DOCSLIB.ORG

Moles and Molarity 6 Equivalent Weights and Normality 7 Dilution Calculations 8 Standard Solutions 12

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text

Load more

This is the table of contents and a sample chapter from WSO Water Treatment, Grade 2, get your full copy from AWWA. awwa.org/wso © 2016 American Water Works Association Contents Chapter 1 Basic Microbiology and Chemistry 1 Chemical Formulas and Equations 1 Moles and Molarity 6 Equivalent Weights and Normality 7 Dilution Calculations 8 Standard Solutions 12 Chapter 2 Operator Math 15 Volume Measurements 15 Conversions 22 Average Daily Flow 30 Surface Overflow Rate 33 Weir Overflow Rate 36 Filter Loading Rate 38 Filter Backwash Rate 41 Mudball Calculation 43 Detention Time 44 Pressure 47 Flow Rate Problems 52 Chemical Dosage Problems 55 Chapter 3 USEPA Water Regulations 71 Types of Water Systems 71 Disinfection By- product and Microbial Regulations 72 Chapter 4 Coagulation and Flocculation Process Operation 89 Operation of the Processes 89 Dosage Control 93 Safety Precautions 93 Record Keeping 94 Chapter 5 Sedimentation and Clarifiers 97 Process Description 97 Sedimentation Facilities 98 Other Clarification Processes 104 Regulations 107 Operation of the Process 107 iii 000200010272023365_ch00_FM_pi-vi.indd 3 5/2/16 9:51 AM iv WSO Water Treatment Grade 2 Chapter 6 Filtration 115 Equipment Associated With Gravity Filters 115 Operation of Gravity Filters 123 Pressure Filtration 135 Regulations 138 Safety Precautions 138 Record Keeping 139 Chapter 7 Chlorine Disinfection 143 Gas Chlorination Facilities 143 Hypochlorination Facilities 155 Operation of the Chlorination Process 157 Chlorination Operating Problems 162 Safety Precautions 165 Record Keeping 170 Chapter 8 Iron and Manganese Treatment 173 Excessive Iron and Manganese 173 Control Processes 175 Control Facilities 178 Regulations 182 Manganese Greensand Filter Operation 182 Process Monitoring 188 Operating Problems 188 Record Keeping 188 Chapter 9 Fluoridation Process Operation 191 Operation of the Fluoridation Process 191 Fluoridation Operating Problems 193 Control Tests 194 Safety Precautions 195 Record Keeping 196 Chapter 10 Water Quality Testing 199 Testing and Laboratory Procedures 199 Physical and Aggregate Properties of Water 209 Chapter 11 Corrosion Control 221 Purposes of Corrosion and Scaling Control 221 Water System Corrosion 222 Scale Formation 226 Corrosion and Scaling Control Methods 227 Corrosion and Scaling Control Facilities 230 Chemical Feed Equipment 233 Chapter 12 Lime Softening 237 Lime Softening Chemical Reactions 237 Lime Softening Facilities 239 Regulations 244 000200010272023365_ch00_FM_pi-vi.indd 4 5/2/16 9:51 AM Contents v Chapter 13 Ion Exchange 247 Ion Exchange Softening 247 Facilities 247 Operation of Ion Exchange Processes 252 Operating Problems 254 Ion Exchange for Removal of Arsenic, Barium, Radium, Nitrate, TOC, and Uranium 255 Activated Alumina Fluoride Removal Process 257 Adsorptive Media 257 Chapter 14 Activated Carbon Adsorption 261 The Principle of Adsorption 261 Adsorption Facilities 262 Powdered Activated Carbon 263 Granular Activated Carbon 265 Regulations 268 Operating Procedures for Adsorption 268 Operating Problems 272 Control Tests 273 Record Keeping 276 Chapter 15 Aeration 279 Water-Into-Air Aerators 279 Air-Into-Water Aerators 284 Combination Aerators 285 Chapter 16 Membrane Treatment 291 Microfiltration Facilities 291 Pleated Membrane Facilities 294 Reverse Osmosis Facilities 297 Chapter 17 Plant Waste Treatment and Disposal 303 Removal of Sludge from Conventional Sedimentation Processes 303 Softening Sludge Handling, Dewatering, and Disposal 305 Solids Separation Technologies 306 Chapter 18 Instrumentation and Control Systems 313 Flow, Pressure, and Level Measurement 313 Other Operational Control Instruments 316 Automation 317 Computerization 318 Chapter 19 Centrifugal Pumps 321 Operation of Centrifugal Pumps 321 Centrifugal Pump Maintenance 325 Record Keeping 336 Pump Safety 336 000200010272023365_ch00_FM_pi-vi.indd 5 5/2/16 9:51 AM vi WSO Water Treatment Grade 2 Chapter 20 Treatment Plant Safety and Security Practices 339 Treatment Plant Safety Review 339 Plant Security 348 Chapter 21 Administration, Records, and Reporting Procedures 355 Process Records 355 Reporting 359 Plant Performance Reports 360 Public Relations 360 Chapter 22 Additional Level 2 Study Questions 363 Study Question Answers 369 Glossary 379 Index 387 000200010272023365_ch00_FM_pi-vi.indd 6 5/2/16 9:51 AM ChapterChapter 11 BasicBasic MicrobiologyMicrobiology andand ChemistryChemistry Chemical Formulas and Equations A group of chemically bonded atoms forms a particle called a molecule. The sim- plest molecules contain only one type of atom, such as when two atoms of oxygen combine (O2) or when two atoms of chlorine combine (Cl2). Molecules of com- pounds are made up of the atoms of at least two different elements; for example, one oxygen atom and two hydrogen atoms form a molecule of the compound water (H2O). “H2O” is called the chemical formula of water. The formula is a shorthand way of writing what elements are present in a molecule of a com- pound, and how many atoms of each element are present in each molecule. Reading Chemical Formulas The following are examples of chemical formulas and what they indicate. Example 1 The chemical formula for calcium carbonate is CaCO3 According to the formula, what is the chemical makeup of the compound? First, the letter symbols given in the formula indicate the three elements that make up the calcium carbonate compound: Ca = calcium C = carbon O = oxygen Second, the subscripts (the small numbers at the lower right corners of the letter symbols) in the formula indicate how many atoms of each element are present in a single molecule of the compound. There is no number just to the right of the Ca or C symbols; this indicates that only one atom of each chemical formula element is present in the molecule. The subscript 3 to the right of the O sym- Using the chemical bolizing oxygen indicates that there are three oxygen atoms in each molecule. symbols for each element, a shorthand CaCO3 way of writing what elements are present in a molecule and how many 1 atom 3 atoms atoms of each element are present in each of the 1 atom molecules. 1 000200010272023365_ch01_p001-014.indd 1 5/2/16 9:05 AM 2 WSO Water Treatment Grade 2 Determining Percent by Weight of Elements in a Compound If 100 lb of sodium chloride (NaCl) were separated into the elements that make up the compound, there would be 39.3 lb of pure sodium (Na) and 60.7 lb of pure chlorine (Cl). We say that sodium chloride is 39.3 percent sodium by weight and that it is 60.7 percent chlorine by weight. The percent by weight of each element in a compound can be calculated using the compound’s chemical formula and atomic weights from the periodic table. The first step in calculating percent by weight of an element in a compound is to determine the molecular weight (sometimes called formula weight) of the compound. The molecular weight of a compound is defined as the sum of the atomic weights of all the atoms in the compound. For example, to determine the molecular weight of sodium chloride, first count how many atoms of each element a single molecule contains: Na Cl 1 atom 1 atom Next, find the atomic weight of each atom, using the periodic table: atomic weight of Na = 22.99 atomic weight of Cl = 35.45 Finally, multiply each atomic weight by the number of atoms of that element in the molecule, and total the weights: Number of Atomic Total Atoms Weight Weight sodium (Na) 1 × 22.99 = 22.99 chlorine (Cl) 1 × 35.45 = 35.45 molecular weight of NaCl = 58.44 Once the molecular weight of a compound is determined, the percent by weight of each element in the compound can be found with the following formula: weight of element in compound percent element by weight = × 100 molecular weight of compound percent by weight Using the formula, first calculate the percent by weight of sodium in the The proportion, compound: calculated as a weight of Na in compound percentage, of each percent Na by weight = × 100 element in a compound. molecular weight of compound 22.99 molecular weight = × 100 The sum of the atomic 58.44 weights of all the atoms = 0.393 × 100 in the compound. Also called formula weight. = 39.3% sodium by weight 000200010272023365_ch01_p001-014.indd 2 5/2/16 9:05 AM Basic Microbiology and Chemistry 3 Then, calculate percent by weight of chlorine in the compound: weight of Cl in compound percent Cl by weight = × 100 molecular weight of compound 35.45 = × 100 58.44 = 0.607 × 100 = 60.7% chlorine by weight To check the calculations, add the percentages. The total should be 100: 39.3% Na + 60.7% Cl 100.0% NaCl Chemical Equations A chemical equation is a shorthand way, through the use of chemical formulas, to write the reaction that takes place when certain chemicals are brought together. As shown in the following example, the left side of the equation indicates the reactants, or chemicals that will be brought together; the arrow indicates which direction the reaction occurs; and the right side of the equation indicates the prod- ucts, or results, of the chemical reaction. calcium calcium react to calcium plus plus water bicarbonate hydroxide form carbonate chemical equation A shorthand way, using Ca(HCO ) + Ca(OH) 2CaCO + 2H O chemical formulas, of 3 2 2 3 2 writing the reaction that takes place when Reactants Products chemicals are brought together. The left side of the equation indicates The 2 in front of CaCO3 is called a coefficient. A coefficient indicates the relative number of molecules of the compound that are involved in the chemical the chemicals brought reaction. If no coefficient is shown, then only one molecule of the compound is together (the reactants); involved. For example, in the preceding equation, one molecule of calcium bi- the arrow indicates in which direction the carbonate reacts with one molecule of calcium hydroxide to form two molecules reaction occurs; and the of calcium carbonate and two molecules of water.
Recommended publications
  • Thermodynamics of Ion Exchange

    Thermodynamics of Ion Exchange

    Chapter 1 Thermodynamics of Ion Exchange Ayben Kilislioğlu Additional information is available at the end of the chapter http://dx.doi.org/10.5772/53558 1. Introduction 1.1. Ion exchange equilibria During an ion exchange process, ions are essentially stepped from the solvent phase to the solid surface. As the binding of an ion takes place at the solid surface, the rotational and translational freedom of the solute are reduced. Therefore, the entropy change (ΔS) during ion exchange is negative. For ion exchange to be convenient, Gibbs free energy change (ΔG) must be negative, which in turn requires the enthalpy change to be negative because ΔG = ΔH - TΔS. Both enthalpic (ΔHo) and entropic (ΔSo) changes help decide the overall selectivity of the ion-exchange process [Marcus Y., SenGupta A. K. 2004]. Thermodynamics have great efficiency on the impulsion of ion exchange. It also sets the equilibrium distribution of ions between the solution and the solid. A discussion about the role of thermodynamics relevant to both of these phenomena was done by researchers [Araujo R., 2004]. As the basic rule of ion exchange, one type of a free mobile ion of a solution become fixed on the solid surface by releasing a different kind of an ion from the solid surface. It is a reversible process which means that there is no permanent change on the solid surface by the process. Ion exchange has many applications in different fields like enviromental, medical, technological,.. etc. To evaluate the properties and efficiency of the ion exchange one must determine the equilibrium conditions.
  • Polymer Exemption Guidance Manual POLYMER EXEMPTION GUIDANCE MANUAL

    Polymer Exemption Guidance Manual POLYMER EXEMPTION GUIDANCE MANUAL

    United States Office of Pollution EPA 744-B-97-001 Environmental Protection Prevention and Toxics June 1997 Agency (7406) Polymer Exemption Guidance Manual POLYMER EXEMPTION GUIDANCE MANUAL 5/22/97 A technical manual to accompany, but not supersede the "Premanufacture Notification Exemptions; Revisions of Exemptions for Polymers; Final Rule" found at 40 CFR Part 723, (60) FR 16316-16336, published Wednesday, March 29, 1995 Environmental Protection Agency Office of Pollution Prevention and Toxics 401 M St., SW., Washington, DC 20460-0001 Copies of this document are available through the TSCA Assistance Information Service at (202) 554-1404 or by faxing requests to (202) 554-5603. TABLE OF CONTENTS LIST OF EQUATIONS............................ ii LIST OF FIGURES............................. ii LIST OF TABLES ............................. ii 1. INTRODUCTION ............................ 1 2. HISTORY............................... 2 3. DEFINITIONS............................. 3 4. ELIGIBILITY REQUIREMENTS ...................... 4 4.1. MEETING THE DEFINITION OF A POLYMER AT 40 CFR §723.250(b)... 5 4.2. SUBSTANCES EXCLUDED FROM THE EXEMPTION AT 40 CFR §723.250(d) . 7 4.2.1. EXCLUSIONS FOR CATIONIC AND POTENTIALLY CATIONIC POLYMERS ....................... 8 4.2.1.1. CATIONIC POLYMERS NOT EXCLUDED FROM EXEMPTION 8 4.2.2. EXCLUSIONS FOR ELEMENTAL CRITERIA........... 9 4.2.3. EXCLUSIONS FOR DEGRADABLE OR UNSTABLE POLYMERS .... 9 4.2.4. EXCLUSIONS BY REACTANTS................ 9 4.2.5. EXCLUSIONS FOR WATER-ABSORBING POLYMERS........ 10 4.3. CATEGORIES WHICH ARE NO LONGER EXCLUDED FROM EXEMPTION .... 10 4.4. MEETING EXEMPTION CRITERIA AT 40 CFR §723.250(e) ....... 10 4.4.1. THE (e)(1) EXEMPTION CRITERIA............. 10 4.4.1.1. LOW-CONCERN FUNCTIONAL GROUPS AND THE (e)(1) EXEMPTION.................
  • Chapter 20 Electrochemistry

    Chapter 20 Electrochemistry

    Chapter 20 Electrochemistry Learning goals and key skills: Identify oxidation, reduction, oxidizing agent, and reducing agent in a chemical equation Complete and balance redox equations using the method of half-reactions. Sketch a voltaic cell and identify its cathode, anode, and the directions in which electrons and ions move. o Calculate standard emfs (cell potentials), E cell, from standard reduction potentials. Use reduction potentials to predict whether a redox reaction is spontaneous. o o Relate E cell to DG and equilibrium constants. Calculate emf under nonstandard conditions. Identify the components of common batteries. Describe the construction of a lithium-ion battery and explain how it works. Describe the construction of a fuel cell and explain how it generates electrical energy. Explain how corrosion occurs and how it is prevented by cathodic protection. Describe the reactions in electrolytic cells. Relate the amounts of products and reactants in redox reactions to electrical charge. Electrochemistry Electrochemistry is the study of the relationships between electricity and chemical reactions. • It includes the study of both spontaneous and nonspontaneous processes. 1 Redox reactions: assigning oxidation numbers Oxidation numbers help keep track of what species loses electrons and what species gains them. • An element is oxidized when the oxidation number increases • An element is reduced when the oxidation number decreases • an oxidizing agent causes another element to be oxidized • a reducing agent causes another element to be reduced. Assigning oxidation numbers (sect. 4.4) 1. Elemental form, each atom has ox. # = 0. Zn O2 O3 I2 S8 P4 2. Simple ions, = charge on ion. -1 for Cl-, +2 for Mg2+ 3.
  • Energy and the Hydrogen Economy

    Energy and the Hydrogen Economy

    Energy and the Hydrogen Economy Ulf Bossel Fuel Cell Consultant Morgenacherstrasse 2F CH-5452 Oberrohrdorf / Switzerland +41-56-496-7292 and Baldur Eliasson ABB Switzerland Ltd. Corporate Research CH-5405 Baden-Dättwil / Switzerland Abstract Between production and use any commercial product is subject to the following processes: packaging, transportation, storage and transfer. The same is true for hydrogen in a “Hydrogen Economy”. Hydrogen has to be packaged by compression or liquefaction, it has to be transported by surface vehicles or pipelines, it has to be stored and transferred. Generated by electrolysis or chemistry, the fuel gas has to go through theses market procedures before it can be used by the customer, even if it is produced locally at filling stations. As there are no environmental or energetic advantages in producing hydrogen from natural gas or other hydrocarbons, we do not consider this option, although hydrogen can be chemically synthesized at relative low cost. In the past, hydrogen production and hydrogen use have been addressed by many, assuming that hydrogen gas is just another gaseous energy carrier and that it can be handled much like natural gas in today’s energy economy. With this study we present an analysis of the energy required to operate a pure hydrogen economy. High-grade electricity from renewable or nuclear sources is needed not only to generate hydrogen, but also for all other essential steps of a hydrogen economy. But because of the molecular structure of hydrogen, a hydrogen infrastructure is much more energy-intensive than a natural gas economy. In this study, the energy consumed by each stage is related to the energy content (higher heating value HHV) of the delivered hydrogen itself.
  • Introduction to Chemistry

    Introduction to Chemistry

    Introduction to Chemistry Author: Tracy Poulsen Digital Proofer Supported by CK-12 Foundation CK-12 Foundation is a non-profit organization with a mission to reduce the cost of textbook Introduction to Chem... materials for the K-12 market both in the U.S. and worldwide. Using an open-content, web-based Authored by Tracy Poulsen collaborative model termed the “FlexBook,” CK-12 intends to pioneer the generation and 8.5" x 11.0" (21.59 x 27.94 cm) distribution of high-quality educational content that will serve both as core text as well as provide Black & White on White paper an adaptive environment for learning. 250 pages ISBN-13: 9781478298601 Copyright © 2010, CK-12 Foundation, www.ck12.org ISBN-10: 147829860X Except as otherwise noted, all CK-12 Content (including CK-12 Curriculum Material) is made Please carefully review your Digital Proof download for formatting, available to Users in accordance with the Creative Commons Attribution/Non-Commercial/Share grammar, and design issues that may need to be corrected. Alike 3.0 Unported (CC-by-NC-SA) License (http://creativecommons.org/licenses/by-nc- sa/3.0/), as amended and updated by Creative Commons from time to time (the “CC License”), We recommend that you review your book three times, with each time focusing on a different aspect. which is incorporated herein by this reference. Specific details can be found at http://about.ck12.org/terms. Check the format, including headers, footers, page 1 numbers, spacing, table of contents, and index. 2 Review any images or graphics and captions if applicable.
  • 1 Some Basic Concepts of Chemistry

    1 Some Basic Concepts of Chemistry

    Some Basic Concepts of Chemistry 1 1 Some Basic Concepts of Chemistry Matter – The three states of matter can be inter-converted by Anything which occupies space, has mass and which can be changing the conditions of temperature and pressure as felt by our senses is called matter. follows : Ev Liq Classification of Matter : Co GasGVa ap as uefacti n po orat tion ndensa – tion Physical Classification : io riza at io on n o tion tion Matter lim ndensa or r Deposi Co Sub or Solid Liquid Solid Liquid Solids Liquids Gases Definite shape Definite No definite Melting or Fusion Freezing or Crystallization and volume volume but no shape and Endothermic state changes Exothermic state changes definite shape volume – Chemical Classification : Matter Pure Substances Mixtures Fixed ratio of masses No fixed ratio of of constituents masses of constituents Elements Compounds Homogeneous Heterogeneous Consists of only one Composed of two Uniform composition Composition is not kind of atoms or more atoms of throughout uniform throughout different elements Solids at room temperature, high density, possess lustre, Metals good conductors of heat and Organic Inorganic electricity Compounds Compounds Originally obtained from Usually obtained from Brittle, do not possess animals and plants, contain minerals and rocks, do not lustre, poor conductors Non-metals carbon and few other elements contain C–H bonds of heat and electricity like H, O, S, N, X (halogens), Possess characteristics etc. having C–H bonds Metalloids of both metals and non- metals Units and Measurements Mass m kilogram kg Fundamental Units : The units which can neither be derived Time t second s from one another nor can be further resolved into any other Temperature T kelvin K units are called fundamental units or basic units.
  • Basic Concepts and Laws of Chemistry. Guidelines and Objectives for Self-Study Courses for Students in All Specialties / O.Y

    Basic Concepts and Laws of Chemistry. Guidelines and Objectives for Self-Study Courses for Students in All Specialties / O.Y

    THE MINISTRY OF EDUCATION AND SCIENCE OF UKRAINE STATE HIGHER EDUCATIONAL INSTITUTION «NATIONAL MINING UNIVERSITY» O.Y. Svietkina, O.B Netyaga, G.V Tarasova BASIC CONCEPTS AND LAWS OF CHEMISTRY. Guidelines and objectives for self-study courses for students in all specialties Dnipro 2016 THE MINISTRY OF EDUCATION AND SCIENCE OF UKRAINE STATE HIGHER EDUCATIONAL INSTITUTION «NATIONAL MINING UNIVERSITY» FACULTY OF GEOLOGICAL PROSPECTING Departament of Chemestry O. Y. Svietkina, O.B Netyaga, G.V Tarasova BASIC CONCEPTS AND LAWS OF CHEMISTRY. Guidelines and objectives for self-study courses for students in all specialties Dnipro NMU 2016 Svietkina O. Y. Basic concepts and laws of chemistry. Guidelines and objectives for self-study courses for students in all specialties / O.Y. Svietkina, O.B. Netyaga, G.V. Tarasova; Ministry of eduk. and sien of Ukrain, Nation. min. univer. – D . : NMU, 2016. – 20 p. Автори: О.Ю. Свєткіна, проф., д-р техн. наук (передмова, розділ 2); О.Б. Нетяга, старш. викл. (розділ 1); Г.В. Тарасова, асист. (розділ 2). Затверджено методичною комісією з галузі знань 10. Природничі науки за поданням кафедри хімії (протокол № 3 від 08.11.2016). The theoretical themes of "Basic concepts and laws of chemistry", are examples of solving common tasks, in order to consolidate the material there are presented self-study tasks for solving. Розглянуто теоретичні положення теми «Основні поняття й закони хімії», наведено приклади розв’язку типових задач з метою закріплення матеріалу, подано задачі для самостійного розв’язування. Відповідальна за випуск завідувач кафедри хімії, д-р техн. наук, проф. О.Ю. Свєткіна. Introduction Chemistry studies such form of substance motion which assumes qualitative change of matters i.e.
  • (I) Determination of the Equivalent Weight and Pka of an Organic Acid

    (I) Determination of the Equivalent Weight and Pka of an Organic Acid

    Experiment 4 (i) Determination of the Equivalent Weight and pKa of an Organic Acid Discussion This experiment is an example of a common research procedure. Chemists often use two or more analytical techniques to study the same system. These experiments can give complementary qualitative and quantitative information concerning an unknown substance. I. Titration of Acids and Bases in Aqueous Solutions The almost instantaneous reaction between acids and bases in aqueous solution produce changes in pH which one can monitor. Two techniques are useful for detecting the equivalence point: (1) colorimetry, using an acid-base color indicator - a dye which undergoes a sharp change in color in a region of pH covering the equivalence point and (2) potentiometry, using a potentiometer (pH meter) to record the sharp change at the equivalence point in the potential difference between an electrode (usually a glass electrode) and the solution whose pH is undergoing change as a result of the addition of acid or base. For example, in the case of the titration of a weak monoprotic acid HA using sodium hydroxide solution we may write: + - NaOH + HA → Na + A + H2O (4.1) Applying the law of mass action to the ionization equilibrium for the weak acid in water: + - HA + H2O H3O + A (4.2) we may write (in dilute solutions [H2O] is essentially constant) [H O+ ][A − ] 3 = K (4.3) [HA] a where Ka is the acid ionization constant (constant at any given temperature). This expression is valid for + - all aqueous solutions containing hydronium ions (H3O ), A ions, and the un-ionized molecules HA.
  • Battle of the Acids Weak Acids and Bases SCIENTIFIC

    Battle of the Acids Weak Acids and Bases SCIENTIFIC

    Battle of the Acids Weak Acids and Bases SCIENTIFIC Introduction Not all acids are created equal. This demonstration compares the “frothing and foaming” activity of different acids with calcium carbonate and examines their behavior in the presence of their conjugate bases to distinguish strong versus weak acids. The use of a “rainbow acid” universal indicator produces a rainbow spectrum of color changes as the mixtures react. Concepts • Strong acid • Weak acid • Conjugate base • pH Materials (for each demonstration) Acetic acid, CH3COOH, 1 M, 400 mL Water, distilled or deionized Calcium carbonate, CaCO3, 40 g Demonstration tray, large Hydrochloric acid, HCl, 1 M, 400 mL Graduated cylinder, 250-mL “Rainbow acid” universal indicator, 5 mL Hydrometer cylinders, 600-mL, 4 (includes accompanying color chart) Pipet, Beral-type Sodium acetate, NaCH3CO2, 16 g Weighing dishes or small beakers, 6 Sodium chloride, NaCl, 12 g Safety Precautions Hydrochloric acid and acetic acid solutions are toxic and corrosive. Avoid contact with skin and eyes. “Rainbow-acid” universal indicator solution is an alcohol-based solution and is flammable. Avoid contact with flames or other ignition sources. Wear chemical splash goggles, chemical-resistant gloves, and a chemical-resistant apron. Please review current Material Safety Data Sheets for additional safety, handling, and disposal information. Preparation To save time in the presentation, pre-measure the amounts of solids needed for the demonstration. Weigh out 12 g of sodium chloride, 16 g of sodium acetate, and 4 × 10-g samples of calcium carbonate in separate, labeled weighing dishes or small beakers. Procedure 1. Obtain 4 large hydrometer cylinders or tall-form beakers and place them on a large demonstration tray.
  • PHARMACY CALCULATIONS •Explain Importance of Calculations in Determining Days Supply •Describe Consequences of Calculation Errors

    PHARMACY CALCULATIONS •Explain Importance of Calculations in Determining Days Supply •Describe Consequences of Calculation Errors

    7/7/2016 THE OBJECTIVES INCLUDE THE FOLLOWING: •Discuss importance of calculations in a pharmacy practice. •Outline steps to avoid calculation errors 2016 ANNUAL MEETING •Explain importance of reading the prescription carefully then performing calculations PHARMACY CALCULATIONS •Explain importance of calculations in determining days supply •Describe consequences of calculation errors. •Perform calculations during the presentation 2016 ANNUAL MEETING 4 ADDITIONAL LEARNING OBJECTIVES •Understand how the concentration of electrolyte 2016 ANNUAL MEETING solutions are expressed and calculations of m.Eq. •Understand the importance of iso-tonicity in SUNIL S. JAMBHEKAR, B. PHARM.; M.S., PH.D ophthalmic solutions. PROFESSOR, PHARMACEUTICAL SCIENCES LECOM BRADENTON, SCHOOL OF PHARMACY •Perform calculations, using a prescription, to BRADENTON, FL34202 determine the quantity of a liquid product required [email protected] to fill the prescription accurately. 2016 ANNUAL MEETING 5 ADDITIONAL LEARNING OBJECTIVES •Perform calculations, using a prescription, to 2016 ANNUAL MEETING determine the # of day supply for a specific DISCLOSURE product. I DO NOT HAVE A VESTED INTEREST IN OR AFFILIATION •Perform calculations to determine m.Eq WITH ANY CORPORATE ORGANIZATION OFFERING FINANCIAL SUPPORT OR GRANT MONIES FOR THIS CONTINUING strength of an electrolyte solution. EDUCATION ACTIVITY, OR ANY AFFILIATION WITH AN ORGANIZATION WHOSE PHILOSOPHY COULD POTENTIALLY •Perform calculations to prepare an isotonic BIAS MY PRESENTATION ophthalmic solution. 2016 ANNUAL MEETING 6 1 7/7/2016 IMPORTANCE OF CALCULATIONS IN THE PHARMACY PRACTICE: •It is consistent with the practice and philosophy of pharmaceutical care. •Insurance companies will reimburse you or •Patient safety is of utmost importance. your employer only for the quantity written on the prescription and not for the quantity •Your pharmacy is the last check point for the dispensed.
  • Stoichiometry of Chemical Reactions 175

    Stoichiometry of Chemical Reactions 175

    Chapter 4 Stoichiometry of Chemical Reactions 175 Chapter 4 Stoichiometry of Chemical Reactions Figure 4.1 Many modern rocket fuels are solid mixtures of substances combined in carefully measured amounts and ignited to yield a thrust-generating chemical reaction. (credit: modification of work by NASA) Chapter Outline 4.1 Writing and Balancing Chemical Equations 4.2 Classifying Chemical Reactions 4.3 Reaction Stoichiometry 4.4 Reaction Yields 4.5 Quantitative Chemical Analysis Introduction Solid-fuel rockets are a central feature in the world’s space exploration programs, including the new Space Launch System being developed by the National Aeronautics and Space Administration (NASA) to replace the retired Space Shuttle fleet (Figure 4.1). The engines of these rockets rely on carefully prepared solid mixtures of chemicals combined in precisely measured amounts. Igniting the mixture initiates a vigorous chemical reaction that rapidly generates large amounts of gaseous products. These gases are ejected from the rocket engine through its nozzle, providing the thrust needed to propel heavy payloads into space. Both the nature of this chemical reaction and the relationships between the amounts of the substances being consumed and produced by the reaction are critically important considerations that determine the success of the technology. This chapter will describe how to symbolize chemical reactions using chemical equations, how to classify some common chemical reactions by identifying patterns of reactivity, and how to determine the quantitative relations between the amounts of substances involved in chemical reactions—that is, the reaction stoichiometry. 176 Chapter 4 Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations By the end of this section, you will be able to: • Derive chemical equations from narrative descriptions of chemical reactions.
  • WO 2019/055177 Al 21 March 2019 (21.03.2019) W 1P O PCT

    WO 2019/055177 Al 21 March 2019 (21.03.2019) W 1P O PCT

    (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 2019/055177 Al 21 March 2019 (21.03.2019) W 1P O PCT (51) International Patent Classification: Declarations under Rule 4.17: C08G 65/02 (2006.01) C08G 18/32 (2006.01) — as to applicant's entitlement to apply for and be granted a C08G 65/26 (2006.01) patent (Rule 4.17(H)) (21) International Application Number: — as to the applicant's entitlement to claim the priority of the PCT/US20 18/047252 earlier application (Rule 4.17(Hi)) (22) International Filing Date: Published: 2 1 August 2018 (21.08.2018) — with international search report (Art. 21(3)) (25) Filing Language: English (26) Publication Language: English (30) Priority Data: 62/559,109 15 September 2017 (15.09.2017) US (71) Applicant: DOW GLOBAL TECHNOLOGIES LLC [US/US]; 2040 Dow Center, Midland, Michigan 48674 (US). (72) Inventors: MASY, Jean-Paul; Herbert H . Dowweg 5, 4542 NM Hoek, Postbus 48, 4530AA Terneuzen (NL). BABB, David A.; 230 1N . Brazosport Boulevard, Freeport, Texas 77541 (US). (74) Agent: Gary C Cohn PLLC; 325 7th Avenue, #203, San Diego, California 92101 (US). (81) Designated States (unless otherwise indicated, for every kind of national protection available) : AE, AG, AL, AM, AO, AT, AU, AZ, BA, BB, BG, BH, BN, BR, BW, BY, BZ, CA, CH, CL, CN, CO, CR, CU, CZ, DE, DJ, DK, DM, DO, DZ, EC, EE, EG, ES, FI, GB, GD, GE, GH, GM, GT, HN, HR, HU, ID, IL, IN, IR, IS, JO, JP, KE, KG, KH, KN, KP, KR, KW, KZ, LA, LC, LK, LR, LS, LU, LY, MA, MD, ME, MG, 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, SD, SE, SG, SK, SL, SM, ST, SV, SY, TH, TJ, TM, TN, TR, TT, TZ, UA, UG, US, UZ, VC, VN, ZA, ZM, ZW.