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Chapter 19: Problem 108

Comment on whether \(\mathrm{F}_{2}\) will become a stronger oxidizing agent with increasing \(\mathrm{H}^{+}\) concentration.

Short Answer

Expert verified
No, the oxidizing power of \( \mathrm{F}_{2} \) is unlikely to be affected by the change in \( \mathrm{H}^{+} \) concentration because this ion is not directly involved in the redox half-reaction of fluorine.

Step by step solution

01

Identify the Redox Half-Reaction

The oxidation half-reaction governing the behavior of \(\mathrm{F}_{2}\) in the solution is: \[ \mathrm{F}_{2}+2e^{-} \rightarrow 2\mathrm{F}^{-}\]. In this reaction, fluorine is reduced as it gains electrons to become fluoride ions.
02

Assess the Effect of \( \mathrm{H}^{+} \)

It is important to note that the addition of \( \mathrm{H}^{+} \) ions does not directly affect the redox half-reaction. However, it increases the acidity of the solution. This changes the overall pH of the solution, which can influence the state of equilibrium.
03

Apply Le Chatelier鈥檚 Principle

Le Chatelier鈥檚 Principle states that if there is a change in concentration of a specific particle in a reaction, the chemical equilibrium will shift to oppose that change. Since the addition of \( \mathrm{H}^{+} \) ions does not directly influence the half-reaction of fluorine, fluorine's ability to act as an oxidizing agent is not likely to increase or decrease with the variation in \( \mathrm{H}^{+} \) concentration.

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Most popular questions from this chapter

Consider the electrolysis of molten barium chloride, \(\mathrm{BaCl}_{2}\). (a) Write the half-reactions. (b) How many grams of barium metal can be produced by supplying 0.50 A for 30 min?

A spoon was silver-plated electrolytically in a \(\mathrm{AgNO}_{3}\) solution. (a) Sketch a diagram for the process. (b) If \(0.884 \mathrm{~g}\) of \(\mathrm{Ag}\) was deposited on the spoon at a constant current of \(18.5 \mathrm{~mA},\) how long (in minutes) did the electrolysis take?

A galvanic cell using \(\mathrm{Mg} / \mathrm{Mg}^{2+}\) and \(\mathrm{Cu} / \mathrm{Cu}^{2+}\) half-cell's operates under standard-state conditions at \(25^{\circ} \mathrm{C}\) and each compartment has a volume of \(218 \mathrm{~mL}\). The cell delivers 0.22 A for \(31.6 \mathrm{~h}\). (a) How many grams of \(\mathrm{Cu}\) are deposited? (b) What is the \(\left[\mathrm{Cu}^{2+}\right]\) remaining?

Consider a galvanic cell consisting of a magnesium electrode in contact with \(1.0 \mathrm{MMg}\left(\mathrm{NO}_{3}\right)_{2}\) and a cadmium electrode in contact with \(1.0 \mathrm{M} \mathrm{Cd}\left(\mathrm{NO}_{3}\right)_{2}\) Calculate \(E^{\circ}\) for the cell, and draw a diagram showing the cathode, anode, and direction of electron flow.

From the following information, calculate the solubility product of AgBr: $$ \begin{array}{ll} \mathrm{Ag}^{+}(a q)+e^{-} \longrightarrow \mathrm{Ag}(s) & E^{\circ}=0.80 \mathrm{~V} \\ \operatorname{AgBr}(s)+e^{-} \longrightarrow \mathrm{Ag}(s)+\mathrm{Br}^{-}(a q) & E^{\circ}=0.07 \mathrm{~V} \end{array} $$
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