In the reduction half reaction of h2o2 in a basic

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Unformatted text preview: plain why the color changes during this process. Question D: An excess of H2O2 has been used in this step since cobalt(II) is oxidized in the presence of the decomposing hydrogen peroxide. In the reduction half reaction of H2O2 in a basic solution hydroxide ions are formed, 2e- + H2O2(aq) 2OH-(aq). Write a balanced ionic equation for the redox reaction occurring in step 4. As a side note: The decomposition of hydrogen peroxide takes place as self-reaction involving both oxidation and reduction processes. Therefore, a by-product reaction occurring here is 2 H2O2(aq) 2 H2O(l) + 2O2(g). This reaction is catalyzed by the presence of transition metal ions. 5. Place the small casserole over the 250 mL beaker that is partially filled with the boiling water (use a hot plate to boil water). Be careful to avoid breathing the vapors that may rise out of the casserole. Next, quickly but carefully, add 12 mL of concentrated HCl and note any color changes. Continue heating the casserole on top of the beaker for about 50 minutes. During the 50 m...
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This note was uploaded on 04/09/2013 for the course CHE CHE 2C taught by Professor Nasiri during the Spring '07 term at UC Davis.

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