SODIUM ACETATE Injection, USP 2 Meq/Ml Rx Only Pharmacy Bulk Package
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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. -
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. -
Salt Effect on Vapor-Liquid Equilibria for Acetone-Water System'
SALT EFFECT ON VAPOR-LIQUID EQUILIBRIA FOR ACETONE-WATER SYSTEM' E1ZO SADA, TOSHIO OHNO** AND SHIGEHARU KITO Department of Chemical Engineering, Nagoya University, Nagoya, Japan Vapor-liquid equilibrium data of acetone-water system saturated with sodium chloride, potassium chloride, sodium nitrate, and calcium chloride dihydrate are determined under atmospheric pressure. These vapor-liquid equilibrium data are correlated by a method which gives approximately the behavior of salt in the liquid. The standard deviation of correlated results is 2.32%. To carry out this correlation, the vapor pressures of aqueous solutions saturated with salts are also determined. Investigations concerned with the effect of salt the portion between Cx and Hj is brought to the addition on the vapor-liquid equilibria of binary- vapor pressure of sample solution. Whenthe system systems are of theoretical and industrial importance, attains equilibrium (about one hour is needed), and not a little knowledge of vapor-liquid equilibrium the heights of Hl5 H2, and H3 aremeasured, and the data in this field is already available2}. However, vapor pressure is calculated from the following most investigations are limited to presentation of equation. P '---(Hi-H,W+(Hg-H,W experimental data with no attempt to develop a cor- LO -% r relation. Among these, only a few correlations />*" (1) are proposed, for example, by Johnson and Furter5), As the density of sample solution is usually an order and Hashitani and Hirata3). In this paper, the vapor-liquid equilibrium data of magnitude lower than for mercury, it does not decrease the accuracy of measurementto use the for the acetone-water system saturated with each density of pure water at measuring temperature in of four kinds of salt, i.e. -
Electrolytic Study of Basic Beryllium Acetate in Carbon Disulphide at 303K, 308K, 313K
IARJSET ISSN (Online) 2393-8021 ISSN (Print) 2394-1588 International Advanced Research Journal in Science, Engineering and Technology Vol. 7, Issue 11, November 2020 DOI 10.17148/IARJSET.2020.71106 Electrolytic Study of Basic Beryllium Acetate in Carbon disulphide at 303K, 308K, 313K Rajeev Kumar Sharma1, Renu Singhal2 Assistant Professor, Department of Chemistry, D.S. College, Aligarh, U.P. (India)1 Associate Professor, Department of Chemistry, D.S. College, Aligarh, U.P. (India)2 Abstract: The electrolytic study of Basic Beryllium Acetate (B.B.A.) in carbon disulphide were reported at 303K, 308K, 313K, the solute solvent interaction have been carried out by computing various Physico-chemical Acoustic Parameters [Apparent Molal adiabatic compressibility (k), Isentropic compressibility (S), Intermolecular free length (Lf), Specific Acoustic Impedance (Z), Relative Association and Solvation Number (Sn)], these parameters have been evaluated by using ultrasonic velocity, density, viscosity data. The results of these parameters indicates the strength of molecular interaction. Keywords: Molecular Interaction, Electrolytic, viscous behavior of Basic Beryllium acetate. I. INTRODUCTION The Isentropic compressibility of dilute aqueous solution of electrolytes decreases with increasing conc. indicating a strong interaction of the dissolved ion with the alkanols1-7, the non-aqueous solution of electrolytes have drawn the attention of same workers.7-9 Now, we are reporting a study of Ultrasound velocity, density and viscosity measurement at 300C, 350C, 400C have 8 been used to calculate isentropic compressibility (s), Intermolecular Free Lenght (Lf) , Specific Acoustic Impedance 9 10 (Z) , Molar sound velocity (R), Relative association (RA) , Apparent molal adiabatic compressibility (k), Wada 11 0 0 constant (B), Shear’s relaxation time (s) and Solvation numbers (Sn) of B.B.A. -
Action of Ammonium Chloride Upon Silicates
Bulletin No. 207 Series E, Chemistry and Physics, 36 DEPARTMENT OF TEiE INTERIOR UNITED STATES GEOLOGICAL SURVEY CHARLES D. WALCOTT, DIRECTOR THE ACTION OF AMMONIUM CHLORIDE UPON SILICATES BY AND GKKOKG-IE Srj::ir, WASHINGTON GOVERNMEN.T PllINTING OFFICE 1902 CONTENTS. Page. Introductory statement......--..-..---.--.------.--.-..--.-.-----------. 7 Analcite-.....-.-.-.--.-.....-.--.'--------....--.-.--..._.-.---.-...---.--. 8 Leucite .....................'.................-....................^-..... 16 The constitution of analcite and leucite.........-..--.-..--...--.---------. 17 Pollucite---. ............................................................ 21 Natrolite--------------------------..-..-----------------.------ --------- 22 Scolecite ................,.:............-.....-.................--.--.... 24 Prehnite .....--.-............--.------------------------------ --------- 25 The trisilicic acids-.--.-.--..---..........-._-----...-.........-...----.- 26 Stilbite.............-..................-....-.-.-----...--.---.......... 29 Henlandite .......... .......................---.-..-.-..-...-----.--..--.. 81 Chabazite............................................................... 32 Thoinsonite...-.-.-..-...._.................---...-.-.-.----..-----..--.. 34 Lanmontite -.-.------.-..-------------.-..-.-..-.-------.-.-----........ 35 Pectolite ......:......... ......................................'.......;.., 36 Wollastonite ....'............................ ................:........... 39 Apophyllite. _.--._..._-....__.....:......___-------------....----..-...._ -
Methanogenesis Rates in Acetate and Nitrate Amended Anoxic Slurries
Methanogenesis rates in acetate and nitrate amended anoxic slurries BIOS 35502: Practicum in Environmental Field Biology Patrick Revord Advisor: William West 2011 Abstract With increasing urbanization and land use changes, pollution of lakes and wetland ecosystems is imminent. Any influx of nutrients, anthropogenic or natural, can have dramatic effects on lake gas production and flux. However, the net effect of simultaneous increase of both acetate and nitrate is unknown. Methane (CH4) production was measured in anoxic sediment and water slurries amended with ammonium nitrate (NH4NO3), which has been shown to inhibit methanogenesis, and sodium acetate (CH3COONa or NaOAc), which is known to increase methanogenesis. The addition of acetate significantly increased the methanogenesis rate, but the nitrate amendment had no significant effect. The simultaneous amendment of both acetate and nitrate showed no significant increase in CH4 compared to the control, indicating that the presence of nitrate may have reduced the effect of acetate amendment. Introduction Methane, a greenhouse gas associated with global warming, continues to increase in concentration in our atmosphere. Global yearly flux of methane into the atmosphere is 566 teragrams of CH4 per year, which is more than double pre-industrial yearly flux (Solomon et al. 2007). Increasing urbanization and land-use changes contribute significantly to increased gas levels (Anderson et al. 2010, Vitousek 1994). Nutrients travel from anthropogenic sources such as wastewater treatment facilities, landfills, and agricultural plots into nearby lakes, rivers, and wetlands, causing increased primary productivity in a process known as eutrophication (Vitousek et al. 1997). The increased nutrients and productivity lead to toxic algal blooms that create products such as acetate, H2, and CO2; a nutrient-rich anoxic environment suitable for anaerobic bacteria to produce unnaturally high levels of methane and other greenhouse gases (Davis and Koop 2006, West unpublished data). -
Isoamyl Acetate
SUMMARY OF DATA FOR CHEMICAL SELECTION Isoamyl Acetate CAS No. 123-92-2 Prepared for NTP by Technical Resources International, Inc Prepared on 11/94 Under NCI Contract No. N01-CP-56019 Table of Contents I. Chemical Identification II. Exposure Information Table 1. Levels of isoamyl acetate reported in foods III. Evidence for Possible Carcinogenic Activity Appendix A: Structural Analogs of Isoamyl Acetate IV. References SUMMARY OF DATA FOR CHEMICAL SELECTION CHEMICAL IDENTIFICATION CAS Registry No.: 123-92-2 Chem. Abstr. Name: 1-Butanol, 3-methyl-, acetate Synonyms: Acetic acid 3-methylbutyl ester; acetic acid, isopentyl ester; AI3-00576; banana oil; isoamyl ethanoate; isopentyl acetate; isopentyl alcohol, acetate; pear oil; 3-methyl-1-butanol acetate; 3-methyl-1-butyl acetate; 3-methylbutyl acetate; 3-methylbutyl ethanoate; i-amyl acetate Structure: Molecular Formula and Molecular Weight: C7H14O2 Mol. Wt.: 130.18 Chemical and Physical Properties: Description: Colorless, flammable liquid with a banana-like odor (ACGIH, 1993). Boiling Point: 142°C (Lide, 1993) Melting Point: -78.5°C (Mark, et al, 1984; Lide, 1993) Solubility: Soluble in water (2000 mg/L at 25°C) (Howard, 1990); soluble in ethanol, diethyl ether, and acetone (Lide, 1993). Vapor 4.5 mm Hg at 20°C (Howard, 1990) Pressure: Refractive 1.4003 (Lide, 1993) Index: Flash Point: closed cup, 33°C; open cup, 38°:C (Budavari, 1989) Density: 0.876 (Lewis, 1993) Reactivity: Thermal decomposition of isoamyl acetate may produce acrid fumes. Contact with strong oxidizing agents, strong acids, and alkaline materials should be avoided (Haarmann & Reimer Corp., 1994). Hazardous decomposition products of isoamyl acetate include CO and CO2 (AESAR/Alfa, 1994) Log 2.13 (Howard, 1990) P(octanol/water partition coefficient): Technical Isoamyl acetate is commercially available as both a natural and synthetic product with a purity Products and range of 95-99+%. -
Bond Distances and Bond Orders in Binuclear Metal Complexes of the First Row Transition Metals Titanium Through Zinc
Metal-Metal (MM) Bond Distances and Bond Orders in Binuclear Metal Complexes of the First Row Transition Metals Titanium Through Zinc Richard H. Duncan Lyngdoh*,a, Henry F. Schaefer III*,b and R. Bruce King*,b a Department of Chemistry, North-Eastern Hill University, Shillong 793022, India B Centre for Computational Quantum Chemistry, University of Georgia, Athens GA 30602 ABSTRACT: This survey of metal-metal (MM) bond distances in binuclear complexes of the first row 3d-block elements reviews experimental and computational research on a wide range of such systems. The metals surveyed are titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, and zinc, representing the only comprehensive presentation of such results to date. Factors impacting MM bond lengths that are discussed here include (a) n+ the formal MM bond order, (b) size of the metal ion present in the bimetallic core (M2) , (c) the metal oxidation state, (d) effects of ligand basicity, coordination mode and number, and (e) steric effects of bulky ligands. Correlations between experimental and computational findings are examined wherever possible, often yielding good agreement for MM bond lengths. The formal bond order provides a key basis for assessing experimental and computationally derived MM bond lengths. The effects of change in the metal upon MM bond length ranges in binuclear complexes suggest trends for single, double, triple, and quadruple MM bonds which are related to the available information on metal atomic radii. It emerges that while specific factors for a limited range of complexes are found to have their expected impact in many cases, the assessment of the net effect of these factors is challenging. -
NMR Chemical Shifts of Common Laboratory Solvents As Trace Impurities
7512 J. Org. Chem. 1997, 62, 7512-7515 NMR Chemical Shifts of Common Laboratory Solvents as Trace Impurities Hugo E. Gottlieb,* Vadim Kotlyar, and Abraham Nudelman* Department of Chemistry, Bar-Ilan University, Ramat-Gan 52900, Israel Received June 27, 1997 In the course of the routine use of NMR as an aid for organic chemistry, a day-to-day problem is the identifica- tion of signals deriving from common contaminants (water, solvents, stabilizers, oils) in less-than-analyti- cally-pure samples. This data may be available in the literature, but the time involved in searching for it may be considerable. Another issue is the concentration dependence of chemical shifts (especially 1H); results obtained two or three decades ago usually refer to much Figure 1. Chemical shift of HDO as a function of tempera- more concentrated samples, and run at lower magnetic ture. fields, than today’s practice. 1 13 We therefore decided to collect H and C chemical dependent (vide infra). Also, any potential hydrogen- shifts of what are, in our experience, the most popular bond acceptor will tend to shift the water signal down- “extra peaks” in a variety of commonly used NMR field; this is particularly true for nonpolar solvents. In solvents, in the hope that this will be of assistance to contrast, in e.g. DMSO the water is already strongly the practicing chemist. hydrogen-bonded to the solvent, and solutes have only a negligible effect on its chemical shift. This is also true Experimental Section for D2O; the chemical shift of the residual HDO is very NMR spectra were taken in a Bruker DPX-300 instrument temperature-dependent (vide infra) but, maybe counter- (300.1 and 75.5 MHz for 1H and 13C, respectively). -
A New Take on the Aspirin Synthesis Lab: a Multi-Step Organic Synthesis Laboratory for High School Students
A new take on the aspirin synthesis lab: A multi-step organic synthesis laboratory for high school students Michael P. Kowalski Rationale The use of the extracts of various plants for the treatment of pain and fever goes back several centuries. A tea made from the leaves or bark of Willow ( Saliaceae ) was found to be especially effective. By the late 19th Century, the active ingredient in these plant extracts, salicylic acid, had been identified. In 1874, the process for the commercial production of salicylic acid was perfected. The use of salicylic acid as an analgesic became widespread. However, side effects, such as gastric bleeding, made long term use of the drug impossible for many patients. In 1895, Felix Hoffman of the Fredrick Bayer Company found a method to acetylate salicylic acid, producing acetyl salicylic acid. This derivative was found to be as effective as salicylic acid as an analgesic but did not have the side effects associated with salicylic acid. The new drug was named “aspirin”, a name inspired by Saint Aspirinius, the patron saint of headaches. The introduction of aspirin marks the beginning of the modern pharmaceutical industry. The mechanism as to how aspirin alleviates pain was not elucidated until the 1970’s, when it was found that aspirin inhibits COX 1 and COX 2, enzymes that catalyze the formation of prostaglandins, substances that cause inflammation (1). The synthesis of aspirin, acetylsalicylic acid, is a standard first year organic chemistry laboratory activity at the college level. In most protocols, salicylic acid is reacted with acetic anhydride producing aspirin and acetic acid by acid catalysis: O OH O O OH O O H2SO4 O CH3 + H3C OH OH H C O CH + 3 3 O The reaction is refluxed for 30 minutes, and then cooled. -
Experiment 1: Synthesis of Acetamides from Aniline and Substituted Anilines
Chem 216 S11 Notes - Dr. Masato Koreeda Date: May 3, 2011 Topic: __Experiment 1____ page 1 of 2. Experiment 1: Synthesis of Acetamides from Aniline and Substituted Anilines Many of the acetylated [CH3–C(=O)-] derivatives of aromatic amines (aka anilines) and phenols are pharmacologically important compounds. Some of these exhibit distinct analgesic activity. Two of the most representative examples are: H HO O N CH3 O CH3 O HO O acetaminophen (Tylenol) acetylsalicylic acid (Aspirin) ======================================================================= The reaction to be carried out in this experiment is: Acetylation of aniline δ- H3C δ+ O acetic O O anhydride H N CH3 N H (electrophile) HO O CH3 + H O CH3 acetanilide acetic acid aniline (nucleophile) Both aniline and acetic anhydride are somewhat viscous liquids. So, simply mixing them together does not result in the efficient formation of acetanilide. Therefore, a solvent (in this case water) is used to dissolve and evenly disperse two reactants in it. R R R Note: O + N R" N R" N CH R' R' R' 3 CH3 - O O O acetyl group amide The amide N is usually not nucleophilic acetamide because of a significant contribution of this resonance form. Reaction mechanism: δ- H H3C H H H3C δ+ O H N O H O N O CH3 O O N + O O H CH3 O CH3 CH3 pKa ~ -5 3 O CH3 tetrahedral (sp ) intermediate B (including ) O H N CH3 O acetanilide Chem 216 S11 Notes - Dr. Masato Koreeda Date: May 3, 2011 Topic: __Experiment 1____ page 2 of 2. Additional comments on the reaction mechanism: 1. -
Aspirin. an Ab Initio Quantum-Mechanical Study of Conformational Preferences and of Neighboring Group Interactions
J. Org. Chem. 2001, 66, 771-779 771 Aspirin. An ab Initio Quantum-Mechanical Study of Conformational Preferences and of Neighboring Group Interactions Rainer Glaser Department of Chemistry, University of MissourisColumbia, Columbia, Missouri 65211 [email protected] Received August 15, 2000 The potential energy surface of acetylsalicylic acid, aspirin, has been explored at the RHF/6-31G* and B3LYP/6-31G* levels, and single-point calculations were performed at levels up to B3LYP/ 6-311G**//B3LYP/6-31G*. All conformational isomers have been located, the thermochemical functions have been computed, and relative energies and free enthalpies were determined. The conformational space of aspirin is spanned by three internal coordinates, and these are the carboxylic acid C-O conformation (s-trans preferred by about 7 kcal/mol), the C-COOH conformation (Z preferred unless there are H-bonding opportunities), and the ester C-O conformation (s-trans preferred by about 4 kcal/mol). There are nine aspirin isomers since one of the conformers realizes hydrogen-bonding structure isomerism as well. Neighboring group interactions are discussed with reference to the intrinsic properties of benzoic acid and phenyl acetate. The intrinsic conformational preference energies for benzoic acid and phenyl acetate are not additive. The acid s-trans preference energies differ by as much as 9 kcal/mol depending on the Ph-COOH and ester conformations. Similarly, the E-preference energies about the Ph-COOH bond vary by as much as 6 kcal/mol depending on the ester conformation. The structural discussion suggests an overall ortho repulsion between the functional groups in all aspirin isomers including the intramolecularly hydrogen- bonded isomers.