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Chapter 22: Problem 13

Freshly prepared solutions containing iodide ion are colorless, but over time they usually turn yellow. Describe a plausible chemical reaction (or reactions) to account for this observation.

Short Answer

Expert verified
Iodide ion (I-) in the solution gets oxidized over time to form iodine (I2), which is yellow. This is why the colorless solution turns yellow over time.

Step by step solution

01

Identifying the initial substance

Identify the initial substance in the solution which is iodide ion (I-). This is a colorless solution.
02

Recognizing the change over time

Recognize that overtime, the solution changes its color to yellow. This indicates that a chemical reaction is taking place.
03

Identifying the product of the reaction

Based on the color change, identify the product of the reaction. Yellow color indicates that the iodide ion (I-) is getting oxidized to iodine (I2). The balanced oxidation reaction is: 2I-(aq) -> I2(s)

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Most popular questions from this chapter

The heavier halogens (Cl, Br, and I) form compounds in which the central halogen atom, \(X\), is bonded directly to oxygen and to fluorine. Several examples are known, including those with formulas of the type \(\mathrm{FXO}_{2}, \mathrm{FXO}_{3, \text { and } \mathrm{F}_{3} \mathrm{XO} . \text { The structures of these }}\) molecules are all consistent with the VSEPR model. Draw Lewis structures and predict the geometries of (a) chloryl fluoride, \(\mathrm{FClO}_{2}\); (b) perchloryl fluoride, \(\mathrm{FClO}_{3} ;(\mathrm{c}) \mathrm{F}_{3} \mathrm{ClO}\).

Explain why the volumes of \(\mathrm{H}_{2}(\mathrm{g})\) and \(\mathrm{O}_{2}(\mathrm{g})\) obtained in the electrolysis of water are not the same.

Show how you would use elemental sulfur, chlorine gas, metallic sodium, water, and air to produce aqueous solutions containing (a) \(\mathrm{Na}_{2} \mathrm{SO}_{3} ;\) (b) \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3} .\) [Hint: You will have to use information from other chapters as well as this one.].

The solubility of \(\mathrm{Cl}_{2}(\mathrm{g})\) in water is \(6.4 \mathrm{g} \mathrm{L}^{-1}\) at \(25^{\circ} \mathrm{C}\) Some of this chlorine is present as \(\mathrm{Cl}_{2},\) and some is found as HOCl or Cl^- For the hydrolysis reaction $$\begin{array}{c}\mathrm{Cl}_{2}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(1) \longrightarrow \\ \mathrm{HOCl}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \\\K_{c}=4.4 \times 10^{-4}\end{array}$$ For a saturated solution of \(\mathrm{Cl}_{2}\) in water, calculate \(\left[\mathrm{Cl}_{2}\right],[\mathrm{HOCl}],\left[\mathrm{H}_{3} \mathrm{O}^{+}\right],\) and \(\left[\mathrm{Cl}^{-}\right]\).

Explain why sulfur can occur naturally as sulfates, but not as sulfites.
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