Kinetics and equilibria for complex formation between palladium(II) and chloroacetate

Kód výsledku v IS VaVaI

<a href="https://www.isvavai.cz/riv?ss=detail&h=RIV%2F00216224%3A14310%2F06%3A00031856" target="_blank" >RIV/00216224:14310/06:00031856 - isvavai.cz</a>

Výsledek na webu

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DOI - Digital Object Identifier

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Jazyk výsledku

angličtina

Název v původním jazyce

Kinetics and equilibria for complex formation between palladium(II) and chloroacetate

Popis výsledku v původním jazyce

Kinetics and equilibria for the formation of a 1:1 complex between palladium(II) and chloroacetate were studied by spectrophotometric measurements in 1.00 mol.dm-3 HClO4 at 298.2 K. The equilibrium constant, K, of the reaction Pd2+ + HL &lt;=&gt; PdL+ +H+ was determined from multi-wavelength absorbance measurements of equilibrated solutions at variable temperatures and spectra of individual species were calculated. Variable-temperature kinetic measurements gave rate constants for the forward and backward reactions at 298.2 K and ionic strength 1.00 mol. dm-3. From the kinetics of the forward and reverse processes, log(10) K = 0.346 +/- 0.007, Delta H_0 = -7.9 +/- 0.9 kJ.mol-1 and Delta S_0 = - 19.8 +/- 3.0 J.K-1.mol-1 were derived, and these values are in good agreement with the results of the equilibrium measurements. The Specific Ion Interaction Theory was employed for determination of thermodynamic equilibrium constants for the protonation of chloroacetate.

Název v anglickém jazyce

Kinetics and equilibria for complex formation between palladium(II) and chloroacetate

Popis výsledku anglicky

Kinetics and equilibria for the formation of a 1:1 complex between palladium(II) and chloroacetate were studied by spectrophotometric measurements in 1.00 mol.dm-3 HClO4 at 298.2 K. The equilibrium constant, K, of the reaction Pd2+ + HL &lt;=&gt; PdL+ +H+ was determined from multi-wavelength absorbance measurements of equilibrated solutions at variable temperatures and spectra of individual species were calculated. Variable-temperature kinetic measurements gave rate constants for the forward and backward reactions at 298.2 K and ionic strength 1.00 mol. dm-3. From the kinetics of the forward and reverse processes, log(10) K = 0.346 +/- 0.007, Delta H_0 = -7.9 +/- 0.9 kJ.mol-1 and Delta S_0 = - 19.8 +/- 3.0 J.K-1.mol-1 were derived, and these values are in good agreement with the results of the equilibrium measurements. The Specific Ion Interaction Theory was employed for determination of thermodynamic equilibrium constants for the protonation of chloroacetate.

Druh

J_x - Nezařazeno - Článek v odborném periodiku (Jimp, Jsc a Jost)

CEP obor

CB - Analytická chemie, separace

OECD FORD obor

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Projekt

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Návaznosti

V - Vyzkumna aktivita podporovana z jinych verejnych zdroju

Rok uplatnění

2006

Kód důvěrnosti údajů

S - Úplné a pravdivé údaje o projektu nepodléhají ochraně podle zvláštních právních předpisů

Název periodika

Journal of Solution CHemistry

ISSN

0095-9782

e-ISSN

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Svazek periodika

35

Číslo periodika v rámci svazku

5

Stát vydavatele periodika

NL - Nizozemsko

Počet stran výsledku

14

Strana od-do

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Kód UT WoS článku

000239310700009

EID výsledku v databázi Scopus

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