Laboratory Solution Preparation
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Experiment 4
Experiment Limiting Reactant 5 A limiting reactant is the reagent that is completely consumed during a chemical reaction. Once this reagent is consumed the reaction stops. An excess reagent is the reactant that is left over once the limiting reagent is consumed. The maximum theoretical yield of a chemical reaction is dependent upon the limiting reagent thus the one that produces the least amount of product is the limiting reagent. For example, if a 2.00 g sample of ammonia is mixed with 4.00 g of oxygen in the following reaction, use stoichiometry to determine the limiting reagent. 4NH3 + 5O2 4NO + 6H2O Since the 4.00 g of O2 produced the least amount of product, O2 is the limiting reagent. In this experiment you will be given a mixture of two ionic solids, AgNO3 and K2CrO4, that are both soluble in water. When the mixture is dissolved into water they will react to form an insoluble compound, Ag2CrO4, which can be collected and weighed. The reaction is the following: 2 AgNO3(aq) + K2CrO4(aq) Ag2CrO4(s) + 2 KNO3(aq) Colorless Yellow Red colorless Precipitate Precipitate is the term used for an insoluble solid which is produced by mixing two solutions. Often the solid particles are so fine that they will pass right through the pores of a filter. Heating the solution for a while causes the particles to clump together, a process called digesting. The precipitate coagulates upon cooling and eventually settles to the bottom of a solution container. The clear liquid above the precipitate is called the supernatant. -
Sodium Chloride (Halite, Common Salt Or Table Salt, Rock Salt)
71376, 71386 Sodium chloride (Halite, Common Salt or Table Salt, Rock Salt) CAS number: 7647-14-5 Product Description: Molecular formula: NaCl Appearance: white powder (crystalline) Molecular weight: 58.44 g/mol Density of large crystals: 2.17 g/ml1 Melting Point: 804°C1 Density: 1.186 g/ml (5 M in water)2 2 Solubility: 1 M in H2O, 20°C, complete, clear, colorless 2 pH: 5.0-8.0 (1 M in H2O, 25°C) Store at room temperature Sodium chloride is geologically stable. If kept dry, it will remain a free-flowing solid for years. Traces of magnesium or calcium chloride in commercial sodium chloride adsorb moisture, making it cake. The trace moisture does not harm the material chemically in any way. 71378 BioUltra 71386 BioUltra for molecular biology, 5 M Solution The products are suitable for different applications like purification, precipitation, crystallisation and other applications which require tight control of elemental content. Trace elemental analyses have been performed for all qualities. The molecular biology quality is also tested for absence of nucleases. The Certificate of Analysis provides lot-specific results. Much of the sodium chloride is mined from salts deposited from evaporation of brine of ancient oceans, or recovered from sea water by solar evaporation. Due to the presence of trace hygroscopic minerals, food-grade salt has a small amount of silicate added to prevent caking; as a result, concentrated solutions of "table salt" are usually slightly cloudy in appearance. 71376 and 71386 do not contain any anti-caking agent. Applications: Sodium chloride is a commonly used chemical found in nature and in all body tissue, and is considered an essential nutrient. -
Review of Calculations for Organic Reactions (Assignment #1B)
Review of Calculations for Organic Reactions (Assignment #1b) In your experiments the quantities of many reactants are given in mass or volume, though chemicals react in mole ratios, because it is not possible to measure a quantity in moles easily. You will have to convert mass or volume (mass = volume x density) to moles before beginning an experiment. You will also have to recognize stoichiometric relationships between reactants and products, which is based on mole ratio, in order to be able to calculate the theoretical yield of product you expect to isolate. You will apply the knowledge from this session to complete the theoretical yield calculation in your prelab reports and postlab reports. In this lab you are expected to be able to differentiate between a limiting reagent and excess reagents, solvents and catalysts which are crucial for the reaction to occur and go to completion. A limiting reagent is a reactant that has the lowest number of moles of all reactants in the chemical reaction and once it is completely consumed the reaction terminates. An excess reagent is a reactant that has a higher number of moles and therefore is not used up when a reaction goes to completion. Solvents and catalysts are not involved in the determination of limiting reagent. An example of calculations that you will be expected to perform is shown using the reaction of phenol with nitric acid. Preparation of picric acid requires the nitration of phenol. Given 5.00 grams of phenol and 15.0 mL concentrated nitric acid (15.9 M), one can determine the MAXIMUM theoretical amount of picric acid formed. -
Cool Reaction the Endothermic Reaction Between SCIENTIFIC Barium Hydroxide and Ammonium Thiocyanate
Cool Reaction The Endothermic Reaction Between SCIENTIFIC Barium Hydroxide and Ammonium Thiocyanate Introduction Many reactions produce heat, in fact when people think of chemical reactions, heat production is often expected. However, endothermic reactions, reactions which consume heat, can be just as exciting. One of the most striking examples of this is when the solids barium hydroxide and ammonium thiocyanate are mixed together in a beaker. Materials Ammonium thiocyanate, NH4SCN, 10 g Stirring rod Barium hydroxide octahydrate, Ba(OH)28H2O, 20 g Thermometer graduated to at least –30 °C Erlenmeyer flask, small, with stopper, or a 50-mL beaker Safety Precautions Barium salts are toxic by ingestion. Ammonium thiocyanate is also toxic by ingestion. Use caution when handling the beaker or flask. Use tongs if available. The temperatures involved are cold enough to freeze skin. Ammonia vapor is very irritating to eyes and the respiratory tract. Do not allow students to inhale this gas. 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. Procedure 1. Transfer 20 g of barium hydroxide and 10 g of ammonium thiocyanate to a flask and mix with a glass or plastic stirring rod. 2. In less than two minutes the solids become liquid. A thermometer placed in the mixture shows the temperature falling far below freezing. An ammonia odor is evident to all who are near the flask. 3. Place the flask in a small puddle of water and your students will clearly see just how cool this reaction is; the water will freeze the flask to the counter top. -
Understanding Variation in Partition Coefficient, Kd, Values: Volume II
United States Office of Air and Radiation EPA 402-R-99-004B Environmental Protection August 1999 Agency UNDERSTANDING VARIATION IN PARTITION COEFFICIENT, Kd, VALUES Volume II: Review of Geochemistry and Available Kd Values for Cadmium, Cesium, Chromium, Lead, Plutonium, Radon, Strontium, Thorium, Tritium (3H), and Uranium UNDERSTANDING VARIATION IN PARTITION COEFFICIENT, Kd, VALUES Volume II: Review of Geochemistry and Available Kd Values for Cadmium, Cesium, Chromium, Lead, Plutonium, Radon, Strontium, Thorium, Tritium (3H), and Uranium August 1999 A Cooperative Effort By: Office of Radiation and Indoor Air Office of Solid Waste and Emergency Response U.S. Environmental Protection Agency Washington, DC 20460 Office of Environmental Restoration U.S. Department of Energy Washington, DC 20585 NOTICE The following two-volume report is intended solely as guidance to EPA and other environmental professionals. This document does not constitute rulemaking by the Agency, and cannot be relied on to create a substantive or procedural right enforceable by any party in litigation with the United States. EPA may take action that is at variance with the information, policies, and procedures in this document and may change them at any time without public notice. Reference herein to any specific commercial products, process, or service by trade name, trademark, manufacturer, or otherwise, does not necessarily constitute or imply its endorsement, recommendation, or favoring by the United States Government. ii FOREWORD Understanding the long-term behavior of contaminants in the subsurface is becoming increasingly more important as the nation addresses groundwater contamination. Groundwater contamination is a national concern as about 50 percent of the United States population receives its drinking water from groundwater. -
Writing Total and Net Ionic Equations
WRITING TOTAL AND NET IONIC EQUATIONS http://www.csun.edu/~hcchm001/FreshChemHandouts.html 1. Write the overall equation including the correct designations for the physical state of the substances (s, l, g, aq). Balance this equation. Most of these kinds of equations are double displacement reactions: AX + BY 6 AY + BX 2. For the total ionic equations, write strong electrolytes in solution in the form of aqueous ions. (a) Strong acids. The common strong acids and their aqueous ions are: HI Hydroiodic acid H+-(aq) + I (aq) HBr Hydrobromic acid H+-(aq) + Br (aq) HCl Hydrochloric acid H+-(aq) + Cl (aq) +- HNO33Nitric acid H (aq) + NO (aq) +- HClO44Perchloric acid H (aq) + ClO (aq) +-2 H24SO Sulfuric acid 2 H (aq) + SO4(aq) (b) Strong bases. Strong bases are the hydroxides of the alkali (Group IA) and alkaline earth (Group IIA) metals ions which are sufficiently soluble. The common strong bases and their aqueous ions are: LiOH Lithium hydroxide Li+-(aq) + OH (aq) NaOH Sodium hydroxide Na+-(aq) + OH (aq) KOH Potassium hydroxide K+-(aq) + OH (aq) +2 - Sr(OH)2Strontium hydroxide Sr (aq) + 2 OH (aq) +2 - Ba(OH)2 Barium hydroxide Ba (aq) + 2 OH (aq) (c) Soluble salts. Determinations of the solubility of a salt may be made by reference to SOLUBILITIES OF IONIC COMPOUNDS. Soluble salts are written as their aqueous ions: NaCl(aq) Sodium chloride Na+-(aq) + Cl (aq) +-2 K24SO (aq) Potassium sulfate 2 K (aq) + SO4(aq) +-2 Li23CO (aq) Lithium carbonate 2 Li (aq) + CO3(aq) +-3 Na34PO (aq) Sodium phosphate 3 Na (aq) + PO4(aq) +-2 (NH42) SO4(aq) Ammonium sulfate 2 NH4(aq) + SO4 (aq) 3. -
Acetal (POM) Chemical Compatibility Chart From
ver 31-Mar-2020 Acetal (POM) Chemical Compatibility Chart Chemical Chemical Acetaldehyde A Ammonium Acetate C Acetamide A Ammonium Bifluoride D Acetate Solvents A Ammonium Carbonate D Acetic Acid D Ammonium Caseinate D Acetic Acid, 20% C Ammonium Chloride, 10% B Acetic Acid, 80% D Ammonium Hydroxide D Acetic Acid, Glacial D Ammonium Nitrate, 10% A Acetic Anhydride D Ammonium Oxalate B Acetone A Ammonium Persulfate D Acetyl Chloride, dry D Ammonium Phosphate, Dibasic B Acetylene A Ammonium Phosphate, Monobasic B Alcohols: Amyl A Ammonium Phosphate, Tribasic B Alcohols: Benzyl A Ammonium Sulfate B Alcohols: Butyl A Ammonium Sulfite D Alcohols: Diacetone A Ammonium Thiosulfate B Alcohols: Ethyl A Amyl Acetate B Alcohols: Hexyl A Amyl Alcohol A Alcohols: Isobutyl A Amyl Chloride A Alcohols: Isopropyl A Aniline A Alcohols: Methyl A Aniline Oil D Alcohols: Octyl A Anise Oil D Alcohols: Propyl (1-Propanol) A Antifreeze D Aluminum chloride, 20% C Aqua Regia (80% HCl, 20% HNO3) D Aluminum Fluoride C Aromatic Hydrocarbons A Aluminum Hydroxide A Arsenic Acid D Aluminum Nitrate B Asphalt B Aluminum Potassium Sulfate, 10% C Barium Carbonate A Aluminum Potassium Sulfate, 100% C Barium Chloride A Aluminum Sulfate, 10% B Barium Cyanide B Alums C Barium Hydroxide D Amines D Barium Nitrate B Ammonia, 10% (Ammonium Hydroxide) C Barium Sulfate B Ammonia, 10% D Barium Sulfide A Ammonia, anhydrous D Bay Oil D Ammonia, liquid D Beer A Ammonia Nitrate C Beet Sugar Liquids B Key to General Chemical Resistance – All data is based on ambient or room temperature conditions, about 64°F (18°C) to 73°F (23°C) A = Excellent C = Fair - Moderate Effect, not recommended B= Good - Minor Effect, slight corrosion or discoloration D = Severe Effect, not recommended for ANY use It is the sole responsibility of the system designer and user to select products suitable for their specific application requirements and to ensure proper installation, operation, and maintenance of these products. -
Magnesium Sulfate
MAGNESIUM SULFATE Prepared at the 68th JECFA (2007), published in FAO JECFA Monographs 4 (2007), superseding the specifications prepared at the 63rd JECFA (2004) and published the Combined Compendium of Food Additive Specifications, FAO JECFA Monographs 1 (2005). An ADI “not specified” was established at the 68th JECFA (2007). SYNONYMS Epsom salt (heptahydrate); INS No.518 DEFINITION Magnesium sulfate occurs naturally in sea water, mineral springs and in minerals such as kieserite and epsomite. It is recovered from them or by reacting sulfuric acid and magnesium oxide. It is produced with one or seven molecules of water of hydration or in a dried form containing the equivalent of between 2 and 3 waters of hydration. Chemical names Magnesium sulfate C.A.S. number Monohydrate: 14168-73-1 Heptahydrate: 10034-99-8 Dried: 15244-36-7 Chemical formula Monohydrate: MgSO4.H2O Heptahydrate: MgSO4.7H2O Dried: MgSO4.xH2O, where x is the average hydration value (between 2 and 3) Formula weight Monohydrate: 138.38 Heptahydrate: 246.47 Assay Not less than 99.0 % and not more than 100.5% on the ignited basis DESCRIPTION Colourless crystals, granular crystalline powder or white powder. Crystals effloresce in warm, dry air. FUNCTIONAL USES Nutrient; flavour enhancer; firming agent; and processing aid (fermentation aid in the production of beer and malt beverages) CHARACTERISTICS IDENTIFICATION Solubility (Vol. 4) Freely soluble in water, very soluble in boiling water, and sparingly soluble in ethanol. Test for magnesium (Vol. 4) Passes test Test for sulfate (Vol. 4) Passes test PURITY Loss on ignition (Vol. 4) Monohydrate: between 13.0 and 16.0 %, Heptahydrate: between 40.0 and 52.0 %, Dried: between 22.0 and 32.0 % (105°, 2h, then 400° to constant weight) pH (Vol. -
Self-Diffusion of Sodium, Chloride and Iodide Ions in Methanol-Water Mixture
Self-Diffusion of Sodium, Chloride and Iodide Ions in Methanol-Water Mixture E. Hawlicka* Institute of Applied Radiation Chemistry, Technical University, Wroblewskiego 15, 93-590, Lodz, Poland Z. Naturforsch. 41 a, 939-943 (1986); received April 25, 1986 The self-diffusion coefficients of Na+, C l- and I- in methanol-water solutions at 35 ± 0.01 °C have been measured in their dependence on the salt molarity in the range 1 • 10-4— 1 • 10-2 mol dm -3. The ionic self-diffusion coefficients in infinitely diluted solutions have been computed. The influence of the solvent composition on the solvation of the ions is discussed. A preferential hydration of Na+, Cl - and I “ ions in water-methanol mixtures has been found. In spite of the great interest in the porperties of aqueous solution with a Nal(Tl) scintillation crystal water-organic solvent electrolyte solutions, data on of the well-type (2 x 2"). the ionic mobilities in such systems are scarce. For the self-diffusion measurements the open-end Usually the ionic mobility is calculated from the capillary method was used. The details of the equivalent conductance and the transference num experimental procedure have been described in [6], ber. Ionic transference numbers have been reported The labelling of the sodium ions with 22Na or for water and 17 organic solvents [1], but only for a 24Na and the iodide ions with i25I or 1311, respective few water-organic solvents mixtures. ly, did not make any difference in the results. Similar information can be obtained from the ionic self-diffusion coefficients, which have been reported for a few water-organic solvent systems Results [2-5], The aim of the present work was to determine the All self-diffusion experiments have been carried self-diffusion coefficients of sodium, chloride and out at 25.0 ± 0.05 °C. -
Mechanosynthesis of Magnesium and Calcium Salt?Urea Ionic Cocrystal
Letter pubs.acs.org/journal/ascecg Mechanosynthesis of Magnesium and Calcium Salt−Urea Ionic Cocrystal Fertilizer Materials for Improved Nitrogen Management Kenneth Honer, Eren Kalfaoglu, Carlos Pico, Jane McCann, and Jonas Baltrusaitis* Department of Chemical and Biomolecular Engineering, Lehigh University, B336 Iacocca Hall, 111 Research Drive, Bethlehem, Pennsylvania 18015, United States *S Supporting Information ABSTRACT: Only 47% of the total fertilizer nitrogen applied to the environment is taken up by the plants whereas approximately 40% of the total fertilizer nitrogen lost to the environment reverts back into unreactive atmospheric dinitrogen that greatly affects the global nitrogen cycle including increased energy consumption for NH3 synthesis, as well as accumulation of nitrates in drinking water. In this letter, we provide a mechanochemical method of inorganic magnesium and calcium salt−urea ionic cocrystal synthesis to obtain enhanced stability nitrogen fertilizers. The solvent-free mechanochemical synthesis presented can result in a greater manufacturing process sustainability by reducing or eliminating the need for solution handling and evaporation. NH3 emission testing suggests that urea ionic cocrystals are capable of decreasing NH3 emissions to the environment when compared to pure urea, thus providing implications for a sustainable global solution to the management of the nitrogen cycle. KEYWORDS: Fertilizers, Nitrogen, urea, Mechanochemistry, Cocrystal, pXRD, NH3 Emissions, Stability ■ INTRODUCTION ammonia as opposed to up to 61.1% of soil treated with urea 7,8 fi only, which suggests that major improvements to the global Atmospheric dinitrogen, N2, xation to synthesize ammonia, 9,10 ’ 1 nitrogen cycle are achievable. Additionally, urea molecular NH3, consumes more than 1% of the world s primary energy. -
The Importance of Minerals in the Long Term Health of Humans Philip H
The Importance of Minerals in the Long Term Health of Humans Philip H. Merrell, PhD Technical Market Manager, Jost Chemical Co. Calcium 20 Ca 40.078 Copper 29 Cu 63.546 Iron Magnesium 26 12 Fe Mg 55.845 24.305 Manganese Zinc 25 30 Mn Zn 55.938 65.380 Table of Contents Introduction, Discussion and General Information ..................................1 Calcium ......................................................................................................3 Copper .......................................................................................................7 Iron ...........................................................................................................10 Magnesium ..............................................................................................13 Manganese ..............................................................................................16 Zinc ..........................................................................................................19 Introduction Daily intakes of several minerals are necessary for the continued basic functioning of the human body. The minerals, Calcium (Ca), Iron (Fe), Copper (Cu), Magnesium (Mg), Manganese (Mn), and Zinc (Zn) are known to be necessary for proper function and growth of the many systems in the human body and thus contribute to the overall health of the individual. There are several other trace minerals requirements. Minimum (and in some cases maximum) daily amounts for each of these minerals have been established by the Institute of -
A Fiber Optic Ammonia Sensor Using a Universal Ph Indicator
Sensors 2014, 14, 4060-4073; doi:10.3390/s140304060 OPEN ACCESS sensors ISSN 1424-8220 www.mdpi.com/journal/sensors Article A Fiber Optic Ammonia Sensor Using a Universal pH Indicator Adolfo J. Rodríguez 1,*, Carlos R. Zamarreño 2, Ignacio R. Matías 2, Francisco. J. Arregui 2, Rene F. Domínguez Cruz 1 and Daniel. A. May-Arrioja 1 1 Fiber and Integrated Optics Laboratory, Electronics Engineering Department, UAM Reynosa Rodhe, Universidad Autónoma de Tamaulipas, Carr. Reynosa-San Fernando S/N, Reynosa, Tamaulipas 88779, Mexico; E-Mails: [email protected] (R.F.D.C.); [email protected] (D.A.M.-A.) 2 Departamento de Ingeniería Eléctrica y Electrónica, Universidad Pública de Navarra, Edif. Los Tejos, Campus Arrosadia, Pamplona España 31006, Spain; E-Mails: [email protected] (C.R.Z.); [email protected] (I.R.M.); [email protected] (F.J.A.) * Author to whom correspondence should be addressed; E-Mail: [email protected]; Tel.: +52-899-9213300 (ext. 8315); Fax: +52-899-921-3300 (ext. 8050). Received: 27 December 2013; in revised form: 12 February 2014 / Accepted: 18 February 2014 / Published: 27 February 2014 Abstract: A universal pH indicator is used to fabricate a fiber optic ammonia sensor. The advantage of this pH indicator is that it exhibits sensitivity to ammonia over a broad wavelength range. This provides a differential response, with a valley around 500 nm and a peak around 650 nm, which allows us to perform ratiometric measurements. The ratiometric measurements provide not only an enhanced signal, but can also eliminate any external disturbance due to humidity or temperature fluctuations.