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Chapter 23: Problem 83

The best oxidizing agent of the following group of ions is (a) \(\mathrm{Ag}^{+}(\mathrm{aq}) ;\) (b) \(\mathrm{Cl}^{-}(\mathrm{aq}) ;\) (c) \(\mathrm{H}^{+}(\mathrm{aq})\) (d) \(\mathrm{Na}^{+}(\mathrm{aq}) ;\) (e) \(\mathrm{OH}^{-}(\mathrm{aq})\)

Short Answer

Expert verified
The best oxidizing agent among the given ions is Ag+.

Step by step solution

01

Understanding Oxidizing agents

An oxidizing agent causes the oxidation of other substances by taking their electrons and is itself reduced in the process. Thus, it can be evaluated with their reduction potential. The species with the highest reduction potential is typically the strongest oxidizing agent.
02

Identifying the strongest oxidizing agent

Looking to the standard reduction potentials for ions, the ions with more positive reduction potentials are the stronger reducing agents. The given ions are: Ag+, Cl-, H+, Na+ and OH-. Referring to a table of standard reduction potentials, these species have the following potentials: \n\nAg+ + e- -> Ag (Eº = +0.80 V)\n2H+ + 2e- -> H2 (Eº = 0.00 V)\n2Cl- -> Cl2 + 2e- (Eº = -1.36 V)\nNa+ + e- -> Na (Eº = -2.71 V)\n2OH- -> O2 + H2O + 4e- (Eº = -0.40 V)
03

Result

From the reduction potentials, the Ag+ ion has the most positive (hence the highest) reduction potential. Therefore, among the options, it is the best oxidizing agent.

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