thesis © Fredrik L. Nordström, 2008 TRITA-CHE Report 2008-32 ISSN 1654-1081 ISBN 978-91-7178-949-5 KTH, Royal Institute of Technology School of Chemical Science and Engineering Department of Chemical Engineering and Technology Division of Transport Phenomena SE-100 44 Stockholm Sweden Paper I: Copyright © 2006 by Wiley InterScience Paper II: Copyright © 2006 by Elsevier Science Paper III: Copyright © 2006 by the American Chemical Society Paper IV: Copyright © 2006 by the American Chemical Society ii In loving memory of my grandparents Aina & Vilmar Nordström iii i v Abstract The Ph.D. project compiled in this thesis has focused on the role of the solvent in solid-liquid phase equilibria and in nucleation kinetics. Six organic substances have been selected as model compounds, viz. ortho-, meta- and para-hydroxybenzoic acid, salicylamide, meta- and para-aminobenzoic acid. The different types of crystal phases of these compounds have been explored, and their respective solid-state properties have been determined experimentally. The solubility of these crystal phases has been determined in various solvents between 10 and 50 oC. The kinetics of nucleation has been investigated for salicylamide by measuring the metastable zone width, in five different solvents under different experimental conditions. A total of 15 different crystal phases were identified among the six model compounds. Only one crystal form was found for the ortho-substituted compounds, whereas the meta-isomeric compounds crystallized as two unsolvated polymorphs. The para-substituted isomers crystallized as two unsolvated polymorphs and as several solvates in different solvents. It was discovered that the molar solubility of the different crystal phases was linked to the temperature dependence of solubility. In general, a greater molar solubility corresponds to a smaller temperature dependence of solubility. The generality of this relation for organic compounds was investigated using a test set of 41 organic solutes comprising a total of 115 solubility curves. A semi-empirical solubility model was developed based on how thermodynamic properties relate to concentration and temperature. The model was fitted to the 115 solubility curves and used to predict the temperature dependence of solubility. The model allows for entire solubility curves to be constructed in new solvents based on the melting properties of the solute and the solubility in that solvent at a single temperature. Based on the test set comprising the 115 solubility curves it was also found that the melting temperature of the solute can readily be predicted from solubility data in organic solvents. The activity of the solid phase (or ideal solubility) of four of the investigated crystal phases was determined within a rigorous thermodynamic framework, by combining experimental data at the melting temperature and solubility in different solvents and temperatures. The results show that the assumptions normally used in the literature to determine the activity of the solid phase may give rise to errors up to a factor of 12. An extensive variation in the metastable zone width of salicylamide was obtained during repeated experiments performed under identical experimental conditions. Only small or negligible effects on the onset of nucleation were observed by changing the saturation temperature or increasing the solution volume. The onset of nucleation was instead considerably influenced by different cooling rates and different solvents. A correlation was found between the supersaturation ratio at the average onset of v nucleation and the viscosity of the solvent divided by the solubility of the solute. The trends suggest that an increased molecular mobility and a higher concentration of the solute reduce the metastable zone width of salicylamide. Keywords: Salicylic acid, m-hydroxybenzoic acid, p-hydroxybenzoic acid, salicylamide, m-aminobenzoic acid, p-aminobenzoic acid, solubility, solid-liquid equilibria, thermodynamics, activity of the solid phase, ideal solubility, activity coefficient, van't Hoff enthalpy of solution, solid state, solution properties, metastable zone width, primary nucleation, nucleation kinetics. v i Popular Scientific Summary Compounds in nature exist as gases, liquids and solids. These states are separated by temperature and pressure. When the temperature of a liquid decreases at constant pressure, it forms a solid. As an example, ice forms on a lake on a cold winter day. When a solid is placed in contact with a liquid, the solid will start to dissolve into the liquid. This is something we see when we for example add sugar to a cup of coffee. As we continue to add a solid to the liquid the solid will at some point no longer dissolve into the liquid. The solution is then said to be saturated and the concentration of the saturated solution is called solubility. In science, we refer to this condition as a state of equilibrium between the solid and the solution. When the solid is in contact with a liquid we also often call the liquid a solvent. The solubility depends on several factors. When we change the solvent or the solid, the solubility will also change. However, we have an additional factor to consider when looking at the solid. The structure of the solid is sometimes different. The element carbon is for example found in nature in different solid forms such as graphite and diamond. These two forms, or phases, of course are very different and also have different solubility. In the pharmaceutical industry, the drug is often found in different solid forms. When we make a tablet of the drug and administer it to humans it will dissolve when it comes in contact with the fluids in the intestines. The drug then travels into the blood's circulatory system giving its purposed medical effect. Since the solid forms of the drug have different solubility they will also dissolve at different rates. This will affect the medical response of the drug, sometimes dramatically. It is therefore very important that we know what the different solid forms of the drug are and how fast they dissolve. When a drug has been discovered it is produced through a series of chemical reactions. To purify the drug from side-products it goes through several industrial purification and separation processes. One of the last and very important processes is the crystallization process. This is when the drug is formed in a solid form from a solution. Crystallization is almost like the opposite of dissolution. We can perform a crystallization process in different ways, but usually we saturate a solution at a certain temperature and then lower the temperature until the solid starts to appear in the form of crystals. Depending on how we perform the crystallization different solid forms of the crystals may appear. The shape and size of these crystals may also be very different. Just as the solubility is important when the drug is given to humans, the solubility is also the most important factor in the crystallization process. To be able to control a crystallization process we need to know the solubility of the different solid forms and how they are related to the solvent and temperature. vii In this research project, six different solid compounds have been investigated together with up to nine different solvents at different temperature. In the first part of the project, we have looked at what different solid forms, or phases, are found among these compounds. We have found that two of the compounds only crystallize as one solid form, whereas the other four compounds crystallize in two to five different solid forms. The solubility of these different solid forms has been determined in different solvents from 10 to 50 oC. It soon became clear that the solubility of these solid forms is directly related to how solubility is dependent on temperature. This connection has not been explored much in the past. To understand why we see this relationship, we used thermodynamic theory, which describes how solubility is related to the properties of the solid and the properties of the solution. Although the science of this connection is interesting to explore we also obtain several practical applications that we can use as an aid in the crystallization process. We can for example more easily estimate how much of the drug is formed as solid depending on what solvent we use. We can also identify different solid forms just by looking at the solubility data. Since the relationship between the solubility and how it depends on temperature was so strong it was decided to investigate whether this connection is something that appears for organic compounds in general. In order to do that, we used a total of 41 different compounds and their solubility data in different solvents. We could verify this behavior and also construct a model that allows us to estimate what the solubility is at different temperature. In addition, it was observed that the solubility at different temperature was predictable to the extent that we could estimate the melting point of the solid. A common problem in the field of crystallization is not being able to measure how the properties of the solid and the properties of the solution affect the solubility. By using this connection and thermodynamic theory it was possible to separate these two properties from each other.
Recommended publications
  • Immersion Cooling of Electronics in Dod Installations

    Immersion Cooling of Electronics in Dod Installations

    LBNL-1005666 Immersion Cooling of Electronics in DoD Installations Henry Coles and Magnus Herrlin Energy Technologies Area May 2016 DISCLAIMER This document was prepared as an account of work sponsored by the United States Government. While this document is believed to contain correct information, neither the United States Government nor any agency thereof, nor The Regents of the University of California, nor any of their employees, makes any warranty, express or implied, or assumes any legal 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 its 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 The Regents of the University of California. The views and opinions of authors expressed herein do not necessarily state or reflect those of the United States Government or any agency thereof or The Regents of the University of California. ABSTRACT A considerable amount of energy is consumed to cool electronic equipment in data centers. A method for substantially reducing the energy needed for this cooling was demonstrated. The method involves immersing electronic equipment in a non-conductive liquid that changes phase from a liquid to a gas. The liquid used was 3M Novec 649. Two-phase immersion cooling using this liquid is not viable at this time. The primary obstacles are IT equipment failures and costs. However, the demonstrated technology met the performance objectives for energy efficiency and greenhouse gas reduction.
  • Working with Hazardous Chemicals

    Working with Hazardous Chemicals

    A Publication of Reliable Methods for the Preparation of Organic Compounds Working with Hazardous Chemicals The procedures in Organic Syntheses are intended for use only by persons with proper training in experimental organic chemistry. All hazardous materials should be handled using the standard procedures for work with chemicals described in references such as "Prudent Practices in the Laboratory" (The National Academies Press, Washington, D.C., 2011; the full text can be accessed free of charge at http://www.nap.edu/catalog.php?record_id=12654). All chemical waste should be disposed of in accordance with local regulations. For general guidelines for the management of chemical waste, see Chapter 8 of Prudent Practices. In some articles in Organic Syntheses, chemical-specific hazards are highlighted in red “Caution Notes” within a procedure. It is important to recognize that the absence of a caution note does not imply that no significant hazards are associated with the chemicals involved in that procedure. Prior to performing a reaction, a thorough risk assessment should be carried out that includes a review of the potential hazards associated with each chemical and experimental operation on the scale that is planned for the procedure. Guidelines for carrying out a risk assessment and for analyzing the hazards associated with chemicals can be found in Chapter 4 of Prudent Practices. The procedures described in Organic Syntheses are provided as published and are conducted at one's own risk. Organic Syntheses, Inc., its Editors, and its Board of Directors do not warrant or guarantee the safety of individuals using these procedures and hereby disclaim any liability for any injuries or damages claimed to have resulted from or related in any way to the procedures herein.
  • Environmental Health and Safety Vacuum Traps

    Environmental Health and Safety Vacuum Traps

    Environmental Health and Safety Vacuum Traps Always place an appropriate trap between experimental apparatus and the vacuum source. The vacuum trap: • protects the pump, pump oil and piping from the potentially damaging effects of the material; • protects people who must work on the vacuum lines or system, and; • prevents vapors and related odors from being emitted back into the laboratory or system exhaust. Improper trapping can allow vapor to be emitted from the exhaust of the vacuum system, resulting in either reentry into the laboratory and building or potential exposure to maintenance workers. Proper traps are important for both local pumps and building systems. Proper Trapping Techniques To prevent contamination, all lines leading from experimental apparatus to the vacuum source must be equipped with filtration or other trapping as appropriate. • Particulates: use filtration capable of efficiently trapping the particles in the size range being generated. • Biological Material: use a High Efficiency Particulate Air (HEPA) filter. Liquid disinfectant (e.g. bleach or other appropriate material) traps may also be required. • Aqueous or non-volatile liquids: a filter flask at room temperature is adequate to prevent liquids from getting to the vacuum source. • Solvents and other volatile liquids: use a cold trap of sufficient size and cold enough to condense vapors generated, followed by a filter flask capable of collecting fluid that could be aspirated out of the cold trap. • Highly reactive, corrosive or toxic gases: use a sorbent canister or scrubbing device capable of trapping the gas. Environmental Health and Safety 632-6410 January 2010 EHSD0365 (01/10) Page 1 of 2 www.stonybrook.edu/ehs Cold Traps For most volatile liquids, a cold trap using a slush of dry ice and either isopropanol or ethanol is sufficient (to -78 deg.
  • A Sample AMS Latex File

    A Sample AMS Latex File

    Li, L. et al. (2021): JoSS, Vol. 10, No. 1, pp. 983–993 (Peer-reviewed article available at www.jossonline.com) www.adeepakpublishing.com www. JoSSonline.com Preliminary Thermal Validation Tests for Education-Class CubeSats and Weather- Balloon Payloads Lingqi Li and Kenjiro S. Lay Penn State University State College, PA, US Masataka Okutsu Penn State University Abington Abington, PA, US Abstract Low development and launch costs of CubeSats, a type of small spacecraft typically one to three liters in volume, have made space science accessible to educational institutions, offering engaging opportunities for stu- dents in the science, technology, engineering, and mathematics (STEM) disciplines. Some university teams work- ing on these education-class CubeSats conduct high-altitude flight experiments using balloons to test their instru- ments in the harsh environment at the edges of the troposphere and the stratosphere. Whether for the balloon experiment or for the actual spaceflight, temperatures of the operating environments are of concern. Instruments flown in space must be qualified for wide thermal ranges (e.g., −40°C to 70°C) in vacuum conditions. Likewise, instruments flown on the balloons must be able to operate in a similarly large range of temperatures (e.g., −50°C to 50°C) in the reduced pressure environment. Unfortunately, a thermal-vacuum chamber—standard testing equipment for spacecraft—is not accessible to many university teams. This paper presents incubator testing and cooling-bath testing methods as preliminary thermal validation tests that may be carried out easily, safely, and inexpensively, without any need for the expensive thermal-vacuum chamber. We also discuss an add-on demon- stration in which a CubeSat prototype was flown on a weather balloon to an altitude of ~16 km.
  • Gas Supersaturation Thresholds for Spontaneous Cavitation in Water with Gas Equilibration Pressures up to 570 Atm1 Wayne A

    Gas Supersaturation Thresholds for Spontaneous Cavitation in Water with Gas Equilibration Pressures up to 570 Atm1 Wayne A

    Gas Supersaturation Thresholds for Spontaneous Cavitation in Water with Gas Equilibration Pressures up to 570 atm1 Wayne A. Gerth and Edvard A. Hemmingsen * Physiological Research Laboratory Scripps Institution of Oceanography University of California, San Diego La Jolla, California 92093 (Z. Naturforsch. 31a, 1711-1716 [1976] ; received October 5, 1976) Supersaturations for the onset of cavitation in water were determined for various gases. At am- bient pressure, the threshold supersaturations (in atm) required for profuse cavitation to initiate both in bulk water and at the glass-water interface were CH4, 120; Ar, 160; N2, 190; He, 360. Exposure of the water and its containing surfaces to hydrostatic pressures up to 1100 atm prior to equilibration with gas had no detectable effect on these threshold values. This indicates that pre- formed gas nuclei are not significantly involved. Cavitation at the glass-water interface was investi- gated for CH4, Ar and N, saturations up to 570 atm. For 320 atm saturations, the threshold super- saturation was about one-half that for decompression directly to ambient pressure, and for 550 atm it was about one-third. These results indicate that the dissolved gas concentration is a critical factor limiting the spontaneous nucleation of bubbles in gas supersaturated liquids. Introduction thereby forcing the resolution of such dissolvable nuclei 4. Water that contains large gas supersaturations The results reported here bear directly upon the can remain stable with the absence of cavitation 2' 3. understanding of the gas supersaturated metastable However, as the gas supersaturation in the water is condition in pure liquids, the factors which limit it, increased, the system eventually fails to tolerate the and the characteristics of its degeneration via the supersaturation and bursts profusely with the for- nucleation and growth of bubbles.
  • Chapter 1 the Fundamentals of Bubble Formation in Water Treatment

    Chapter 1 the Fundamentals of Bubble Formation in Water Treatment

    Chapter 1 The Fundamentals of Bubble Formation in Water Treatment Paolo Scardina and Marc Edwards1 Keywords: bubble, air binding, filters, nucleation, equilibrium, water treatment, headloss, filtration, gas transfer Abstract: Water utilities can experience problems from bubble formation during conventional treatment, including impaired particle settling, filter air binding, and measurement as false turbidity in filter effluent. Coagulation processes can cause supersaturation and bubble formation by converting bicarbonate alkalinity to carbon dioxide by acidification. A model was developed to predict the extent of bubble formation during coagulation which proved accurate, using an apparatus designed to physically measure the actual volume of bubble formation. Alum acted similar to hydrochloric acid for initializing bubble formation, and higher initial alkalinity, lower final solution pH, and increased mixing rate tended to increase bubble formation. Lastly, the protocol outlined in Standard Methods for predicting the degree of supersaturation was examined, and when compared to this work, the Standard Methods approach produces an error up to 16% for conditions found in water treatment. Introduction: Gas bubble formation is of established importance to divers and fish (i.e., the bends), carbonated beverages, solid liquid separation in mining, cavitation in pumps, gas transfer, stripping, and dissolved air flotation processes. Moreover, it is common knowledge that formation of gas bubbles in conventional sedimentation and filtration facilities is a significant nuisance at many utilities, because bubbles are believed to hinder sedimentation, cause headloss in filters through a phenomenon referred to as “air binding,” and measure as turbidity in effluents without posing a microbial hazard. Utilities have come to accept these problems, and to the knowledge of these authors there is currently no rigorous basis for predicting when such problems will occur or correcting them when they do.
  • Cloud Microphysics

    Cloud Microphysics

    1. Microphysics of Clouds Changes in phase are basic to cloud microphysics. The possible changes are: vapor-liquid evaporation, condensation liquid-solid freezing, melting vapor-solid deposition, sublimation The changes from left to right correspond to increasing molecular order. These transitions don’t occur at thermodynamic equilibrium. There is a strong free en- ergy barrier that must be overcome for droplets to form. To form a droplet by condensation of vapor, surface tension must be overcome by a strong gradient of vapor pressure. This means that phase transitions don’t occur at es(1), or sat- uration over a plane surface of water. Even if a sample of moist air is cooled adiabatically to the equilibrium saturation point for bulk water, droplets should not be expected to form. In fact, water droplets do begin to condense in pure wa- ter vapor only when the relative humidity reaches several hundred percent! This is called Homogeneous Nucleation. The reason why cloud droplets are observed to form in the atmosphere when ascending air just reaches equilibrium saturation is because the atmosphere con- tains significant concentrations of particles of micron and sub-micron size which have an affinity for water. This is called Heterogeneous Nucleation. There are many types of condensation nuclei in the atmosphere. Some become wetted at RH less than 100% and account for haze. Larger condensation nuclei may grow to cloud droplet size. As moist air is cooled adiabatically and RH is close to 100 the hygroscopic CCN begin to serve as centers of condensation. If ascent con- tinues, there is supersaturation by cooling which is depleted by condensation on the nuclei.
  • Rapid Cryogenic Fixation of Biological Specimens for Electron Microscopy

    Rapid Cryogenic Fixation of Biological Specimens for Electron Microscopy

    RAPID CRYOGENIC FIXATION OF BIOLOGICAL SPECIMENS FOR ELECTRON MICROSCOPY KEITH PATRICKRYAN A thesis submitted in partial fulfilment of the requirements of the Council for National Academic Awards for the degree of Doctor of Philosophy September 1991 Polytechnic South West in collaboration with the Marine Biological Association of the United Kingdom and Plymouth Marine Laboratory ----- . \ ~ ,, '' - .... .._~ .. ·=·~-·-'-·-'" --······ --~....... ~=.sn.-.......... .r.=-..-> POL VTECHNIC SOUTH WEST liBRARY SERVICES Item C!O 00 7 9 4 9 3-0 No. ', )'; I Class 1 !) -, C!f -RYA !No. rr ... · ,Contl No. :x70ZS\0253 ·. ' COPYRIGHT This copy of the thesis has been supplied on condition that anyone who consults it is understood to recognise that its copyright rests with its author and that no quotation from the thesis and no information derived from it may be published without the authors prior written consent. 2 CONTENTS Page List of Figures 8 List of Tables 10 Abstract 11 Acknowledgements 12 1 Introduction 13 2 Literature Review 23 2.1 Background to specimen preservation for microscopy 23 2.2 Problems of chemical processing for electron rhlcroscopy 23 2.3 Introduction of cryotechniques into microscopy methods 24 2.4 The potential of cryofixation 25 2.5 The problems of cryofixation 25 2.6 Water, cooling and crystal nucleation 26 2. 7 Cell water 29 2.8 Crystallisation and latent heat release 29 2.9 Phase separation and eutectic temperature 30 2.10 Types of ice 31 2.11 Phase transitions 32 2.12 Ice crystal growth in frozen specimens after freezing 34 2.13 Cryoprotection against ice crystal damage 37 2.14 Modelling the cooling process 38 2.15 Cooling methods 45 2.16 Coolants (liquid) 46 2.17 Coolants (solid) 46 2.18 Plunge cooling methods 48 2.19 Jet cooling methods 51 2.20 Cryoblock methods 54 2.21 Rapid cooling experiments 59 3 2.22 Specimen rewarming during handling after freezing 74 2.23 Conclusions 74 3.
  • Carbonate Chemistry

    Carbonate Chemistry

    CHAPTER 3 SOLUTION-MINERAL EQUILIBRIA PART 1: CARBONATES Carbonic acid and the carbonate minerals provide another good illustration of the use of equilibrium reasoning in geochemistry. Interactions among these compounds determine the conditions under which limestones and dolomites are fomied or dissolved, and likewise the conditions of formation of carbonate minerals as cements in soils and sandstones and as vein fillings. We start with some qualitative remarks about the most common of these substances, the carbonate of calcium, then go on to a more quantitative treatment and to the reactions of other common carbonate minerals. • 3-1 SOLUBILITY OF CALCITE Calcium carbonate occurs in nature as the two common minerals calcite and aragonite (Sec. 3-3). A third crystal form (vaterite) can be prepared artificially, and is known as a very rare mineral in nature. Under usual conditions near the Earth's surface calcite is the most stable and most abundant of the three forms, and for the discussion in this section and the next it will be the center of attention. Aragonite and vaterite may be assumed to show similar chemical behavior, but in general to react more rapidly and to have greater solubility. 61 62 INTRODUCTION TO GEOCHEMISTRY A strong acid dissolves calcite by the familiar reaction CaC03 + 2H+ ---+ Ca2+ + H20 + C02. (3-1 ) calcite At low acid concentrations a more accurate equation would be CaC03 + H+ - • Ca2+ + HCO) (3-2) calcite showing that W takes co~ - away from Ca2+ to form the very weak (little dissociated) acid HCO:J. (Still greater accuracy would require consideration of the complex ion CaHCOj , but under usual conditions its concentration is small and for the present can be neglected.) These reactions would take place in nature, for example, where acid solutions from the weathering of pyrite encounter limestone.
  • The Role of Evolving Surface Tension in the Formation of Cloud Droplets James F

    The Role of Evolving Surface Tension in the Formation of Cloud Droplets James F

    Technical Note: The Role of Evolving Surface Tension in the Formation of Cloud Droplets James F. Davies1, Andreas Zuend2, Kevin R. Wilson3 1Department of Chemistry, University of California Riverside, CA USA 5 2Department of Atmospheric and Oceanic Sciences, McGill University, Montreal, Quebec, Canada 3Chemical Sciences Division, Lawrence Berkeley National Laboratory, Berkeley, CA USA Correspondence to: James F. Davies ([email protected]) Abstract. The role of surface tension (σ) in cloud droplet activation has long been ambiguous. Recent studies have reported observations attributed to the effects of an evolving surface tension in the activation 10 process. However, adoption of a surface-mediated activation mechanism has been slow and many studies continue to neglect the composition-dependence of aerosol/droplet surface tension, using instead a value equal to the surface tension of pure water (σw). In this technical note, we clearly describe the fundamental role of surface tension in the activation of multicomponent aerosol particles into cloud droplets. It is demonstrated that the effects of surface tension in the activation process depend primarily on the evolution 15 of surface tension with droplet size, typically varying in the range 0.5σw ≲ σ ≤ σw due to the partitioning of organic species with a high surface affinity. We go on to report some recent laboratory observations that exhibit behavior that may be associated with surface tension effects, and propose a measurement coordinate that will allow surface tension effects to be better identified using standard atmospheric measurement techniques. Unfortunately, interpreting observations using theory based on surface film and liquid-liquid 20 phase separation models remains a challenge.
  • Microbubble Treatment of Gas Supersaturated Water

    Microbubble Treatment of Gas Supersaturated Water

    MICROBUBBLE TREATMENT OF GAS SUPERSATURATED WATER Contract No. GS-23F-0339K/01PE810319 Desalination and Water Purification R&D Program Report No. 70 December 2001 U.S. Department of Interior Bureau of Reclamation Denver Office Technical Service Center Environmental Resources Team Water Treatment Engineering and Research Group MICROBUBBLE TREATMENT OF GAS SUPERSATURATED WATER Mark A. Lichtwardt ARCADIS G&M, Inc. Highlands Ranch, Colorado Co-Author Andrew Murphy Bureau of Reclamation Denver, Colorado Contract No. GS-23F-0339K/01PE810319 Desalination and Water Purification R&D Program Report No. 70 December 2001 U.S. Department of Interior Bureau of Reclamation Denver Office Technical Service Center Environmental Resources Team Water Treatment Engineering and Research Group Mission Statements U.S. Department of the Interior The mission of the Department of the Interior is to protect and provide access to our Nation’s natural and cultural heritage and honor our trust responsibilities to tribes. Bureau of Reclamation The mission of the Bureau of Reclamation is to manage, develop, and protect water and related resources in an environmentally and economically sound manner in the interest of the American public. Disclaimer The information contained in this report regarding commercial products or firms may not be used for advertising or promotional purposes and is not to be construed as an endorsement of any product or firm by the Bureau of Reclamation. The information contained in this report was developed for the Bureau of Reclamation; no warranty as to the accuracy, usefulness, or completeness is expressed or implied. Acknowledgements This work was financially supported by the U.S. Department of Interior, Bureau of Reclamation under Contract No.
  • Heating and Cooling Chemical Mixtures Revision Date: 11/01/19 Prepared By: Michael Roy P.I.: Prof

    Heating and Cooling Chemical Mixtures Revision Date: 11/01/19 Prepared By: Michael Roy P.I.: Prof

    Section 5.7 Title: Heating and Cooling Chemical Mixtures Revision Date: 11/01/19 Prepared By: Michael Roy P.I.: Prof. John F. Berry Prior Approval: This procedure is NOT considered hazardous enough that prior approval is needed from the Principal Investigator. Involves Use of Particularly Hazardous Substance (PHS)? No ___ Carcinogen ___ Reproductive Toxin ___ High Acute Toxicity Does this procedure require medical surveillance? No Does this require use of a fit-tested respirator? No Brief Description of Procedure: Overview of common heating and cooling methods used in the Berry labs. Location: List the locations (buildings/rooms) where this procedure may be performed. For use of a PHS indicate a more precise location within the room, if appropriate, as a designated area. Daniels Chemistry - All Berry group labs Chemicals Involved: Chemical Physical or Health Hazard (e.g. carcinogen, corrosive) Organic solvents (cooling) Consult relevant SDSs for more details Dry ice Frostbite Liquid nitrogen Frostbite, asphyxiation Other Hazards: Include hazards, other than chemical, that may be present during operation of the procedure. Burns (heating) and frostbite (cooling). Exposure Controls: (Check all that apply) PPE: _X_ Safety Glasses ___ Face Shield ___Chemical Splash Goggles ___Chemical Apron _X_ Gloves (Nitrile) _X_ Lab Coat ___Respirator (type) ___Other: Engineering Controls: _X_ Fume Hood ___Biosafety Cabinet ___ Glove box ___ Vented gas cabinet ___Other: Administrative Controls: List any specific work practices needed to perform this procedure (e.g., cannot be performed alone, must notify other staff members before beginning, etc.). N/A Task Hazard Control Table: For procedures involving numerous steps, it may be convenient to indicate specific requirements for individual tasks in the table below: N/A Waste Disposal: Describe any chemical waste generated and the disposal method used.