Which metal could you use to reduce Mn 2+ ions but not Mg 2+ ions?

everyone in this example, we need to identify the metals that can be oxidized with lead two plus, but not with cadmium two plus. So what we should recall is that for a metal to be oxidized easily. That will correspond to a lower value for the cell potential reduction. Or rather the cell potential cell electrode potential. So when we refer to our standard electrode potential table, which we can find either online or in our textbooks, we're going to first look for the lead two plus ion and we would see that For the oxidation of its product, which is solid lead. We would gain two electrons here and this will correspond to a cell potential value equal to negative 0.13V. Now, what we're going to look for next beneath this chart is we would have the formation of our metal tin And we would see that from the Catalan of Tin which is a 2-plus cat ion. We would gain two electrons in the oxidation of solid tin. And so this has a self potential value equal to negative 0.14 and sorry, this is negative 0.14V. So beneath tin, we would also recognize that we have nickel two plus which to form solid nickel, we would gain two electrons to our carry on and we would see that for this oxidation of solid nickel, we have a self potential value equal to negative 0.23 volts. And then last in our chart we have cadmium beneath nickel. So we have the two plus captain of cadmium. And we would see that to form solid cadmium, We would gain two electrons. And this oxidation of solid cadmium corresponds to a self potential value equal to negative 0.40V. And so we need to determine what metals can be oxidized with lead two plus, but not with cadmium two plus. So we would find the metals that fall beneath lead because we want to find the metals that can be oxidized with lead two plus. And we would see that those metals are the middleton And the metal nickel. And so we can say therefore 10 and nickel can be oxidized Only with lead two plus. So this statement here would be our final answer to complete this example. So I hope that everything that I reviewed was clear and sorry about that. If you have any questions, just leave them down below. Otherwise, I will see everyone in the next practice video.

Ch.19 - Electrochemistry

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Tro 4th Edition

Ch.19 - Electrochemistry

Problem 55

Chapter 19, Problem 55

Which metal could you use to reduce Mn²⁺ ions but not Mg²⁺ ions?

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Identify the reduction potentials of Mn^{2+} and Mg^{2+}.

Find a metal with a reduction potential between those of Mn^{2+} and Mg^{2+}.

Ensure the metal can reduce Mn^{2+} by having a more negative reduction potential than Mn^{2+}.

Check that the metal cannot reduce Mg^{2+} by having a less negative reduction potential than Mg^{2+}.

Select the appropriate metal based on these criteria.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reduction Potential

Reduction potential is a measure of the tendency of a chemical species to acquire electrons and be reduced. Metals with higher reduction potentials can reduce ions with lower reduction potentials. Understanding the standard reduction potentials of Mn2+ and Mg2+ is essential to determine which metal can reduce Mn2+ but not Mg2+.

Electrochemical Series

The electrochemical series is a list of elements organized by their standard electrode potentials. It helps predict the feasibility of redox reactions. By comparing the positions of Mn2+ and Mg2+ in this series, one can identify which metals can reduce specific ions based on their relative potentials.

Redox Reactions

Redox reactions involve the transfer of electrons between two species, where one is oxidized (loses electrons) and the other is reduced (gains electrons). Identifying the correct metal for the reduction of Mn2+ ions requires understanding the redox behavior of the metals in question and their ability to donate electrons in the reaction.

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Identifying Redox Reactions

Related Practice

Textbook Question

Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ni(s) + Zn²⁺(aq) → Ni²⁺(aq) + Zn(s)

b. Ni(s) + Pb²⁺(aq) → Ni²⁺(aq) + Pb(s)

c. Al(s) + 3 Ag⁺(aq) → Al³⁺(aq) + 3 Ag(s)

d. Pb(s) + Mn²⁺(aq) → Pb²⁺(aq) + Mn(s)

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Textbook Question

Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ca²⁺(aq) + Zn(s) → Ca(s) + Zn²⁺(aq)

b. 2 Ag⁺(aq) + Ni(s) → 2 Ag(s) + Ni²⁺(aq)

c. Fe(s) + Mn²⁺(aq) → Fe²⁺(aq) + Mn(s)

d. 2 Al(s) + 3 Pb²⁺(aq) → 2 Al³⁺(aq) + 3 Pb(s)

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Textbook Question

Which metal can be oxidized with an Sn²⁺ solution but not with an Fe²⁺ solution?

648

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Textbook Question

Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Al b. Ag c. Pb

Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu b. Fe c. Au

Which metal could you use to reduce Mn2+ ions but not Mg2+ ions?

Verified video answer for a similar problem:

Key Concepts

Reduction Potential

Electrochemical Series

Redox Reactions

Which metal could you use to reduce Mn²⁺ ions but not Mg²⁺ ions?