Final answer:
In the reaction Ag+ + Ti3+ → Ag + Ti4+, Ag+ acts as the oxidizing agent as it gets reduced, and Ti3+ acts as the reducing agent as it gets oxidized.
Step-by-step explanation:
In the reaction Ag+ + Ti3+ → Ag + Ti4+, we determine the role of each species by following the electron transfer. An oxidizing agent gains electrons and gets reduced, while a reducing agent loses electrons and gets oxidized.
Here, silver (Ag+) is gaining an electron to become neutral silver (Ag), which means silver ions get reduced and therefore, Ag+ is the oxidizing agent. Conversely, titanium (Ti3+) loses an electron to become Ti4+, getting oxidized, which makes Ti3+ the reducing agent.
To elaborate, the half-reactions for this redox process are:
- Oxidation (reducing agent): Ti3+ → Ti4+ + e−
- Reduction (oxidizing agent): Ag+ + e− → Ag
Therefore, option 1) where Ag+ is the oxidizing agent and Ti3+ is the reducing agent is correct.