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Journal articles on the topic 'Potentiometric titration'

Author: Grafiati

Published: 4 June 2021

Last updated: 18 February 2022

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1

Gibson, Graham, Alexei A. Neverov, and R. S. Brown. "Potentiometric titration of metal ions in methanol." Canadian Journal of Chemistry 81, no. 6 (June 1, 2003): 495–504. http://dx.doi.org/10.1139/v03-035.

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The potentiometric titrations of nine lanthanideIII triflates, ZnII and CuII triflate, and the NiII, CoII, MgII, and TiIV perchlorates were obtained in methanol to determine the titration constants (defined as the sspH at which the [OCH3]/[Mx+]t ratios are 0.5 and 1.5) as well as the apparent sspKa values for deprotonation of the metal-bound solvent molecules. The titrations were performed under various conditions with and without added salts as electrolytes, and the variations in the titration constants are discussed. In selected cases (La3+, Zn2+) the titration profiles were analyzed using a complex fitting program to obtain information about the species present in solution.Key words: potentiometric titration, methanol, sspH, metal ion, lanthanides, apparent sspKa.

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2

Денисов, О. С., and Е. Н. Корчуганова. "ПОТЕНЦИОМЕТРИЧЕСКОЕ ТИТРОВАНИЕ СОЛЕЙ ЦИНКА." Труды БГТУ Серия 2, № 1, no. 1 (241) 2021 (February 12, 2021): 24–29. http://dx.doi.org/10.52065/2520-2669-2021-241-1-24-29.

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3

Zhang, Lina, Toshiyuki Takematsu, and Takashi Norisuye. "Potentiometric titration of xanthan." Macromolecules 20, no. 11 (November 1987): 2882–87. http://dx.doi.org/10.1021/ma00177a041.

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4

Price, Randi, and Ping Wan. "Determination of Quaternary Ammonium Compounds by Potentiometric Titration with an Ionic Surfactant Electrode: Single-Laboratory Validation." Journal of AOAC INTERNATIONAL 93, no. 5 (September 1, 2010): 1542–52. http://dx.doi.org/10.1093/jaoac/93.5.1542.

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Abstract A potentiometric titration for determining the quaternary ammonium compounds (QAC) commonly found in antimicrobial products was validated by a single laboratory. Traditionally, QACs were determined by using a biphasic (chloroform and water) manual titration procedure. Because of safety considerations regarding chloroform, as well as the subjectivity of color indicator-based manual titration determinations, an automatic potentiometric titration procedure was tested with quaternary nitrogen product formulations. By using the Metrohm Titrando system coupled with an ionic surfactant electrode and an Ag/AgCl reference electrode, titrations were performed with various QAC-containing formulation products/matrixes; a standard sodium lauryl sulfate solution was used as the titrant. Results for the products tested are sufficiently reproducible and accurate for the purpose of regulatory product enforcement. The robustness of the method was measured by varying pH levels, as well as by comparing buffered versus unbuffered titration systems. A quantitation range of 11000 ppm quaternary nitrogen was established. Eight commercially available antimicrobial products covering a variety of matrixes were assayed; the results obtained were comparable to those obtained by the manual titration method. Recoveries of 94 to 104% were obtained for spiked samples.

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5

Gündüz, Turgut, Esma Kiliç, Güleren Özkan, Muhammed F. Awaad, and Mustafa Tastekin. "Conductimetric and potentiometric investigation of effect of acidity on formation of homoconjugates in acetonitrile solvent." Canadian Journal of Chemistry 68, no. 5 (May 1, 1990): 674–78. http://dx.doi.org/10.1139/v90-103.

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In the present work, 11 aromatic and nine aliphatic carboxylic acids, namely benzoic, 2-nitrobenzoic, 3-nitrobenzoic, 4-nitrobenzoic, 2,4-dinitrobenzoic, 3,5-dinitrobenzoic, 2-aminobenzoic, 3-aminobenzoic, 4-aminobenzoic, o-phthalic, salicylic, formic, acetic, monochloroacetic, dichloroacetic, trichloroacetic, propionic, n-butyric, caprylic, and myristic acids, were titrated conductimetrically and potentiometrically with triethylamine in acetonitrile solvent, under a nitrogen atmosphere, at 25 °C. Closer investigation of the conductimetric titration curves of these acids showed that the acidity of an acid, rather than the basicity of its conjugate base, plays a major part in the formation of homoconjugate ions, at least in acetonitrile solvent. If the acid is strong enough, there is a maximum before the experimental end point at about the half-neutralization point. To determine the minimum strength for an acid to show this maximum before the end point, all acids were also titrated potentiometrically. It was found that those acids which have half-neutralization potentials over −85 mV give a strong homoconjugation reaction and show a maximum before the experimental end point. Moreover, the acids that show maxima before the experimental end point in the conductimetric titration also show rather well-shaped potentiometric titration curves. Keywords: nonaqueous media, conductimetric titrations, potentiometric titrations, titration in acetonitrile, acidity and homoconjugation.

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6

Al-Ghannam, Sheikha M., Abdalla M. S. Abulkibash, and Abeer M. Al-Olyyan. "Differential Electrolytic Potentiometric Determination of Some Amino Acids in Dosage Forms." Journal of AOAC INTERNATIONAL 87, no. 3 (May 1, 2004): 671–76. http://dx.doi.org/10.1093/jaoac/87.3.671.

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Abstract The application of direct-current differential electrolytic potentiometry to the nonaqueous titration of amino acids was investigated. The basic character of amino acids in acetic acid was enhanced to permit their direct titration with perchloric acid. A pair of antimony electrodes was used as an indicating system. The shapes of the titration curves obtained were almost symmetrical with sharp peaks. The optimum current density for those titrations was found to be 1–2 μA/cm2. The procedure was applied successfully to the determination of certain amino acids in drug formulations, and the results were favorably compared statistically with those obtained by official methods.

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7

Khil’ko, S. L., A. I. Kovtun, and V. I. Rybachenko. "Potentiometric titration of humic acids." Solid Fuel Chemistry 45, no. 5 (October 2011): 337–48. http://dx.doi.org/10.3103/s0361521911050028.

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8

Soldatov, V. S. "Potentiometric titration of ion exchangers." Reactive and Functional Polymers 38, no. 2-3 (November 1998): 73–112. http://dx.doi.org/10.1016/s1381-5148(98)00018-2.

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9

Shul’ga, N. V., L. A. Gomolko, and N. P. Krut’ko. "Potentiometric titration of lignosulfonic acids." Russian Journal of Applied Chemistry 81, no. 7 (July 2008): 1278–82. http://dx.doi.org/10.1134/s107042720807029x.

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10

Pezzatini, G., G. Loglio, and S. Becagli. "Potentiometric titration of diprotic systems." Fresenius' Journal of Analytical Chemistry 358, no. 4 (June 17, 1997): 465–70. http://dx.doi.org/10.1007/s002160050447.

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11

Ciesielski, Witold, and Robert Zakrzewski. "Potentiometric Titration of 2-Thiouracils." Archiv der Pharmazie 331, no. 11 (November 1998): 371–72. http://dx.doi.org/10.1002/(sici)1521-4184(199811)331:11<371::aid-ardp371>3.0.co;2-z.

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12

Prasad, S., V. D. Leite, R. A. C. Santana, and E. A. Medeiros. "Electrometric studies on formation of cerium vanadates as a function of pH." Eclética Química 31, no. 2 (2006): 31–38. http://dx.doi.org/10.1590/s0100-46702006000200005.

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The precise nature of the reaction between nitric acid and sodium ortho-vanadate solutions has been studied by means of electrometric techniques involving potentiometric and conductometric titrations. The well defined inflections and breaks in the titration curves confirm the existence of the anions, pyro-V2O7(4-), meta-VO3- and poly-H2V10O28(4-) corresponding to the ratios of VO4(3-):H+ as 1:1, 1:2 and 1:2.6 in the neighborhood of pH 10.5, 7.4 and 3.6, respectively. The interaction of cerium(III) nitrate with sodium vanadate solutions, at specific pH levels 12.4, 10.5, 7.4 and 3.6 was also studied by potentiometric and conductometric titrations between the reactants. The end-points obtained from the sharp inflections in the titration curves provide definite evidence for the formation and precipitation of cerium ortho-Ce2O3.V2O5, pyro-2Ce2O3.3V2O5 and meta-Ce2O3.3V2O5 vanadates in the neighborhood of pH 7.4, 6.2 and 4.8, respectively. Analytical investigations on the precipitates formed confirm the results of the electrometric study.

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13

Sołtysik, Barbara. "A quick method to determine the content of sulfates in silicic and aluminosilicate fillers." Polish Journal of Chemical Technology 9, no. 1 (January 1, 2007): 33–35. http://dx.doi.org/10.2478/v10026-007-0009-8.

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A quick method to determine the content of sulfates in silicic and aluminosilicate fillers The paper presents the possibility of using barium-selective electrode to a potentiometric determination of sulfates in silicic and aluminosilicate fillers. The results of sulfates potentiometric titration in silicic and aluminosilicate fillers are described. A statistical interpretation of the results was carried out. The recommended method is based on the end-point detection of sulfates potentiometric titration in hydro-alcoholic medium by means of barium chlorate(VII) titrant. The potentiometric titration, which uses an ion-selective electrode as the indicator for the end-point was applied as the analytical technique. The parameter ranges for accurate sulfates determination in model solutions and the method of samples' preparation for analysis were investigated.

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14

Besenhard, J. O., H. P. Gansmann, and H. Meyer. "Bestimmung von Oberflächenoxiden auf Rußen durch potentiometrische Direkttitration in nichtwäßrigen Lösungsmitteln / Determination of Surface Oxides on Carbon Blacks by Direct Potentiometric Titration in Non-Aqueous Solvents." Zeitschrift für Naturforschung B 45, no. 6 (June 1, 1990): 857–63. http://dx.doi.org/10.1515/znb-1990-0617.

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An attempt is made to quantitatively determine acidic and basic surface oxides on carbon blacks and also to monitor their acid and base strength distribution by direct potentiometric titrations in non-aqueous media.In contrast to direct titration procedures proposed so far, our method allows to distinguish clearly between several types of acidic surface oxides of different acid strength. This is mainly achieved by improvements of the non-aqueous titration media. The total contents of weakly and strongly acidic and also of basic oxides determined by this very fast method is comparable to results obtained by slow and laborious indirect titrations.

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15

Mustafa, S., A. Naeem, N. Rehana, and H. Y. Samad. "Cation-Exchange Properties of Aluminium(III) Phosphate." Adsorption Science & Technology 13, no. 4 (August 1996): 261–79. http://dx.doi.org/10.1177/026361749601300404.

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Potentiometric titrations of aluminium(III) phosphate have been performed in the presence of aqueous electrolyte solutions containing Cu2+, Zn2+, Ni2+ and K+ ions as a function of the concentration of the latter, the pH and the temperature. The sorption of Zn2+ ions has also been studied and the data for metal ion sorption shown to correlate with the Potentiometric titration data, indicating that the process responsible for metal ion uptake is ion exchange. The pKa value of the exchanger and its thermodynamic parameters have been evaluated.

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16

Kamalasekaran, Kavitha. "Potentiometric Titration of Vanadium (V) with Iron (II) in the Presence of NTA and DTPA Using Dry-Cell Graphite Electrode." Revista de Chimie 72, no. 3 (July 29, 2021): 144–58. http://dx.doi.org/10.37358/rc.21.3.8445.

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A sensitive potentiometric titration for vanadium (V) based effect of ligands such as nitrilotriacetic acid (NTA) and diethylenetriaminepenta-acetic acid (DTPA) are reviewed. The potential iron system decreased the presence of NTA and DTPA. In this case, iron (III) increased with respect to the vanadium (IV) volume. The production of iron (III)-ligand complex has increased. This result suggested that the formation of V(V)-NTA and V(V)-DTPA complexes were less favoured than that of V(IV)-NTA and V(IV)-DTPA complexes. The calculated correlation coefficients (r) conveyed the effectiveness of the graphite electrode as the indicator electrode for the potentiometric titrations. On comparing the potential jump values, the extent of potential caused by DTPA was found to be more than that of NTA. The utilization of graphite electrode has facilitated the potentiometric titration by significantly causing larger potential jump. This method was precise and accurate as no interference of foreign ions was observed. Hence, the approach could be applied to the vanadium (V) of any samples.

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17

Isvoranu, Marian, Constantin Luca, Maria Pleniceanu, and Cezar Spinu. "Studies on a Pb2+ - selective electrode with a macrocyclic liquid membrane: Potentiometric determination of pb2+ ions." Journal of the Serbian Chemical Society 71, no. 12 (2006): 1345–52. http://dx.doi.org/10.2298/jsc0612345i.

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This paper presents experimental and theoretical data regarding the design, characterization and analytical applications of a non-expensive, liquid-membrane ion-selective electrode for Pb2+ ions. The membrane is a solution of the active complex formed by Pb2+ ions with dibenzo-18-crown-6-ionophore (DB-[18]-C-6) extracted in propylene carbonate (PC). The successful application of the developed electrode for the determination of Pb2+ ions in aqueos solution samples by direct potentiometry and potentiometric titration is presented. For the presented analytical results, there are insignificant systematic errors between the direct potentiometric method with the developed ion-selective electrode and atomic absorption spectrometry. .

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18

Golovko, Dmitriy, Virender Sharma, Olga Pavlova, Elena Belyanovskaya, Igor Golovko, Victoria Suprunovich, and Radek Zboril. "Determination of submillimolar concentration of ferrate(VI) in alkaline solutions by amperometric titration." Open Chemistry 9, no. 5 (October 1, 2011): 808–12. http://dx.doi.org/10.2478/s11532-011-0069-8.

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AbstractA new amperometric titration method was developed for quantitative determination of ferrate(VI) (FeVIO42−) in the 7.06×10−5−5.73×10−3 M concentration range. Chromium(III) hydroxide solution was used as the titrant. The diffusion current (Id) had a linear relationship with the concentration of ferrate(VI) and slopes were dependent on the concentration of NaOH. The amperometric titration could detect a lower concentration of ferrate(VI) than could potentiometric and colorimetric titrations. The method was applied successfully to determine concentrations of ferrate(VI), generated electrochemically, in strong alkaline solutions.

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19

Bensacia, Nabila, Saâd Moulay, François Garin, Ioana Fechete, and Anne Boos. "Effect of Grafted Hydroquinone on the Acid-Base Properties of Poly(acrylic acid) in the Presence of Copper (II)." Journal of Chemistry 2015 (2015): 1–7. http://dx.doi.org/10.1155/2015/913987.

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Potentiometric titration of poly(acrylic acid) and hydroquinone-functionalized poly(acrylic acid) was conducted in the presence of copper (II). The effects of hydroquinone functionalizing and copper (II) complexing on the potentiometric titration of poly(acrylic acid) were studied in an ionic environment and in its absence. Henderson-Hasselbalch equation was applied to assess its validity for this titration. Coordination number and the stability constants of the copper- (II-)complexed polymers were determined, and results showed the formation of mostly monodentate and bidentate copper- (II-)polymer complexes.

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20

Abulkibash, Abdallah M., Munir Al-Absi, and Abdul aziz Nabil Amro. "Microtitrimetry by Controlled Current Potentiometric Titration." Журнал аналитической химии 68, no. 1 (2013): 60–63. http://dx.doi.org/10.7868/s0044450213010027.

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21

Young, San-Land, Miriam Martino, Carlos Kienzle-Sterzer, and J. Antonio Torres. "Potentiometric titration studies on xanthan solutions." Journal of the Science of Food and Agriculture 64, no. 1 (January 1994): 121–27. http://dx.doi.org/10.1002/jsfa.2740640118.

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22

Hernlem, Bradley J., and Lee-Shin Tsai. "Titration of Chlorine: Amperometric versus Potentiometric." Journal - American Water Works Association 92, no. 12 (December 2000): 101–7. http://dx.doi.org/10.1002/j.1551-8833.2000.tb09075.x.

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23

Abulkibash, Abdallah M., Munir Al-Absi, and Abdul aziz Nabil Amro. "Microtitrimetry by controlled current potentiometric titration." Journal of Analytical Chemistry 68, no. 1 (December 29, 2012): 57–60. http://dx.doi.org/10.1134/s1061934813010024.

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24

Lu, Weiping, and Edward H. Smith. "Modeling potentiometric titration behavior of glauconite." Geochimica et Cosmochimica Acta 60, no. 18 (September 1996): 3363–73. http://dx.doi.org/10.1016/0016-7037(96)00180-9.

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25

Anderson, Leif G., Conny Haraldsson, and Roger Lindegren. "Gran linearization of potentiometric Winkler titration." Marine Chemistry 37, no. 3-4 (April 1992): 179–90. http://dx.doi.org/10.1016/0304-4203(92)90077-n.

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26

Shi-nan, Xie, Ji Hong, Wu Ai-qin, and Chen Guo-hua. "Potentiometric titration of calcium in seawater." Chinese Journal of Oceanology and Limnology 15, no. 1 (March 1997): 32–35. http://dx.doi.org/10.1007/bf02850579.

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27

Qayoom, Amtul, Syed Arif Kazmi, and Saeeda Nadir Ali. "Turmeric Powder as a Natural Heavy Metal Chelating Agent: Surface Characterisation." Pakistan Journal of Scientific & Industrial Research Series A: Physical Sciences 60, no. 1 (February 28, 2017): 1–8. http://dx.doi.org/10.52763/pjsir.phys.sci.60.1.2017.1.8.

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The present study was conducted to investigate surface properties of turmeric in order to evaluateits detoxification potential and ability to sequester toxic metals ions. Scanning Electron Microscopy (SEM),Energy Dispersion Spectroscopy (EDS), Infra-Red (IR) spectroscopy and potentiometric titrations wereemployed for characterisation of the surface of turmeric powder. Spectroscopic studies revealed that thesurface of turmeric powder was porous mainly composed of polymeric -OH , -NH , -CH2 , -COO and-OH groups of polysaccharides. From potentiometric titrations and modelling of batch titration data, it wasfound that surface of the turmeric contains at least four binding sites with pKa values 3.56 (pK1), 4.83(pK2), 7.68 (pK3) and 10.4 (pK4). Turmeric powder contains highest concentration of amino and hydroxylgroups for the pK4 values i.e., 0.55 mmol/ g. The total binding sites concentration for turmeric powderwas 1.2 mmol/ g.

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28

Partanen, Jaakko I., Pekka M. Juusola, and Virginie Verraes. "Re-evaluation of the second thermodynamic dissociation constants of α-alanine, valine, and leucine using potentiometric data measured for aqueous potassium chloride solutions at 298.15 K." Canadian Journal of Chemistry 83, no. 1 (January 1, 2005): 46–56. http://dx.doi.org/10.1139/v04-164.

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Equations were developed for the calculation of the second stoichiometric (molality scale) dissociation constants (Km2) of α-alanine, valine, and leucine in aq. KCl solutions at 298.15 K from the revised thermodynamic dissociation constants (Ka2) of these acids and the ionic strength (Im) of the solutions. The ionic strength of the solutions considered in this study is determined mostly by KCl alone, and the equations for Km2 were based on the single-ion activity coefficient equations of the Hückel type. The existing literature data obtained from Harned cell measurements and new potentiometric titration data were used to revise the Ka2 values of the three amino acids. The values (1.295 ± 0.013) × 1010, (1.894 ± 0.009) × 1010, and (1.685 ± 0.011) × 1010 were obtained from the new potentiometric titration data for α-alanine, valine, and leucine, respectively. For alanine and valine, the new Ka2 values are also supported by the Harned cell data used, but the value (1.80 ± 0.02) × 1010 obtained for leucine from these data is significantly different. The potentiometric values are recommended here. The activity coefficient equations for the calculation of Km2 values were also determined from the new potentiometric data. By means of the activity coefficient equations obtained for these three amino acids for KCl solutions, Km2 can be evaluated almost within experimental error up to an Im of about 1.0 mol kg1. The Km2 values calculated by this method are also compared with the values suggested in the literature.Key words: ionic strength dependence, stoichiometric dissociation constant, Debye-Hückel equation, potentiometry, α-alanine, valine, leucine.

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29

Vytřas, Karel, Tomáš Čapoun, Emil Halámek, Jan Souček, and Blanka Štajerová. "Potentiometric ion-pair formation titrations of N-alkyl-N-ethylpyrrolidinium cations using plastic membrane electrodes." Collection of Czechoslovak Chemical Communications 55, no. 4 (1990): 941–50. http://dx.doi.org/10.1135/cccc19900941.

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Cations of the homologous series of N-alkyl-N-ethylpyrrolidinium salts were determined with a good precision by a titration using sodium tetraphenylborate titrant and potentiometric indication with a simple PVC membrane coated-wire electrode. The value of the potentiometric titration break depended on the number of carbon atoms in the alkyl chain. To explain the role of the equilibria involved, the values of both the distribution ratios and the extraction constants as well as the solubility products of N-alkyl-N-ethylpyrrolidinium tetraphenylborates were determined. The value of the titration break could readily be correlated with the logarithmic values of the extraction parameters.

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30

H�zi, J., L. Daruh�zi, O. Pint�r, and Zs Szak�ly. "Critical comparison of evaluation methods of potentiometric titration data using a microcomputer-controlled automatic potentiometric titration system." Mikrochimica Acta 89, no. 1-6 (January 1986): 379–88. http://dx.doi.org/10.1007/bf01207330.

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31

Ramamurthy, Narayanan, Narayan Baliga, Joyce A. Wahr, Ulrich Schaller, Victor C. Yang, and Mark E. Meyerhoff. "Improved protamine-sensitive membrane electrode for monitoring heparin concentrations in whole blood via protamine titration§." Clinical Chemistry 44, no. 3 (March 1, 1998): 606–13. http://dx.doi.org/10.1093/clinchem/44.3.606.

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Abstract An improved protamine-sensitive electrode based on a polymeric membrane doped with the charged ion exchanger dinonylnaphthalenesulfonate (DNNS) is used for monitoring heparin concentrations in whole blood. The electrode exhibits significant nonequilibrium potentiometric response to polycationic protamine over the concentration range of 0.5–20 mg/L in undiluted whole-blood samples. The sensor can serve as a simple end point detector for the determination of heparin via potentiometric titrations with protamine. Whole-blood heparin concentrations determined by the electrode method (n ≥157) correlate well with other protamine titration-based methods, including the commercial Hepcon HMS assay (r = 0.934) and a previously reported potentiometric heparin sensor-based method (r = 0.973). Reasonable correlation was also found with a commercial chromogenic anti-Xa heparin assay (r = 0.891) with corresponding plasma samples and appropriate correction for whole-blood hematocrit levels. Whereas a significant positive bias (0.62 kU/L; P <0.001) is observed between the anti-Xa assay and the protamine sensor methods, insignificant bias is observed between the protamine sensor and the Hepcon HMS tests (0.08 kU/L; P = 0.02). The possibility of fully automating these titrations offers a potentially simple, inexpensive, and accurate method for monitoring heparin concentrations in whole blood.

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32

Mustafa, S., A. Naeem, N. Rehana, and T. Hussain. "Exchange of Some Divalent Metal Cations and Their Effect on the Dissociation of Iron(III) Phosphate." Adsorption Science & Technology 13, no. 4 (August 1996): 241–60. http://dx.doi.org/10.1177/026361749601300403.

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Potentiometric titrations of iron(III) phosphate have shown an apparently weak monobasic acid behaviour towards alkali, alkaline earth and divalent transition metal ions. The selectivity sequence and dissociation of the exchanger was found to increase in the order Cu2+ > Zn2+ > Ni2+ > Ca2+ > K+. The dissociation constants of iron(III) phosphate have been determined from Potentiometric titration data in the temperature range 303–323 K. In addition, the exchange of Cu2+, Zn2+ and Co2+ on iron(III) phosphate and the effect of these ions on dissociation were also studied as a function of concentration, temperature and solution pH value. The thermodynamic parameters ΔH0, ΔS0 and ΔG0 for the dissociation of iron(III) phosphate are also presented.

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33

Pleniceany, Maria, Marian Isvoranu, and Cezar Spinu. "Liquid membrane ion-selective electrodes for potentiometric dosage of coper and nickel." Journal of the Serbian Chemical Society 70, no. 2 (2005): 269–76. http://dx.doi.org/10.2298/jsc0502269p.

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This paper presents experimental and theoretical data regarding the preparation and characterization of three liquid-membrane electrodes, which have not been mentioned in the specialized literature so far. The active substances, the solutions of which in nitrobenzene formed the membranes on a graphite rod, are simple complex combinations of Cu(II) and Ni(II) ions with an organic ligand belonging to the Schiff base class: N-[2-thienylmethilidene]-2-aminoethanol (TNAHE). The Cu2+ -selective and Ni2+ -selective electrodes were used to determine the copper and nickel ions in aqueous solutions, both by direct potentiometry and by potentiometric titration with EDTA. They were also used for the determination of Cu2+ and Ni2+ ions in industrial waters by direct potentiometry.

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34

Grabowski, Lauren E., and Scott R. Goode. "Determining a Solubility Product Constant by Potentiometric Titration To Increase Students’ Conceptual Understanding of Potentiometry and Titrations." Journal of Chemical Education 94, no. 5 (March 15, 2017): 636–39. http://dx.doi.org/10.1021/acs.jchemed.6b00460.

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35

Jokic, Anja, Radmila Dzudovic, Ljiljana Jaksic, and Snezana Nikolic-Mandic. "The application of hydrogen-palladium electrode for potentiometric acid-base determinations in tetrahydrofuran." Journal of the Serbian Chemical Society 78, no. 8 (2013): 1203–12. http://dx.doi.org/10.2298/jsc120927018j.

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The application of the hydrogen-palladium electrode (H2/Pd) as the indicator electrode for the determination of relative acidity scale (Es, mV) of tetrahydrofuran (THF) and the potentiometric titrations of acids in this solvent was investigated. The relative acidity scale tetrahydrofuran was determined from the difference half-neutralization potentials of perchloric acid and tetrabutylammonium hydroxide (TBAH), which were measured by using both H2/Pd-SCE and glass-SCE electrode pairs. The experimentally obtained value of Es scale THF with a H2/Pd-SCE electrode pair was 1155 mV, and those obtained with glass-SCE electrode pair 880 mV. By using a H2/Pd indicator electrode, the individual acids (benzoic acid, palmitic acid, maleic acid, acetyl acetone, ?-naphthol) and two component acid mixtures (benzoic acid + ?-naphthol, palmitic acid + ?-naphthol, maleic acid + ?-naphthol and maleic acid + ftalic acid) were titrated with a standard solution of TBAH. In addition, sodium methylate and potassium hydroxide proved to be very suitable titrating agents for titrating of the individual acids and the acids in mixtures, respectively. The relative error of the determination of acids in mixture was less than 3%. The results are in agreement with those obtained by a conventional glass electrode. The advantages of H2/Pd electrode over a glass electrode in potentiometric acid-base determinations in tetrahydrofuran lie in the following: this electrode gives wider relative acidity scale THF, higher the potential jumps at the titration end-point and relatively fast response time; furthermore, it is very durable, simple to prepare and can be used in the titrations of small volumes.

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36

Gélinas, Stéphanie, James A. Finch, and Andrew J. Vreugdenhil. "Determination of Monolayer Density by Potentiometric Titration." Journal of Physical Chemistry B 103, no. 29 (July 1999): 5988–91. http://dx.doi.org/10.1021/jp990067c.

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37

Gibson, Graham T. T., Mark F. Mohamed, Alexei A. Neverov, and R. S. Brown. "Potentiometric Titration of Metal Ions in Ethanol." Inorganic Chemistry 45, no. 19 (September 2006): 7891–902. http://dx.doi.org/10.1021/ic060517x.

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38

Verbeek, A. A. "A FORTH-language, computer-controlled potentiometric titration." Journal of Chemical Education 62, no. 8 (August 1985): 687. http://dx.doi.org/10.1021/ed062p687.

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39

Muroga, Yoshio, and Mitsuru Nagasawa. "Potentiometric Titration Behavior of Poly(crotonic acid)." Polymer Journal 18, no. 1 (January 1986): 15–19. http://dx.doi.org/10.1295/polymj.18.15.

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40

Grant, D., W. F. Long, and F. B. Williamson. "Zn2+-heparin interaction studied by potentiometric titration." Biochemical Journal 287, no. 3 (November 1, 1992): 849–53. http://dx.doi.org/10.1042/bj2870849.

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Measurement of the decrease in pH that accompanies the addition of Zn2+ to heparin in solution provided an indirect method of examining cation-polyanion interaction. Construction of plots analogous to isothermal saturation binding plots revealed the existence, for defined conditions of interaction, of a [heparin]-independent direct proportionality between the fraction of the maximal pH change occurring and the [Zn2+]/[heparin disaccharide] ratio. This accords with results from polarimetric examination of Ca(2+)- and Cu(2+)-heparin interactions. It suggests that, under the conditions used, cation-heparin interaction may result in the formation of a complex that exists in a colloid-like phase, between which and the aqueous phase, exchange of cations does not follow simple solution-phase reversible equilibrium thermodynamic behaviour. The results suggest that the putative Zn(2+)-containing complex is less stable in the presence of NaCl than is the corresponding Ca(2+)-containing complex. Addition of Zn2+ to low concentrations of heparins is accompanied by the usual decrease in pH, followed by a removal of H+ from solution as the [Zn2+]/[heparin disaccharide] ratio increases, suggesting dissolution of the putative complex. This reversal of the initial pH change was not seen for most other cation-heparin interactions under the conditions studied.

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41

Zuyi, Tao, Du Jinzhou, and Chu Taiwei. "Potentiometric titration in studies of ion exchangers." Reactive and Functional Polymers 31, no. 1 (August 1996): 17–24. http://dx.doi.org/10.1016/1381-5148(96)00036-3.

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42

Gayda, Jean-Pierre, Patrick Bertrand, Claude More, Françoise Guerlesquin, and Mireille Bruschi. "EPR potentiometric titration of c3-type cytochromes." Biochimica et Biophysica Acta (BBA) - Protein Structure and Molecular Enzymology 829, no. 2 (June 1985): 262–67. http://dx.doi.org/10.1016/0167-4838(85)90196-7.

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43

Jordan, Arthur. "Potentiometric titration of chlorides in biological fluids." Recueil des Travaux Chimiques des Pays-Bas 74, no. 5 (September 2, 2010): 522–29. http://dx.doi.org/10.1002/recl.19550740502.

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44

Aktaş, Hakan, and Pekcan Ertokuş. "Potentiometric determination of ibuprofen, indomethacin and naproxen using an artificial neural network calibration." Journal of the Serbian Chemical Society 73, no. 1 (2008): 87–95. http://dx.doi.org/10.2298/jsc0801087a.

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In this study, three anti-inflammatory agents, namely ibuprofen, indomethacin and naproxen, were titrated potentiometrically using tetrabutyl?ammonium hydroxide in acetonitrile solvent under a nitrogen atmosphere at 25?C. MATLAB 7.0 software was applied for data treatment as a multivariate calibration tool in the potentiometric titration procedure. An artificial neural network (ANN) was used as a multivariate calibration tool in the potentiometric titration to model the complex non-linear relationship between ibuprofen, indomethacin and naproxen concentrations and the millivolt (mV) of the solutions measured after the addition of different volumes of the titrant. The optimized network predicted the concentrations of agents in synthetic mixtures. The results showed that the employed ANN can precede the titration data with an average relative error of prediction of less than 2.30%.

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45

Sakač, Nikola, Dubravka Madunić-Čačić, Dean Marković, Lucija Hok, Robert Vianello, Bojan Šarkanj, Bojan Đurin, et al. "Potentiometric Surfactant Sensor Based on 1,3-Dihexadecyl-1H-benzo[d]imidazol-3-ium for Anionic Surfactants in Detergents and Household Care Products." Molecules 26, no. 12 (June 14, 2021): 3627. http://dx.doi.org/10.3390/molecules26123627.

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A 1,3-dihexadecyl-1H-benzo[d]imidazol-3-ium-tetraphenylborate (DHBI-TPB) ion-pair implemented in DHBI-TPB surfactant sensor was used for the potentiometric quantification of anionic surfactants in detergents and commercial household care products. The DHBI-TPB ion-pair was characterized by FTIR spectroscopy and computational analysis which revealed a crucial contribution of the C–H∙∙∙π contacts for the optimal complex formation. The DHBI-TPB sensor potentiometric response showed excellent analytical properties and Nernstian slope for SDS (60.1 mV/decade) with LOD 3.2 × 10−7 M; and DBS (58.4 mV/decade) with LOD 6.1 × 10−7 M was obtained. The sensor possesses exceptional resistance to different organic and inorganic interferences in broad pH (2–10) range. DMIC used as a titrant demonstrated superior analytical performances for potentiometric titrations of SDS, compared to other tested cationic surfactants (DMIC > CTAB > CPC > Hyamine 1622). The combination of DHBI-TPB sensor and DMIC was successfully employed to perform titrations of the highly soluble alkane sulfonate homologues. Nonionic surfactants (increased concentration and number of EO groups) had a negative impact on anionic surfactant titration curves and a signal change. The DHBI-TPB sensor was effectively employed for the determination of technical grade anionic surfactants presenting the recoveries from 99.5 to 101.3%. The sensor was applied on twelve powered samples as well as liquid-gel and handwashing home care detergents containing anionic surfactants. The obtained results showed good agreement compared to the outcomes measured by ISE surfactant sensor and a two-phase titration method. The developed DHBI-TPB surfactant sensor could be used for quality control in industry and has great potential in environmental monitoring.

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Vasilyeva, Marina S., Vladimir S. Rudnev, E. S. Zykova, Alexander Yu Ustinov, Ksenia A. Sergeeva, A. V. Nepomnyaschiy, I. V. Lukiyanchuk, and Galina I. Marinina. "Ti/TiO₂, Au Electrodes Prepared by Plasma Electrolytic Oxidation and Electron Beam Evaporation." Defect and Diffusion Forum 386 (September 2018): 326–31. http://dx.doi.org/10.4028/www.scientific.net/ddf.386.326.

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Ti/TiO2,Au electrodes were prepared via plasma electrolytic oxidation (PEO) of Ti plate, followed by deposition of a thin (10 nm) Au layer by electron beam evaporation (EBE). The electrodes obtained were used for potentiometric indication of different types of chemical reactions. Ti/TiO2,Au electrodes showed an excellent performance for end point indication in the oxidation-reduction and complexometric titrations similar to the traditional Pt and in the acid-base titration similar to glass electrode.

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47

Rajkovic, Milos, Ivana Novakovic, and Aleksandar Petrovic. "Determination of titratable acidity in white wine." Journal of Agricultural Sciences, Belgrade 52, no. 2 (2007): 169–84. http://dx.doi.org/10.2298/jas0702169r.

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The amount of titration acid in must is in the largest number of cases with in the range 5.0-8.0 g/dm3. Wines, as a rule, contain less acids than must, and according to Regulations, titratable acidity is in the range of 4.0-8.0 g/dm3 expressed in tartaric acid, because a part of tartaric acid is deposited in the form of salts (tartar or argol) during alcohol fermentation. For wines that contain less than 4 g/dm3 of titratable acids there arises a suspicion about their origin, that is, that during the preparation some illegal acts were done. Because of that, the aim of this paper is to determine titratable acidity in white wine, using standard methods of determination, which are compared with the results received by potentiometric titration using ion-selective electrode. According to the received results it can be seen that wine titration with indicator gives sufficient reliable values of wine titration acidity. However, as potentiometric titration at pH value 7.00 is more reliable and objective method, the values of titratable acids content in wine, expressed through tartaric acid, are given according to this result. The analysis of differential potentiometric curves shows that these curves can give us an answer to the question of the presence of a larger amount of other nonorganic substances, which have already existed in wine. However, none of the used methods gives absolutely reliable answer what substances are present in analysed samples.

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TANIA, L., C. DIAWATI, M. SETYARINI, N. KADARITNA, and A. SAPUTRA. "USING POTENTIOMETRIC ACID-BASE TITRATION TO DETERMINE PKA FROM MANGOSTEEN PERICARPS EXTRACT." Periódico Tchê Química 16, no. 32 (August 20, 2019): 768–73. http://dx.doi.org/10.52571/ptq.v16.n32.2019.786_periodico32_pgs_768_773.pdf.

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One of the uses of acid-base indicators is to show the end point of the titration, so the accurate determination of acidity constant and pH range of indicators needs to be done. This study aims to determine the acidity constant (pKa) of mangosteen pericarp extract and its accuracy as an indicator of acid-base titration. Determination of pKa was done by a simple potentiometric titration method. The titration data were plotted in three graphs, i.e., pH, ΔpH/ΔV (the (the first derivative), and Δ2pH/ΔV2 (the second derivative) versus titrant volume to determine the equivalence point of the titration. The accuracy test was carried out by comparing the volume of oxalic acid used to titrate NaOH solution using the indicator of mangosteen pericarp extract and phenolphthalein indicator. The result showed that the equivalence point was found on the titrant volume of 8.6 mL and a measured pH of 9.84. so the pKa value of mangosteen pericarp extract was 7.20, and the pH range was 6.20 to 8.20. the average volume of oxalic acid used to titrate 5 mL of NaOH using phenolphthalein as the indicator was 5.2 mL while the titration used mangosteen pericarp extract was 5.23 mL. The accuracy of mangosteen pericarp extract was 99.42%. By the result, it can be concluded that potentiometric titration can be used as a simple way to determine the acidity constant of mangosteen pericarp extract. Moreover, the mangosteen pericarp extract can be used as an alternative acid-base titration indicator to substitute the common acid-base titration in the laboratory.

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Abu Ghalwa, Nasser. "Development of a Novel Solid-State Sensor Electrode Based on Titanium Thin Film as an Indicator Electrode in Potentiometric and Conductometric Acid-Base Titration in Aqueous Solution." Journal of Sensors 2012 (2012): 1–8. http://dx.doi.org/10.1155/2012/681826.

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A modified Ti/(SnO2+ Sb2O3) electrode was prepared by thermal deposition on titanium substrate and its use as indicator electrode to potentiometric and conductometric acid-base titration in aqueous solution at 298 K was developed. The E-pH curve is linear with slope of 0.0512 V/dec at 298 K. The standard potential of this electrode,E0, was determined with respect to the SCE as reference electrode. The recovery percentages for potentiometric and conductometric acid-base titration for acetic acid against NaOH were calculated. The cell constant, specific conductance, and the molar conductance with dilution for some common electrolytes were measured.

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50

Zubenya, Natalia, Natalia Zubenya, Zholt Kormosh, Diana Saribekova, Diana Saribekova, Sergei Sukharev, and Sergei Sukharev. "Potentiometric Membrane Sensors for Levamisole Determination." Mediterranean Journal of Chemistry 6, no. 2 (November 15, 2016): 7–14. http://dx.doi.org/10.13171/mjc61/016111516/kormosh.

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The ion pair (IP) of levamisole with BiI4 - (SbI4 - ) for the levamisole-selective sensor with a PVC membrane containing - ions were developed. Thermal behavior of obtained IP was investigated by differential thermal analysis that would show the thermal stability and the character of the decomposition of the complex. The thermolysis of Lev+BiI4 - IP undergoes three stages that fit a theoretical interpretation. The linearity ranges of levamisole sensors function are 7.9 ×10-6 – 1×10-1 (7.9 ×10-5 – 1×10-1 ) M. The Nernstian slope of 50.6 – 53.4 mV pC−1 and detection limit of 5.0 × 10−5 – 1.5 × 10−4) M. The working range of pH is 2.8 – 6.0. The efficiency of the use of electrodes for levamisole content control in pharmaceutical preparations was shown by direct potentiometry and potentiometric titration methods.

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