Provide an example of the oxidation and reduction in aqueous solutions.

Oxidation and reduction in aqueous solutions can be seen in the reaction between iron and copper sulfate.

When iron is added to copper sulfate solution, the iron atoms lose electrons and become positively charged ions, while the copper ions gain electrons and become neutral copper atoms. This process is known as reduction, as the copper ions have gained electrons. The iron atoms, on the other hand, have lost electrons and are said to have been oxidized.

The reaction can be represented by the following equation: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)

In this equation, the iron atoms are oxidized (Fe → Fe2+ + 2e-) and the copper ions are reduced (Cu2+ + 2e- → Cu). The iron atoms are said to be the reducing agent, as they cause the reduction of the copper ions, while the copper ions are the oxidizing agent, as they cause the oxidation of the iron atoms.

This reaction is an example of a redox reaction, which involves the transfer of electrons between species. In aqueous solutions, redox reactions are common and play important roles in many biological processes, such as respiration and photosynthesis.

Overall, the reaction between iron and copper sulfate is a useful example of oxidation and reduction in aqueous solutions, and highlights the importance of redox reactions in biological systems.