DOCSLIB.ORG

Solutions and Their Behavior

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Solutions and Their Behavior Solutions and Their Behavior Shonna Robinson, (ShonnaR) Therese Forsythe, (ThereseF) Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) AUTHORS Shonna Robinson, (ShonnaR) To access a customizable version of this book, as well as other Therese Forsythe, (ThereseF) interactive content, visit www.ck12.org EDITOR Richard Parsons, (RichardP) CK-12 Foundation is a non-profit organization with a mission to reduce the cost of textbook materials for the K-12 market both in the U.S. and worldwide. Using an open-content, web-based collaborative model termed the FlexBook®, CK-12 intends to pioneer the generation and distribution of high-quality educational content that will serve both as core text as well as provide an adaptive environment for learning, powered through the FlexBook Platform®. Copyright © 2014 CK-12 Foundation, www.ck12.org The names “CK-12” and “CK12” and associated logos and the terms “FlexBook®” and “FlexBook Platform®” (collectively “CK-12 Marks”) are trademarks and service marks of CK-12 Foundation and are protected by federal, state, and international laws. Any form of reproduction of this book in any format or medium, in whole or in sections must include the referral attribution link http://www.ck12.org/saythanks (placed in a visible location) in addition to the following terms. Except as otherwise noted, all CK-12 Content (including CK-12 Curriculum Material) is made available to Users in accordance with the Creative Commons Attribution-Non-Commercial 3.0 Unported (CC BY-NC 3.0) License (http://creativecommons.org/ licenses/by-nc/3.0/), as amended and updated by Creative Com- mons from time to time (the “CC License”), which is incorporated herein by this reference. Complete terms can be found at http://www.ck12.org/terms. Printed: April 6, 2014 www.ck12.org Chapter 1. Solutions and Their Behavior CHAPTER 1 Solutions and Their Behavior CHAPTER OUTLINE 1.1 Properties of Solutions 1.2 Solution Formation 1.3 Measuring Concentration 1.4 Factors Affecting Solubility 1.5 Solubility Graphs 1.6 Colligative Properties 1.7 Separating Mixtures 1.8 Reactions Between Ions in Solutions 1.9 References 1 1.1. Properties of Solutions www.ck12.org 1.1 Properties of Solutions Lesson Objectives The student will: • define a solution. • describe the composition of solutions. • define the terms solute and solvent. • identify the solute and solvent in a solution. • describe the different types of solutions and give examples of each type. • define colloids and suspensions. • explain the differences among solutions, colloids, and suspensions. • list some common examples of colloids. Vocabulary colloid type of mixture in which the size of the particles is between 1 × 103 pm and 1 × 106 pm solute the substance in a solution present in the least amount solution a homogeneous mixture solvent the substance in a solution present in the greatest amount suspension type of mixture in which the particles settle to the bottom of the container and can be separated by filtration Tyndall effect the scattering of light by particles Introduction In this chapter, we begin our study of solution chemistry. We all might think that we know what a solution is, listing a drink like tea or soda as an example of a solution. What you might not have realized, however, is that the air or alloys such as brass are all classified as solutions. Why are these classified as solutions? Why wouldn’t milk be classified as a true solution? To answer these questions, we have to learn some specific properties of solutions. Let’s begin with the definition of a solution and look at some of the different types of solutions. 2 www.ck12.org Chapter 1. Solutions and Their Behavior Homogeneous Mixtures A solution is a homogeneous mixture (remember the prefix “homo-” means “same”), meaning that the properties are the same throughout the solution. Take, for example, the vinegar that is used in cooking. Vinegar is approximately 5% acetic acid in water. This means that every teaspoon of vinegar contains 5% acetic acid and 95% water by mass. When a solution is said to have uniform properties, the definition is referring to properties at the particle level. What does this mean? Consider brass as an example, which is an alloy made from copper and zinc. An alloy is a homogeneous mixture formed when one solid is dissolved in another. To the naked eye, a brass coin seems like it is just one substance, but at a particle level two substances are present (copper atoms and zinc atoms). Now consider a pile of zinc filings and copper pieces. Is this now a homogeneous solution? The properties of any spoonful of the mixture you are holding would not be consistent with any other spoonful you removed from the mixture, so the combination of zinc filings and copper pieces in a pile does not represent a homogeneous mixture. The solvent and solute are the two basic parts of a solution. The solvent is the substance present in the greatest amount. The solute, then, is the substance present in the least amount. When you are making a cup of hot chocolate, you take a teaspoon of cocoa powder and dissolve it in a cup of hot water. Since much less cocoa powder is used than water, the cocoa powder is the solute and the water is the solvent. Just because solutions have the same composition throughout does not mean the composition cannot be varied. If you were to dissolve a quarter teaspoon of table salt in one cup of water, a solution would form. You can, however, vary the composition of this solution to a point. If you were to add another half teaspoon of salt to the cup of water, you would still make a solution, but the composition of this solution would be different from the last one. What would happen if you tried to dissolve half cup of salt in the water? At this point, the solution has passed its limit as to the amount of salt that can be dissolved in it, so it would no longer be a homogeneous solution. As a result, solutions have a constant composition that can be varied up to a point. There are usually limits, however, to the amount of substance that can be dissolved into another substance and still remain homogeneous. Types of Solutions There are three states of matter: solid, liquid, and gas. If we think about solutions and the possibilities of combining these states together to form solutions, we have nine possibilities of solutions. Look at Table 1.1. TABLE 1.1: Types of Solutions Solid Solvent Liquid Solvent Gaseous Solvent Solid Solute Solid in a Solid Solid in a Liquid Solid in a Gas Liquid Solute Liquid in a Solid Liquid in a Liquid Liquid in a Gas Gaseous Solute Gas in a Solid Gas in a Liquid Gas in a Gas Although there are nine possibilities, there are really only four common types of solutions. For example, a solid in a liquid solution can be anything from a sugar solution to seawater. Liquid in liquid solutions include vinegar and the antifreeze/coolant used in cars. For a gas in a liquid solution, the most common example is in soft drinks: carbon dioxide is a gas dissolved in water. Another example is the ammonia solution used for cleaning. Finally, to understand a gas in a gas solution, take a deep breath. Air is a solution made up of mostly oxygen gas and nitrogen gas. A solid in a solid solution is often a metallic alloy like steel or brass. The other types of solutions are still solutions, but they are less common in everyday lives. Example: Name the solute and solvent in each of the following mixtures. a. salt water b. air 3 1.1. Properties of Solutions www.ck12.org Solution: a. solute = salt; solvent = water b. solute = oxygen, argon, carbon dioxide, + more; solvent = nitrogen Colloids and Suspensions Unlike solutions, colloids are mixtures in which the size of the particles is between 1 × 103 pm and 1 × 106 pm. In meters, these sizes translate to 1 × 10−9 m to 1 × 10−6 m. As a comparison, a small grain of sand has a diameter of 2 × 10−5 m. A common example of a colloid is milk. One way to tell that milk is a colloid is by the Tyndall effect. The Tyndall effect is the scattering of light by particles. This involves shining a light through the mixture: when the light cannot pass through the mixture, the mixture is considered a colloid. This is why milk appears “cloudy” –or what we think of as “milky.” When light is passed through a true solution, the particles are so small that they do not obstruct the light. For example, the solution vinegar is clear and allows light to pass through easily. In comparison, when light is passed through a colloid, the larger particles act as an obstruction to the light, causing the light to scatter. The particles, however, are still small enough so that they do not settle out of solution. Look at Table 1.2 for some common colloid products that are formed when different phase solutes and solvents are mixed. TABLE 1.2: Some Common Colloidal Materials Solid Solvent Liquid Solvent Gaseous Solvent Solid Solute Ruby, brass, steel Butter, cheese, mustard, Marshmallow Jell-o Liquid Solute Paint, milk of magnesia Milk, mayonnaise, face Whipping cream, shaving creams cream Gaseous Solute Airborn viruses, car ex- Fog, clouds Aerosol Sprays haust, smoke Suspensions are mixtures where the particles settle to the bottom of the container.
Load more

Recommended publications
  • Paclitaxel-Loaded Glycyrrhizic Acid Micelles
    Molecules 2015, 20, 4337-4356; doi:10.3390/molecules20034337 OPEN ACCESS molecules ISSN 1420-3049 www.mdpi.com/journal/molecules Article Bioavailability Enhancement of Paclitaxel via a Novel Oral Drug Delivery System: Paclitaxel-Loaded Glycyrrhizic Acid Micelles Fu-Heng Yang †, Qing Zhang †, Qian-Ying Liang, Sheng-Qi Wang, Bo-Xin Zhao, Ya-Tian Wang, Yun Cai and Guo-Feng Li * Department of Pharmacy, Nanfang Hospital, Southern Medical University, Guangzhou 510515, China; E-Mails: [email protected] (F.-H.Y.); [email protected] (Q.Z.); [email protected] (Q.-Y.L.); [email protected] (S.-Q.W.); [email protected] (B.-X.Z.); [email protected] (Y.-T.W.); [email protected] (Y.C.) † These authors contributed equally to this work. * Author to whom correspondence should be addressed; E-Mail: [email protected]; Tel.: +86-20-6278-7236; Fax: +86-20-6278-7724. Academic Editor: Derek J. McPhee Received: 7 November 2014 / Accepted: 25 February 2015 / Published: 6 March 2015 Abstract: Paclitaxel (PTX, taxol), a classical antitumor drug against a wide range of tumors, shows poor oral bioavailability. In order to improve the oral bioavailability of PTX, glycyrrhizic acid (GA) was used as the carrier in this study. This was the first report on the preparation, characterization and the pharmacokinetic study in rats of PTX-loaded GA micelles The PTX-loaded micelles, prepared with ultrasonic dispersion method, displayed small particle sizes and spherical shapes. Differential scanning calorimeter (DSC) thermograms indicated that PTX was entrapped in the GA micelles and existed as an amorphous state. The encapsulation efficiency was about 90%, and the drug loading rate could reach up to 7.90%.
    [Show full text]
  • Types of Solutions
    Chemistry 51 Chapter 8 TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present in larger amount. Solutes and solvents may be of any form of matter: solid, liquid or gas. Some Examples of Solutions Type Example Solute Solvent Gas in gas Air Oxygen (gas) Nitrogen (gas) Gas in liquid Soda water CO2 (gas) Water (liquid) Liquid in liquid Vinegar Acetic acid (liquid) Water (liquid) Solid in liquid Seawater Salt (solid) Water (liquid) Liquid in solid Dental amalgam Mercury (liquid) Silver (solid) Solid in solid Brass Zinc (solid) Copper (solid) Solutions form between solute and solvent molecules because of similarities between them. (Like dissolves Like) Ionic solids dissolve in water because the charged ions (polar) are attracted to the polar water molecules. Non-polar molecules such as oil and grease dissolve in non-polar solvents such as kerosene. 1 Chemistry 51 Chapter 8 ELECTROLYTES & NON-ELECTROLYTES Solutions can be characterized by their ability to conduct an electric current. Solutions containing ions are conductors of electricity and those that contain molecules are non- conductors. Substances that dissolve in water to form ions are called electrolytes. The ions formed from these substances conduct electric current in solution, and can be tested using a conductivity apparatus (diagram below). Electrolytes are further classified as strong electrolytes and weak electrolytes. In water, a strong electrolyte exists only as ions. Strong electrolytes make the light bulb on the conductivity apparatus glow brightly. Ionic substances such as NaCl are strong electrolytes.
    [Show full text]
  • Addendum.Solubility
    Addendum to Hebden: Chemistry 11 SOLUBILITY I. CALCULATING SOLUBILITY AND ION CONCENTRATIONS Once the mass of a substance present in 1 L of a solution has been experimentally measured, calculating the solubility of the substance is straightforward. EXAMPLE: It is experimentally found that 1.00 L of saturated AgBrO3(aq) contains 1.96 g of AgBrO3. What is the molar solubility of AgBrO3? (That is, what is the solubility expressed in moles per litre?) g 1mol –3 [AgBrO3] = 1.96 x = 8.31 x 10 M L 235 .8 g –3 EXAMPLE: The molar solubility of PbI2 is 1.37 x 10 M. Express this value in grams per litre. –3 mol 461.0 g g Solubility (g/L) = 1.37 x 10 x = 0.632 L 1mol L o EXAMPLE: It is experimentally found that 0.250 L of saturated CaCl2 contains 18.6 g of CaCl2 at 20 C. What is the molar solubility of CaCl2? 18.6 g 1mol [CaCl2] = x = 0.670 M 0 .250L 111 .1g Note: Unless otherwise indicated, assume all solutions are at a temperature of 25oC. EXERCISES: o 1. Aluminum fluoride, AlF3 , has a solubility of 5.59 g/L at 20 C. Express this solubility in moles per litre. o 2. Lead (II) chloride, PbCl2 , has a solubility of 0.99 g/100.0 mL at 20 C. Calculate the molar solubility of PbCl2 . –3 o 3. The molar solubility of MgCO3 is 1.26 x 10 M at 25 C. Express this value in grams per litre. –4 o 4.
    [Show full text]
  • Chemistry Curriculum L1
    1 CHEMISTRY The Nature of Chemistry Topic(s) Concepts Competencies (Eligible Anchor Descriptions Vocabulary Textbook Duration (with Standards) Content) Pages (in days) The Scientific 3.2.10.A6: CHEM.A.1.1.1: CHEM.A.1.1: The Nature of Chemistry L1: Ch 1 (p3-27) 2-5 Method • Compare and contrast • Classify physical or • Identify and describe how Analytical chemistry scientific theories. chemical changes within a observable and measurable Biochemistry Laboratory • Know that both direct system in terms of matter properties can be used to Chemistry Procedure(s) and indirect observations and/or energy. classify and describe matter Inorganic chemistry and Safety are used by scientists to and energy. Organic chemistry study the natural world CHEM.A.1.1.2: Physical chemistry The Metric and universe. • Classify observations as Science System, • Identify questions and qualitative and/or Technology Significant concepts that guide quantitative. Figures, and scientific investigations. Scientific Methods and L1 and L2: 2-5 Measurement • Formulate and revise CHEM.A.1.1.3: Laboratory Safety & Teacher and explanations and models • Utilize significant figures to Procedures department using logic and evidence. communicate the Control generated • Recognize and analyze uncertainty in a quantitative Control experiment materials; Flinn alternative explanations observation. Dependent variable Scientific Safetly and models. Erlenmeyer flask (E-flask) Contract • Explain the importance of Graduated cylinder accuracy and precision in Hypothesis making valid Independent variable measurements. Laboratory balance Laboratory burner 3.2.C.A6: Law • Examine the status of Observation existing theories. Science Scientific method • Evaluate experimental Theory information for relevance Variable and adherence to Laboratory equipment science processes.
    [Show full text]
  • Through-Process Modeling of Aluminum Alloys for Cold Spray: EXPERIMENTAL CHARACTERIZATION and VERIFICATION of MODELS
    Through-Process Modeling of Aluminum Alloys for Cold Spray: EXPERIMENTAL CHARACTERIZATION AND VERIFICATION OF MODELS by Baillie McNally A Dissertation Submitted to the Faculty of the WORCESTER POLYTECHNIC INSTITUTE In partial fulfillment of the requirements for the Degree of Doctor of Philosophy in Materials Science and Engineering January 2016 Approved: Richard D. Sisson, Jr., Advisor Director of the Material Science and Engineering Program George F. Fuller Professor Mechanical Engineering ABSTRACT The cold spray process is a cost-effective process for repairing damaged parts or creating thin coatings and structural bulk materials for military vehicles and aircraft that require high maneuverability, durability, and energy efficiency. This process can be made even more robust with a predictive tool that would tailor the material and processing parameters to a variety of applications. A through-process model that includes powder production, powder processing, cold spray particle impact, and post-processing would benefit the current trial and error efforts immensely and would aid in the search for optimal cold spray alloys for different applications. The powder production stage addresses the microstructure, phases and strength that result from the gas atomization process. The powder processing stage takes into account microstructural effects from heat treating or degassing the powder before it is cold sprayed. The particle impact stage includes a finite element model that simulates the temperature generation and strain that occurs during cold spray. An additive strength model, which is applied to the powder and used as an input into the impact model, determines the contributions of solid solution, microstructural, and precipitation strengthening and is a function of particle diameter, and time and temperature of powder processing.
    [Show full text]
  • Table of Contents
    TABLE OF CONTENTS SECTION 1: BASIC CONSTANTS, UNITS, AND CONVERSION FACTORS CODATA Recommended Values of the Fundamental Physical Constants: 2014 ............................................................................. 1-1 Standard Atomic Weights .............................................................................................................................................................. 1-10 Atomic Masses and Abundances ................................................................................................................................................... 1-12 Electron Configuration and Ionization Energy of Neutral Atoms in the Ground State .............................................................. 1-16 International Temperature Scale of 1990 (ITS-90) ....................................................................................................................... 1-17 International System of Units (SI) ................................................................................................................................................. 1-18 Units for Magnetic Properties ........................................................................................................................................................ 1-22 Conversion Factors for Energy Units ............................................................................................................................................ 1-23 Descriptive Terms for Solubility ..................................................................................................................................................
    [Show full text]
  • Solid in Liquid Solution Example
    Solid In Liquid Solution Example Mohammad is covetous: she circling aloft and jarrings her somatoplasm. Phoebean and anglophobic fragmentarilyErny demagnetises, or primly but after Oliver Poul roundabout socialise andconfesses touzle uneasily,her Senusis. tintless Wadsworth and Lupercalian. tars his limping services Make a solution of the solutes will dissolve in all throughout and composition all matter that the type of liquid in water molecules are In hydrogen is strongly flavored water or screen to respond to mix with water molecules and chocolate recently developed in solid liquid solution is? What happens due to strain out. Weak electrolytes are removed, when frozen into silver, they vibrate a measure out a clustering effect on. Mass of examples of it makes sense it from water example, liquid type of a volume. Students to get the solution in water is an important role, matter distinct state, vapor pressure of solute is oil and the validity or dispersed particles. Was evaporated all specimens of evaluation of molecular, carbon dioxide gas or composition. In a solution ions in vinegar salad dressing is in a solution in an example of examples might not. This example of examples of springer nature of a cake and cold water but the teakettle or not. In particular solvents in industry, quis nostrud exercitation ullamco laboris nisi ut aliquip ex ea commodo consequat. Solutions to be liquid. Learning family and zinc are convenient units when a solvent, and petrol and drink with increase. See them again form a gas dissolved ions in your name. Macro scale somewhere between. Their mouth such as you ever wondered what do ionic compounds are classified as calcium ions.
    [Show full text]
  • Experiment 16 87 Interpreting the Table of Solubility Properties S the Solubility in Water Is at Least 0.1 M
    Appendix: Solubility Properties of Ions and Solids – 2– – 2– 3– – 2– 2– Cl SO4 C2H3O2 CO3 , PO4 OH , O S + + + Na , K , NH4 S S S S S S Ba2+ S I S A S– S Ca2+ S S– S A S– S Mg2+ S S S A A S Fe3+ (yellow) S S S A A A Fe2+ (pale aqua) S S S A A A Cr3+ (blue-violet) S S S A A A Al3+ S S S A, B A, B A, B Ni2+ (green) S S S A, N A, N A+, O+ Co2+ (pink) S S S A A A+, O+ Zn2+ S S S A, B, N A, B, N A Mn2+ (light pink) S S S A A A Cu2+ (blue) S S S A, N A, N O Cd2+ S S S A, N A, N A+, O Ag+ A+, N S–, N S–, N A, N A, N O Pb2+ HW, B, B S A, B A, B O A+ Note: Br– and I– have solubility properties similar to Cl–, but they have significantly different oxidation potentials. Key: S soluble in water S– slightly soluble in water HW soluble in hot water A soluble in acid (6 M HCl or other non-precipitating, non-oxidizing acid) A+ soluble in 12 M HCl O soluble in hot 6 M HNO3 (an oxidizing acid) + O soluble in aqua regia (12 M HNO3 and 12 M HCl mixed in a 1:3 ratio) B soluble in 6 M NaOH N soluble in 6 M NH3 I insoluble in any common reagent Chemistry 1B Experiment 16 87 Interpreting the table of solubility properties S The solubility in water is at least 0.1 M.
    [Show full text]
  • Solubility Handbook Collected from Wikipedia by Khaled Gharib ([email protected])
    Solubility handbook Collected from wikipedia by Khaled Gharib ([email protected]) PDF generated using the open source mwlib toolkit. See http://code.pediapress.com/ for more information. PDF generated at: Sat, 31 Mar 2012 09:49:23 UTC Contents Articles What is solubility 1 Solubility 1 Solubility chart 8 Solubility chart 8 Solubility table 10 Solubility table 10 References Article Sources and Contributors 39 Image Sources, Licenses and Contributors 40 Article Licenses License 41 1 What is solubility Solubility Solubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a solid, liquid, or gaseous solvent to form a homogeneous solution of the solute in the solvent. The solubility of a substance fundamentally depends on the used solvent as well as on temperature and pressure. The extent of the solubility of a substance in a specific solvent is measured as the saturation concentration where adding more solute does not increase the concentration of the solution. Most often, the solvent is a liquid, which can be a pure substance or a mixture.[1] One may also speak of solid solution, but rarely of solution in a gas (see vapor-liquid equilibrium instead). The extent of solubility ranges widely, from infinitely soluble (fully miscible[2]) such as ethanol in water, to poorly soluble, such as silver chloride in water. The term insoluble is often applied to poorly or very poorly soluble compounds. Under certain conditions, the equilibrium solubility can be exceeded to give a so-called supersaturated solution, which is metastable.[3] Solubility is not to be confused with the ability to dissolve or liquefy a substance, because the solution might occur not only because of dissolution but also because of a chemical reaction.
    [Show full text]
  • Design and Testing of an Apparatus to Measure Carbon Dioxide Solubility in Liquid Foods
    DESIGN AND TESTING OF AN APPARATUS TO MEASURE CARBON DIOXIDE SOLUBILITY IN LIQUID FOODS By THELMA FRANCISCA CALIX LARA A THESIS PRESENTED TO THE GRADUATE SCHOOL OF THE UNIVERSITY OF FLORIDA IN PARTIAL FULFILLMENT OF THE REQUIREMENTS FOR THE DEGREE OF MASTER OF SCIENCE UNIVERSITY OF FLORIDA 2008 1 © 2008 Thelma Francisca Calix Lara 2 To those that have guided and inspired me 3 ACKNOWLEDGMENTS I wish to express my special gratitude to my major advisor, Dr. Murat O. Balaban, for his valuable support, guidance and for being an example of motivation and hard work to us. I also like to thank my advising committee, Dr. Charles A. Sims and Dr. Allen F. Wysocki, for their guidance, assistance and time for my research. I am very grateful for my lab partners and friends, Luis, Jose, Max, Milena, Alberto, Zareena, Mutlu, Diana, Wendy, Yavuz, Maria and Giovanna for their assistance and for making the work in the lab such an enjoyable experience. I thank infinitely to my parents, Winston and Sagrario, my sister and my brother, Lourdes and Winston, for their unconditional love and support during my entire life. They have been my primary inspiration to pursue my goal. Finally, my dearest thanks to Jorge, for all the support and happiness he brought to my life. 4 TABLE OF CONTENTS page ACKNOWLEDGMENTS ...............................................................................................................4 LIST OF TABLES...........................................................................................................................7 LIST
    [Show full text]
  • WO 2016/183279 Al 17 November 2016 (17.11.2016) P O P C T
    (12) INTERNATIONAL APPLICATION PUBLISHED UNDER THE PATENT COOPERATION TREATY (PCT) (19) World Intellectual Property Organization I International Bureau (10) International Publication Number (43) International Publication Date WO 2016/183279 Al 17 November 2016 (17.11.2016) P O P C T (51) International Patent Classification: (81) Designated States (unless otherwise indicated, for every C09D 175/16 (2006.01) C08G 18/73 (2006.01) kind of national protection available): AE, AG, AL, AM, C08G 18/67 (2006.01) AO, AT, AU, AZ, BA, BB, BG, BH, BN, BR, BW, BY, BZ, CA, CH, CL, CN, CO, CR, CU, CZ, DE, DK, DM, (21) Number: International Application DO, DZ, EC, EE, EG, ES, FI, GB, GD, GE, GH, GM, GT, PCT/US20 16/03 1997 HN, HR, HU, ID, IL, IN, IR, IS, JP, KE, KG, KN, KP, KR, (22) International Filing Date: KZ, LA, LC, LK, LR, LS, LU, LY, MA, MD, ME, MG, 12 May 2016 (12.05.2016) MK, MN, MW, MX, MY, MZ, NA, NG, NI, NO, NZ, OM, PA, PE, PG, PH, PL, PT, QA, RO, RS, RU, RW, SA, SC, (25) Filing Language: English SD, SE, SG, SK, SL, SM, ST, SV, SY, TH, TJ, TM, TN, (26) Publication Language: English TR, TT, TZ, UA, UG, US, UZ, VC, VN, ZA, ZM, ZW. (30) Priority Data: (84) Designated States (unless otherwise indicated, for every 62/160,094 12 May 2015 (12.05.2015) US kind of regional protection available): ARIPO (BW, GH, GM, KE, LR, LS, MW, MZ, NA, RW, SD, SL, ST, SZ, (71) Applicant: RHODIA OPERATIONS [FR/FR]; 25, Rue TZ, UG, ZM, ZW), Eurasian (AM, AZ, BY, KG, KZ, RU, De Clichy, 75009 Paris (FR).
    [Show full text]
  • Application and Optimization of Membrane Processes Treating Brackish and Surficial Groundwater for Potable Water Production
    University of Central Florida STARS Electronic Theses and Dissertations, 2004-2019 2012 Application And Optimization Of Membrane Processes Treating Brackish And Surficial Groundwater For Potable Water Production Jayapregasham Tharamapalan University of Central Florida Part of the Environmental Engineering Commons Find similar works at: https://stars.library.ucf.edu/etd University of Central Florida Libraries http://library.ucf.edu This Doctoral Dissertation (Open Access) is brought to you for free and open access by STARS. It has been accepted for inclusion in Electronic Theses and Dissertations, 2004-2019 by an authorized administrator of STARS. For more information, please contact [email protected]. STARS Citation Tharamapalan, Jayapregasham, "Application And Optimization Of Membrane Processes Treating Brackish And Surficial Groundwater For Potable Water Production" (2012). Electronic Theses and Dissertations, 2004-2019. 2503. https://stars.library.ucf.edu/etd/2503 APPLICATION AND OPTIMIZATION OF MEMBRANE PROCESSES TREATING BRACKISH AND SURFICIAL GROUNDWATER FOR POTABLE WATER PRODUCTION by JAYAPREGASHAM THARAMAPALAN B.Eng (Civil & Structural), Nanyang Technological University, Singapore, 1994 MSc (Environmental), Nanyang Technological University, Singapore, 2003 A dissertation submitted in partial fulfillment of the requirements for the degree of Doctor of Philosophy in the Department of Civil, Environmental, and Construction Engineering in the College of Engineering and Computer Science at the University of Central Florida Orlando, Florida Fall Term 2012 Major Professor: Steven J. Duranceau © 2012 Jayapregasham Tharamapalan ii ABSTRACT The research presented in this dissertation provides the results of a comprehensive assessment of the water treatment requirements for the City of Sarasota. The City’s drinking water supply originates from two sources: (1) brackish groundwater from the Downtown well field, and (2) Floridan surficial groundwater from the City’s Verna well field.
    [Show full text]