Atropine and quinine ionic associates with some acid dyes

1988 ◽  
Vol 53 (8) ◽  
pp. 1655-1663 ◽  
Author(s):  
Jan Souček ◽  
Emil Halámek ◽  
Roman Kysilka
Keyword(s):  
Ionic Strength ◽  
Aqueous Solutions ◽  
Aqueous Phase ◽  
Bromothymol Blue ◽  
Acid Dyes ◽  
Extraction Recovery ◽  
Extraction Constants ◽  
Ionic Associates ◽  
Metanil Yellow ◽  
Extraction Spectrophotometry

The formation of ionic associates of atropine and quinine with bromothymol blue, metanil yellow and cresol red was studied by extraction spectrophotometry. In aqueous solutions, formation of ionic associates was only observed for quinine with bromothymol blue; ionic associates of both dyes with all of the three dyes could be, however, studied by their extraction into chloroform. The conditional extraction constants were calculated for the equilibria involved. The ability of atropine, quinine and bromothymol blue to be extracted into chloroform was examined in dependence on pH and ionic strength of the aqueous phase. The pH1/2 value corresponding to 50% extraction recovery decreases with increasing ionic strength for quinine whereas for atropine the extraction recovery is only slightly affected by a higher ionic strength and for bromothymol blue the pH1/2 (E = 50%) value increases with increasing ionic strength.

Extraction of some metals into solutions of 1-phenyl-3-methyl-4-benzoylpyrazolone-5 in freon 113

1980 ◽  
Vol 45 (4) ◽  
pp. 1221-1226 ◽  
Author(s):  
Oldřich Navrátil ◽  
Pavel Linhart
Keyword(s):  
Ionic Strength ◽  
Aqueous Solutions ◽  
Stability Constants ◽  
Aqueous Phase ◽  
Organic Phase ◽  
Extraction Constants ◽  
Distribution Constants ◽  
The Stability

The partition of 1-phenyl-3-methyl-4-benzoylpyrazolone-5 (HA) between aqueous solutions of HClO4 and NaClO4, ionic strength 0.1, and Freon 113 or its 2 : 1 mixture with benzene was studied. The logarithms of the HA distribution constants are 2.84 ± 0.10 and 3.39 ± 0.15 for the two organic phases, respectively. The extraction curves of cerium(III) and europium(III) revealed that in dependence on the pH of the aqueous phase, the metals are transferred into the organic phase in the form of the MA3 complexes (M = Ce, Eu). The stability constants of the complexes MAn in the aqueous phase were determined along with their distribution and extraction constants. For cobalt, zinc, and hafnium, a part of the extraction curves could only be studied, only the extraction constants were therefore determined. The sparing solubility of HA in Freon 113 can be circumvented by using a Freon-benzene mixture 2 : 1, which is still practically incombustible.

Extraction of hafnium by means of some substituted 1-phenyl-3-methyl-4-benzoyl-pyrazol-5-ones

1981 ◽  
Vol 46 (8) ◽  
pp. 1901-1905 ◽  
Author(s):  
Oldřich Navrátil ◽  
Jiří Smola
Keyword(s):  
Ionic Strength ◽  
Aqueous Phase ◽  
Dissociation Constants ◽  
Parent Substance ◽  
Benzoyl Group ◽  
Extraction Constants ◽  
Extraction Parameters ◽  
Substituted 1

Distribution between aqueous phase and benzene or chloroform was studied for 1-phenyl-3-methyl-4-benzoylpyrazol-5-ones with 2-chloro, 4-methoxy, 3-nitro, and 4-nitro substitution in the benzoyl group (ionic strength of the aqueous phase 0.1) and for hafnium in their presence (ionic strength 2.0). The distribution and dissociation constants of the reagents and the extraction constants of their hafnium complexes were determined. Hafnium was found to be extracted as the HfA4 species. The extraction parameters of the derivatives in question do not differ substantially from those of the parent substance.

Extraction of iron(III) from the citric medium by the toluene solution of trilaurylamine

1980 ◽  
Vol 45 (11) ◽  
pp. 3116-3129 ◽  
Author(s):  
Petr Vaňura ◽  
Libor Kuča
Keyword(s):  
Citric Acid ◽  
Ionic Strength ◽  
Aqueous Phase ◽  
Organic Phase ◽  
Toluene Solution ◽  
Constant Ionic Strength ◽  
Extraction Constants ◽  
Equilibrium Concentrations

The composition of Fe(III) complexes extracted from the aqueous phase of constant ionic strength (1M-(H3,Na3,Fe)A, where H3A denotes citric acid) by the toluene solution of trilaurylamine (TLA) has been determined and the respective extraction constants have been calculated. In the concentration range cFe < 10-2 mol l-1 FeA(TLA)2 and FeA(TLA)4(H3A)2-4 are the predominant complexes in the organic phase. The abundance of the (FeA)3(TLA)6(H3A)2 complex in the organic phase increases at higher equilibrium concentrations of Fe(III) in the aqueous phase and at higher concentrations of TLA.

Investigation of the Conditions of Extraction of Ion-Associates of 3-Quinuclidinyl Benzilate with Acidic Dyes

1993 ◽  
Vol 58 (2) ◽  
pp. 315-319 ◽  
Author(s):  
Emil Halámek ◽  
Zbyněk Kobliha
Keyword(s):  
Aqueous Phase ◽  
Bromocresol Green ◽  
Limits Of Detection ◽  
Extraction Constants ◽  
Optimum Ph ◽  
Metanil Yellow ◽  
Quinuclidinyl Benzilate

Ion-associates of 3-quinuclidinyl benzilate (BZ) with thirteen acidic dyes were examined after their extraction into chloroform. Based on spectrophotometric measurements, the optimum pH of the aqueous phase was established and the extraction yields, distribution ratios, conditional extraction constants and limits of detection were calculated. Bromocresol green and metanil yellow are suggested as reagents for the analysis of BZ.

Extraction of scandium, cerium, promethium, and europium with dibutylphosphoric, bis(2-ethylhexyl)phosphoric, and dioctylphosphoric acids in Freon 113

1987 ◽  
Vol 52 (2) ◽  
pp. 322-328 ◽  
Author(s):  
Petr Linhart ◽  
Oldřich Navrátil ◽  
Josef Havel ◽  
Milan Vrchlabský
Keyword(s):  
Aqueous Solutions ◽  
Aqueous Phase ◽  
Acid Concentration ◽  
Organic Phase ◽  
Hydrogen Ions ◽  
Inorganic Acid ◽  
Extraction Constants ◽  
Distribution Constants ◽  
Phosphoric Acids

The extraction of Sc, Ce, Pm, and Eu from aqueous solutions of HClO4 and HNO3 into organic phases constituted by solutions of dialkylphosphoric acids in Freon 113 was studied. The effects of the kind of inorganic acid, concentration of hydrogen ions in the aqueous phase and concentration of the extracting agent in the organic phase were examined. Based on the dependences of the distribution ratios of the metals on the above variables, the compositions of the extractable complexes were determined and the extraction constants calculated. The dimerization constants and distribution constants of the monomer were also determined for dibutylphosphoric and bis(2-ethylhexyl)phosphoric acids.

Competitive Extraction of Some Bases by Carbollylcobaltate Anion from Water Into Chloroform

1999 ◽  
Vol 64 (7) ◽  
pp. 1111-1118 ◽  
Author(s):  
Oldřich Navrátil ◽  
Zdeněk Skaličan ◽  
Zbyněk Kobliha ◽  
Emil Halámek
Keyword(s):  
Aqueous Phase ◽  
Organic Phase ◽  
Azo Dyes ◽  
Analytical Methods ◽  
Extraction Method ◽  
Organic Bases ◽  
Quaternary Salts ◽  
Ionic Associates ◽  
Complementary Study ◽  
Extraction Spectrophotometry

The bis[undecahydro-7,8-dicarbaundecaborato(2-)]cobaltate(1-) (X-) has been used for complementary study of its ionic associates with some cations of organic bases and quaternary salts. For the optimization of present analytical methods, quinuclidin-3-yl hydroxy(diphenyl)acetate, 1-(1-phenylcyclohexyl)piperidine, dibenzo[b,f][1,4]oxazepine and cocaine, were studied by competitive extraction method. X- labelled with 60Co was used as carrier anion, triphenylmethane and azo dyes as competitive anions. The aqueous phase was 0.1 and 0.01 M HCl, the organic phase was chloroform. A comparison was made with earlier results obtained by extraction spectrophotometry.

Extraction of hafnium(IV) with organophosphorus reagents from solutions of mineral acids mixtures

1979 ◽  
Vol 44 (12) ◽  
pp. 3656-3664
Author(s):  
Oldřich Navrátil ◽  
Jiří Smola ◽  
Rostislav Kolouch
Keyword(s):  
Ionic Strength ◽  
Aqueous Phase ◽  
Organic Phase ◽  
Perchloric Acid ◽  
Synergic Effect ◽  
Salting Out ◽  
Initial Concentration ◽  
Mixed Complexes ◽  
Synergic Extraction ◽  
Mineral Acids

Extraction of hafnium(IV) was studied from solutions of mixtures of perchloric and nitric acids and of perchloric and hydrochloric acids for constant ionic strength, I = 2, 4, 6, or 8, and for cHf 4 . 10-4 mol l-1. The organic phase was constituted by solutions of some acidic or neutral organophosphorus reagents or of 2-thenoyltrifluoroacetone, 1-phenyl-3-methyl-4-benzoyl-5-pyrazolone, or N-benzoyl-N-phenylhydroxylamine in benzene, chloroform, or n-octane. A pronounced synergic extraction of hafnium proceeds only on applying organophosphorus reagents from an aqueous phase whose acidity is not lower than 3M-(HClO4 + HNO3) or 5M-(HClO4 + HCl). The synergic effect was not affected markedly by a variation of the initial concentration of hafnium in the range 1 . 10-8 -4 .10-4 mol l-1, it lowered with increasing initial concentration of the organophosphorus reagent and decreasing concentration of the H+ ions. It is suggested that the hafnium passes into the organic phase in the form of mixed complexes, the salting-out effect of perchloric acid playing an appreciable part.

Sorption of Cadmium and Lead by Chelating Ion Exchangers Ostsorb OXIN, Ostsorb DETA, and Ostsorb DTTA

1994 ◽  
Vol 59 (6) ◽  
pp. 1311-1318 ◽  
Author(s):  
Ladislav Svoboda ◽  
Petr Vořechovský
Keyword(s):  
Ionic Strength ◽  
Aqueous Solutions ◽  
Sodium Perchlorate ◽  
Exchange Capacity ◽  
Chloride Ions ◽  
Point Of View ◽  
Alkaline Media ◽  
Ion Exchangers ◽  
Acidic Media ◽  
Cadmium And Lead

The properties of cellulose chelating ion exchangers Ostsorb have been studied in the sorption of cadmium and lead from aqueous solutions. The Cd(II) and Pb(II) ions are trapped by the Ostsorb OXIN and Ostsorb DETA ion exchangers most effectively in neutral and alkaline media but at these conditions formation of stable hydrolytic products of both metals competes with the exchange equilibria. From this point of view, Ostsorb DTTA appears to be a more suitable sorbent since it traps the Pb(II) and Cd(II) ions in acidic media already. Chloride ions interfere with the sorption of the two metals by Ostsorb DTTA whereas the ionic strength adjusted by the addition of sodium perchlorate does not affect the exchange capacity of this ion exchanger.

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