Question

(i) Select oxidising and reducing agents with reason in the following reactions:
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Hint:

The species that loses electrons (oxidized) is the reducing agent, and the species that gains electrons (reduced) is the oxidizing agent.

Answer 1

In each reaction, we need to identify the species being oxidized (losing electrons) and reduced (gaining electrons). The species that loses electrons is the reducing agent, and the species that gains electrons is the oxidizing agent. (a) Sn^{++} (aq) $\rightarrow$ \text{Sn}^{+++} (aq):}
In this reaction, Sn\(^{++}\) loses an electron to form Sn\(^{+++}\). Hence, Sn\(^{++}\) is oxidized. The species that gains the electron is the oxidizing agent. Reducing agent: Sn^{++} (aq)
Oxidizing agent: Sn^{+++} (aq)
(b) Fe^{+++} (aq) $\rightarrow$ \text{Fe}^{++} (aq):}
In this reaction, Fe\(^{+++}\) gains an electron to form Fe\(^{++}\), so Fe\(^{+++}\) is reduced. The species that loses the electron is the reducing agent. Reducing agent: Fe^{+++} (aq)
Oxidizing agent: Fe^{++} (aq)
(c) Na(s) $\rightarrow$ Na^{+} (aq):}
Here, Na (sodium) loses an electron to form Na\(^+\). Therefore, sodium (Na) is oxidized. The species that accepts the electron is the oxidizing agent. Reducing agent: Na (s)
Oxidizing agent: Na^{+} (aq)