We can determine the standard potencies for several chemical substances. A few of these substances are listed in Table P2. These data help compare the oxidative/reductive strengths of various substances. Table 1 shows the half-reaction to the standard hydrogen electrode (SHE). It’s more than halfway down.
All reactants below the H+ in the table have more potent oxidants than those above. F2 is by far the most potent oxidant. It has a standard electrode potential of 2.87 V.
Answer: The order of the species in their decreasing oxidizing agent ability is Ag^+>Sn^2+>Cr^3+>Na^+
Answer and explanation
Ag+ is the only ion that was mentioned in the query.
It has the most significant potential to reduce. Due to its high reduction potency, it is easily reduced down to Ag. Cu2+ is next, followed by Cr2+. Finally, Mg2+ has a low reduction potential.
These agents act as reducing agents and help the element get reduced. These agents have a lower potential to reduce other aspects. The reducing agent is more effective if it has a negative value.
The following elements have reduced potential:
Ag^+:0.80V\Cr^3+:-0.74V\Sn^2+:-0.14V\Na^+:-2.71V
These reduction potentials show that Ag+ is best as an oxidizing agent, and Na+ is best as a reducing agent.
Order in the decreasing oxidizing agent ability of the species is Ag^+>Sn^2+>Cr^3+>Na^+
Example 1 – Silver Sulfide
Ag2S is what causes the black tarnish to form on silver objects. The following is the half-reaction to reverse the process of tarnishing.
Ag2S(s)+2e–2Ag(s)+S2-(aq)Edeg=-0.69V
Referring Table 1, determine which species–H2O2[aq], I-[aq], and Sn2+[aq] –can reduce Ag2S below standard conditions.
These five species–H2O2[aq], Zn[s], I-[aq], Sn2+[aq] – can be identified as the strongest reducing agent for aqueous solution. This will help you to choose the best product candidate.
The data in Table 1 suggests an alternative agent for removing tarnish that is easily accessible, affordable, and potentially more effective.
Conclusion
This is the correct order for oxidizing agents: Ag+>Cu2+>Cr2+>Mg2+.
Eo values allow you to predict the relative strengths of different oxidants and reducers. Standard electrode potentials can be used to determine other substances’ oxidative and reduction strengths. An explanation for apparent anomalies may be found in the fact that electrode potentials are measured in an aqueous solution. This allows intermolecular solid electrostatic interactions.
