Ch.20 - Electrochemistry

Problem 59

Chapter 20, Problem 59

Which metal could you use to reduce Zn2+ ions but not Al3+ ions?

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Identify the reduction potentials of the metals involved: Zn^{2+} \rightarrow Zn and Al^{3+} \rightarrow Al.

Consult a standard reduction potential table to find the reduction potentials for Zn^{2+}/Zn and Al^{3+}/Al.

Determine the reduction potential of the metal you are considering using for reduction.

The metal you choose should have a reduction potential that is more negative than Zn^{2+}/Zn but more positive than Al^{3+}/Al.

Select a metal that fits these criteria, meaning it can reduce Zn^{2+} to Zn but not Al^{3+} to Al.

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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. In this context, understanding the standard reduction potentials of Zn2+ and Al3+ is crucial to determine which metal can reduce Zn2+ but not Al3+.

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 consulting this series, one can identify metals that can reduce specific metal ions based on their relative positions and potentials in the series.

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). Understanding the principles of oxidation and reduction is essential for determining which metals can reduce certain ions, as it directly relates to their ability to donate electrons in a 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)

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)

Textbook Question

Which metal can be oxidized with an Mn2+ solution but not with an Mg2+ solution?

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. Cu

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. Ag