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Chapter 23: Problem 43

Write plausible equations for the following reactions occurring in the hydrometallurgy of the coinage metals. (a) Copper is precipitated from a solution of copper(II) sulfate by treatment with \(\mathrm{H}_{2}(\mathrm{g})\) (b) Gold is precipitated from a solution of \(\mathrm{Au}^{+}\) by adding iron(II) sulfate. (c) Copper(II) chloride solution is reduced to copper(I) chloride when treated with \(\mathrm{SO}_{2}(\mathrm{g})\) in acidic solution.

Short Answer

Expert verified
The balanced chemical reactions are: \n (a) \(\mathrm{CuSO}_{4}(\mathrm{a.q.}) + \mathrm{H}_{2}(\mathrm{g}) \rightarrow \mathrm{Cu(s)} + \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{a.q.})\) \n (b) \(2 \, \mathrm{Au}^{+}(\mathrm{a.q.}) + 3 \, \mathrm{FeSO}_{4}(\mathrm{a.q.}) \rightarrow 2 \, \mathrm{Au(s)} + 3 \, \mathrm{Fe}^{2+}(\mathrm{a.q.}) + 3 \, \mathrm{SO}_{4}^{2-}(\mathrm{a.q.})\) \n (c) \(2 \, \mathrm{CuCl}_{2}(\mathrm{a.q.}) + \mathrm{SO}_{2}(\mathrm{g}) + 2 \, \mathrm{H}^{+}(\mathrm{a.q.}) \rightarrow 2 \, \mathrm{CuCl}(\mathrm{s}) + \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{a.q.})\)

Step by step solution

01

Write Equation for Precipitation of Copper

Copper(II) sulfate reacts with hydrogen gas to precipitate copper. The reaction can be written as: \[ \mathrm{CuSO}_{4}(\mathrm{a.q.}) + \mathrm{H}_{2}(\mathrm{g}) \rightarrow \mathrm{Cu(s)} + \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{a.q.}) \] This equation is already balanced.
02

Write Equation for Precipitation of Gold

Gold ions react with iron(II) sulfate to precipitate gold. The reaction can be written as: \[ 2 \, \mathrm{Au}^{+}(\mathrm{a.q.}) + 3 \, \mathrm{FeSO}_{4}(\mathrm{a.q.}) \rightarrow 2 \, \mathrm{Au(s)} + 3 \, \mathrm{Fe}^{2+}(\mathrm{a.q.}) + 3 \, \mathrm{SO}_{4}^{2-}(\mathrm{a.q.}) \] Here, we needed to balance the equation by multiplying the gold ions and gold solids by 2, and iron(II) sulfate, iron ions and sulfate ions by 3.
03

Write Equation for Reduction of Copper(II) Chloride

Copper(II) chloride is reduced to copper(I) chloride when treated with sulfur dioxide gas in acidic solution. The reaction can be written as follows: \[ 2 \, \mathrm{CuCl}_{2}(\mathrm{a.q.}) + \mathrm{SO}_{2}(\mathrm{g}) + 2 \, \mathrm{H}^{+}(\mathrm{a.q.}) \rightarrow 2 \, \mathrm{CuCl}(\mathrm{s}) + \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{a.q.}) \] This equation was balanced by multiplying copper(II) chloride and copper(I) chloride by 2.

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Most popular questions from this chapter

By means of a chemical equation, give an example to represent the reaction of (a) a transition metal with a nonoxidizing acid; (b) a transition metal oxide with \(\mathrm{NaOH}(\mathrm{aq}) ;(\mathrm{c})\) an inner transition metal with \(\mathrm{HCl}(\mathrm{aq})\).

Why is it reasonable to expect the chemistry of dichromate ion to involve mainly oxidation-reduction reactions and that of chromate ion to involve mainly precipitation reactions?

Balance the following oxidation-reduction equations. $$\text { (a) } \mathrm{Fe}_{2} \mathrm{S}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{S}(\mathrm{s})$$ $$\begin{aligned} &\text { (b) } \mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\\ &&\mathrm{MnO}_{4}^{-}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}$$ $$\begin{aligned} &\text { (c) } \mathrm{Ag}(\mathrm{s})+\mathrm{CN}^{-}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\\ &&\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \end{aligned}$$

In your own words, define the following terms: (a) domain; (b) flotation; (c) leaching; (d) amalgam.

When a soluble lead compound is added to a solution containing primarily orange dichromate ion, yellow lead chromate precipitates. Describe the equilibria involved.
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