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The relative stabilities of the copper hydroxyl sulphates

Published online by Cambridge University Press:  05 July 2018

C. H. Yoder ,
T. M. Agee ,
K. E. Ginion ,
A. E. Hofmann ,
J. E. Ewanichak ,
C. D. Schaeffer Jr. ,
M. J. Carroll ,
R. W. Schaeffer  and
P. F. McCaffrey
C. H. Yoder*
Affiliation:
Department of Chemistry, Franklin and Marshall College, Lancaster, PA 17604-3303, USA
T. M. Agee
Affiliation:
Department of Chemistry, Franklin and Marshall College, Lancaster, PA 17604-3303, USA
K. E. Ginion
Affiliation:
Department of Chemistry, Franklin and Marshall College, Lancaster, PA 17604-3303, USA
A. E. Hofmann
Affiliation:
Department of Chemistry, Franklin and Marshall College, Lancaster, PA 17604-3303, USA
J. E. Ewanichak
Affiliation:
Department of Chemistry, Franklin and Marshall College, Lancaster, PA 17604-3303, USA
C. D. Schaeffer Jr.
Affiliation:
Department of Chemistry and Biochemistry, Elizabethtown College, Elizabethtown, PA 17022-2298, USA
M. J. Carroll
Affiliation:
Department of Chemistry and Biochemistry, Elizabethtown College, Elizabethtown, PA 17022-2298, USA
R. W. Schaeffer
Affiliation:
Department of Chemistry and Biochemistry, Messiah College, Grantham, PA 17027-9800, USA
P. F. McCaffrey
Affiliation:
Department of Chemistry and Biochemistry, Messiah College, Grantham, PA 17027-9800, USA
*
E-mail: claude.yoder@fandm.edu
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Abstract

The literature contains considerable disagreements on the relative stabilities of the members of the copper hydroxyl sulphate family. Titration of copper sulphate with sodium hydroxide is claimed by some to produce only brochantite, while other reports indicate that antlerite and a dihydrate of antlerite are produced in the titration. Most stability field diagrams show that antlerite is the more stable stoichiomer at pH 4 and sulphate activity of 0.05–1. We have reexamined this stoichiometric family by titration of aqueous copper sulphate with sodiumhydroxide and sodium carbonate, reverse titration of sodiumhydroxide with copper sulphate and simultaneous addition of copper sulphate and sodium hydroxide at a variety of mole ratios, concentrations, temperatures and reaction times. We have also explored the reaction of copper hydroxide with copper sulphate and the reaction of weak bases, such as sodiumacetate, sodiumcarbonate and urea, with copper sulphate. Our work indicates that: (1) antlerite is not formed in reactions of 0.05 to 1.2 M CuSO4 with 0.05–1.0 M NaOH or Na2CO3 at room temperature; (2) antlerite is formed in the addition of small concentrations of base (≤0.01 M) to 1 M CuSO4 at 80°C, but not at roomtem perature or with 0.01 M CuSO4 at 80°C; (3) the formation of Cu5(SO4)2(OH)6·4H2O occurs at large Cu2+ to base mole ratios; (4) the compound described in the literature as antlerite dihydrate is actually Cu5(SO4)2(OH)6.4H2O; (5) at mole ratios of Cu2+ to OH– ranging from 2:1 to 1:2 the predominant product is brochantite; and (6) brochantite and Cu5(SO4)2(OH)6.4H2O are converted to antlerite in the presence of 1 M CuSO4 (the latter requires temperatures of 80°C or greater).

The Ksp (ion activity product) values of antlerite and brochantite were determined to be 2.53 (0.01)⨯10−48 and 1.01 (0.01)⨯10−69, respectively, using atomic absorption spectroscopy and Visual MINTEQ after equilibration in solutions of varying ionic strength and pH for six days. These values are in good agreement with those from the literature. However, after 6 months, antlerite in contact with solution is partially converted to brochantite and hence is metastable with a relatively low conversion rate. The Ksp value for antlerite must therefore be considered approximate. The relative stabilities of the copper hydroxyl sulphates are rationalized using appropriate equations and Gibbs energy calculations. A Gibbs free energy of formation for Cu5(SO4)2(OH)6.4H2O of –3442 kJ/mol was obtained from the simple salt approximation.

Keywords

antleritebrochantiteXRDAAStitrationcopper hydroxyl sulphates
Type
Research Article
Information
Mineralogical Magazine , Volume 71 , Issue 5 , October 2007 , pp. 571 - 577
Copyright
Copyright © The Mineralogical Society of Great Britain and Ireland 2007

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