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Chapter 18: Problem 3

You want to "plate out" nickel metal from a nickel nitrate solution onto a piece of metal inserted into the solution. Should you use copper or zinc? Explain.

Short Answer

Expert verified
Zinc should be used instead of copper for the plating process because it has a more negative reduction potential (\(E掳_{Zn} = -0.76 V\)), making it more reactive than copper (\(E掳_{Cu} = +0.34 V\)). This higher reactivity will allow zinc to more easily lose electrons, enabling the deposition of nickel metal from the nickel nitrate solution.

Step by step solution

01

Identify the Metals' Standard Reduction Potentials

The first step is to identify the standard reduction potentials of the metals in question, which will allow us to determine which metal is more reactive. The standard reduction potentials of copper, zinc, and nickel are as follows: Copper (Cu): \[E掳_{Cu} = +0.34 V\] Zinc (Zn): \[E掳_{Zn} = -0.76 V\] Nickel (Ni): \[E掳_{Ni} = -0.25 V\]
02

Compare the Reactivities

Next, compare the reactivity of the metals by comparing their standard reduction potentials. Remember that the more negative the reduction potential, the more likely a metal is to lose electrons, which is indicative of its reactivity. Since \(E掳_{Zn} = -0.76 V\) and \(E掳_{Cu} = +0.34 V\), it is clear that zinc (\(Zn\)) has a more negative reduction potential than copper (\(Cu\)). Consequently, zinc is more reactive than copper.
03

Choose the Metal for the Plating Process

Given that zinc is more reactive than copper, when placed in a nickel nitrate solution, zinc would be more likely to lose electrons. This would result in the zinc dissolving into the solution and the nickel ions in the solution gaining electrons and depositing as metallic nickel onto the zinc metal surface. Therefore, to plate out nickel metal from a nickel nitrate solution, zinc should be used instead of copper.

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Most popular questions from this chapter

The black silver sulfide discoloration of silverware can be removed by heating the silver article in a sodium carbonate solution in an aluminum pan. The reaction is $$3 \mathrm{Ag}_{2} \mathrm{~S}(s)+2 \mathrm{Al}(s) \rightleftharpoons 6 \mathrm{Ag}(s)+3 \mathrm{~S}^{2-}(a q)+2 \mathrm{Al}^{3+}(a q)$$ a. Using data in Appendix 4 , calculate \(\Delta G^{\circ}, K\), and \(\mathscr{C}^{\circ}\) for the above reaction at \(25^{\circ} \mathrm{C}\). (For \(\mathrm{Al}^{3+}(a q), \Delta G_{\mathrm{f}}^{\circ}=-480 . \mathrm{kJ} / \mathrm{mol}\).) b. Calculate the value of the standard reduction potential for the following half-reaction: $$2 \mathrm{e}^{-}+\mathrm{Ag}_{2} \mathrm{~S}(s) \longrightarrow 2 \mathrm{Ag}(s)+\mathrm{S}^{2-}(a q)$$

Is the following statement true or false? Concentration cells work because standard reduction potentials are dependent on concentration. Explain.

What reactions take place at the cathode and the anode when each of the following is electrolyzed? a. molten \(\mathrm{NiBr}_{2}\) b. molten \(\mathrm{AlF}_{3}\) c. molten \(\mathrm{MnI}_{2}\)

Consider the following half-reactions: $$\begin{aligned}\mathrm{Pt}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pt} & & \mathscr{E}^{\circ}=1.188 \mathrm{~V} \\ \mathrm{PtCl}_{4}^{2-}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pt}+4 \mathrm{Cl}^{-} & & \mathscr{C}^{\circ}=0.755 \mathrm{~V} \\ \mathrm{NO}_{3}^{-}+4 \mathrm{H}^{+}+3 \mathrm{e}^{-} \longrightarrow \mathrm{NO}+2 \mathrm{H}_{2} \mathrm{O} & & \mathscr{C}^{\circ}=0.96 \mathrm{~V}\end{aligned}$$ Explain why platinum metal will dissolve in aqua regia (a mixture of hydrochloric and nitric acids) but not in either concentrated nitric or concentrated hydrochloric acid individually.

Consider only the species (at standard conditions) $$\mathrm{Br}^{-}, \mathrm{Br}_{2}, \mathrm{H}^{+}, \quad \mathrm{H}_{2}, \quad \mathrm{La}^{3+}, \quad \mathrm{Ca}, \quad \mathrm{Cd}$$ in answering the following questions. Give reasons for your answers. a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by \(\mathrm{MnO}_{4}^{-}\) in acid? d. Which species can be reduced by \(\mathrm{Zn}(s)\) ?
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