You isolate a compound with the formula PtCl4 ·2 KCl. From electrical conductance tests of an aq

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You isolate a compound with the formula PtCl4 ·2 KCl. From...

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.

Key Concepts

Electrical Conductivity Measurements in Ionic Solutions

Electrical conductivity tests help determine the number of ions present in solution by measuring the ease with which electrical current passes through the solution. The observation of three ions per formula unit aligns with the dissociation of the coordination compound into one complex anion and two potassium cations, thereby confirming the structure of the compound.

Precipitation Reactions for Detecting Free Ions

Precipitation reactions are used to probe the presence of free ions in a solution. In this case, the addition of AgNO3 would precipitate free chloride ions as AgCl if they were present. The absence of a precipitate confirms that the chloride ions are coordinated to the metal rather than being free, reinforcing the idea that the complex ion has no counter chloride anions.

Coordination Compound

This concept involves a central metal ion bonded to surrounding molecules or ions (ligands) through coordinate covalent bonds. In the problem, the platinum ion bonds with chloride ions to form a complex ion. Understanding coordination compounds is key to predicting their chemical formula, geometry, and properties such as solubility and ionization behavior in solution.

Complex Ion Formation and Ion Counting

Complex ion formation explains how ligands, such as chloride, coordinate with a central metal ion to form a charged species. The ion counting from the conductivity tests indicates that the compound dissociates into three ions. This suggests that the complex ion [PtCl4]2– is paired with two counter cations (K+), fitting the experimental data, and confirms that all chloride ions are bound within the complex, not free in solution.

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