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Synthesis of Solids
Published in Elaine A. Moore, Lesley E. Smart, Solid State Chemistry, 2020
Elaine A. Moore, Lesley E. Smart
The second method was precursor synthesis. The starting materials are barium chloride, titanium butoxide (Ti(OC4H9)4), and oxalic acid. Overall, this process produces more carbon dioxide per molecule of barium salt and so more waste product than the first method (Principle 1). A lower percentage of the starting atoms are found in the product (Principle 2). Barium chloride is also toxic if swallowed and harmful if inhaled. Titanium butoxide is an irritant for eyes, skin, and respiratory and digestive tracts (Principle 3). This process requires a solvent, but the solvent is water (Principle 5). The temperature used is not as high as that for the first method (Principle 6).
Inorganic Chemicals in Drinking Water
Published in Joseph Cotruvo, Drinking Water Quality and Contaminants Guidebook, 2019
Barium is an alkaline earth metal in the same category as magnesium, calcium, strontium, and radium, so it has very similar chemical properties. It forms Ba2+ salts with many anions, and many of the salts such as barium sulfate and barium carbonate have low water solubility. However, barium chloride is 37.4 percent water soluble at 25°C.
List of Chemical Substances
Published in T.S.S. Dikshith, and Safety, 2016
Exposures to barium chloride cause sore throat, coughing, and labored breathing, and become harmful and fatal if swallowed or inhaled. Prolonged exposures cause irritation to the skin, eyes, and respiratory tract, and involve the heart, respiratory system, and the CNS. An accidental ingestion of barium chloride causes severe gastroenteritis, abdominal pain, vomiting, diarrhea, tremors, faintness, paralysis of arms and legs, and a slow or irregular heartbeat. In severe cases, barium chloride may cause collapse and death from respiratory failure.
Effect of alcohol on the crystallization process of MgCO3·3H2O: an experimental and molecular dynamics simulation study
Published in Energy Sources, Part A: Recovery, Utilization, and Environmental Effects, 2020
Xingfu Song, Chaoyan Dai, Guilan Chen, Chunhua Dong, Jianguo Yu
Alcohol precipitation has been extensively applied for crystallization (Guan et al. 2011; Jones, Piana, and Gale 2008; Kowacz, Putnis, and Putnis 2007; Sand et al. 2012). In general, with the presence of alcohol (C1~ C3), the solubility of inorganic salts decreases while the rate of crystallization increases. Jones, Piana, and Gale (2008) have studied the effect of methanol on the solubility of barium sulfate and the reactive crystallization rate between barium chloride and sodium sulfate. With the increase of methanol mass fraction, the solubility of barium sulfate becomes smaller and crystallization induction period between barium chloride and sodium sulfate becomes shorter. Liu et al. (2014) have studied the crystallization thermodynamics and nucleation kinetics of Disodium 5-Inosinate (IMP) in water-ethanol system and obtained the similar result that alcohol can significantly increase the nucleation rate of IMP. Hence, alcohol has a significant effect on the crystallization kinetics and thermodynamics.
Chemical, biological, and trophic status of temperate lakes can be strongly influenced by the presence of late-glacial marine sediments
Published in Lake and Reservoir Management, 2020
Stephen A. Norton, Aria Amirbahman, Linda Bacon, Holly A. Ewing, Martin Novak, Andrea Nurse, Michael Retelle, J. Curt Stager, Martin Yates
Total S from sediment samples was extracted as sulfate (SO42-) by the Eschka procedure (ASTM D3177-02 2007) by thoroughly mixing a sample with the Eschka mixture (2 parts calcined magnesium oxide and 1 part anhydrous sodium carbonate). The mixture was ashed in a muffle furnace at 800 C. The ashed sample was leached with hot water, filtered, and the S was precipitated as barium sulfate with a 10% barium chloride solution. The precipitate was filtered, dried, and combusted at 800 C to constant weight to calculate the amount of precipitated S. The barium sulfate was mixed with silica, vanadium pentoxide, and copper, decomposed in vacuum at 1050 C (Yanagisawa and Sakai 1983), and collected as sulfur dioxide for determination of δ34S (equation 1). The 34S/32S ratios were determined on a Delta V isotope ratio mass spectrometer (ThermoFisher Scientific). The overall reproducibility of the δ34S measurement was 0.3‰, which includes the uncertainty of measurement (external reproducibility is ∼0.1‰) and the uncertainty of the preparation method (∼0.2‰). The detection limit for total S, and thus determination of δ34S, was 0.01%.
Surfactant mediated synthesis of barium sulfate, strontium sulfate and barium-strontium sulfate nanoparticles
Published in Inorganic and Nano-Metal Chemistry, 2019
Prutviraj K., Thimmasandra Narayan Ramesh
Figure 1 shows the pXRD patterns of the barium sulfate/strontium sulfate/barium-strontium sulfate samples obtained by the addition of barium chloride/strontium chloride/equimolar mixture of barium-strontium sulfate solution to sodium sulfate solution at 28–30 °C. X-ray powder diffraction patterns of barium sulfate/strontium sulfate/barium-strontium sulfate samples obtained could be indexed to orthorhombic crystal system and the lattice parameters are given in Table 1. The pXRD pattern of all the samples exhibit strong and sharp diffraction peaks indicating better crystallinity. The reflections in the pXRD patterns of barium sulfate, strontium sulfate and Ba0.5Sr0.5–SO4 sample could be indexed to single phase in orthorhombic system. Barium sulfate, strontium sulfate and Ba0.5Sr0.5–SO4 samples match with JCPDS cards (i) 24–1035 (ii) 05–0593 and (iii) 39–1468, respectively. The lattice parameters, space groups and cell volumes of barium sulfate/strontium sulfate/barium-strontium sulfate obtained by precipitation methods are given in Table 1. The cell volume of Ba0.5Sr0.5–SO4 is 326.80 Ǻ3 is an intermediate value compared to BaSO4 and SrSO4 indicating that Ba0.5Sr0.5–SO4 forms a solid solution.