Which metal can be oxidized with an Sn 2+ solution but not with an Fe 2+ solution?

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 56

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Chapter 19, Problem 56

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

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Identify the standard reduction potentials (E°) for Sn2+/Sn and Fe2+/Fe from a standard reduction potential table.

Understand that a metal can be oxidized by an ion if the ion has a higher reduction potential than the metal's corresponding ion.

Compare the reduction potential of Sn2+ with the reduction potential of the metal in question to determine if Sn2+ can oxidize the metal.

Similarly, compare the reduction potential of Fe2+ with the reduction potential of the metal in question to determine if Fe2+ can oxidize the metal.

Find a metal whose corresponding ion has a reduction potential between those of Sn2+ and Fe2+, indicating that it can be oxidized by Sn2+ but not by Fe2+.

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Key Concepts

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

Oxidation and Reduction

Oxidation refers to the loss of electrons by a substance, while reduction is the gain of electrons. In redox reactions, one species is oxidized and another is reduced. Understanding these processes is crucial for determining which metals can be oxidized by specific ions, as the ability of a metal to be oxidized depends on its position in the electrochemical series.

Electrochemical Series

The electrochemical series is a list of metals and their standard electrode potentials, which indicates their tendency to be oxidized or reduced. Metals higher in the series are more easily oxidized than those lower down. This series helps predict which metals can be oxidized by certain ions, such as Sn2+ and Fe2+, based on their relative positions.

Metal Reactivity

Metal reactivity refers to how readily a metal can lose electrons and undergo oxidation. More reactive metals can displace less reactive metals from their compounds in solution. In the context of the question, identifying a metal that can be oxidized by Sn2+ but not by Fe2+ requires understanding the reactivity of the metals involved and their respective positions in the electrochemical series.

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Related Practice

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

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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

Textbook Question

Determine whether or not each metal dissolves in 1 M HNO₃. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu b. Au

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

Verified Solution

Key Concepts

Oxidation and Reduction

Electrochemical Series

Metal Reactivity

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