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Academic literature on the topic 'Thiosulfate'

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Published: 4 June 2021
Last updated: 20 February 2023

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Journal articles on the topic "Thiosulfate"

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Munawarah, Fitriatul, Budy Wiryono, and Muliatiningsih Muliatiningsih. "PERANAN FITOREMEDIASI PADA LAHAN BEKAS TAMBANG EMAS DI KECAMATAN JONGGAT KABUPATEN LOMBOK TENGAH." Jurnal Agrotek Ummat 4, no. 2 (August 20, 2017): 73. http://dx.doi.org/10.31764/agrotek.v4i2.982.

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Abstrak: Penelitian ini bertujuan untuk mengetahui peranan Amonium thiosulfat dan Sodium thiosulfat sebagai bahan pengkhelat pada proses Fitoremediasi dengan menggunakan tanaman Paspalum conjugatum (Rumput Paitan). Metode yang digunakan dalam penelitian ini adalah metode eksperimental yang dilakukan di lapangan pada bulan Mei sampai Juli 2017. Penelitian dirancang menggunakan Rancangan Acak Kelompok (RAK) dengan variasi perlakuan: PAT1 = pemberian Amonium thiosulfat sebanyak 1 gr, PAT2 = pemberian Amonium thiosulfat sebanyak 2 gr, PST1 = pemberian Sodium thiosulfat sebanyak 1 gr, PST2 = pemberia Sodium thiosulfat sebanyak 2 gr. Setiap perlakuan diulang sebanyak 3 kali sehingga diperoleh 12 unit percobaan. Parameter yang diamati dalam penelitian ini meliputi konsentrasi Hg pada tanaman, berat berangkasan, dan tinggi tanaman. Data hasil pengamatan dianalisis dengan menggunakan standar deviasi mean. Bahan pengkhelat Amonium thiosulfat lebih tinggi mengikat Hg di bandingkan dengan Sodium thiosulfat. Konsentrasi kadar total Hg tertinggi terdapat pada perlakuan Amonium thiosulfat dosis 2 gr/15 liter sebesar 1137,87 ppm. Semakin tinggi konsentrasi Hg pada tanah mengakibatkan pertumbuhan tanaman terhambat.Abstract: Ammonium thiosulfate and Sodium thiosulfate as chelating material in the Phytoremediation process using Paspalum conjugatum (Paitan Grass). The method used in this study is an experimental method conducted in the field from May to July 2017. The study was designed using Randomized Block Design (RBD) with a variety of treatments: PAT1 = giving 1 gr Ammonium thiosulfate, PAT2 = giving 2 gr Ammonium thiosulfate giving, PST1 = giving 1 gr Sodium thiosulfate, PST2 = giving 2 grams of Sodium thiosulfate. Each treatment was repeated three times to obtain 12 experimental units. The parameters observed in this study include the concentration of Hg in plants, the weight of stature, and plant height. Observation data were analyzed using the standard deviation of the mean. The chelating agent Ammonium thiosulfate is higher in binding to Hg compared to Sodium thiosulfate. The highest concentration of total Hg was found in Ammonium thiosulfate treatment with a dose of 2 gr / 15 liters of 1137.87 ppm. The higher the concentration of Hg on the soil resulted in stunted plant growth.
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González Lara, Juan, Francisco Cardona, Antonio Vallmajor, and Montserrat Cadevall. "Oxidation of Thiosulfate with Oxygen Using Copper (II) as a Catalyst." Metals 9, no. 4 (March 28, 2019): 387. http://dx.doi.org/10.3390/met9040387.

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Thiosulfate effluents are generated in the photography and radiography industrial sectors, and in a plant in which thiosulfates are used to recover the gold and silver contained in ores. Similar effluents also containing thiosulfate are those generated from the petrochemical, pharmaceutical and pigment sectors. In the future, the amounts of these effluents may increase, particularly if the cyanides used in the extraction of gold and silver from ores are substituted by thiosulfates, or if the same happens to electronic scrap or in metallic coating processes. This paper reports a study of the oxidation of thiosulfate, with oxygen using copper (II) as a catalyst, at a pH between 4 and 5. The basic idea is to avoid the formation of tetrathionate and polythionate, transforming the thiosulfate into sulfate. The nature of the reaction and a kinetic study of thiosulfate transformation, by reaction with oxygen and Cu2+ at a ppm level, are determined and reported. The best conditions were obtained at 60 °C, pH 5, with an initial concentration of copper of 53 ppm and an oxygen pressure of 1 atm. Under these conditions, the thiosulfate concentration was reduced from 1 g·L−1 to less than 20 ppm in less than three hours.
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Okuniewski, Andrzej, Jaroslaw Chojnacki, Katarzyna Baranowska, and Barbara Becker. "Bis(diisopropylammonium) thiosulfate and bis(tert-butylammonium) thiosulfate." Acta Crystallographica Section C Crystal Structure Communications 69, no. 2 (January 26, 2013): 195–98. http://dx.doi.org/10.1107/s0108270113001327.

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Two new dialkylammonium thiosulfates, namely bis(diisopropylammonium) thiosulfate, 2C6H16N+·S2O32−, (I), and bis(tert-butylammonium) thiosulfate, 2C4H12N+·S2O32−, (II), have been characterized. The secondary ammonium salt (I) crystallizes withZ= 4, while the primary ammonium salt (II), with more hydrogen-bond donors, crystallizes withZ= 8 and a noncrystallographic centre of inversion. In both salts, the organic cations and thiosulfate anions are linked within extensive N—H...O and N—H...S hydrogen-bond networks, forming extended two-dimensional layers. Layers are parallel to (10\overline{1}) in (I) and to (002) in (II), and have a polar interior and a nonpolar hydrocarbon exterior. The layered structure and hydrogen-bond motifs observed in (I) and (II) are similar to those in related ammonium sulfates.
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Sari, Alifiana Permata, Fadila Arum Rhamadani, Nur Layli Amanah, and Agung Nugroho. "Study of Efficiency and Reaction Rates Dechlorination of Nata De Coco Wastewater Using Sodium Thiosulfate." Journal of Emerging Supply Chain, Clean Energy, and Process Engineering 1, no. 2 (December 31, 2022): 107–16. http://dx.doi.org/10.57102/jescee.v1i2.17.

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Chemical reduction with sodium thiosulfate is commonly used to dechlorinate chlorinated waste. U.S. Environmental Protection Agency recommends sodium thiosulfate (Na2S2O3) as a dechlorinating agent for waste samples containing residual chlorine before being released into the environment or entering the distribution system. However, sodium thiosulfate's efficiency and chlorination kinetics at different concentrations are still unknown due to a lack of information on chlorination kinetics. The study was conducted by determining the number of efficient doses of sodium thiosulfate and observing chlorination kinetics using sodium thiosulfate as a dechlorination agent observed at different stoichiometric ratios (1x, 1.5x, and 2x). Sodium thiosulfate at a stoichiometric dose of 2x can reduce chlorine residue by up to 0.4 ppm. The regression analysis of and constant rate are used in the kinetic analysis of sodium thiosulfate dechlorination processes. The kinetics of the chlorination process employing sodium thiosulfate is first order to the total concentration of chlorine in solution at a stoichiometric dosage of 2x, according to the findings.
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Loučka, Tomáš. "Adsorption and Oxidation of Thiosulfate on the Platinum Electrode in a Slightly Alkaline Medium." Collection of Czechoslovak Chemical Communications 65, no. 1 (2000): 1–8. http://dx.doi.org/10.1135/cccc20000001.

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The aim of this research was to study the oxidation and reduction of the adsorbed thiosulfate on the platinum electrode in a slightly alkaline medium. The adsorption was performed at the open circuit conditions. The reduction of the adsorbed layer in the hydrogen region is slower in a slightly alkaline medium than in acid. The mechanism of reduction and oxidation of adsorbed molecules is probably the same. The nonstationary currents measured in presence of thiosulfates showed that the change in the oxidation number does not take place during the adsorption in the double layer region. In the hydrogen region, thiosulfate replaces the adsorbed hydrogen while beeing reduced. Nonstationary currents at higher concentrations of thiosulfate indicate the presence of more layers on the electrode. Upon reaching higher concentrations of thiosulfate the oxidation reaction takes place between thiosulfate in solution and adsorbed product of its reduction. The open circuit potential of the platinum electrode measured in a thiosulfate solution was 0.780 and 0.783 V against the hydrogen electrode in the same solution.
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Al-Khazaal, A. Z., F. Ahmad, and N. Ahmad. "Study on the Removal of Thiosulfate from Wastewater by Catalytic Oxidation." Engineering, Technology & Applied Science Research 9, no. 2 (April 10, 2019): 4053–56. http://dx.doi.org/10.48084/etasr.2553.

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Wastewater streaming from industrial plants, including petroleum refineries, chemical plants, pulp and paper plants, mining operations, electroplating operations, and food processing plants, can contain offensive substances such as cyanide, sulfides, sulfites, thiosulfates, mercaptans and disulfides that tend to increase the chemical oxygen demand (COD) of the streams. In the present work, removal of thiosulfate from wastewater by catalytic oxidation using aluminum oxide as a catalyst was studied. Four main factors were considered, namely the initial thiosulfate concentration, the hydrogen peroxide concentrations, the amount of the catalyst and the operating temperatures. The analysis of thiosulfate and sulfate was carried out by using UV Visible Spectrophotometer. An empirical rate equation was developed.
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Orzeszko, Andrzej, Anna Niedźwiecka-Komaś, Ryszard Stolarskic, and Zygmunt Kazimierczuk. "Synthesis and Conformation of Nucleoside 5'-S-Thiosulfates." Zeitschrift für Naturforschung B 53, no. 10 (October 1, 1998): 1191–96. http://dx.doi.org/10.1515/znb-1998-1015.

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AbstractReaction between 5′-bromo-5′-deoxy- (or 5′-tosyl-) nucleosides and sodium thiosulfate gives the respective 5′-S-thiosulfates (nucleoside Bunte salts). Conformation and some physicochemical properties of the new nucleotide analogs are described
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Lehner, Anna J., Lisa V. Schindler, and Caroline Röhr. "Kristallstrukturen der Alkalimetall-Thiosulfate A2S2O3 nH2O (A/n = K/0, K/⅓ , Rb=1) / Crystal Structures of the Alkali Thiosulfates A2S2O3 · nH2O (A/n = K/0, K/⅓ , Rb=1)." Zeitschrift für Naturforschung B 68, no. 4 (April 1, 2013): 323–37. http://dx.doi.org/10.5560/znb.2013-3089.

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The potassium and rubidium thiosulfates (hydrates) considered in this work were originally obtained as by-products during several syntheses of mixed sulfido=oxido metallates. The interesting complexity of their structural chemistry has motivated us to investigate them in detail. The crystal structures of all title compounds have been determined using single-crystal X-ray data. The structure of the anhydrous potassium thiosulfate K2S2O3 (monoclinic, space group P21/c, a=1010.15(14), b=910.65(12), c=1329.4(2) pm, b =111.984(11)º, Z =8, R1=0.0665) exhibits two crystallographically different thiosulfate anions, overall coordinated by 9=10 potassium cations. Their packing in the structure leads to a complex structure with a pseudo orthorhombic unit cell. The structure of the anhydrous salt is discussed in comparison with the known even more complicated 1=3 hydrate K2S2O3·1/3H2O (monoclinic, space group P21/c, a=938.27(6), b=602.83(4), c=3096.0(2) pm, b =98.415(6)º, Z =12, R1=0.0327). Under the chosen experimental conditions, rubidium forms the monohydrate Rb2S2O3 ·H2O, which also crystallizes with a new, in this case less complex structure (monoclinic, space group C2/m, a=1061.4(1), b=567.92(4), c=1096.4(1) pm, b =97.40(1)º, Z =4, R1=0.0734). Its thiosulfate ions form double layers of equally oriented tetrahedral units. The bond lengths and angles of the thiosulfate ions in all title compounds and in the sodium salts used for comparison vary only very slightly (dS-S =199.8 - 203.0 pm, dS-O =144.8 - 147.4 pm), and the deviation from the ideal C3v symmetry is very small, despite their complex packing. The overall coordination number of the thiosulfate ions by the alkali cations (and water molecules) increases systematically with the ionic radius of the counter cations and the amount of water molecules. For all known alkali thiosulfates, both the conventional and the calculated effective coordination numbers (ECoN) of the alkali cations as well as the partial molar volumes of the cations and the water molecules are compared and discussed.
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Landry, Greg M., Taku Hirata, Jacob B. Anderson, Pablo Cabrero, Christopher J. R. Gallo, Julian A. T. Dow, and Michael F. Romero. "Sulfate and thiosulfate inhibit oxalate transport via a dPrestin (Slc26a6)-dependent mechanism in an insect model of calcium oxalate nephrolithiasis." American Journal of Physiology-Renal Physiology 310, no. 2 (January 15, 2016): F152—F159. http://dx.doi.org/10.1152/ajprenal.00406.2015.

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Nephrolithiasis is one of the most common urinary tract disorders, with the majority of kidney stones composed of calcium oxalate (CaOx). Given its prevalence (US occurrence 10%), it is still poorly understood, lacking progress in identifying new therapies because of its complex etiology. Drosophila melanogaster (fruitfly) is a recently developed model of CaOx nephrolithiasis. Effects of sulfate and thiosulfate on crystal formation were investigated using the Drosophila model, as well as electrophysiological effects on both Drosophila (Slc26a5/6; dPrestin) and mouse (mSlc26a6) oxalate transporters utilizing the Xenopus laevis oocyte heterologous expression system. Results indicate that both transport thiosulfate with a much higher affinity than sulfate Additionally, both compounds were effective at decreasing CaOx crystallization when added to the diet. However, these results were not observed when compounds were applied to Malpighian tubules ex vivo. Neither compound affected CaOx crystallization in dPrestin knockdown animals, indicating a role for principal cell-specific dPrestin in luminal oxalate transport. Furthermore, thiosulfate has a higher affinity for dPrestin and mSlc26a6 compared with oxalate These data indicate that thiosulfate's ability to act as a competitive inhibitor of oxalate via dPrestin, can explain the decrease in CaOx crystallization seen in the presence of thiosulfate, but not sulfate. Overall, our findings predict that thiosulfate or oxalate-mimics may be effective as therapeutic competitive inhibitors of CaOx crystallization.
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Anandham, R., P. Indiragandhi, M. Madhaiyan, Kyounga Kim, Woojong Yim, V. S. Saravanan, Jongbae Chung, and Tongmin Sa. "Thiosulfate oxidation and mixotrophic growth of Methylobacterium oryzae." Canadian Journal of Microbiology 53, no. 7 (July 2007): 869–76. http://dx.doi.org/10.1139/w07-057.

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Thiosulfate oxidation and mixotrophic growth with succinate or methanol plus thiosulfate was examined in nutrient-limited mixotrophic condition for Methylobacterium oryzae CBMB20, which was recently characterized and reported as a novel species isolated from rice. Methylobacterium oryzae was able to utilize thiosulfate in the presence of sulfate. Thiosulfate oxidation increased the protein yield by 25% in mixotrophic medium containing 18.5 mmol·L–1of sodium succinate and 20 mmol·L–1of sodium thiosulfate on day 5. The respirometric study revealed that thiosulfate was the most preferable reduced inorganic sulfur source, followed by sulfur and sulfite. Thiosulfate was predominantly oxidized to sulfate and intermediate products of thiosulfate oxidation, such as tetrathionate, trithionate, polythionate, and sulfur, were not detected in spent medium. It indicated that bacterium use the non-S4intermediate sulfur oxidation pathway for thiosulfate oxidation. Thiosulfate oxidation enzymes, such as rhodanese and sulfite oxidase activities appeared to be constitutively expressed, but activity increased during growth on thiosulfate. No thiosulfate oxidase (tetrathionate synthase) activity was detected.
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Dissertations / Theses on the topic "Thiosulfate"

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Ullah, Mohammad Barkat. "Mercury stabilization using thiosulfate and thioselenate." Thesis, University of British Columbia, 2012. http://hdl.handle.net/2429/41930.

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Mercury is commonly present with gold in nature. As a result it has a tendency to follow gold through the cyanide recovery circuit and ends up in the electro-winning cell as elemental mercury. The laws on the sale and international transport of this mercury are changing. Ultimately, it appears that it will be necessary to stabilize and dispose in a stable form. Mercury sulfide (HgS) and mercury selenide (HgSe) have significantly lower solubilities. The concept of using a thiosulfate dissolution/precipitation method to stabilize mercury as mercury sulfide has been investigated. Comparing the solubilities of mercury sulfide and mercury selenide, mercury selenide is much less soluble. For this reason, the second idea in this thesis is to use sodium thioselenate as a source of selenium in mercury solution to produce mercury selenide. To pursue this project, mercury analysis, mercury leaching and mercury precipitation tests were performed at different temperatures and solution conditions. The resulting solutions were analyzed by Atomic Absorption Spectroscopy (AAS) and the solid precipitates were analyzed by X-ray Diffraction. The EDTA titration method for mercury analysis is effective for a simple mercury nitrate solution. If sodium thiosulfate was added in the solution, thiosulfate interfered with the solution and the titration method was not effective. As a result the AAS method was adopted. Red mercury sulfide can be precipitated by simple aging of mercury thiosulfate solution. Parameters such as temperature, pH and thiosulfate concentration have an effect on the rate and extent of mercury sulfide precipitation. With an increase of temperature, thiosulfate concentration and at lower pH, the mercury precipitation rate increases. However at very high temperature such as 70ºC and 80ºC mercury precipitates as a mixture of red and black mercury sulfide. Thioselenate synthesis was attempted from a mixture of sodium sulfite and selenium powder. The reaction between sulfite and elemental selenium was too slow to be useful. The environmental stability of the mercury sulfide precipitates produced from thiosulfate solutions was investigated. Solid Waste Disposal Characterization (SWDC) tests were done to check the precipitation limit for land disposal and Resource Conservation and Recovery Act (RCRA).
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Zhou, Zizheng. "Mercury stabilization using thiosulfate or selenosulfate." Thesis, University of British Columbia, 2013. http://hdl.handle.net/2429/44276.

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Mercury is often found associated with gold and silver minerals in ore bodies. It is recovered as liquid elemental mercury in several stages including carbon adsorption, carbon elution, electrowinning and retorting. Thus a great amount of mercury is produced as a by-product in gold mines. The Mercury Export Ban Act of 2008 prohibits conveying, selling and distributing elemental mercury by federal agencies in United States. It also bans the export of elemental mercury starting January 1, 2013. As a result, a long-term mercury management plan is required by gold mining companies that generate liquid mercury as a by-product. This thesis will develop a process to effectively convert elemental mercury into much more stable mercury sulfide and mercury selenide for safe disposal. The process consists of 1) extraction of elemental mercury into solution to form aqueous mercury (II) and 2) mercury precipitation as mercury sulfide or mercury selenide. Elemental mercury can be effectively extracted by using hypochlorite solution in acidic environment to form aqueous mercury (II) chloride. The effect of different parameters on the extent and rate of mercury extraction were studied, such as pH, temperature, stirring speed and hypochlorite concentration. Results show that near complete extraction can be achieved within 8 hours by using excess sodium hypochlorite at pH 4 with a fast stirring speed of 1000RPM. Mercury precipitation was achieved by using thiosulfate and selenosulfate solution. In thiosulfate precipitation, cinnabar, metacinnabar or a mixture of both can be obtained depending on the experimental conditions. Elevated temperatures, acidic environment and high reagent concentrations favour the precipitation reaction. Complete mercury removal can be achieved within 4 hours. However, it appears that the less stable metacinnabar tends to form when the precipitation rate increases. Selenosulfate solution can be produced by dissolving elemental selenium in sulfite solution at elevated temperature. Precipitation of mercury selenide using selenosulfate reagent was found to be very effective. The precipitation rate proved to be extremely fast, and the formed precipitates have been confirmed to be tiemannite (HgSe) in all experiments. Finally, Solid Waste Disposal Characterization (SWDC) experiments were conducted to examine the mobility of the formed mercury sulfide and mercury selenide. The results show that none of the formed precipitates exceed the Ultimate Treatment Standard (UTS) limit.
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Muslim, Abrar. "Thiosulfate leaching process for gold extraction." Thesis, Curtin University, 2010. http://hdl.handle.net/20.500.11937/896.

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Increasing environmental concerns over the use of cyanide for gold recovery has intensified the need to deeply understand gold thiosulfate leaching system. Therefore, experimental and modelling work for the kinetics and equilibrium adsorption of thiosulfate, polythionates, gold and copper onto strong based anion exchange resin have been conducted in this study, and the results are concisely discussed in the thesis. Experimental procedures, reaction mechanisms and novel dynamic models for the adsorption phenomena were also proposed.
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Sitando, Onias. "Gold Leaching in Thiosulfate-Oxygen Solutions." Thesis, Sitando, Onias (2017) Gold Leaching in Thiosulfate-Oxygen Solutions. PhD thesis, Murdoch University, 2017. https://researchrepository.murdoch.edu.au/id/eprint/38239/.

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Gibbins, Matthew Thomas George. "Metabolic and vascular effects of thiosulfate sulfurtransferase deletion." Thesis, University of Edinburgh, 2018. http://hdl.handle.net/1842/31558.

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Hydrogen sulfide (H2S), is a gasotransmitter with several key roles in metabolism and vascular function. The effects of H2S are dependent on concentration and target organ. For example, increased H2S concentrations impair liver metabolic function but protect against vascular dysfunction and atherosclerosis. Thiosulfate sulfurtransferase (TST), a nuclear encoded mitochondrial matrix enzyme, is proposed to be a component of the sulfide oxidising unit (SOU) which metabolises H2S. Preliminary data has shown that Tst deletion in mice (Tst-/-) increases circulating H2S levels measured in whole blood. Therefore, it was hypothesised that Tst-/- mice would exhibit worsened metabolic function in the liver but also protection of vascular function under conditions of vascular stress e.g. atherosclerosis. Liver metabolism was assessed by extensive metabolic phenotyping of Tst-/-mice fed control diet and in conditions of metabolic dysfunction induced by a high fat diet (HFD). Tst deletion altered glucose metabolism in mice; gluconeogenesis was increased in liver from Tst-/-mice fed control diet. Glucose intolerance in HFD-fed Tst-/-mice was also more severe than HFDfed C57BL/6 controls. In vitro metabolic investigations in primary hepatocytes isolated from Tst-/-mice demonstrated that mitochondrial ATP-linked and leak respiration were increased compared to controls. The effect of Tst deletion on vascular function was investigated in Tst- /-mice fed control or HFD using myography. Tst deletion did not alter vessel function when mice were maintained on a normal diet. HFD feeding (20 weeks) reduced maximal vessel constriction in the presence of endothelial nitric oxide synthase and cyclooxygenase inhibitors in C57BL/6 aorta. However, in Tst-/-mice fed HFD there was no reduction in maximal constriction suggesting a protective action of Tst deletion. The effects of Tst deletion on atherosclerotic lesions was investigated by generating double knock-out (DKO) mice by deletion of the Tst gene in ApoE-/- mice and (ApoE-/-Tst-/-). Atherosclerotic lesion formation was accelerated by feeding mice a western diet. Within the brachiocephalic branch lesion volume and total vessel volume were reduced in DKO mice fed western diet for 12 weeks, indicating that Tst deletion reduced lesion formation. Plasma cholesterol was reduced in DKO mice compared to ApoE-/- controls and a trend towards reduced systolic blood pressure was also noted. Overall this work supported the hypothesis that Tst deletion engenders metabolic dysfunction but vascular protection. The findings are consistent with the reported effects of increased H2S signalling. Overall inhibition of TST represents a novel target for treatment of atherosclerosis, with the caveat that glycaemia may be worsened due to hepatic metabolic dysfunction.
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com, seanzhang06@hotmail, and Xin-min Zhang. "The dissolution of gold colloids in aqueous thiosulfate solutions." Murdoch University, 2008. http://wwwlib.murdoch.edu.au/adt/browse/view/adt-MU20090807.121135.

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The kinetics of the dissolution of gold and silver colloids in ammoniacal thiosulfate solutions has been studied using oxygen, copper(II) or oxygenated copper(II) as oxidants at pH 9 - 11 and temperature 22oC to 48oC. The effects of the concentration of the main reagents such as copper(II), ammonia and thiosulfate as well as various background reagents have been investigated. Gold and silver colloids have characteristic absorption peaks at 530 nm and 620 nm respectively. Thus, the extent of gold or silver dissolution in different lixiviant systems was monitored using an ultraviolet-visible spectrophotometer. A comparison of the behaviour of gold colloids and powders has also been made. The beneficial or detrimental effects of silver colloid, and background reagents such as silver nitrate, and sodium salts of nitrate, carbonate, sulfite, sulfate, trithionate, tetrathionate anions have also been investigated. Experimental results show that the relative rates and the extent of gold colloid dissolution at 25ºC in different lixiviant systems in a given time interval are in the order: oxygen-cyanide > copper(II)-ammonia-thiosulfate ≈ oxygen-copper(II)- ammonia-thiosulfate > oxygen ammonia-thiosulfate ≥ oxygen-ammonia > copper(II) ammonia. The analysis of electrode potentials shows that Au(S2O3)23- is the predominant gold(I) species in the lixiviant solutions containing oxygen or copper(II) as oxidant and thiosulfate or mixed ammonia-thiosulfate as ligands. During the reaction of copper(II) with thiosulfate in ammoniacal solution without oxygen, the measured potential using a platinum electrode represent the redox couple Cu(NH3)n2+/Cu(S2O3)m1-2m (n = 4 or 3, m = 3 or 2) depending on the concentrations of thiosulfate and ammonia. The initial dissolution rates of gold colloid by oxygen in copper-free solutions show a reaction order of 0.28 with respect to the concentration of dissolved oxygen, but independent of the concentration of ammonia and thiosulfate. The reaction activation energy of 25 kJ/mol in the temperature range 25°C to 48°C indicated a diffusion controlled reaction. The initial dissolution rates of gold colloid by oxidation with copper(II) in oxygenfree solutions show reaction orders of 0.41, 0.49, 0.60, 0.15 and 0.20 with respect to the concentrations of copper(II), thiosulfate, ammonia, chloride and silver respectively. The presence of silve (I) or chloride ions enhances the rate of gold dissolution, indicating their involvement in the surface reaction, possibly by interfering with or preventing a passivating sulfur rich film on gold surface. An activation energy of 40-50 kJ/mol for the dissolution of gold by oxidation with copper(II) in the temperature range 22°C to 48°C suggests a mixed chemically/diffusion controlled reaction. The dissolution of gold by oxidation with copper(II) in oxygen-free solutions appears to be a result of the reaction between gold, thiosulfate ions and the mixed complex Cu(NH3)p(S2O3)0. The half order reactions support electrochemical mechanisms in some cases. The initial dissolution rates of gold colloid, massive gold and gold-silver alloys by oxygenated copper(II) solutions also suggest a reaction that is first order with respect to copper(II) concentration. High oxygen concentration in solutions has a negative effect on the initial rate of gold dissolution and overall percentage of gold dissolution, indicating that oxygen affects the copper(II), copper(I) or sulfur species which in turn affects the gold dissolution. The surface reaction produces Au(NH3)(S2O3)- and Cu(NH3)p+. The mixed complexes Au(NH3)(S2O3)- and Cu(NH3)p+ re-equilibrate to the more stable complexes Au(S2O3)23- and Cu(S2O3)35- in solution. The dissolution of gold powder by oxidation with copper(II) in oxygen-free solutions shows the same trends as that of gold colloid. The presence of silver(I) or chloride ions enhances the initial rate and percentage dissolution of gold colloid and powder. The dissolution kinetics of gold powder and colloid follow a shrinking sphere kinetic model in solutions of relatively low concentrations of thiosulfate and ammonia, with apparent rate constants being inversely proportional to particle radius. The best system for dissolving gold based on the results of this work is the copper(II)-ammonia-thiosulfate solution in the absence of oxygen or in the presence of oxygen. In the absence of oxygen, copper(II) 1.5-4.5 mM, thiosulfate 20-50 mM, ammonia 120-300 mM and pH 9.3-10 are the best conditions. The presences of carbonate and sulfite have a significant negative effect on the dissolution of gold. The presence of sodium trithionate shows a beneficial effect in the first two hours, while sodium tetrathionate or lead nitrate have a small negative effect and sodium nitrate showed no effect on the dissolution of gold. Silver nitrate and sodium chloride also show beneficial effects. In the presence of oxygen, copper(II) 2.0-3.0 mM, thiosulfate 50 mM, ammonia 240 mM and pH 9.3-9.5 are the best conditions.
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Zhang, Xin-min. "The dissolution of gold colloids in aqueous thiosulfate solutions." Zhang, Xin-min (2008) The dissolution of gold colloids in aqueous thiosulfate solutions. PhD thesis, Murdoch University, 2008. http://researchrepository.murdoch.edu.au/672/.

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The kinetics of the dissolution of gold and silver colloids in ammoniacal thiosulfate solutions has been studied using oxygen, copper(II) or oxygenated copper(II) as oxidants at pH 9 - 11 and temperature 22oC to 48oC. The effects of the concentration of the main reagents such as copper(II), ammonia and thiosulfate as well as various background reagents have been investigated. Gold and silver colloids have characteristic absorption peaks at 530 nm and 620 nm respectively. Thus, the extent of gold or silver dissolution in different lixiviant systems was monitored using an ultraviolet-visible spectrophotometer. A comparison of the behaviour of gold colloids and powders has also been made. The beneficial or detrimental effects of silver colloid, and background reagents such as silver nitrate, and sodium salts of nitrate, carbonate, sulfite, sulfate, trithionate, tetrathionate anions have also been investigated. Experimental results show that the relative rates and the extent of gold colloid dissolution at 25ºC in different lixiviant systems in a given time interval are in the order: oxygen-cyanide > copper(II)-ammonia-thiosulfate ≈ oxygen-copper(II)- ammonia-thiosulfate > oxygen ammonia-thiosulfate ≥ oxygen-ammonia > copper(II) ammonia. The analysis of electrode potentials shows that Au(S2O3)23- is the predominant gold(I) species in the lixiviant solutions containing oxygen or copper(II) as oxidant and thiosulfate or mixed ammonia-thiosulfate as ligands. During the reaction of copper(II) with thiosulfate in ammoniacal solution without oxygen, the measured potential using a platinum electrode represent the redox couple Cu(NH3)n2+/Cu(S2O3)m1-2m (n = 4 or 3, m = 3 or 2) depending on the concentrations of thiosulfate and ammonia. The initial dissolution rates of gold colloid by oxygen in copper-free solutions show a reaction order of 0.28 with respect to the concentration of dissolved oxygen, but independent of the concentration of ammonia and thiosulfate. The reaction activation energy of 25 kJ/mol in the temperature range 25°C to 48°C indicated a diffusion controlled reaction. The initial dissolution rates of gold colloid by oxidation with copper(II) in oxygenfree solutions show reaction orders of 0.41, 0.49, 0.60, 0.15 and 0.20 with respect to the concentrations of copper(II), thiosulfate, ammonia, chloride and silver respectively. The presence of silve (I) or chloride ions enhances the rate of gold dissolution, indicating their involvement in the surface reaction, possibly by interfering with or preventing a passivating sulfur rich film on gold surface. An activation energy of 40-50 kJ/mol for the dissolution of gold by oxidation with copper(II) in the temperature range 22°C to 48°C suggests a mixed chemically/diffusion controlled reaction. The dissolution of gold by oxidation with copper(II) in oxygen-free solutions appears to be a result of the reaction between gold, thiosulfate ions and the mixed complex Cu(NH3)p(S2O3)0. The half order reactions support electrochemical mechanisms in some cases. The initial dissolution rates of gold colloid, massive gold and gold-silver alloys by oxygenated copper(II) solutions also suggest a reaction that is first order with respect to copper(II) concentration. High oxygen concentration in solutions has a negative effect on the initial rate of gold dissolution and overall percentage of gold dissolution, indicating that oxygen affects the copper(II), copper(I) or sulfur species which in turn affects the gold dissolution. The surface reaction produces Au(NH3)(S2O3)- and Cu(NH3)p+. The mixed complexes Au(NH3)(S2O3)- and Cu(NH3)p+ re-equilibrate to the more stable complexes Au(S2O3)23- and Cu(S2O3)35- in solution. The dissolution of gold powder by oxidation with copper(II) in oxygen-free solutions shows the same trends as that of gold colloid. The presence of silver(I) or chloride ions enhances the initial rate and percentage dissolution of gold colloid and powder. The dissolution kinetics of gold powder and colloid follow a shrinking sphere kinetic model in solutions of relatively low concentrations of thiosulfate and ammonia, with apparent rate constants being inversely proportional to particle radius. The best system for dissolving gold based on the results of this work is the copper(II)-ammonia-thiosulfate solution in the absence of oxygen or in the presence of oxygen. In the absence of oxygen, copper(II) 1.5-4.5 mM, thiosulfate 20-50 mM, ammonia 120-300 mM and pH 9.3-10 are the best conditions. The presences of carbonate and sulfite have a significant negative effect on the dissolution of gold. The presence of sodium trithionate shows a beneficial effect in the first two hours, while sodium tetrathionate or lead nitrate have a small negative effect and sodium nitrate showed no effect on the dissolution of gold. Silver nitrate and sodium chloride also show beneficial effects. In the presence of oxygen, copper(II) 2.0-3.0 mM, thiosulfate 50 mM, ammonia 240 mM and pH 9.3-9.5 are the best conditions.
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Jeffery, Y. Masau Rosemarie. "The mechanism of thiosulfate oxidation by Thiobacillus thiooxidans 8085." Thesis, National Library of Canada = Bibliothèque nationale du Canada, 1999. http://www.collectionscanada.ca/obj/s4/f2/dsk1/tape7/PQDD_0012/MQ41722.pdf.

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Sen, Gupta Supriya Kumar. "Oxidation of sodium thiosulfate in weak kraft black liquor." Thesis, McGill University, 1987. http://digitool.Library.McGill.CA:80/R/?func=dbin-jump-full&object_id=66124.

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Zhang, Xin-Min. "The dissolution of gold colloids in aqueous thiosulfate solutions /." Murdoch University Digital Theses Program, 2008. http://wwwlib.murdoch.edu.au/adt/browse/view/adt-MU20090807.121135.

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Books on the topic "Thiosulfate"

1

Laitinen, Tarja. Thiosulfate pitting corrosion of stainless steels in paper machine environment. Espoo, Finland: VTT, Technical Research Centre of Finland, 1999.

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Siu, Tung. Kinetic and mechanistic study of aqueous sulfide-sulfite-thiosulfate system. Ottawa: National Library of Canada, 1999.

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McKenzie, David J. From a closed to an open system: PH oscillations in the oxidation of thiosulfate by hydrogen peroxide. Sudbury, Ont: Laurentian University, 1997.

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Cepuch, C. Cyanide blood concentration following sodium nitroprusside administration: effect of sodium thiosulfate. 1993.

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Engelhardt, Wolfgang von. Untersuchungen über das Extracelluläre Flüssigkeitsvolumen und Die Thiosulfat-Totalclearance Wachsender Schweine. Springer London, Limited, 2013.

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Parker, Philip M. The World Market for Sulfites and Thiosulfates: A 2007 Global Trade Perspective. ICON Group International, Inc., 2006.

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The World Market for Sulfites and Thiosulfates: A 2004 Global Trade Perspective. Icon Group International, Inc., 2005.

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Parker, Philip M. The 2007 Import and Export Market for Sulfites and Thiosulfates in China. ICON Group International, Inc., 2006.

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Parker, Philip M. The 2007 Import and Export Market for Sulfites and Thiosulfates in United States. ICON Group International, Inc., 2006.

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Parker, Philip M. The 2007 Import and Export Market for Sulfides, Polysulfides, Dithionites, Sulfoxylates, Sulfites, Thiosulfates, Sulfates and Alums in India. ICON Group International, Inc., 2006.

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Book chapters on the topic "Thiosulfate"

1

Cantrell, F. Lee. "Thiosulfate." In Critical Care Toxicology, 1–4. Cham: Springer International Publishing, 2016. http://dx.doi.org/10.1007/978-3-319-20790-2_156-1.

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Cantrell, F. Lee. "Thiosulfate." In Critical Care Toxicology, 3001–4. Cham: Springer International Publishing, 2017. http://dx.doi.org/10.1007/978-3-319-17900-1_156.

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Gooch, Jan W. "Sodium Thiosulfate." In Encyclopedic Dictionary of Polymers, 675. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_10841.

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Schomburg, D., M. Salzmann, and D. Stephan. "Thiosulfate dehydrogenase." In Enzyme Handbook 7, 537–41. Berlin, Heidelberg: Springer Berlin Heidelberg, 1994. http://dx.doi.org/10.1007/978-3-642-78521-4_104.

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Bährle-Rapp, Marina. "Sodium Thiosulfate." In Springer Lexikon Kosmetik und Körperpflege, 519. Berlin, Heidelberg: Springer Berlin Heidelberg, 2007. http://dx.doi.org/10.1007/978-3-540-71095-0_9766.

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Schomburg, Dietmar, and Dörte Stephan. "Thiosulfate sulfurtransferase." In Enzyme Handbook, 883–89. Berlin, Heidelberg: Springer Berlin Heidelberg, 1997. http://dx.doi.org/10.1007/978-3-642-59025-2_163.

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Schomburg, Dietmar, and Dörte Stephan. "Thiosulfate-thiol sulfurtransferase." In Enzyme Handbook, 895–97. Berlin, Heidelberg: Springer Berlin Heidelberg, 1997. http://dx.doi.org/10.1007/978-3-642-59025-2_165.

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Schomburg, Dietmar, and Dörte Stephan. "Thiosulfate-dithiol sulfurtransferase." In Enzyme Handbook, 903–5. Berlin, Heidelberg: Springer Berlin Heidelberg, 1997. http://dx.doi.org/10.1007/978-3-642-59025-2_167.

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Bährle-Rapp, Marina. "Sodium Propoxyhydroxypropyl Thiosulfate Silica." In Springer Lexikon Kosmetik und Körperpflege, 516. Berlin, Heidelberg: Springer Berlin Heidelberg, 2007. http://dx.doi.org/10.1007/978-3-540-71095-0_9695.

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Trüper, H. G., C. Lorenz, M. Schedet, and M. Steinmetz. "Metabolism of Thiosulfate in Chlorobium." In Green Photosynthetic Bacteria, 189–200. Boston, MA: Springer US, 1988. http://dx.doi.org/10.1007/978-1-4613-1021-1_24.

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Conference papers on the topic "Thiosulfate"

1

de Koning, Marie-Sophie, and Rachel Giles. "Sodium thiosulfate ineffective at cardiac protection." In 71st ACC Scientific Session, edited by Marc Bonaca. Baarn, the Netherlands: Medicom Medical Publishers, 2022. http://dx.doi.org/10.55788/bd75f31a.

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Corwin, D., J. Kamau, R. Snyder, and M. Dunn. "Sodium Thiosulfate Induced Severe Anion Gap Metabolic Acidosis." In American Thoracic Society 2020 International Conference, May 15-20, 2020 - Philadelphia, PA. American Thoracic Society, 2020. http://dx.doi.org/10.1164/ajrccm-conference.2020.201.1_meetingabstracts.a1670.

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Povar, Igor, Stefano Ubaldini, Tudor Lupascu, Oxana Spinu, and Boris Pintilie. "THE SOLUTION CHEMISTRY OF THE COPPER (II) - AMMONIA THIOSULFATE AQUEOUS SYSTEM." In International Symposium "The Environment and the Industry". National Research and Development Institute for Industrial Ecology, 2018. http://dx.doi.org/10.21698/simi.2018.fp20.

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Belobaba, A. G., D. V. Sukhorukov, and A. I. Masliy. "Oxidation of sulfite and thiosulfate anions on a porous carbon fiber anode." In 2008 Third International Forum on Strategic Technologies (IFOST). IEEE, 2008. http://dx.doi.org/10.1109/ifost.2008.4602952.

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Li, Jing-Ying, and Xiu-Li Xu. "Notice of Retraction: Thiosulfate Leaching of Gold and Silver from Waste Mobile Phones." In 2011 5th International Conference on Bioinformatics and Biomedical Engineering. IEEE, 2011. http://dx.doi.org/10.1109/icbbe.2011.5781413.

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Koizhanova, Aigul. "EFFECTIVE EXTRACTION OF GOLD AND SILVER FROM SULPHIDIC ORE BY CYANIDE-THIOSULFATE SOLUTIONS." In SGEM2011 11th International Multidisciplinary Scientific GeoConference and EXPO. Stef92 Technology, 2011. http://dx.doi.org/10.5593/sgem2011/s03.116.

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Goossens, J., M. Courbebaisse, V. Ratsimbazafy, D. Bazin, M. Daudon, V. Frochot, P. Richette, F. Lioté, H.-K. Ea, and V. Guigonis. "AB0882 Efficacy of intralesionnal sodium thiosulfate in disabling tumoral calcinosis: about two cases." In Annual European Congress of Rheumatology, 14–17 June, 2017. BMJ Publishing Group Ltd and European League Against Rheumatism, 2017. http://dx.doi.org/10.1136/annrheumdis-2017-eular.2809.

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Almubarak, Tariq, Majed Almubarak, Abdullah Almoajil, and Fares Alotaibi. "Vitamin C: An Environmentally Friendly Multifunctional Additive for Hydraulic Fracturing Fluids." In ADIPEC. SPE, 2022. http://dx.doi.org/10.2118/211113-ms.

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Abstract There exists a need for high temperature fracturing fluids as we expand exploration into deeper, lower permeability, and hotter formations. Fracturing fluid stability depends on two main bonds: the crosslinker to polymer bond and the monomer to monomer bond. To preserve the crosslinker to polymer bond, a proper crosslinker with a suitable delay additive is typically utilized. On the other hand, the monomer to monomer bond is challenging to protect since it’s susceptible to a variety of factors with the main culprit being oxygen radical attacks. Consequently, the most common high temperature stabilizers used are oxygen scavengers such as sodium thiosulfate or sodium sulfite. Unfortunately, both additives create their own issues. Sodium thiosulfate is known to degrade at high temperature to generate H2S, while sulfites generate sulfates that end up causing inorganic scale precipitation or feeding sulfate reducing bacteria creating another source of H2S in the reservoir. Additionally, Sodium thiosulfate is a high pH additive which can cause formation damage through fines migration and precipitation of hydroxides. Vitamin C is renowned for its antioxidative and oxygen scavenging properties throughout many industries. It is commonly used as an extremely cheap supplement to boost the immune system and as a food preservative to increase shelf life. Moreover, it has an acidic pH and offers a chemical structure capable of delaying crosslinking reactions. For that reason, this work aims to study the influence of Vitamin C as a multifunctional additive in fracturing fluids. The tests mainly utilized the high-pressure/high-temperature (HPHT) rheometer. The performance of Vitamin C was assessed with a guar derivative at temperatures between 250-300°F for 1.5 hours. Moreover, zeta potential and coreflood were used to evaluate the formation damage tendencies of using this additive. The results showed that the use of Vitamin C was able to provide a pH reduction, crosslinking delay, and enhance the high temperature stability of fracturing fluids. Zeta potential and coreflood experiments showed that clays were more stable at lower pH conditions minimizing fines migration. Vitamin C is a cheap and readily manufactured environmentally friendly additive that offers solutions to the use of fracturing fluids at high temperatures. Utilizing it not only offers oxygen scavenging ability, but also replaces additives that lower pH and provides crosslinking delaying properties.
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Jarvis, Ian W. H., Chris J. Ottley, D. Graeme Pearson, Michael J. Tilby, and Gareth J. Veal. "Abstract 3501: Characterisation of cisplatin-DNA adducts formed in the presence of sodium thiosulfate." In Proceedings: AACR 101st Annual Meeting 2010‐‐ Apr 17‐21, 2010; Washington, DC. American Association for Cancer Research, 2010. http://dx.doi.org/10.1158/1538-7445.am10-3501.

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Yang, Xiaqiong, Chaoyi Chen, Junqi Li, Bianli Quan, and Xiangqian Zhang. "Influence of thiosulfate on corrosion behavior of 16 Mn steel in sodium hydroxide solution." In 2016 International Conference on Advanced Materials and Energy Sustainability (AMES2016). WORLD SCIENTIFIC, 2017. http://dx.doi.org/10.1142/9789813220393_0029.

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Reports on the topic "Thiosulfate"

1

Oji, L. N., M. L. Restivo, M. R. Duignan, and W. R. Wilmarth. Gaseous Diffusion Membrane Leaching with Select Lixiviants: Ammonium Carbonate, Sodium Phosphate and Ammonium thiosulfate. Office of Scientific and Technical Information (OSTI), November 2018. http://dx.doi.org/10.2172/1485269.

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SONG, Yuhuan, guangyan CAI guangyan, and Ting PENG. Can sodium thiosulfate delay the progression of cardiovascular calcification in dialysis patients? a systematic review and meta-analysis. INPLASY - International Platform of Registered Systematic Review and Meta-analysis Protocols, March 2022. http://dx.doi.org/10.37766/inplasy2022.3.0018.

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Sodium thiosulfate reduces hearing loss in children treated with chemotherapy. National Institute for Health Research, November 2018. http://dx.doi.org/10.3310/signal-000669.

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