Abstract
The stability constants of highly concentrated copper(II)–lactate alkaline aqueous solutions for Cu2O electrodeposition were determined by factor analysis of UV-vis absorption spectra. The stability constant is 107.05 ± 0.05 for the chemical equilibrium expression CuL2 + OH– = Cu(H–1L)L– + H2O, while that for the chemical equilibrium expression Cu(H–1L)L– + OH– = Cu(H–1L)22– + H2O is 105.05 ± 0.05; here, L– is the lactate ion (CH3CH(OH)COO–) and H–1L2– is the deprotonated lactate ion (CH3CH(O–)COO–). By refining the potential–pH and pH speciation diagrams for the Cu–lactate–H2O system, it appears that the pH dependence of the preferential orientation of Cu2O is due to differences in the dissolved species.
Highlights
The stability constants of highly concentrated copper(II)–lactate alkaline aqueous solutions for Cuprous oxide (Cu2 O) electrodeposition were determined by factor analysis of UV-vis absorption spectra
By refining the potential–pH and pH speciation diagrams for the Cu–lactate–H2 O system, it appears that the pH dependence of the preferential orientation of Cu2 O is due to differences in the dissolved species
Cuprous oxide (Cu2 O) is a low-cost p-type semiconductor with low toxicity that has attracted the attention of researchers as a solar-cell and photocathode material.[1,2,3,4,5,6,7,8,9,10,11,12]
Summary
In the pH range of 6.04–13.15, there are three significant eigenvalues, 648698.1852, 25774.8143, and 255.1911, which are the principal factors These results confirmed that only three optical active species, CuL2 , Cu(H–1 L)L– , and Cu(H–1 L)2 2– , existed in these solutions. Only two significant eigenvalues, 291864.4077 and 1555.0453, were obtained from the solutions for pH 6.04–7.11, confirming that only two copper(II)–containing species, CuL2 and Cu(H–1 L)L– , were in equilibrium in this region. 3.9724 should be considered as a principal factor due to the small quantity of existing CuL2 , only two significant eigenvalues, 374403.0872 and 6902.8214, were obtained from the solutions for pH 7.80–13.15 This confirmed that mainly two copper(II)–lactate complexes, Cu(H–1 L)L– and Cu(H–1 L)2 2– , were in equilibrium in this region. The potential–pH diagram of the Cu–HL–H2 O system based on reported thermochemical data (Fig. 7b) indicates that Cu(OH)[2]
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