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Chapter 21: Problem 32

A coordination compound of cobalt(III) contains four ammonia molecules, one sulfate ion, and one chloride ion. Addition of aqueous \(\mathrm{BaCl}_{2}\) solution to an aqueous solution of the compound gives no precipitate. Addition of aqueous \(\mathrm{AgNO}_{3}\) to an aqueous solution of the compound produces a white precipitate. Propose a structure for this coordination compound.

Short Answer

Expert verified
The structure of the coordination compound can be represented as \(\mathrm{[Co(NH_3)_4SO_4Cl]}\), where cobalt(III) is at the center, coordinating with four ammonia molecules and one sulfate ion, while the chloride ion is free in the solution. The sulfate ion acts as a bidentate ligand coordinating to cobalt(III), and its presence prevents the formation of a precipitate when aqueous BaCl鈧� is added to the solution. However, the free chloride ion in the solution forms a white precipitate of AgCl upon the addition of aqueous AgNO鈧�.

Step by step solution

01

Analyse the behavior with BaCl鈧�

When aqueous BaCl鈧� is added to the compound, there is no precipitate. This indicates that the sulfate ion must be coordinating with the cobalt(III) ion. If the sulfate ion was free in solution, adding Ba虏鈦� ions would lead to the formation of solid barium sulfate (BaSO鈧�), a compound that is poorly soluble in water. Since there is no precipitate, we can assume that the sulfate ion is not free; instead, it is coordinated to the cobalt ion.
02

Analyse the behavior with AgNO鈧�

When aqueous AgNO鈧� is added to the solution, a white precipitate is observed. This precipitate is likely silver chloride (AgCl), which forms when chloride ions (Cl鈦�) are present in the solution. Since there is a precipitate, it means that the chloride ion in the compound is free in the solution and available to form the AgCl precipitate.
03

Propose the structure of the coordination compound

Based on the behavior of the coordination compound in the presence of BaCl鈧� and AgNO鈧�, we can propose the following structure for the compound: Cobalt(III) ion is at the center, coordinating with four ammonia molecules, one sulfate ion, and one chloride ion. The sulfate ion is directly bonded to the cobalt ion, while the chloride ion is free in the solution. Therefore, the structure can be represented as: \[ \mathrm{[Co(NH_3)_4SO_4Cl]} \] The cobalt(III) complex ion has the sulfate ion and chloride ion as counterions, with sulfate ion being a bidentate ligand coordinating to cobalt(III), and the chloride ion is present as a free ion in the solution.

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Most popular questions from this chapter

Name the following coordination compounds. a. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2}\) d. \(\mathrm{K}_{4}\left[\mathrm{PtCl}_{6}\right]\) b. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{I}_{3}\) e. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\) c. \(\mathrm{K}_{2}\left[\mathrm{PtCl}_{4}\right]\) f. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]\)

Name the following coordination compounds. a. \(\mathrm{Na}_{4}\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) b. \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\) c. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) d. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)

Draw all the geometrical isomers of \(\left[\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{BrCl}\right]^{+} .\) Which of these isomers also have an optical isomer? Draw the various isomers.

One of the classic methods for the determination of the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas. This solution is then reacted with an acidic solution containing periodate ion; the products are the permanganate and iodate ions. Write balanced chemical equations for both of these steps.

The \(\mathrm{CrF}_{6}^{4-}\) ion is known to have four unpaired electrons. Does the \(\mathrm{F}^{-}\) ligand produce a strong or weak field?
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