Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons. (b) For the reaction $\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\( \)\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\( is the reducing agent and \)\mathrm{Co}^{2+}(a q)$ is the oxidizing agent. (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

Recall the concept of oxidation and reduction in redox reactions: - Oxidation refers to the loss of electrons. - Reduction refers to the gain of electrons. Since the statement says that if something is oxidized, it is formally losing electrons, the statement is correct. Thus, the answer is: Statement (a): True

In the given reaction: \(\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{Co}^{3+}(a q)\) We need to find the change in oxidation state of \(\mathrm{Fe}\) and \(\mathrm{Co}\) : - \(\mathrm{Fe}\): \(\mathrm{Fe}^{3+}(aq)\) has an oxidation state of +3 and \(\mathrm{Fe}^{2+}(aq)\) has an oxidation state of +2, so the change is (-1), which means reduction has occurred. - \(\mathrm{Co}\): \(\mathrm{Co}^{2+}(aq)\) has an oxidation state of +2 and \(\mathrm{Co}^{3+}(aq)\) has an oxidation state of +3, so the change is (+1), which means oxidation has occurred. Now, we can identify the reducing and oxidizing agents: - Reducing agent: The substance that reduces another substance by losing electrons (undergoes oxidation). In this case, it is \(\mathrm{Co}^{2+}(aq)\). - Oxidizing agent: The substance that oxidizes another substance by gaining electrons (undergoes reduction). In this case, it is \(\mathrm{Fe}^{3+}(aq)\). Therefore, the claim that \(\mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent is incorrect. Thus, the answer is: Statement (b): False

The statement claims that if there are no changes in the oxidation state of the reactants or products in a reaction, it is not a redox reaction. Remember that redox reactions involve oxidation and reduction processes, where one substance loses electrons and another gains electrons. Therefore, if no changes in oxidation state occur, then neither oxidation nor reduction has taken place, and the reaction is not a redox reaction. Thus, the answer is: Statement (c): True