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Chapter 23: Problem 16

Suggest a series of reactions, using common chemicals, by which each of the following syntheses can be performed. (a) \(\mathrm{Cu}(\mathrm{OH})_{2}(\mathrm{s})\) from \(\mathrm{CuO}(\mathrm{s})\) (b) \(\operatorname{Cr} \mathrm{Cl}_{3}\left(\text { aq) } \text { from }\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{s})\right.\)

Short Answer

Expert verified
a) Copper(II) Hydroxide can be synthesized from Copper(II) Oxide by combining it with water. \n b) Chromium(III) Chloride can be synthesized from ammonium dichromate through a two-step process involving a redox reaction with zinc and sulfuric acid to form Chromium(III) ions, which can then combine with Chloride ions from hydrochloric acid to form Chromium(III) Chloride.

Step by step solution

01

Part (a): Synthesis of Copper(II) Hydroxide

The reaction needed to transform CuO into Cu(OH)2 requires adding a substance that can produce hydroxide ions in solution. A common source of this is water (H2O). As the reaction occurs, CuO reacts with H2O to form Cu(OH)2. This can be represented as: \[ \mathrm{CuO(s)} + \mathrm{H2O(l)} \rightarrow \mathrm{Cu(OH)2(s)} \] This reaction is a type of chemical reaction called a combination reaction.
02

Part (b): Synthesis of Chromium(III) Chloride

We will first transform the dichromate ion into a chromium(III) ion with a redox reaction involving zinc and sulfuric acid. This is done using the reaction: \[ \left(\mathrm{NH4}\right)_{2}\mathrm{Cr2O7} + 14\mathrm{Zn} + 8\mathrm{H2SO4} \rightarrow 2\mathrm{Cr^{3+}} + 7\mathrm{Zn^{2+}} + 16\mathrm{OH^-} + 2\mathrm{N2} + 8\mathrm{SO4^{2-}} \] Then, we turn the Cr3+ ion into CrCl3, this is achieved by introducing a Chlorine ion source such as hydrochloric acid (HCl). The reaction can be expressed as follows: \[ \mathrm{Cr^{3+}} + 3\mathrm{Cl^-} \rightarrow \mathrm{CrCl3} \] These reactions are both redox reactions as there are changes in the oxidation state of elements.

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Most popular questions from this chapter

All of the following elements have an ion displaying the +6 oxidation state except (a) Mo; (b) Cr; (c) Mn; (d) \(\mathrm{V} ;\) (e) S.

Write plausible half-equations to represent each of the following in basic solution. (a) oxidation of \(\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})\) to \(\mathrm{FeO}_{4}^{2-}\) (b) reduction of \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\) to silver metal

The metallic radii of \(\mathrm{Ni}\), \(\mathrm{Pd}\), and \(\mathrm{Pt}\) are \(125,138,\) and \(139 \mathrm{pm},\) respectively. Why is the difference in radius between Pt and Pd so much less than between Pd and Ni?

Explain the important distinctions between each pair of terms: (a) ferromagnetism and paramagnetism; (b) roasting and reduction; (c) hydrometallurgy and pyrometallurgy; (d) chromate and dichromate.

Complete and balance the following equations. If no reaction occurs, so state. (a) \(\operatorname{TiCl}_{4}(\mathrm{g})+\mathrm{Na}(1) \stackrel{\Delta}{\longrightarrow}\) (b) \(\mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{Al}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\) (c) \(\mathrm{Ag}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow\) (d) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{aq})+\mathrm{KOH}(\mathrm{aq}) \longrightarrow\) (e) \(\mathrm{MnO}_{2}(\mathrm{s})+\mathrm{C}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\)
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