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Chapter 10: Problem 109

You create a battery using a zinc anode in a solution of \(\mathrm{Zn}^{2+}\) ions connected to a nickel cathode in a solution of \(\mathrm{Ni}^{2+}\) ions. The two beakers are also connected with a salt bridge containing \(\mathrm{K}^{+}\) ions and \(\mathrm{Cl}^{-}\) ions. (a) Toward which electrode do \(\mathrm{K}^{+}\) ions flow? (b) Toward which electrode do \(\mathrm{Cl}^{-}\) ions flow?

Short Answer

Expert verified
(a) The \(\mathrm{K}^{+}\) ions flow towards the anode. (b) The \(\mathrm{Cl}^{-}\) ions flow towards the cathode.

Step by step solution

01

Identify the half-reactions at each electrode

First, let's identify the half-reactions happening at both the anode and the cathode. At the anode, oxidation takes place, whereas at the cathode, reduction takes place. For the given galvanic cell, the half-reactions are as follows: Anode (oxidation): \[ \mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2 e^{-} \] Cathode (reduction): \[ \mathrm{Ni}^{2+} + 2 e^{-} \rightarrow \mathrm{Ni} \]
02

Determine the direction of electron flow

In a galvanic cell, the electrons flow from the anode (where oxidation occurs) to the cathode (where reduction occurs). In this problem, electrons flow from the zinc electrode to the nickel electrode.
03

Determine the flow of \(\mathrm{K}^{+}\) ions

Now, let's determine in which direction the \(\mathrm{K}^{+}\) ions flow. Recall that at the anode, oxidation takes place, leading to the production of \(\mathrm{Zn}^{2+}\) ions. To maintain electro-neutrality in the anode beaker, some positive ions have to flow from the salt bridge to the anode solution. Because \(\mathrm{K}^{+}\) ions are positively charged, they will flow towards the anode compartment to balance the increase in \(\mathrm{Zn}^{2+}\) ions. Answer (a): The \(\mathrm{K}^{+}\) ions flow towards the anode.
04

Determine the flow of \(\mathrm{Cl}^{-}\) ions

Finally, let's determine in which direction the \(\mathrm{Cl}^{-}\) ions flow. At the cathode, reduction takes place, and \(\mathrm{Ni}^{2+}\) ions are consumed from the solution. To maintain electro-neutrality in the cathode beaker, some negative ions have to flow from the salt bridge to the cathode solution. Since \(\mathrm{Cl}^{-}\) ions are negatively charged, they will flow towards the cathode compartment to balance the decrease in \(\mathrm{Ni}^{2+}\) ions. Answer (b): The \(\mathrm{Cl}^{-}\) ions flow towards the cathode.

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Most popular questions from this chapter

Consider the following molecules. Without using the shortcut rules, determine the oxidation state for each atom in the molecules and show how you calculated it. (a) \(\mathrm{H}_{2}\) (b) \(\mathrm{O}_{2}\) (c) \(\mathrm{Cl}_{2}\) (d) IF

Consider a battery made from lead, \(\mathrm{Pb}\), and copper, \(\mathrm{Cu}\), along with \(\mathrm{Pb}^{2+}\) ions and \(\mathrm{Cu}^{2+}\) ions. In such a battery, what is the oxidizing agent, and what is the reducing agent? (Hint: Start by consulting the EMF series, and determine which metal oxidizes and which metal ion gets reduced.)

A battery is constructed from tin and copper by dipping strips of each metal into a solution of its ions \(\left(\mathrm{Sn}^{2+}\right.\) and \(\mathrm{Cu}^{2+}\), respectively). As the battery operates, the \(\mathrm{Sn}^{2+}\) concentration increases and the \(\mathrm{Cu}^{2+}\) concentration decreases. (a) What is getting oxidized? (b) What is getting reduced? (c) Draw a battery similar to the one you drew for WorkPatch 10.7. Make sure you label which way the electrons flow, and also label the cathode, \(+\), and anode, \(=\)

Draw a Lewis dot diagram for \(\mathrm{H}_{2} \mathrm{O}_{2}\) (hydrogen peroxide), and use the oxidation-state method of electron bookkeeping to determine how many electrons each atom should be assigned.

How are oxidation states useful in determining whether a reaction is a redox reaction?
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