By Glenn Dryhurst (Auth.)
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Additional info for Biological Electrochemistry
It was thus proposed that the failure to observe reduction peak ll c of ubiquinone-30 at slow sweep rates was due to formation of the Q H ~ species, according to the scheme just described and shown in Eq. (19), which upon reaction with tetraethylammonium perchlorate Q + e~ • Q^ H + > QH- QH- (from water) insoluble precipitate then forms a precipate on the electrode. The electrochemical reduction of ubiquinone-30 in acetonitrile in the presence of ethanol has also been studied briefly . A cyclic voltammogram of ubiquinone-30 in a 1 :1 mixture of acetonitrile and ethanol is shown in Fig.
2 V. This potential is that of the more positive peak. The more negative peak was due to reduction of protons . b Cr + e - ^ Q * * Peak II, (14b) Reduction peak ll c thus corresponded to a further 1e~ reduction of the radi2 cal anion (Q~) formed in the peak l c process to give a dianion (Q ~) [Eq. (14b)]. Peak ll a was proposed to represent the reverse reaction. However, it is clear from the data in Table VI that peaks ll c and ll a do not form a reversible couple. Addition of the weak acid diethyl malonate caused oxidation peak ll a to disappear and caused a shift of the peak potential for reduction peak ll c to more positive values (Table VI).
In addition, the polarographic diffusion current was linearly dependent on the concentration of ubiquinone-50 at a given concentration of sodium dodecyl sulfate, indicating that the observed wave must be due to electrochemical reduction of the ubiquinone-50. It appeared to be clear from the experimental results that the diffusing particle was a micelle of sodium dodecyl sulfate with ubiquinone-50. The diffusion coefficient of the latter micelle would be expected to depend on the size of the micelle formed and hence on the concentration of the sodium dodecyl sulfate.
Biological Electrochemistry by Glenn Dryhurst (Auth.)