ISSN:
1436-5073
Source:
Springer Online Journal Archives 1860-2000
Topics:
Chemistry and Pharmacology
Description / Table of Contents:
Zusammenfassung Eine Semimikro-Technik zur Bestimmung der Löslichkeitskonstanten von Metalloxiden, -hydroxiden, -carbonaten und -sulfiden wurde entwickelt und mit Erfolg auf Kupfer (II)- und Eisen (II)-carbonat angewendet. Alle experimentellen Daten konnten mit Hilfe der beiden folgenden heterogenen Gleichgewichte erklärt werden $$\begin{gathered} CuCO_{3(s)} + 2H_{(l)}^ + \rightleftharpoons Cu_{(l)}^{2 + } + CO_{2(g)} + H_2 O_{(l)} ; \hfill \\ ^* K_{ps0} (CuCO_3 ) = [Cu^{2 + } ] \cdot p_{CO_2 } \cdot [H^ + ]^{ - 2} \hfill \\ FeCO_{3(s)} + 2H_{(l)}^ + \rightleftharpoons Fe_{(l)}^{2 + } + CO_{2(g)} + H_2 O_{(l)} ; \hfill \\ ^* K_{ps0} (FeCO_3 ) = [Fe^{2 + } ] \cdot p_{CO_2 } \cdot [H^ + ]^{ - 2} . \hfill \\ \end{gathered} $$ Folgende Löslichkeitskonstanten wurden gefunden (Fehlergrenze 1δ): $$\begin{gathered} \log ^* K_{ps 0} (CuCO_3 ) = 6,95 \pm 0,04; 25^0 C, I = 0.20 mol dm^{ - 3} (NaClO_4 ), \hfill \\ \log ^* K_{ps 0} (FeCO_3 ) = 7,61 \pm 0,05; 50^0 C, I = 1,0 mol kg^{ - 1} (NaClO_4 ). \hfill \\ \end{gathered} $$ Mit diesen Werten ergaben sich die freien Bildungsenthalpien von Kupfer (II)-und Eisen(II)-carbonat zu $$\begin{gathered} \Delta _f G_{298}^ \ominus (CuCO_3 ) = - 126,21 \pm 0,06 kcal mol^{ - 1} , \hfill \\ \Delta _f G_{298}^ \ominus (FeCO_3 ) = - 159,90 \pm 0,11 kcal mol^{ - 1} . \hfill \\ \end{gathered} $$ Thermodynamische Konsequenzen dieser Resultate werden diskutiert.
Notes:
Summary A semimicro technique for the determination of solubility constants of metal oxides, hydroxides, carbonates and sulphides has been developed and successfully applied to copper(II) and iron(II) carbonate. All experimental data can be interpreted according to the heterogeneous equilibria $$\begin{gathered} CuCO_{3(s)} + 2H_{(l)}^ + \rightleftharpoons Cu_{(l)}^{2 + } + CO_{2(g)} + H_2 O_{(l)} ; \hfill \\ ^* K_{ps0} (CuCO_3 ) = [Cu^{2 + } ] \cdot p_{CO_2 } \cdot [H^ + ]^{ - 2} , \hfill \\ FeCO_{3(s)} + 2H_{(l)}^ + \rightleftharpoons Fe_{(l)}^{2 + } + CO_{2(g)} + H_2 O_{(l)} ; \hfill \\ ^* K_{ps0} (FeCO_3 ) = [Fe^{2 + } ] \cdot p_{CO_2 } \cdot [H^ + ]^{ - 2} . \hfill \\ \end{gathered} $$ The individual solubility constants obtained are (errors 1δ): $$\begin{gathered} \log ^* K_{ps 0} (CuCO_3 ) = 6.95 \pm 0.04, 25^0 C, I = 0.20M (NaClO_4 ), \hfill \\ \log ^* K_{ps 0} (FeCO_3 ) = 7.61 \pm 0.05, 50^0 C, I = 1.0 mole/kg (NaClO_4 ). \hfill \\ \end{gathered} $$ With these values the free enthalpies of formation of copper(II) and iron (II) carbonate have been calculated as $$\begin{gathered} \Delta _f G_{298}^ \ominus (CuCO_3 ) = - 126.21 \pm 0.06 kcal/mole \hfill \\ \Delta _f G_{298}^ \ominus (FeCO_3 ) = - 159.90 \pm 0.11 kcal/mole. \hfill \\ \end{gathered} $$ Thermodynamic implications of these results are discussed.
Type of Medium:
Electronic Resource
URL:
http://dx.doi.org/10.1007/BF01198705
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