Pure and Applied Chemistry

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• Pratt Kenneth W.: Measurement of pHT values of Tris buffers in artificial seawater at varying mole ratios of Tris:Tris·HCl. Marine Chemistry 2014, 162, 89. <http://dx.doi.org/10.1016/j.marchem.2014.03.003>
• Shibata Manabu, Kato Makoto, Iwamoto Yasukazu, Nomura Satoshi, Kakiuchi Takashi: Potentiometric determination of pH values of dilute sulfuric acid solutions with glass combination electrode equipped with ionic liquid salt bridge. Journal of Electroanalytical Chemistry 2013, 705, 81. <http://dx.doi.org/10.1016/j.jelechem.2013.07.024>
• Waters Jason F., Millero Frank J.: The free proton concentration scale for seawater pH. Marine Chemistry 2013, 149, 8. <http://dx.doi.org/10.1016/j.marchem.2012.11.003>
• Pires M. José R. G. R., Ferra M. Isabel A., Marques Albertina M.: Ionization of Acid Orange 7 in Various Ionic Media. J. Chem. Eng. Data 2013, 58, 2181. <http://dx.doi.org/10.1021/je400466m>
• Padr� Juan M., Acquaviva Agust�n, Tascon Marcos, Gagliardi Leonardo G., Castells Cecilia B.: Effect of temperature and solvent composition on acid dissociation equilibria, I: Sequenced determination of compounds commonly used as buffers in high performance liquid chromatography coupled to mass spectroscopy detection. Analytica Chimica Acta 2012, 725, 87. <http://dx.doi.org/10.1016/j.aca.2012.03.015>
• Roy Lakshmi N., Roy Rabindra N., Allen Kathleen A., Mehrhoff Casey J., Henson Isaac B., Stegner Jessica M.: Buffer standards for the physiological pH of the zwitterionic compound of 3-(N-morpholino)propanesulfonic acid (MOPS) from T=(278.15 to 328.15)K. K J CHEM THERMODYN 2012, 47, 21. <http://dx.doi.org/10.1016/j.jct.2011.09.010>
• Roy Rabindra N., Roy Lakshmi N., Henson Isaac B., Stegner Jessica M., Dinga John J., Summers Clark E., Suhrheinrich Gregory L., Veliz Jaime A., Dieterman Lauren A.: Buffer standards for the physiological pH of N-[2-hydroxy-1,1-bis(hydroxymethyl)ethyl]glycine (TRICINE) from T=(278.15 to 328.15)K. The Journal of Chemical Thermodynamics 2012, 52, 11. <http://dx.doi.org/10.1016/j.jct.2012.02.019>
• Pires M. José R.G.R., Ferra M. Isabel A., Marques Albertina M.M.: Ionization of methyl orange in aqueous sodium chloride solutions. The Journal of Chemical Thermodynamics 2012, 53, 93. <http://dx.doi.org/10.1016/j.jct.2012.04.023>
• Baeza-Baeza Juan J., García-Álvarez-Coque M. Celia: Systematic Approach for Calculating the Concentrations of Chemical Species in Multiequilibrium Problems: Inclusion of the Ionic Strength Effects. J. Chem. Educ. 2012, 89, 900. <http://dx.doi.org/10.1021/ed200594u>
• Fraenkel Dan: Electrolytic Nature of Aqueous Sulfuric Acid. 2. Acidity. J. Phys. Chem. B 2012, 116, 11678. <http://dx.doi.org/10.1021/jp306042q>
• Spitzer Petra, Pratt Kenneth W.: The history and development of a rigorous metrological basis for pH measurements. J Solid State Electrochem 2011, 15, 69. <http://dx.doi.org/10.1007/s10008-010-1106-9>
• Kakiuchi Takashi: Salt bridge in electroanalytical chemistry: past, present, and future. J Solid State Electrochem 2011, 15, 1661. <http://dx.doi.org/10.1007/s10008-011-1373-0>
• Ferse Armin, Müller Hans-Otfried: Factorizing of a concentration function for the mean activity coefficients of aqueous strong electrolytes into individual functions for the ionic species. J Solid State Electrochem 2011, 15, 2149. <http://dx.doi.org/10.1007/s10008-011-1413-9>
• Zapała Lidia: Potentiometric Studies on the Equilibria of Flufenamic Acid in Aqueous Solutions and in Two-phase Organic Solvent + Water Systems. J Solution Chem 2011, 40, 198. <http://dx.doi.org/10.1007/s10953-010-9642-6>
• Stoica Daniela, Yardin Catherine, Ebrard Géraldine, Vaslin-Reimann Sophie, Fisicaro Paola: Evaluation of the Standard Potential of the Ag/AgCl Electrode in a 50 wt-% Water–Ethanol Mixture. J Solution Chem 2011, 40, 1819. <http://dx.doi.org/10.1007/s10953-011-9758-3>
• Marion G.M., Millero F.J., Camões M.F., Spitzer P., Feistel R., Chen C.-T.A.: pH of seawater. Mar Chem 2011, 126, 89. <http://dx.doi.org/10.1016/j.marchem.2011.04.002>
• Ferra M. Isabel A., Graça Joaquim R., Marques Albertina M. M.: Ionization of Acetic Acid in Aqueous Potassium Chloride Solutions. J Chem Engg Data 2011, 56, 3673. <http://dx.doi.org/10.1021/je200584a>
• Roy Lakshmi N., Roy Rabindra N., Wollen Joshua T., Harmon Meagan A., Stegner Jessica M., Shah Ankita A., Henson Isaac B.: Buffer Standards for the Biological pH of the Amino Acid N-[2-Hydroxyethyl]piperazine-N′-[3-propanesulfonic acid], HEPPS, From (278.15 to 328.15) K. J Chemical & Engineering Data 2011, 56, 4126. <http://dx.doi.org/10.1021/je200629y>
• Fraenkel Dan: Effect of Solvent Permittivity on the Thermodynamic Behavior of HCl Solutions: Analysis Using the Smaller-Ion Shell Model of Strong Electrolytes. Chem B 2011, 115, 14634. <http://dx.doi.org/10.1021/jp207878f>
• Haya Luisa, Sayago Francisco J., Mainar Ana M., Cativiela Carlos, Urieta José S.: Quantum-chemical predictions of redox potentials of carbamates in methanol. PCCP 2011, 13, 17696. <http://dx.doi.org/10.1039/c1cp21576k>
• Bates Roger G.: Acidity Functions in Aqueous and Nonaqueous Media. Bull Soc Chim Belges 2010, 84, 1139. <http://dx.doi.org/10.1002/bscb.19750841201>
• Partanen J. I., Salmimies R. K., Partanen L. J., Louhi-Kultanen M.: Prediction of Activity Coefficients for Uni-univalent Electrolytes in Pure Aqueous Solution. Chem Eng Technol 2010, 33, 730. <http://dx.doi.org/10.1002/ceat.200900617>
• Spitzer Petra, Seitz Steffen: Metrological traceability chain for pH measurement results. MAPAN 2010, 25, 191. <http://dx.doi.org/10.1007/s12647-010-0019-5>
• Spitzer Petra, Fisicaro Paola, Seitz Steffen, Champion Rachel: pH and electrolytic conductivity as parameters to characterize bioethanol. Accred Qual Assur 2009, 14, 671. <http://dx.doi.org/10.1007/s00769-009-0565-0>
• Roy Rabindra N., Roy Lakshmi N., Ashkenazi Shahaf, Wollen Joshua T., Dunseth Craig D., Fuge Michael S., Durden Jared L., Roy Chandra N., Hughes Hannah M., Morris Brett T.: Buffer Standards for pH Measurement of N-(2-Hydroxyethyl)piperazine-N′-2-ethanesulfonic Acid (HEPES) for I=0.16 mol⋅kg−1 from 5 to 55 °C. J Solution Chem 2009, 38, 449. <http://dx.doi.org/10.1007/s10953-009-9378-3>
• Ferra M. I. A., Graça J. R., Marques A. M. M.: Application of the Pitzer Model to Assignment of pH to Phthalate Standard Buffer Solutions. J Solution Chem 2009, 38, 1433. <http://dx.doi.org/10.1007/s10953-009-9421-4>
• Roy Rabindra N., Roy Lakshmi N., Denton Cole E., LeNoue Sean R., Dunseth Craig D., Fuge Michael S., Ashkenazi Shahaf, Durden Jared L., Roy Chandra N., Wollen Joshua T.: Buffer Standards for the Physiological pH of the Zwitterionic Compound, HEPPSO from 5 to 55 °C. J Solution Chem 2009, 38, 1417. <http://dx.doi.org/10.1007/s10953-009-9442-z>
• Roy Rabindra N., Roy Lakshmi N., Denton Cole E., LeNoue Sean R., Fuge Michael S., Dunseth Craig D., Durden Jared L., Roy Chandra N., Bwashi Adonis, Wollen Joshua T., DeArmon Samantha J.: Buffer Standards for the Physiological pH of 3-[(1,1-Dimethyl-2-hydroxymethyl)amino]-2-hydroxypropanesulfonic Acid from (278.15 to 328.15) K†. J. Chem. Eng. Data 2009, 54, 428. <http://dx.doi.org/10.1021/je8004563>
• Máriássy Michal, Pratt Kenneth W, Spitzer Petra: Major applications of electrochemical techniques at national metrology institutes. Metrologica 2009, 46, 199. <http://dx.doi.org/10.1088/0026-1394/46/3/007>
• Kohonen Jarno, Qu Haiyan, Hatakka Henry, Alatalo Hannu, Reinikainen Satu-Pia, Louhi-Kultanen Marjatta, Kallas Juha: In-line monitoring of reactive crystallization process based on ATR-FTIR and Raman spectroscopy. J Chemometrics 2008, 22, 644. <http://dx.doi.org/10.1002/cem.1161>
• Box Karl J., Völgyi Gergely, Ruiz Rebeca, Comer John E., Takács-Novák Krisztina, Bosch Elisabeth, Ràfols Clara, Rosés Martí: Physicochemical Properties of a New Multicomponent Cosolvent System for the pKa Determination of Poorly Soluble Pharmaceutical Compounds. HCA 2007, 90, 1538. <http://dx.doi.org/10.1002/hlca.200790161>
• Prenesti Enrico, Fisicaro Paola, Berto Silvia, Ferrara Enzo, Daniele Pier Giuseppe: Monitoring the traceability of the pH of a primary tetraborate buffer: comparison of results from primary and secondary apparatus. Anal Bioanal Chem 2007, 387, 2595. <http://dx.doi.org/10.1007/s00216-007-1117-2>
• Guiomar M. J., Lito H. M., Camões M. Filomena, Viçoso Catarina M.: Improving the quality of potentiometric pH measurements. Accred Qual Assur 2007, 12, 447. <http://dx.doi.org/10.1007/s00769-007-0296-z>
• Falciola Luigi, Mussini Patrizia R., Mussini Torquato, Rossi Manuela: A Determination of Standard Potentials and Related Primary pH Standards in the 50 Mass Percent (N-Methyl-2-Pyrrolidinone + Water) Mixture at Various Temperatures. J Solution Chem 2007, 36, 1037. <http://dx.doi.org/10.1007/s10953-007-9162-1>
• Pratt Kenneth W., Duewer David L.: Visualization technique for uncertainty budgets: Onion charts. Accred Qual Assur 2006, 10, 527. <http://dx.doi.org/10.1007/s00769-005-0035-2>
• Lito M.J. Guiomar H.M., Camões M. Filomena, Viçoso Catarina M.: Effect of condensation phenomena on potentiometric measurements. Analytica Chimica Acta 2006, 575, 45. <http://dx.doi.org/10.1016/j.aca.2006.05.078>
• Wilczek-Vera Grazyna, Rodil Eva, Vera Juan H.: A complete discussion of the rationale supporting the experimental determination of individual ionic activities. Fluid Phase Equilb 2006, 244, 33. <http://dx.doi.org/10.1016/j.fluid.2006.03.011>
• Partanen Jaakko I., Covington Arthur K.: Re-evaluation of the First and Second Stoichiometric Dissociation Constants of Phthalic Acid at Temperatures from (0 to 60) °C in Aqueous Phthalate Buffer Solutions with or without Potassium Chloride. 1. Estimation of the Parameters for the Hückel Model Activity Coefficient Equations for Calculation of the Second Dissociation Constant. J Chemical & Engineering Data 2006, 51, 777. <http://dx.doi.org/10.1021/je0504921>
• Fisicaro Paola, Ferrara Enzo, Prenesti Enrico, Berto Silvia: Role of the activity coefficient in the dissemination of pH: comparison of primary (Harned cell) and secondary (glass electrode) measurements on phosphate buffer considering activity and concentration scales. Anal Bioanal Chem 2005, 383, 341. <http://dx.doi.org/10.1007/s00216-005-3417-8>
• Wilczek-Vera Grazyna, Vera Juan H.: On the measurement of individual ion activities. Fluid Phase Equilb 2005, 236, 96. <http://dx.doi.org/10.1016/j.fluid.2005.05.021>
• Vera Guillem, Hidalgo Ana, Climent Miguel Angel, Andrade Carmen, Alonso Cruz: Chloride-Ion Activities in Simplified Synthetic Concrete Pore Solutions: The Effect of the Accompanying Ions. J Amer Ceram Soc 2004, 83, 640. <http://dx.doi.org/10.1111/j.1151-2916.2000.tb01245.x>
• Liljenzin J.‐O., Mesmin C.: Determination of H₂TPTZ₂ ²⁺ Stability Constant by TPTZ Solubility in Nitric Acid. Sol Extr Ion Exch 2003, 21, 783. <http://dx.doi.org/10.1081/SEI-120025922>
• Antonini D, Falciola L, Mussini P.R, Mussini T: Medium effects, comparability and predictability of pH-standards in aqueous+organic solvent mixtures: behavior of the (ethylene carbonate+water) and (propylene carbonate+water) systems. Journal of Electroanalytical Chemistry 2001, 503, 153. <http://dx.doi.org/10.1016/S0022-0728(01)00345-X>
• de Mendonça António J.G., Vaz Margarida I.P.M., de Mendonça Dina I.M.D.: Activity coefficients in the evaluation of food preservatives. Innovative Food Science and Emerging Technology 2001, 2, 175. <http://dx.doi.org/10.1016/S1466-8564(01)00037-6>
• Tishchenko P. Ya.: Standardization of pH measurements based on the ion interaction approach. Russ Chem Bull 2000, 49, 680. <http://dx.doi.org/10.1007/BF02495481>
• Barták Petr, Pěchová Danuše, Tarkowski Petr, Bednář Petr, Kotouček Milan, Stránský Zdeněk, Vespalec Radim: Determination of the first dissociation constant of 6-benzylaminopurine. Analytica Chimica Acta 2000, 421, 221. <http://dx.doi.org/10.1016/S0003-2670(00)01037-0>
• Nazari K., Moosavi-Movahedi A.A.: Potentiometric titration and enthalpy evaluation of horseradish peroxidase in the presence of n-dodecyl trimethylammonium bromide. Colloids Surface B 2000, 18, 63. <http://dx.doi.org/10.1016/S0927-7765(99)00127-7>
• Partanen Jaakko I., Minkkinen Pentti O.: Equations for calculation of the pH of buffer solutions containing sodium or potassium dihydrogen phosphate, sodium hydrogen phosphate, and sodium chloride at 25°C. J Solution Chem 1997, 26, 709. <http://dx.doi.org/10.1007/BF02767623>
• Richter W, Dube G: Measurement standards and the general problem of reference points in chemical analysis. Metrologica 1997, 34, 13. <http://dx.doi.org/10.1088/0026-1394/34/1/3>
• Bosch Elisabeth, Ràfols Clara, Rosés Martí: Variation of acidity constants and pH values of some organic acids in water—2-propanol mixtures with solvent composition. Effect of preferential solvation. Analytica Chimica Acta 1995, 302, 109. <http://dx.doi.org/10.1016/0003-2670(94)00435-O>
• Rondinini S., Mussini P.R., Vertova A., Bortoluzzi A., Bono L., Longhi P.: A new, long-lived Ca-selective electrode. Actuat B 1995, 23, 27. <http://dx.doi.org/10.1016/0925-4005(94)01514-I>
• Covington A. K., Ferra M. I. A.: A pitzer mixed electrolyte solution theory approach to assignment of pH to standard buffer solutions. J Solution Chem 1994, 23, 1. <http://dx.doi.org/10.1007/BF00972604>
• Ràfols Clara, Rosés Martí, Bosch Elisabeth: Standardization of potentiometric cells in propan-2-ol-water. Analytica Chimica Acta 1993, 280, 75. <http://dx.doi.org/10.1016/0003-2670(93)80244-F>
• Dickson Andrew G.: The measurement of sea water pH. Mar Chem 1993, 44, 131. <http://dx.doi.org/10.1016/0304-4203(93)90198-W>
• Millero Frank J, Zhang Jia-Zhong, Fiol Sarah, Sotolongo Sara, Roy Rabindra N, Lee Kitack, Mane Sanjay: The use of buffers to measure the pH of seawater. Mar Chem 1993, 44, 143. <http://dx.doi.org/10.1016/0304-4203(93)90199-X>
• Bagg J.: Temperature and salinity dependence of seawater-KCl junction potentials. Mar Chem 1993, 41, 337. <http://dx.doi.org/10.1016/0304-4203(93)90265-P>
• Grigera J.Raul: Water and electrolyte solutions concentration and activity. Life Sci Oxford 1992, 50, 1567. <http://dx.doi.org/10.1016/0024-3205(92)90443-S>
• Mussini Torquato, Longhi Paolo, Marcolungo Irene, Mussini Patrizia R., Rondinini Sandra: Status and problems of standardization of pH scales for controls in different media. Reference value standards in ethylene glycol/water mixed solvents. Fresenius J Anal Chem 1991, 339, 608. <http://dx.doi.org/10.1007/BF00325546>
• Bagg John: Computer calculation of liquid-junction potentials—II. Junction potentials for junctions with concentrated KCl. Electrochimica Acta 1990, 35, 367. <http://dx.doi.org/10.1016/0013-4686(90)87012-Q>
• White D.Richard: Standard potential of the silver-silver chloride electrode and mean activity coefficient of hydrochloric acid in 10 wt% sucrose/water from 0 to 25°C. Food Chem 1990, 37, 1. <http://dx.doi.org/10.1016/0308-8146(90)90039-7>
• H.M. Lito M.J.Guiomar, G.F.C. Camões M.Filomena, Ferra M.Isabel A., Covington Arthur K.: Calculation of reference pH values for standard solutions from the corresponding acid dissociation constants. Analytica Chimica Acta 1990, 239, 129. <http://dx.doi.org/10.1016/S0003-2670(00)83843-X>
• Mussini T., Mazza F.: Medium effects as key electrochemical variables for corrosion and electrochemistry studies in non-aqueous and mixed solvents. Electrochimica Acta 1987, 32, 855. <http://dx.doi.org/10.1016/0013-4686(87)87074-3>
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• Covinton A.K., Rebelo M.J.F.: Determination of pH values over the temperature range –60°C for some operational reference standard solutins and values of the conventional residual liquid-junction potentials. Analytica Chimica Acta 1987, 200, 245. <http://dx.doi.org/10.1016/S0003-2670(00)83773-3>
• Longhi P., Mussini P.R., Mussini T., Rondinini S.: Evaluating membrane cell e.m.f.ś from different schems of integration of the relevant nernstian equations. J Membr Sci 1987, 34, 345. <http://dx.doi.org/10.1016/S0376-7388(00)83174-9>
• Roy Rabindra N., Gibbons James J., McGinnis Timothy, Woodmansee Ray: Standard electromotive force of the H2-AgCl;Ag cell in 30, 40, and 50 mass% glycerol/water from −20 to 25 °C: pK2 and pH values for a standard “Mops” buffer in 50 mass% glycerol/water. Crybiology 1985, 22, 578. <http://dx.doi.org/10.1016/0011-2240(85)90035-5>
• Roy Rabindra N., Gibbons James J., Baker Gigi E.: Acid dissociation constants and pH values for standard “bes” and “tricine” buffer solutions in 30, 40, and 50 mass% dimethyl sulfoxide/water between 25 and −25 °C. Crybiology 1985, 22, 589. <http://dx.doi.org/10.1016/0011-2240(85)90036-7>
• Covington A.K., Ferra M.I.A., Zou Z-Y.: Application of multilinear regression analysis to the evaluation of standard pH values for potassium hydrogen phthalate reference value standard solutions at temperatures up to 498 K. Electrochimica Acta 1985, 30, 805. <http://dx.doi.org/10.1016/0013-4686(85)80131-6>
• Mussini Torquato, Longhi Paolo, Rondinini Sandra, Tettamanti Michele, Covington Arthur K.: Reference value standards for pH measurements in 5, 15 and 30% (w/w) acetonitrile/water solvent mixtures at temperatures from 288.15 to 308.15 K. Analytica Chimica Acta 1985, 174, 331. <http://dx.doi.org/10.1016/S0003-2670(00)84395-0>
• Roy Rabindra N., Gibbons James J., Baker Gigi, Bates Roger G.: Standard electromotive force of the H2AgCl;Ag cell in 30, 40, and 50 mass% dimethyl sulfoxide/water from −20 to 25 °C: pK2 and pH values for a standard “Bicine” buffer solution at subzero temperatures. Crybiology 1984, 21, 672. <http://dx.doi.org/10.1016/0011-2240(84)90227-X>
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