Solubility, activity coefficients and acid–base properties of three naphthol derivatives in NaCl(aq) at different ionic strengths and at T=298.15K

Bretti, Clemente; Stefano, Concetta De; Manfredi, Giuseppe; Sammartano, Silvio

doi:10.1016/j.molliq.2010.10.008

Cited by 15 publications

(10 citation statements)

References 29 publications

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“…For Debye–Hückel type equation: where log K i H0 is the protonation constant at infinite dilution for the i th protonation step, I is the ionic strength in molarity, C is an empirical parameter for the depencence of the protonation constants on ionic strength, and z * = Σ(charge) 2 reactants – Σ(charge) 2 products ; for higher ionic strengths, C has been defined as below − where c ∞ and c 0 are equal to C for ionic strength I → ∞ and I → 0, respectively.…”

Section: Resultsmentioning

confidence: 99%

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca²⁺and Mg²⁺at Different Ionic Strengths and Ionic Media at 298.15 K

et al. 2016

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The protonation constants (log K i H ) of L-glutamic acid N,Ndiacetic acid tetrasodium salt (GLDA) were determined at T = 298.15 K and various ionic strengths in NaCl (aq) , 0.18 ≤ I ≤ 3.20 mol•kg −1 , (CH 3 ) 4 NCl (aq) 0.17 ≤ I ≤ 4.00 mol•kg −1 , and (C 2 H 5 ) 4 NI (aq) 0.13 ≤ I ≤ 1.10 mol•kg −1 by using the potentiometric method. The calculation of ionic strength dependence parameters was performed by Debye−Huckel type equation, Specific ion Interaction Theory (SIT). and Pitzer equations (only for NaCl (aq) ). These equations make it feasible to calculate and predict the protonation constants of GLDA in the desired range of ionic strength theoretically. The values of pure water protonation constants are log K 1 H 10.558 ± 0.028, log K 2 H 5.348 ± 0.011, log K 3 H 3.088 ± 0.015 and log K 4 H 1.918 ± 0.009, the first protonation refers to the nitrogen group and the other three to carboxylate groups. The different values of log K i H obtained in NaCl (aq) , (CH 3 ) 4 NCl (aq) , and (C 2 H 5 ) 4 NI (aq) were interpreted in terms of formation of weak complexes between GLDA and the cations of the supporting electrolytes. Binding constants referring to the weak species formed by GLDA with sodium and tetramethylammonium cations were calculated. For example, the stability of the NaL and (CH 3 ) 4 NL species, at infinite dilution, are log K = 2.5 ± 0.2 and 1.6 ± 0.3, respectively. The complexing ability of GLDA versus calcium and magnesium was also determined in NaCl (aq) at various ionic strength values. The pure water formation constants are for calcium log K CaL 0 = 8.181 ± 0.024 and for magnesium log K MgL 0 = 7.263 ± 0.028.

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Section: Resultsmentioning

confidence: 99%

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca²⁺and Mg²⁺at Different Ionic Strengths and Ionic Media at 298.15 K

et al. 2016

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“…In order to remove O 2 and CO 2 , purified N 2 was bubbled through the solution. Titrand solutions were prepared and pH measurements were performed as reported earlier [8,9]. The reported data are the mean of three independent experiments.…”

Section: Methodsmentioning

confidence: 99%

“…On comparing the effect of KCl on the protonation constant of the naphthols compounds under study with that of NaCl on the same naphthols [9], we can note that the effect of NaCl may be identical to that of KCl. This can be shown from the nearly equal values of the parameters ∞ and 0 at 298.15 K.…”

Section: Protonation Constantsmentioning

confidence: 99%

“…The pH measurements for the ligands under study (naphthalen-1-ol, naphthalene-1,5-diol, and 4-amino-3-hydroxynaphthalene-1-sulphonic acid) in aqueous solution, at the temperature range of = (293.15 to 213.15) K at 5 K intervals, were performed as reported earlier [8,9]. The number of protons associated with the molecules of the ligands under study, , was calculated as reported earlier [10].…”

Section: Protonation Constantsmentioning

confidence: 99%

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Protonation and Solvation Thermodynamics of Some Naphthol Derivatives in KCl Aqueous Solution of Different Ionic Strengths

El–Dossoki

2016

Journal of Chemistry

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The acid-base properties of naphthalen-1-ol (L1), naphthalene-1,5-diol (L2), and 4-amino-3-hydroxynaphthalene-1-sulphonic acid (L3) were characterized from pH-metric measurements in pure water and in different concentrations (0–4 mol kg−1) of aqueous KCl solutions at the temperature range ofT= (293.15 to 213.15) K at 5 K intervals. The results reveal that naphthalen-1-ol and naphthalene-1,5-diol molecules have two ionisable protons (of the hydroxyl groups) while 4-amino-3-hydroxynaphthalene-1-sulphonic acid has three ionisable protons (hydrogen ion of the hydroxyl group, SO3H, andNH3+). Modeling of the data was done by applying Debye-Hückel model. The protonation and the solvation processes of all studied ligands are spontaneous and endothermic processes. Also the solubilities of naphthalen-1-ol, naphthalene-1,5-diol, and 4-amino-3-hydroxynaphthalene-1-sulphonic acid were determined. The data were analyzed using Setschenow equation and the values of Setschenow coefficients (km) were determined. From the solubility data, the activity coefficients were obtained. The values of the total solubilities (ST) for naphthalen-1-ol and naphthalene-1,5-diol were found equal to the values of their neutral species (S0). On the other hand, the total solubility for 4-amino-3-hydroxynaphthalene-1-sulphonic acid is different from that of its neutral species. The results also indicate solubility decrease in pure water from L1-L2-L3.

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“…12 shows the non-specific long-range contribution of the electrostatic region, while the second reflects the contribution due to short-range ion-ion, ion-neutral, or neutralneutral interactions in accordance with the Brønsted postulate that ε(j, k) = 0 if ions have the same charge sign. There are many papers in the literature about the SIT [29][30][31][32][33][34][35][36]. Sammartano [29] proposed a modified version of the SIT approach in which the specific coefficients are expressed as a function of I by:…”

Section: Ionic Strength Dependence Of the Dissociation And Stability mentioning

confidence: 99%

Complexation of Dioxovanadium(V) with D-(-)-Quinic Acid at Different Ionic Strengths Using Different Models Based on the Debye-Hückel Theory

Majlesi

Rezaienejad

2011

J Solution Chem

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The complex formation reaction between the dioxovanadium(V) cation VO + 2 and D-(-)-quinic acid {(1R,3R,4S,5R)-(-)-1,3,4,5-tetrahydroxycyclohexane-1-carboxylic acid} has been studied in aqueous solutions. The UV data and the values of the derived conditional stability constants are presented and discussed in the light of one stoichiometric model for the reaction at T = 298 K and different ionic strengths (0.10 to 1.00) mol·dm −3 of sodium chloride. Speciation diagrams and dissociation constants were obtained on the basis of UV spectroscopic measurements and potentiometric titrations, respectively. Our results show that one complex species, VO 2 L, exists in solution in the pH range of about 1.00 to 3.00. The parabolic, Specific Ion Interaction Theory (SIT), and extended Debye-Hückel type (EDH) models successfully describe the ionic strength dependence of the stability constants. A comparison with literature data is also reported.

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Solubility, activity coefficients and acid–base properties of three naphthol derivatives in NaCl(aq) at different ionic strengths and at T=298.15K

Cited by 15 publications

References 29 publications

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca²⁺and Mg²⁺at Different Ionic Strengths and Ionic Media at 298.15 K

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca²⁺and Mg²⁺at Different Ionic Strengths and Ionic Media at 298.15 K

Protonation and Solvation Thermodynamics of Some Naphthol Derivatives in KCl Aqueous Solution of Different Ionic Strengths

Complexation of Dioxovanadium(V) with D-(-)-Quinic Acid at Different Ionic Strengths Using Different Models Based on the Debye-Hückel Theory

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Solubility, activity coefficients and acid–base properties of three naphthol derivatives in NaCl(aq) at different ionic strengths and at T=298.15K

Cited by 15 publications

References 29 publications

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca2+and Mg2+at Different Ionic Strengths and Ionic Media at 298.15 K

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca2+and Mg2+at Different Ionic Strengths and Ionic Media at 298.15 K

Protonation and Solvation Thermodynamics of Some Naphthol Derivatives in KCl Aqueous Solution of Different Ionic Strengths

Complexation of Dioxovanadium(V) with D-(-)-Quinic Acid at Different Ionic Strengths Using Different Models Based on the Debye-Hückel Theory

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Thermodynamic Study on the Protonation and Complexation of GLDA with Ca²⁺and Mg²⁺at Different Ionic Strengths and Ionic Media at 298.15 K

Thermodynamic Study on the Protonation and Complexation of GLDA with Ca²⁺and Mg²⁺at Different Ionic Strengths and Ionic Media at 298.15 K