Additional Related Projects

• Find in the literature other UV-resistant dyes and test them instead of rhodamine B.

• Quantify the amount of CO2 produced, by mass spectrometry or gravimetry for example.

• Use UV light of different wavelengths to observe any possible effects on the overall process described in the present experiment.

• Oxidize a small amount (e.g., a few drops) of an aromatic species with Fenton's reagent and do a qualitative test for the presence of the corresponding phenolic derivative (Caution: many aromat-ics are highly toxic). (See Greenberg, 1998).

• Use an Fe(III)L complex (e.g., Fe(III)EDTA, see Experiment 8) to produce Fe(Il) by photoreduc-tion. Add H2O2 and use the mixture in the same fashion as the normal Fenton's reagent, as described in the procedure above.

• Perform Fenton's reaction on a halogenated aromatic hydrocarbon (e.g., C2CU) and test for the presence of CI and CO2 in the products. (See Leung, 1992).

• Repeat the original experiment done by Fenton by adding a drop of an Fe2+ solution and a drop of a H2O2 solution to a basic solution of tartaric acid (see Fenton, 1894). He reported observing an intense violet color. Could this color be due to the presence of ferrate ions? How can this be tested? Search the literature as needed to see if such a hypothesis is plausible, and if possible, find an analytical tool to test for it. (See Ibanez, 2004).

• Try recently proposed alternative systems that circumvent some of the inherent limitations in the Fenton system (e.g., the requirement of a low working pH, the narrow pH range for solubility of the iron species, and the easiness of oxidation of Fe2+ by ambient dioxygen). For exam ple, try a Cu(II)/H202/organic acid system, or a Co/H202/ascorbic acid system. (See Verma, 2003 and 2004).

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