3. Write half-reactions that show how H2O2 can act as either an oxidizing agent

Question

3. Write half-reactions that show how H2O2 can act as either an oxidizing agent or a reducing agent, and describe where each of these situations occurred in your testing.

4. In your testing, several precipitates are formed, and then dissolved as complexes. Select three of these situations for which to write a balanced reaction equation.

5. When Mn2+ ions are separated from the mixture, they go through a series of oxidizing andreducing steps. Write the reaction equations that describe this process.

Test Procedure results conclusion results conclusion 1 Add HCl to test tube #1 White ppt Ag+,Pb+,Hg2+ White ppt Ag+,Pb+,Hg2+ 2 Add H2SO4 to check for Pb+ White ppt Pb+ No white ppt No Pb+ 3 Add NH3 to check for Hg2^2+ Grey ppt Hg2^2+ Grey ppt Hg2^2+ present 4 Add 15 drops HCl check pH White ppt Ag+ No ppt No Ag+ 5 Add HNO3 and NaBiO3 Purple Mn+ No purple No Mn+ 6 Add KNO2 to check for Co2+ Yellow ppt Co2+ No yellow No Co2+ 7 Add NH3 to check for Cu2+ Blue color Cu2+ No blue No Cu2+ 8 Add KSCN for Fe+ Deep red Fe+ Red color Fe+ present 9 Add HCl, drop to H2O for Bi3+ White cloud Bi3+ No cloud No Bi3+ 10 Add HCl & NH3 for Al3+ Gelatinous Al3+ No Gelatine No Al3+ 11 Add HCl & FeCN for Zn2+ White ppt Zn2+ No ppt No Zn2+

Explanation / Answer

5. + 2OH

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