Rank the given metal ions in order of increasing strength as an oxidizing agent. Pb 2+ (-0.13 V), Mn 2+ (-1.18 V), Cu 2+ (+0.16 V), Co 3+ (+1.82 V), Fe 3+ (+0.77 V)

Here on this practice problem it says, rank the given metal ions in order of increasing strength as an oxidizing agent. Within this question we have lead 2 ion, manganese 2 ion, copper 2 ion, cobalt 3 ion, and iron 3 ion, each with their respective standard reduction potentials. Now going back to the question itself, it says oxidizing agent. Remember, oxidizing agent means that you are being reduced. And remember, the larger your standard reduction potential value is, then the more likely reduction is going to occur. So when they're saying rank in terms of increasing strength of oxidizing agent, they want us to rank them in terms of increasing ability to be reduced. So they want us to or it from smallest standard reduction potential to largest standard reduction potential. So let's take a look at our options. Manganese 2 ion would start it out because it has the smallest standard reduction potential of negative 1.18 volts. Who's the next smallest? That would be lead 2. And then who's the next smallest after that? That would be copper 2. Then we have iron 3 ion, and then finally cobalt 3 has the largest standard reduction potential, which means it represent the strongest oxidizing agent from the list. So this would be ordering it from smallest ability to be reduced to largest ability to be reduced with cobalt III ion.

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20. Electrochemistry

Standard Reduction Potentials

General Chemistry

20. Electrochemistry

Standard Reduction Potentials

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Multiple Choice

Rank the given metal ions in order of increasing strength as an oxidizing agent.
Pb²⁺ (-0.13 V), Mn²⁺ (-1.18 V), Cu²⁺ (+0.16 V), Co³⁺ (+1.82 V), Fe³⁺(+0.77 V)

Pb2+ < Cu2+ < Mn2+ < Co3+ < Fe3+

Co3+ < Fe3+ < Cu2+ < Pb2+ < Mn2+

Mn2+ < Pb2+ < Cu2+ < Fe3+ < Co3+

Mn2+ < Pb2+ < Cu2+ < Co3+ < Fe3+

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Verified step by step guidance

Understand that the strength of an oxidizing agent is related to its standard reduction potential. The higher the reduction potential, the stronger the oxidizing agent.

List the given metal ions along with their standard reduction potentials: Pb²⁺ (-0.13 V), Mn²⁺ (-1.18 V), Cu²⁺ (+0.16 V), Co³⁺ (+1.82 V), Fe³⁺ (+0.77 V).

Rank the metal ions based on their standard reduction potentials from lowest to highest: Mn²⁺ (-1.18 V), Pb²⁺ (-0.13 V), Cu²⁺ (+0.16 V), Fe³⁺ (+0.77 V), Co³⁺ (+1.82 V).

The order of increasing strength as an oxidizing agent is the same as the order of increasing standard reduction potential.

Conclude that Mn²⁺ is the weakest oxidizing agent and Co³⁺ is the strongest oxidizing agent based on their standard reduction potentials.

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Struggling with General Chemistry?

Rank the given metal ions in order of increasing strength as an oxidizing agent.Pb2+ (-0.13 V), Mn2+ (-1.18 V), Cu2+ (+0.16 V), Co3+ (+1.82 V), Fe3+ (+0.77 V)

Watch next

Standard Reduction Potentials practice set

Rank the given metal ions in order of increasing strength as an oxidizing agent.
Pb²⁺ (-0.13 V), Mn²⁺ (-1.18 V), Cu²⁺ (+0.16 V), Co³⁺ (+1.82 V), Fe³⁺(+0.77 V)