(b) Arrange the following in order of increasing strength as reducing agents in acidic solution: Zn, I^-, Sn²⁺, H₂O₂, Al.

Verified step by step guidance

1. Understand the concept of reducing agents: A reducing agent is a substance that donates electrons to another substance, reducing it. The strength of a reducing agent is determined by its ability to lose electrons easily.
2. Consider the standard reduction potentials: In acidic solutions, the standard reduction potential (E°) values can help determine the strength of reducing agents. A more negative E° value indicates a stronger reducing agent.
3. List the standard reduction potentials for each species: Look up the standard reduction potentials for Zn, I-, Sn2+, H2O2, and Al in a table of standard reduction potentials.
4. Compare the E° values: Arrange the species in order of increasing reduction potential. The species with the most negative E° value is the strongest reducing agent, and the one with the least negative (or most positive) E° value is the weakest.
5. Arrange the species: Based on the comparison of their standard reduction potentials, list the species in order of increasing strength as reducing agents.

Key Concepts

Reducing Agents

Reducing agents are substances that donate electrons in a chemical reaction, thereby reducing another species. Their strength as reducing agents is determined by their ability to lose electrons easily. In acidic solutions, the relative strength of reducing agents can vary based on their standard reduction potentials, which indicate how readily they can be oxidized.

Standard Reduction Potential

Standard reduction potential (E°) is a measure of the tendency of a chemical species to be reduced, expressed in volts. A higher E° value indicates a stronger oxidizing agent and a weaker reducing agent. Conversely, a lower E° value suggests a stronger reducing agent. This concept is crucial for comparing the reducing strengths of different substances in a given reaction environment.

Acidic Solution

An acidic solution is characterized by a higher concentration of hydrogen ions (H⁺) than hydroxide ions (OH⁻). In such environments, certain reactions may be favored, and the behavior of reducing agents can change. For example, some metals may react differently in acidic conditions compared to neutral or basic conditions, affecting their reducing power.