Abstract
The solubility of crystalline Ni(OH)2 was studied in solutions of 0.01M NaC104 with pH ranging from 7 to near 14. Equilibrium was approached both from over-and undersaturation, and the equilibration times extended from 3 to 90 days. The solubility of Ni(OH)2(c) in the pH range of approximately 7 to 11.3 was effectively modeled by including aqueous Ni2+ and NiOH+ species. Values of the logarithm of the thermodynamic equilibrium constants for the reactions [Ni(OH)2(c) ⇌ Ni2+ + 2OH-] and [Ni2+ + OH- ⇌ Ni(OH)+] were determined to be -16.1±0.1 and 5.65 ± 0.10, respectively. These data, in conjunction with Pitzer ion interaction parameters given in the literature, were used to model the reported solubilities of Ni(OH)2(c) in chloride, sodium acetate, and potassium chloride solutions. The model predictions for these systems were in excellent agreement with the experimental data from the literature.
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References
R. NÄsÄnen,Ann. Acad. Sci. Fenn. A2, 59 (1942).
K. H. Gayer and A. B. Garrett,J. Amer. Chem. Soc. 71, 2973 (1949).
P. K. Jena and B. Prasad,J. Ind. Chem. Soc. 33(2), 122 (1956).
G. Blaszkiewicz,Z. Chem. 7, 245 (1967).
D. F. Novak-Adamic, B. Cosovic, H. Bilinski, and M. Branica,J. Inorg. Chem. 35, 2371 (1973).
N. S. Chickerur, B. B. Sabat, and P. P. Mahapatra,Thermochimica Acta 41, 375 (1980).
H. T. S. Britton,J. Chem. Soc. 127, 2110 (1925).
K. Murahe,Bull. Chem. Soc. Jpn. 3, 267 (1928).
C. N. R. Rao,A Handbook of Chemistry and Physics, (East West Press, New Delhi, 1970).
G. Almkvist,Z. Anorg. Chem. 103, 240 (1918).
P. R. Tremaine and J. C. Leblanc,J. Chem. Thermodyn. 12, 521 (1980).
F. M. Doyle-Garner and A. J. Monhemius,Metallurgical Transactions B 16B, 671 (1985).
W. Feitknecht and L. Hartmann,Chimia 8, 95 (1954).
C. F. Baes, Jr. and R. E. Mesmer,The Hydrolysis of Cations (Wiley, New York 1976).
D. Rai,Radiochim. Acta 35, 97 (1984).
D. Rai, A. R. Felmy, and T. W. Szelmeczka,J. Solution Chem. 20(4), 375 (1991).
NONLIN, developed by A. R. Felmy, uses the MINPACK nonlinear least-squares programs with a chemical equilibrium routine based on the Gibbs free energy minimization procedure.
K. S. Pitzer,J. Phys. Chem. 77, 268 (1973).
D. P. Wagman, W. H. Evans, V. B. Parker, R. H. Schumm, I. Halow, S. W. Bailey, K. L. Churney, and R. L. Nuttall,J. Phys. Chem. Ref. Data 11(2) (American Chemical Society and the American Institute of Physics, New York 1982).
C. E. Harvie, N. Moller, and J. H. Weare,Geochim. Cosmochim. Acta 48, 723 (1984).
Felmy, A. R., D. Rai, J. A. Schramke, and J. A. Ryan,Radiochimica Acta 48, 29 (1989).
K. S. Pitzer and G. Mayorga,J. Phys. Chem. 77, 2300 (1973).
H. Kim and W. J. Frederick,J. Chem. Eng. Data 33, 177 (1988).
G. B. Naumov, B. N. Ryzenko, and I. L. Khodakovsky,Handbook of Thermodynamic Data (National Technical Information Service (NTIS), PB226 722 1974).
S. Liu, W. Wang, and Y. Zhang,Huaxue Tongbao 11, 28 (1994).
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Mattigod, S.V., Rai, D., Felmy, A.R. et al. Solubility and solubility product of crystalline Ni(OH)2 . J Solution Chem 26, 391–403 (1997). https://doi.org/10.1007/BF02767678
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DOI: https://doi.org/10.1007/BF02767678