Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 50: Problem 16

Which is the stronger oxidizing agent, \(\mathrm{Cu}^{2+}(\mathrm{aq})\) or \(\mathrm{H}^{+}(\mathrm{aq})\) ?

Short Answer

Expert verified
The stronger oxidizing agent is determined by comparing the standard reduction potentials of \(\mathrm{Cu}^{2+}(\mathrm{aq})\) and \(\mathrm{H}^{+}(\mathrm{aq})\). Without the specific values from a standard electrode potential table, a definitive answer can't be given in this context. However, once the numbers are available, the ion with the higher reduction potential will be the stronger oxidizing agent.

Step by step solution

01

Refer to Standard Electrode Potential Table

Refer to a Standard Electrode Potential Table which will have reduction potentials listed for various half-reactions. The reduction potential values for \(\mathrm{H}^{+} \rightarrow \mathrm{H_{2}} (g)\) and \(\mathrm{Cu}^{2+} \rightarrow \mathrm{Cu} (s)\) are required.
02

Compare the Standard Reduction Potentials

Compare the standard reduction potentials. Use the values obtained from the standard electrode potential table. The species with the higher standard reduction potential will be the stronger oxidizing agent.
03

Draw a conclusion

The species with the higher standard reduction potential is the stronger oxidizing agent, because it is more prone to be reduced (gain electrons).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

What use(s) could be made of the flow of electrons in the wire?

The standard reduction potentials for \(\mathrm{Ag}^{+}(\mathrm{aq})\) and \(\mathrm{Au}^{+}(\mathrm{aq})\) are \(\begin{array}{lr} & E_{\mathrm{red}}^{\circ} \\ \mathrm{Ag}^{+}+1 \mathrm{e}^{-} \rightleftarrows \mathrm{Ag}(\mathrm{s}) & .80 \\\ \mathrm{Au}^{+}+1 \mathrm{e}^{-} \rightleftarrows \mathrm{Au}(\mathrm{s}) & 1.68\end{array}\) Which ion, \(\mathrm{Ag}^{+}(\mathrm{aq})\) or \(\mathrm{Au}^{+}(\mathrm{aq})\), exhibits the stronger pull on electrons?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free