Some Graphical Methods for Determining Equilibrium Constants. IV. On Methods for Three-Variable Data w(x,y).

Sillén, Lars Gunnar; Terjesen, S. G.; Cox, R. A.; Peacocke, A. R.

doi:10.3891/acta.chem.scand.10-0803

Cited by 32 publications

(3 citation statements)

References 0 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…No systematic deviation was observed assuming the stoichiometric compositions and the formation constants reported in Table 3. They have been used to construct the model curves 16 A = 0.024 M; B = 0.0050 M 0.061(6.126); 0.083(6.202); 0.104(6.267); 0.126(6.326); 0.148(6.38); 0.169(6.434); 0.191(6.482); 0.213(6.502); 0.235(6.544); 0.256 (6.591); 0.278(6.628); A = 0.025 M; B = 0.0050 M 0.001(5.908); 0.022(6.006); 0.043(6.085); 0.063(6.16); 0.084(6.224); 0.105(6.289); 0.125(6.347); 0.146(6.398); 0.167(6.453); 0.188 (6.501); A = 0.025 M; B = 0.0050 M 0.057(6.214); 0.105(6.334); 0.172(6.453); 0.202(6.499); 0.238(6.562); 0.307(6.663); 0.363(6.741); 0.416(6.819); 0.454(6.856); 0.554 (7.013); 0.656(7.15); 0.763(7.284); 0.853(7.39); 0.949(7.506); 1.043(7.628); A = 0.025 M; B = 0.0052 M 0.108 (6.445); 0.309 (6.711); 0.424 (6.86); 0.474 (6.93); 0.52 (6.993); 0.583 (7.068); 0.621 (7.11); 0.683 (7.191); 0.742 (7.267); 0.881 (7.42); 1.043 (7.606); 1.088 (7.652); 1.139 (7.686); A = 0.025 M; B = 0.0051 M 0.011 (6.008); 0.054 (6.14); 0.108 (6.226); 0.203 (6.426); 0.297 (6.637); 0.352 (6.706); 0.407 (6.767); 0.479 (6.871); 0.532 (6.972); 0.567 (7.018); 0.602 (7.086); 0.654 (7.139); 0.74 (7.28); 0.799 (7.357); 0.856 (7.428); 0.986 (7.593); A = 0.050 M; B = 0.0050 M 0.068 (6.62); 0.281 (6.987); 0.37 (7.094); 0.541 (7.357); A = 0.0089 M, B = 0.0052 M; -0.097(2.267); -0.090(2.326); -0.080(2.393); -0.078(2.432); -0.072(2.473); -0.067(2.518); -0.062(2.569); -0.059(2.601); -0.056(2.634); -0.051(2.669); -0.049(2.710); -0.039(2.797); -0.032(2.846); -0.024(2.922); -0.014(3.01); -0.005(3.124); 0.006(3.267); 0.013(3.359); 0.026(3.628); 0.035(3.836); 0.046(4.159); 0.063(4.636); 0.086(5.020); 0.112(5.269); 0.138(5.444); 0.164(5.583); 0.190(5.702); 0.216(5.802); 0.242(5.889); 0.268(5.971); 0.294(6.044); 0.311(6.088); 0.329(6.129); 0.346(6.171); 0.364(6.209); 0.381(6.243); 0.398(6.279); 0.416(6.313); 0.433(6.344); 0.445(6.376); 0.463(6.404); 0.485(6.431); 0.503(6.461). Table 3.…”

Section: Methods and Resultsmentioning

confidence: 99%

On the Hydrolysis of the Dioxouranium(VI) Ion in Oxalate Solutions

et al. 2005

View full text Add to dashboard Cite

The complex formation between the dioxouranium (VI) and the oxalate ions has been investigated by measuring the potential of a glass electrode, at 25.00 degrees C, in 1 and 3 M NaClO4, at lower acidities than 10(-4.5) M, in order to favour the formation of (mixed) ternary species. The upper limits of concentration of all the analytical parameters have been imposed by the modest solubility of Na2C2O4 in the ionic media. The experimental measurements at different ionic strengths have been treated by means of the computerised least square programme LETAGROP - ETITR. Ternary complexes of general composition (p, q, r) are formed according to reaction (1), in addition to the already reported binary complexes. pUO2(2+) + qH2O + rC2O4(2-) <==> (UO2)p(OH)q(C2O4)r(2p-q-2r)(+) + qH+ (1). The stoichiometric compositions of the ternary species are (1, 1, 1), (2, 4, 2), (2, 2, 4). Their formation constants, expressed in molality, obtained in the two ionic media, are listed below. [table: see text]. For reasons discussed in the present work in the last column only the value of the constant in 1 M ionic medium is reported for the species (2, 4, 2). Additional evidence on the stoichiometric composition of the species formed is afforded by the mass-spectrometric measurements, collected in solutions of known composition.

show abstract

Section: Methods and Resultsmentioning

confidence: 99%

On the Hydrolysis of the Dioxouranium(VI) Ion in Oxalate Solutions

et al. 2005

View full text Add to dashboard Cite

show abstract

“…3. After that, the values of p and r and the constants β 1,p,r of AgH p L r are obtained from the set c H , c L c Ag ,c H according to the procedure suggested by Sillèn [23], which entails deducing from a three variable function such as η, relationships between two of the variable concentrations by keeping the third constant [20]. By applying the proposed graphic procedure, keeping c H constant, Eq.…”

Section: Complex Formationmentioning

confidence: 99%

Stability and Structure of Silver–l-methionine Complexes

Bottari

Festa

et al. 2022

J Solution Chem

View full text Add to dashboard Cite

Stability and structure of complexes between silver (I) and l-methionine (L) deduced from potentiometric and 1H NMR measurements allow to assume the prevailing of several protonated species. The experimental data are compatible with the formation of the following complexes: AgL, AgL2, AgH2L, AgH1L2, AgH2L2, AgH3L2 and AgH4L2. The coordination sites are obtained by 1H NMR spectra, showing that only the bond between the methylthioether sulfur atom and silver (I) is responsible of the complex stability. The system is studied potentiometrically with silver and glass electrodes at 25 °C and 1.00 mol·dm−3 NaClO4 as ionic medium. Amino acids containing sulfur are few and not extensively studied. In particular, l-methionine, even if it is the most important, enantiomer and their complexes with silver (I) present anticarcinogenic properties, is quite not investigated. In the same experimental conditions, l-methionine protonation constants are determined. The 1H NMR data allow one to assume that, in moderately alkaline solution, silver (I) is bond with six membered chelate rings with sulfur and amino nitrogen, while carboxylic groups are not involved. No polynuclear species are present. The high stability of the complex with ratio 1:2 (silver (I)/l-methionine), involving also two hydrogen ions, predominating in a wide range of hydrogen ion concentration suggests to propose a study for the preparation of an electrode to measure the deprotonated l-methionine concentration.

show abstract

“…• Bjerrum (1950), Irving et al (1952Irving et al ( , 1953, Sullivan and Hindman (1952), Rossotti and Rossotti (1955), Sillen (1956Sillen ( , 1958 West (1956), Stuart Tobias (1958), Costing (1959).…”

Section: Table Imentioning

confidence: 99%

Studies in Analytical Chemistry

1988

Studies in Analytical Chemistry

View full text Add to dashboard Cite

Some Graphical Methods for Determining Equilibrium Constants. IV. On Methods for Three-Variable Data w(x,y).

Cited by 32 publications

References 0 publications

On the Hydrolysis of the Dioxouranium(VI) Ion in Oxalate Solutions

On the Hydrolysis of the Dioxouranium(VI) Ion in Oxalate Solutions

Stability and Structure of Silver–l-methionine Complexes

Studies in Analytical Chemistry

Contact Info

Product

Resources

About