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Journal articles on the topic 'Aerated sulfuric acid aqueous solutions'

Author: Grafiati

Published: 4 June 2021

Last updated: 2 February 2022

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1

Autsavapromporn, Narongchai, Jintana Meesungnoen, Ianik Plante, and Jean-Paul Jay-Gerin. "Monte Carlo simulation study of the effects of acidity and LET on the primary free-radical and molecular yields of water radiolysis — Application to the Fricke dosimeter." Canadian Journal of Chemistry 85, no. 3 (March 1, 2007): 214–29. http://dx.doi.org/10.1139/v07-021.

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Monte Carlo simulations are used to investigate the effects of acidity (pH) on the primary yields of various chemical species produced in the radiolysis of de-aerated aqueous sulfuric acid solutions over the range from neutral solution to 0.4 mol/L H2SO4. The effects of the quality of radiation, measured in terms of linear energy transfer (LET), have also been studied for LET varying from ~0.3 to 15 keV/µm at ambient temperature. Our results show that an increase in acidity (1 < pH < 4) leads to an increase in the yield [Formula: see text] of the "reducing" free radicals (hydrated electron and H atom) and a slight increase in G·OH and [Formula: see text], while there is a slight decrease in [Formula: see text] At pH < 1, OH radicals react with HSO4- anions to form SO4·– radicals, resulting in a steep decrease in G.OH. By contrast, in the range of pH from ~4 to 7, the calculated yield values are independent of sulfuric acid concentration. In both neutral water and 0.4 mol/L H2SO4 (pH 0.46) solutions, the primary molecular yields increase upon increasing LET to ~15 keV/µm with a concomitant decrease in those of free radicals. As an exception, GH. at first increases with LET, reaching a maximum near 6.5 keV/µm before decreasing steeply at higher LET. The results obtained are generally in good agreement with available experimental data over the whole acidity and LET ranges studied. Finally, as an application, we have simulated the radiation-induced oxidation of ferrous sulfate solutions in aerated aq. 0.4 mol/L H2SO4 (Fricke dosimeter) as a function of time up to ~50 s and addressed the effects of LET on the resulting ferric ion yield at 25 °C. The production of Fe3+ ions is highly sensitive to free-radical yields, especially H atoms (via formation of HO2), resulting in a marked decline of G(Fe3+) with increasing LET. The general trend of the observed variation of G(Fe3+) with radiation quality is well reproduced by our computed Fe3+ ion yield values.Key words: liquid water, acidic (H2SO4) aqueous solutions, radiolysis, free-radical and molecular yields, linear energy transfer (LET), Fricke dosimeter, Monte Carlo simulations.

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2

Sanders, Stephen J. "Modeling organics in aqueous sulfuric acid solutions." Industrial & Engineering Chemistry Process Design and Development 24, no. 4 (October 1985): 942–48. http://dx.doi.org/10.1021/i200031a008.

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3

Casas, J. M., F. Alvarez, and L. Cifuentes. "Aqueous speciation of sulfuric acid–cupric sulfate solutions." Chemical Engineering Science 55, no. 24 (December 2000): 6223–34. http://dx.doi.org/10.1016/s0009-2509(00)00421-8.

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4

Kameda, Yasuo, Kiyohiko Hosoya, Shuji Sakamoto, Hirohito Suzuki, Takeshi Usuki, and Osamu Uemura. "Hydrogen-bonded structure in aqueous sulfuric acid solutions." Journal of Molecular Liquids 65-66 (November 1995): 305–8. http://dx.doi.org/10.1016/0167-7322(95)00882-8.

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5

Hayduk, Walter, Haruki Asatani, and Benjamin C. Y. Lu. "Solubility of sulfur dioxide in aqueous sulfuric acid solutions." Journal of Chemical & Engineering Data 33, no. 4 (October 1988): 506–9. http://dx.doi.org/10.1021/je00054a033.

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6

Kruchinin, N. P., V. V. Romanov, V. G. Kulichikhin, A. S. Semenova, and V. E. Sorokin. "Creep of oksalon fibres in aqueous sulfuric acid solutions." Fibre Chemistry 16, no. 6 (1985): 431–33. http://dx.doi.org/10.1007/bf00546266.

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7

Lisitsyn, Yu A., and L. V. Grigor’eva. "Electrochemical amination. Dilute aqueous organic solutions of sulfuric acid." Russian Journal of Electrochemistry 45, no. 2 (February 2009): 132–38. http://dx.doi.org/10.1134/s1023193509020025.

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8

Jankovska, Katica, Lidija Soptrajanova, and Ilinka Spirevska. "Protonation of maleic and fumaric acid in aqueous sulfuric acid solutions." Journal of the Serbian Chemical Society 65, no. 10 (2000): 695–708. http://dx.doi.org/10.2298/jsc0010695j.

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The protonations of maleic and fumaric acid in an acidic medium (aqueous solutions of sulfuric acid) were followed spectrophotometrically at room temperature. The acid-base equilibria were characterised qualitatively and quantitatively. The pKBH+ values were determined using the Hammett equation, employing several acid functions in order to determine which of them describes best the protonation process of the studied organic acids. The thermodynamic pKBH+ values as well as those of the solvation parameters m, m* and ? and of the thermodynamic protonation constants (or, rather, the pKa,p values) were also defermined. The method of characteristic vector analysis (CVA) was used to reconstruct the experimental spectra.

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9

Zhestkova, T. P., T. N. Zhukova, and I. E. Makarov. "Specifics of radiolytic degradation of oxalic acid in aerated aqueous solutions." High Energy Chemistry 45, no. 2 (March 2011): 85–88. http://dx.doi.org/10.1134/s0018143911020159.

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10

Keeffe, J. R., A. J. Kresge, and J. Toullec. "Acid-catalyzed enolization of acetophenone: catalysis by bisulfate ion in sulfuric acid solutions." Canadian Journal of Chemistry 64, no. 6 (June 1, 1986): 1224–27. http://dx.doi.org/10.1139/v86-203.

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Rates of acid-catalyzed enolization of acetophenone in dilute aqueous solution, measured under conditions where the solvated proton is the only acidic species present, give a hydrogen ion catalytic coefficient, [Formula: see text], that is 35% smaller than the value obtained by X acidity function extrapolation of measurements made in moderately concentrated sulfuric acid solutions. The difference may be attributed to catalysis by bisulfate ion in the sulfuric acid solutions; this is supported by direct measurement of the bisulfate ion catalytic coefficient in dilute sulfuric acid. This revised value of [Formula: see text] leads to new, but only slightly different, values of the keto–enol equilibrium constant for acetophenone in aqueous solution, pKE = 7.96 ± 0.04, the acidity constant for acetophenone ionizing as a carbon acid, [Formula: see text] and the encounter-controlled rate constant for the reaction of acetophenone enol with molecular bromine, k = (3.2 ± 0.4) × 109 M−1 s−1.

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11

Young Kim, Ki, Ki-Taek Byun, and Ho-Young Kwak. "Characteristics of Sonoluminescing Bubbles in Aqueous Solutions of Sulfuric Acid." Journal of the Physical Society of Japan 75, no. 11 (November 15, 2006): 114705. http://dx.doi.org/10.1143/jpsj.75.114705.

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12

Choe, Yoong-Kee, Eiji Tsuchida, and Tamio Ikeshoji. "First-principles molecular dynamics study on aqueous sulfuric acid solutions." Journal of Chemical Physics 126, no. 15 (April 21, 2007): 154510. http://dx.doi.org/10.1063/1.2718526.

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13

Sharipov, G. L., A. M. Abdrakhmanov, and R. Kh Gainetdinov. "Sonoluminescence of aqueous solutions of sulfuric acid and sulfur dioxide." Russian Chemical Bulletin 52, no. 9 (September 2003): 1966–68. http://dx.doi.org/10.1023/b:rucb.0000009639.39650.14.

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14

Lisitsyn, Yu A., and A. V. Sukhov. "Electrochemical Amination of Chlorobenzene in Aqueous-Organic Solutions of Sulfuric Acid." Russian Journal of Electrochemistry 54, no. 11 (November 2018): 886–92. http://dx.doi.org/10.1134/s1023193518130268.

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15

Lisitsyn, Yu A., and A. V. Sukhov. "Electrochemical amination of benzene in aqueous-acetic solutions of sulfuric acid." Russian Journal of General Chemistry 87, no. 5 (May 2017): 929–33. http://dx.doi.org/10.1134/s1070363217050061.

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16

Casas, J. M., J. P. Etchart, and L. Cifuentes. "Aqueous speciation of arsenic in sulfuric acid and cupric sulfate solutions." AIChE Journal 49, no. 8 (August 2003): 2199–210. http://dx.doi.org/10.1002/aic.690490827.

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17

Bolsaitis, P., and J. F. Elliott. "Thermodynamic activities and equilibrium partial pressures for aqueous sulfuric acid solutions." Journal of Chemical & Engineering Data 35, no. 1 (January 1990): 69–85. http://dx.doi.org/10.1021/je00059a022.

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18

Marziano, Nunziata C., Alberto Tomasin, Claudio Tortato, and Paolo Isandelli. "The problem of acidity in concentrated aqueous solutions of sulfuric acid." Journal of the Chemical Society, Perkin Transactions 2, no. 11 (1998): 2535–40. http://dx.doi.org/10.1039/a803473g.

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19

Zhao, Hong-Kun, and Fang Zhang. "Solubility of Sodium Naphthalene Disulfonate in Aqueous Solutions of Sulfuric Acid." Journal of Chemical & Engineering Data 55, no. 9 (September 9, 2010): 3955–57. http://dx.doi.org/10.1021/je100020v.

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20

Noulty, Robert A., and Derek G. Leaist. "Diffusion in aqueous copper sulfate and copper sulfate-sulfuric acid solutions." Journal of Solution Chemistry 16, no. 10 (October 1987): 813–25. http://dx.doi.org/10.1007/bf00650751.

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21

Leaist, Derek G. "The Soret effect with chemical reaction in aqueous sulfuric acid solutions." Journal of Solution Chemistry 18, no. 7 (July 1989): 651–61. http://dx.doi.org/10.1007/bf00651001.

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22

Lisitsyn, Yu A., and A. V. Sukhov. "Electrochemical Amination of Isomeric Chloroanilines in Aqueous Solutions of Sulfuric Acid." Russian Journal of Electrochemistry 56, no. 5 (May 2020): 426–30. http://dx.doi.org/10.1134/s1023193520050080.

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23

Iraci, L. T., R. R. Michelsen, S. F. M. Ashbourn, T. A. Rammer, and D. M. Golden. "Uptake of hypobromous acid (HOBr) by aqueous sulfuric acid solutions: low-temperature solubility and reaction." Atmospheric Chemistry and Physics 5, no. 6 (June 21, 2005): 1577–87. http://dx.doi.org/10.5194/acp-5-1577-2005.

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Abstract. Hypobromous acid (HOBr) is a key species linking inorganic bromine to the chlorine and odd hydrogen chemical families. We have measured the solubility of HOBr in 45-70wt% sulfuric acid solutions representative of upper tropospheric and lower stratospheric aerosol composition. Over the temperature range 201-252 K, HOBr is quite soluble in sulfuric acid, with an effective Henry's law coefficient, H*=104-107mol L-1atm-1. H* is inversely dependent on temperature, with ΔH=-45.0±5.4 kJ mol-1 and ΔS=-101±24 J mol-1K-1 for 55-70wt% H2SO4 solutions. Our study includes temperatures which overlap both previous measurements of HOBr solubility. For uptake into 55-70wt% H2SO4, the solubility is described by log H*=(2349±280)/T-(5.27±1.24). At temperatures colder than ~213K, the solubility of HOBr in 45wt% H2SO4 is at least a factor of five larger than in 70wt% H2SO4, with log H*=(3665±270)/T-(10.63±1.23). The solubility of HOBr is comparable to that of HBr, indicating that upper tropospheric and lower stratospheric aerosols should contain equilibrium concentrations of HOBr which equal or exceed those of HBr. Upon uptake of HOBr into aqueous sulfuric acid in the presence of other brominated gases, particularly for 70wt% H2SO4 solution, our measurements demonstrate chemical reaction of HOBr followed by evolution of gaseous products including Br2O and Br2.

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24

Iraci, L. T., R. R. Michelsen, S. F. M. Ashbourn, T. A. Rammer, and D. M. Golden. "Uptake of hypobromous acid (HOBr) by aqueous sulfuric acid solutions: low-temperature solubility and reaction." Atmospheric Chemistry and Physics Discussions 5, no. 2 (March 9, 2005): 1213–39. http://dx.doi.org/10.5194/acpd-5-1213-2005.

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Abstract. Hypobromous acid (HOBr) is a key species linking inorganic bromine to the chlorine and odd hydrogen chemical families. We have measured the solubility of HOBr in 45–70 wt% sulfuric acid solutions representative of upper tropospheric and lower stratospheric aerosol composition. Over the temperature range 201–252 K, HOBr is quite soluble in sulfuric acid, with an effective Henry's law coefficient, H*=104-107 mol L-1 atm-1. H* is inversely dependent on temperature, with ΔH=-45.0±5.4 kJ mol-1 and ΔS=-101±24 J mol-1 K-1 for 55–70 wt% H2SO4 solutions. Our study includes temperatures which overlap both previous measurements of HOBr solubility. For uptake into 55–70 wt% H2SO4, the solubility is described by log H*=(2349±280)/T–(5.27±1.24). At temperatures colder than ~213 K, the solubility of HOBr in 45 wt% H2SO4 is at least a factor of five larger than in 70 wt% H2SO4, with log H*=(3665±270)/T–(10.63±1.23). The solubility of HOBr is comparable to that of HBr, indicating that upper tropospheric and lower stratospheric aerosols should contain equilibrium concentrations of HOBr which equal or exceed those of HBr. Upon uptake of HOBr into aqueous sulfuric acid in the presence of other brominated gases, particularly for 70 wt% H2SO4 solution, our measurements demonstrate chemical reaction of HOBr followed by evolution of gaseous products including Br2O and Br2.

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25

Swanson, Brian D. "How Well Does Water Activity Determine Homogeneous Ice Nucleation Temperature in Aqueous Sulfuric Acid and Ammonium Sulfate Droplets?" Journal of the Atmospheric Sciences 66, no. 3 (March 1, 2009): 741–54. http://dx.doi.org/10.1175/2008jas2542.1.

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Abstract Frozen fraction measurements made using a droplet free-fall freezing tube apparatus are presented and used, along with other recent laboratory measurements, to evaluate how well both the water activity idea and the translated melting-point curve idea of Koop et al. predict homogeneous freezing-point temperatures for aqueous ammonium sulfate and sulfuric acid solution droplets. The new freezing-point temperature datasets agree with the previous lowest-temperature results for both solutes. The lowest measured freezing-point temperatures for aqueous ammonium sulfate solutions agree with a curve shaped like the translated melting-point curve. However, those for aqueous sulfuric acid solutions are significantly lower than predicted by the translated melting-point curve idea, and a single water activity freezing-point temperature curve does not represent the lowest-temperature freezing-point temperature data for both solutes. A linear extrapolation of the new aqueous sulfuric acid solution freezing data to low temperatures predicts that high critical supersaturations in cloud-free regions of the upper troposphere will occur when homogeneous ice nucleation in an aqueous sulfuric acid aerosol is the primary ice formation mechanism.

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26

Verbrugge, Mark W., and Robert F. Hill. "Experimental and theoretical investigation of perfluorosulfonic acid membranes equilibrated with aqueous sulfuric acid solutions." Journal of Physical Chemistry 92, no. 23 (November 1988): 6778–83. http://dx.doi.org/10.1021/j100334a056.

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27

Brandani, Stefano, Vincenzo Brandani, and Francesco Vegliò. "On the Purification of β-Naphthalenesulfonic Acid from Dilute Aqueous Solutions Containing Sulfuric Acid." Industrial & Engineering Chemistry Research 37, no. 11 (November 1998): 4528–30. http://dx.doi.org/10.1021/ie980088d.

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28

Chiang, Y., A. J. Kresge, R. A. More O'ferrall, B. A. Murray, N. P. Schepp, and J. Wlrz. "The ketonization of acetophenone enol in concentrated aqueous sulphuric and perchloric acid solutions. Implication on X acidity function correlations of the enolization reaction and determination of the keto–enol equilibrium constant as a function of acidity." Canadian Journal of Chemistry 68, no. 10 (October 1, 1990): 1653–56. http://dx.doi.org/10.1139/v90-257.

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Rates of ketonization of the enol of acetophenone, generated by flash photolytic photohydration of phenylacetylene, were measured in aqueous sulfuric and perchloric acid solutions over the concentration range 1–50 wt.% acid; rates of enolization of acetophenone, monitored by bromine scavenging, were also measured in aqueous perchloric acid solutions over the same concentration range. The results suggest that the curvature observed in a previous X acidity function correlation of the rate of enolization in sulfuric acid solutions was an artifact produced by insufficiently efficient scavenging, and that introduction of the activity of water in the correlating expression, used previously to eliminate the curvature and believed to reflect covalent involvement of water in the enolization reaction, is unnecessary. The present results also show that the keto–enol equilibrium constant for acetophenone decreases with increasing acidity in these concentrated sulfuric and perchloric acid solutions. Key words: acetophenone, enolization, ketonization, keto–enol equilibrium, concentrated acid solutions.

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29

Koter, Stanisław, and Monika Kultys. "Electric transport of sulfuric acid through anion-exchange membranes in aqueous solutions." Journal of Membrane Science 318, no. 1-2 (June 2008): 467–76. http://dx.doi.org/10.1016/j.memsci.2008.03.010.

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30

Liu, Ze, Ling-Yan Wu, Tian-He Wang, Mao-Fa Ge, and Wei-Gang Wang. "Uptake of Methacrolein into Aqueous Solutions of Sulfuric Acid and Hydrogen Peroxide." Journal of Physical Chemistry A 116, no. 1 (December 15, 2011): 437–42. http://dx.doi.org/10.1021/jp2100649.

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31

Michelsen, H. A. "A parameterization for the activity of H+in aqueous sulfuric acid solutions." Geophysical Research Letters 25, no. 19 (October 1, 1998): 3571–73. http://dx.doi.org/10.1029/98gl02756.

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32

Merrill, Daniel R., Ionel C. Stefan, Daniel A. Scherson, and J. Thomas Mortimer. "Electrochemistry of Gold in Aqueous Sulfuric Acid Solutions under Neural Stimulation Conditions." Journal of The Electrochemical Society 152, no. 7 (2005): E212. http://dx.doi.org/10.1149/1.1921850.

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33

Hinatsu, James T., and Frank R. Foulkes. "Diffusion Coefficients for Copper (II) in Aqueous Cupric Sulfate‐Sulfuric Acid Solutions." Journal of The Electrochemical Society 136, no. 1 (January 1, 1989): 125–32. http://dx.doi.org/10.1149/1.2096571.

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34

Danzer, Gerald D., and James R. Kincaid. "Resonance Raman spectra of Ru(bpz) 32+ in aqueous sulfuric acid solutions." Journal of Raman Spectroscopy 23, no. 12 (December 1992): 681–89. http://dx.doi.org/10.1002/jrs.1250231205.

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35

Yoshida, Masafumi, Noriyuki Sakamoto, Kimiyoshi Ikemi, and Shizuo Arichi. "Solution Properties of Poly(4-vinylpyridine) in Aqueous Solutions of Sulfuric Acid." Bulletin of the Chemical Society of Japan 65, no. 11 (November 1992): 3108–11. http://dx.doi.org/10.1246/bcsj.65.3108.

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36

Lisitsyn, Yu A., and A. V. Sukhov. "Electrochemical amination. synthesis of aniline in aqueous–acetonitrile solutions of sulfuric acid." Russian Journal of Electrochemistry 51, no. 11 (November 2015): 1092–95. http://dx.doi.org/10.1134/s1023193515110099.

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37

Vielma, Tuomas, Lubomir Hnedkovsky, and Glenn Hefter. "Chemical speciation effects on the volumetric properties of aqueous sulfuric acid solutions." Journal of Chemical Thermodynamics 158 (July 2021): 106408. http://dx.doi.org/10.1016/j.jct.2021.106408.

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38

Markovic, Smiljana, Novica Rakicevic, and Djuro Misljenovic. "The temperature dependence of the disproportionation reaction of iodous acid in aqueous sulfuric acid solutions." Journal of the Serbian Chemical Society 67, no. 5 (2002): 347–51. http://dx.doi.org/10.2298/jsc0205347m.

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The aim of this work was to examine the disproportionation reaction of iodous acid, HOIO, in aqueous 0.18 mol/dm3H2SO4 solution, by spectrophotometric measurements of the absorbance. The absorbing HgI+-ion species were generated during the observed disproportionation process. The specific rate constants of disproportionation were calculated in the temperature range from 12 to 30 ?C. The average values ranged from 1.20 to 2.94 mol-1dm3 s-1, respectively. In addition, the values of the activation energies were determined by a graphical method. An average value of 71.20 kJ/mol was found for the chosen temperature interval.

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39

Maynard-Casely, Helen E., Helen E. A. Brand, and Kia S. Wallwork. "Structure and thermal expansion of sulfuric acid octahydrate." Journal of Applied Crystallography 45, no. 6 (October 10, 2012): 1198–207. http://dx.doi.org/10.1107/s0021889812037752.

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Synchrotron X-ray powder diffraction has been used to structurally characterize crystallization products from 37.8 and 40.5 wt% aqueous sulfuric acid solutions. It is confirmed that, despite speculation in the literature, the structure that predominately crystallized from these solutions is sulfuric acid octahydrate (SAO). The existence of an uncharacterized phase is also noted. It was found that existing models proposed for the crystal structure of SAO did not satisfactorily fit to the data acquired here, and hence a new structure solution was sought. It is reported here that the structure of SAO is contained within a unit cell withI2 symmetry witha= 7.44247 (11),b= 7.4450 (1),c= 26.1168 (3) Å, β = 125.0428 (7)°,V= 1184.78 (3) Å3at 80 K. Data were collected at temperatures between 80 and 198 K, which enabled determination of the thermal expansion of SAO.

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40

Gonçalves, Reinaldo Simões, and Roni Fábio Dalla Costa. "Electrochemical evidence of the influence of light on the corrosion processes of low-carbon steel in diluted sulfuric acid." Ciência e Natura 15, no. 15 (December 13, 1993): 35. http://dx.doi.org/10.5902/2179460x26356.

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Two different electrochemical methods confirm the influence of ligth on the anodic current values observad when low carbon steel electrodes were polarizad in deaerated 1.0 N H2SO4 solutions in the anodic potential range. The highest density values were obtained when the system is under illumination. The effect of natural illumination conditions on the weigh-loss experiments in aerated 1.0 N H2SO4, confirms that the corrosion rate is higher in an illuminated medium than in the dark.

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41

Zhang, Runhu, Hongzhu Ma, and Bo Wang. "Removal of Chromium(VI) from Aqueous Solutions Using Polyaniline Doped with Sulfuric Acid." Industrial & Engineering Chemistry Research 49, no. 20 (October 20, 2010): 9998–10004. http://dx.doi.org/10.1021/ie1008794.

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42

Krissmann, J., M. A. Siddiqi, and K. Lucas. "Absorption of sulfur dioxide in dilute aqueous solutions of sulfuric and hydrochloric acid." Fluid Phase Equilibria 141, no. 1-2 (December 1997): 221–33. http://dx.doi.org/10.1016/s0378-3812(97)00203-3.

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43

Boyd, Mary K., Ho Yin Lai, and Keith Yates. "Water quenching behavior of excited 9-xanthylium cations in aqueous sulfuric acid solutions." Journal of the American Chemical Society 113, no. 19 (September 1991): 7294–300. http://dx.doi.org/10.1021/ja00019a029.

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44

Das, Kaushik. "Single ion activities in aqueous sulfuric acid solutions: A new extra-thermodynamic assumption." Journal of Solution Chemistry 17, no. 4 (April 1988): 327–36. http://dx.doi.org/10.1007/bf00650413.

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45

Al-Owais, A. A., and I. S. El-Hallag. "Voltammetric and chronoamperometric studies of aniline electropolymerization in different aqueous sulfuric acid solutions." Polymer Bulletin 76, no. 9 (November 17, 2018): 4571–84. http://dx.doi.org/10.1007/s00289-018-2610-9.

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46

MacHardy, S. J., and L. J. J. Janssen. "The diffusion coefficient of Cu(II) ions in sulfuric acid–aqueous and methanesulfonic acid–methanol solutions." Journal of Applied Electrochemistry 34, no. 2 (February 2004): 169–74. http://dx.doi.org/10.1023/b:jach.0000009956.75577.ef.

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47

Kish, J. R., M. B. Ives, and J. R. Rodda. "Corrosion Mechanism of Nickel-Containing Stainless Steels in Concentrated Aqueous Solutions of Sulfuric Acid." CORROSION 60, no. 6 (June 2004): 523–37. http://dx.doi.org/10.5006/1.3287756.

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48

Lisitsyn, Yu A., and A. V. Sukhov. "Electrochemical Amination. Selective Functionalization of para- and ortho-Anisidines in Aqueous Sulfuric Acid Solutions." Russian Journal of Electrochemistry 54, no. 12 (December 2018): 1294–97. http://dx.doi.org/10.1134/s102319351813027x.

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49

Lotnik, S. V., L. A. Khamidullina, and V. P. Kazakov. "Temperature Quenching of Uranyl Ion Photoluminescence in Frozen Deuterated Aqueous Solutions of Sulfuric Acid." High Energy Chemistry 38, no. 5 (September 2004): 323–29. http://dx.doi.org/10.1023/b:hiec.0000041343.46247.4d.

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50

Lisitsyn, Yu A., and Yu M. Kargin. "Electrochemical Amination of Benzene in Aqueous Solutions of Sulfuric Acid and an Organic Solvent." Russian Journal of Electrochemistry 39, no. 12 (December 2003): 1279–85. http://dx.doi.org/10.1023/b:ruel.0000009092.47297.5a.

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