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Chapter 21: Problem 1

You isolate a compound with the formula \(\mathrm{PtCl}_{4} \cdot 2 \mathrm{KCl}\). From electrical conductance tests of an aqueous solution of the compound, you find that three ions per formula unit are present, and you also notice that addition of \(\mathrm{AgNO}_{3}\) does not cause a precipitate. Give the formula for this compound that shows the complex ion present. Explain your findings. Name this compound.

Short Answer

Expert verified
The compound's formula showing the complex ion present is K鈧俒PtCl鈧凨鈧俔, and its name is Potassium hexachloroplatinate(IV). This formula shows that all the chloride ions are included in the complex ion, satisfying the given criteria of three ions per formula unit and no precipitate with AgNO鈧�.

Step by step solution

01

List Possible Dissociation Reactions

We are given the compound's formula as PtCl鈧劼�2KCl. In water, the possible dissociation reactions for this compound can be: 1. PtCl鈧劼测伝 + 2K鈦� 2. [PtCl鈧凨鈧俔鲁鈦� + 2K鈦� 3. [PtCl鈧侹鈧俔虏鈦� + 2K鈦�
02

Verify the Number of Ions per Formula Unit

Given that the compound dissociates into three ions per formula unit, we can compare the possible reactions from Step 1 and eliminate the reactions that do not meet this requirement. 1. PtCl鈧劼测伝 + 2K鈦� 鈫� 3 ions 鉃� Correct 2. [PtCl鈧凨鈧俔鲁鈦� + 2K鈦� 鈫� 3 ions 鉃� Correct 3. [PtCl鈧侹鈧俔虏鈦� + 2K鈦� 鈫� 4 ions 鉃� Incorrect Since the compound shouldn't cause a reaction with AgNO鈧�, this suggests silver chloride (AgCl) is not precipitated. To identify which dissociation reaction satisfies this condition, the complex ion must contain all the chloride ions.
03

Check the AgNO鈧� Reaction

Comparing candidate reactions from Step 2, we need the one where all chloride ions are included in the complex ion and not free chloride ions are present. 1. PtCl鈧劼测伝 + 2K鈦� 鈫� Free chloride ions available, AgCl can precipitate 鉃� Incorrect 2. [PtCl鈧凨鈧俔鲁鈦� + 2K鈦� 鈫� No free chloride ions available, AgCl won't precipitate 鉃� Correct
04

Identify the Compound's Formula and Name

From the analysis above, we found that the dissociation reaction which agrees with the given criteria (three ions/formula unit and no precipitate with AgNO鈧�) is: [PtCl鈧凨鈧俔鲁鈦� + 2K鈦� Hence the compound's formula showing the complex ion present is K鈧俒PtCl鈧凨鈧俔. This compound can be named as Potassium hexachloroplatinate(IV).

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Most popular questions from this chapter

There are three salts that contain complex ions of chromium and have the molecular formula \(\mathrm{CrCl}_{3} \cdot 6 \mathrm{H}_{2} \mathrm{O}\). Treating \(0.27 \mathrm{~g}\) of the first salt with a strong dehydrating agent resulted in a mass loss of \(0.036 \mathrm{~g}\). Treating \(270 \mathrm{mg}\) of the second salt with the same dehydrating agent resulted in a mass loss of \(18 \mathrm{mg}\). The third salt did not lose any mass when treated with the same dehydrating agent. Addition of excess aqueous silver nitrate to \(100.0-\mathrm{mL}\) portions of \(0.100 M\) solutions of each salt resulted in the formation of different masses of silver chloride; one solution yielded 1430 \(\mathrm{mg} \mathrm{AgCl} ;\) another, \(2870 \mathrm{mg} \mathrm{AgCl}\); the third, \(4300 \mathrm{mg} \mathrm{AgCl}\). Two of the salts are green and one is violet. Suggest probable structural formulas for these salts, defending your answer on the basis of the preceding observations. State which salt is most likely to be violet. Would a study of the magnetic properties of the salts be helpful in determining the structural formulas? Explain.

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 complex ion \(\mathrm{Fe}(\mathrm{CN})_{6}{ }^{3-}\) is paramagnetic with one unpaired electron. The complex ion \(\mathrm{Fe}(\mathrm{SCN})_{6}{ }^{3-}\) has five unpaired electrons. Where does \(\mathrm{SCN}^{-}\) lie in the spectrochemical series relative to \(\mathrm{CN}^{-}\) ?

Write electron configurations for the following metals. a. \(\mathrm{Ni}\) b. \(\mathrm{Cd}\) c. \(\mathrm{Zr}\) d. \(\mathrm{Os}\)

What is the electron configuration for the transition metal ion(s) in each of the following compounds? a. \(\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{4}\right]\) b. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{2}\right] \mathrm{I}_{2}\) c. \(\mathrm{Na}_{2}\left[\mathrm{TaF}_{7}\right]\) d. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{Pt} \mathrm{I}_{4}\right]\) Pt forms \(+2\) and \(+4\) oxidation states in compounds.
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