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Chapter 18: Problem 53

Ferrous sulfate \(\left(\mathrm{FeSO}_{4}\right)\) is often used as a coagulant in water purification. The iron(II) salt is dissolved in the water to be purified, then oxidized to the iron(III) state by dissolved oxygen, at which time gelatinous \(\mathrm{Fe}(\mathrm{OH})_{3}\) forms, assuming the \(\mathrm{pH}\) is above approximately \(6 .\) Write balanced chemical equations for the oxidation of \(\mathrm{Fe}^{2+}\) to \(\mathrm{Fe}^{3+}\) by dissolved oxygen and for the formation of \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\) by reaction of \(\mathrm{Fe}^{3+}(a q)\) with \(\mathrm{HCO}_{3}^{-}(a q)\).

Short Answer

Expert verified
The balanced chemical equations for the water purification process using ferrous sulfate are: 1. The oxidation of iron(II) ions to iron(III) ions by dissolved oxygen: \(4 \ Fe^{2+} (aq) + O_{2} (aq) + 4 \ H^{+} (aq) \rightarrow 4 \ Fe^{3+} (aq) + 2 \ H_{2}O (l)\) 2. The formation of gelatinous iron(III) hydroxide precipitate by the reaction of iron(III) ions with bicarbonate ions: \(Fe^{3+} (aq) + 3 \ HCO_{3}^{-} (aq) \rightarrow Fe(OH)_{3} (s) + 3 \ CO_{2} \ (g) + 3 \ H^{+} (aq)\)

Step by step solution

01

Oxidation of Fe虏鈦� to Fe鲁鈦� by Dissolved Oxygen

First, we have to write a balanced equation for the oxidation of iron(II), which is represented as Fe虏鈦�, to iron(III), represented as Fe鲁鈦�, by dissolved oxygen (O鈧�). In this process, the iron ions will lose one electron (e鈦�) due to oxidation. To balance the equation, we must ensure that there are the same number of atoms of each element on both sides of the equation. Here is the balanced equation for the oxidation of Fe虏鈦� to Fe鲁鈦� by dissolved oxygen: \(4 \ Fe^{2+} (aq) + O_{2} (aq) + 4 \ H^{+} (aq) \rightarrow 4 \ Fe^{3+} (aq) + 2 \ H_{2}O (l)\)
02

Formation of Fe(OH)鈧� by the Reaction of Fe鲁鈦� with HCO鈧冣伝

Now we need to write a balanced chemical equation for the formation of gelatinous Fe(OH)鈧�(s) from the reaction of Fe鲁鈦� with bicarbonate ions (HCO鈧冣伝). This dissolved iron(III) will react with the bicarbonate ions to form the precipitate Fe(OH)鈧�(s) and the gaseous carbon dioxide (CO鈧�). Here is the balanced equation for the formation of Fe(OH)鈧�(s) by the reaction of Fe鲁鈦� with HCO鈧冣伝: \(Fe^{3+} (aq) + 3 \ HCO_{3}^{-} (aq) \rightarrow Fe(OH)_{3} (s) + 3 \ CO_{2} \ (g) + 3 \ H^{+} (aq)\) In summary, the balanced equations for the water purification process using ferrous sulfate are: 1. The oxidation of iron(II) ions to iron(III) ions by dissolved oxygen: \(4 \ Fe^{2+} (aq) + O_{2} (aq) + 4 \ H^{+} (aq) \rightarrow 4 \ Fe^{3+} (aq) + 2 \ H_{2}O (l)\) 2. The formation of gelatinous iron(III) hydroxide precipitate by the reaction of iron(III) ions with bicarbonate ions: \(Fe^{3+} (aq) + 3 \ HCO_{3}^{-} (aq) \rightarrow Fe(OH)_{3} (s) + 3 \ CO_{2} \ (g) + 3 \ H^{+} (aq)\)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation-Reduction Reactions
In the world of chemistry, oxidation-reduction reactions, often simply called redox reactions, are vital processes. These reactions involve the transfer of electrons between substances.

Oxidation occurs when a substance loses electrons, while reduction happens when a substance gains electrons.
  • In our specific exercise, iron(II) ions, represented as \( Fe^{2+} \), lose an electron to become iron(III) ions, \( Fe^{3+} \). This is the oxidation part of the reaction.
  • Meanwhile, the oxygen molecule, \( O_2 \), is reduced, as it gains electrons from the iron ions.
This balanced exchange ensures that the number of electrons lost and gained is equal.

Understanding these reactions is key in many fields such as energy storage, metallurgy, and indeed water purification, where controlling electron transfers can help modify the chemical state of pollutants for easier removal.
Iron Hydroxide Formation
Iron hydroxide formation is an important process in the water treatment industry. This is because the creation of iron hydroxide solids can help get rid of contaminants.

For this to happen, iron(III) ions \( Fe^{3+} \) from a previous oxidation step react with bicarbonate ions \( HCO_3^- \) in water.
  • The chemical reaction results in the formation of gelatinous iron(III) hydroxide, represented as \( Fe(OH)_3 \), which is seen as a solid precipitate.
  • At the same time, carbon dioxide gas \( CO_2 \) is released and hydrogen ions \( H^+ \) are produced.
This complex reaction is helpful in water purification as the formed gelatinous iron hydroxide clusters together impurities, making them easier to remove.

Thus, understanding this reaction is essential to leveraging its benefits in the purification process.
Water Purification Chemistry
Water purification chemistry often relies on a series of chemical reactions to remove impurities and make water safe for consumption. Coagulation is a critical process in this field, which involves clumping together of particles so that they can be easily separated from the water.

In the context of ferrous sulfate, \( FeSO_4 \), being used as a coagulant:
  • First, the chemical reactions convert dissolved iron(II) ions, \( Fe^{2+} \), to iron(III) ions, \( Fe^{3+} \).
  • The iron(III) ion subsequently reacts to form iron(III) hydroxide, \( Fe(OH)_3 \), which is a substantive agent of purification.
This system of reactions ensures efficient coagulation and is crucial for removing contaminants from water, including suspended solids and some heavy metals.

Mastering water purification chemistry can significantly improve water quality and protect public health.

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Most popular questions from this chapter

A reaction that contributes to the depletion of ozone in the stratosphere is the direct reaction of oxygen atoms with ozone: \(\mathrm{O}(g)+\mathrm{O}_{3}(g) \longrightarrow 2 \mathrm{O}_{2}(g)\) At \(298 \mathrm{~K}\) the rate constant for this reaction is \(4.8 \times 10^{5} \mathrm{M}^{-1} \mathrm{~s}^{-1}\). (a) Based on the units of the rate constant, write the likely rate law for this reaction. (b) Would you expect this reaction to occur via a single elementary process? Explain why or why not. (c) From the magnitude of the rate constant, would you expect the activation energy of this reaction to be large or small? Explain. (d) Use \(\Delta H_{f}^{\circ}\) values from Appendix \(\mathrm{C}\) to estimate the enthalpy change for this reaction. Would this reaction raise or lower the temperature of the stratosphere?

The Ogallala aquifer is the largest in the United States, covering \(450,000 \mathrm{~km}^{2}\) across eight states, from South Dakota to Texas. This aquifer provides \(82 \%\) of the drinking water for the people who live in this region, although most \((>75 \%)\) of the water that is pumped from it is for irrigation. Irrigation withdrawals are approximately 18 billion gallons per day. (a) The Ogallala aquifer might run dry, according to some estimates, in 25 years. How many cubic kilometers of water would be withdrawn in a 25 -year period? (b) Explain the processes that would recharge the aquifer.

The concentration of \(\mathrm{H}_{2} \mathrm{O}\) in the stratosphere is about \(5 \mathrm{ppm}\). It undergoes photodissociation according to: $$ \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{H}(g)+\mathrm{OH}(g) $$ (a) Write out the Lewis-dot structures for both products and reactant. (b) Using Table \(8.4,\) calculate the wavelength required to cause this dissociation. (c) The hydroxyl radicals, OH, can react with ozone, giving the following reactions: $$ \begin{array}{l} \mathrm{OH}(g)+\mathrm{O}_{3}(g) \longrightarrow \mathrm{HO}_{2}(g)+\mathrm{O}_{2}(g) \\ \mathrm{HO}_{2}(g)+\mathrm{O}(g) \longrightarrow \mathrm{OH}(g)+\mathrm{O}_{2}(g) \end{array} $$ What overall reaction results from these two elementary reactions? What is the catalyst in the overall reaction? Explain.

(a) What are trihalomethanes (THMs)? (b) Draw the Lewis structures of two example THMs.

One of the principles of green chemistry is that it is better to use as few steps as possible in making new chemicals. How does this principle relate to energy efficiency?
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