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Chapter 15: Problem 34

The reaction of lime \((\mathrm{CaO})\) with \(\mathrm{SO}_{2}\) in the scrubber of a power plant is a Lewis acid-base reaction. Explain.

Short Answer

Expert verified
\(\text{CaO}\) donates an electron pair, functioning as a Lewis base; \(\text{SO}_2\) accepts it, acting as a Lewis acid.

Step by step solution

01

Identify the substances involved

The substances involved in the reaction within the scrubber are calcium oxide (\(\text{CaO}\)), which is commonly referred to as lime, and sulfur dioxide (\(\text{SO}_2\)).
02

Define Lewis acid and base

In a Lewis acid-base reaction, a Lewis acid is defined as a species that can accept an electron pair, while a Lewis base is a species that can donate an electron pair.
03

Determine the role of CaO

Calcium oxide (\(\text{CaO}\)) acts as a Lewis base in this reaction because the oxygen atom in \(\text{CaO}\) has lone pairs of electrons that it can donate.
04

Determine the role of SO2

Sulfur dioxide (\(\text{SO}_2\)) acts as a Lewis acid because the sulfur atom can accept an electron pair due to its electron-deficient sites.
05

Explain the reaction

In the scrubber, \(\text{CaO}\) donates an electron pair to form an ionic bond with \(\text{SO}_2\), resulting in the formation of calcium sulfite (\(\text{CaSO}_3\)). This interaction is characteristic of a Lewis acid-base reaction, where \(\text{CaO}\) is the Lewis base and \(\text{SO}_2\) is the Lewis acid.

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Key Concepts

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

Calcium Oxide
Calcium oxide, often known as lime, is a widely used chemical compound with the formula \( \text{CaO} \). It forms by heating limestone at high temperatures to remove carbon dioxide. Once formed, calcium oxide serves various purposes but is particularly significant in industrial processes.

In the context of chemistry, calcium oxide plays the role of a Lewis base. This is because the oxygen atom in \( \text{CaO} \) has lone pairs of electrons available. When \( \text{CaO} \) encounters other chemical species, such as sulfur dioxide, these lone pairs can be donated to form new chemical bonds.
  • Industrial Uses: Calcium oxide is often used in construction, agriculture, and as a desiccant due to its ability to react with water and gases.
  • Role in Reactions: As a Lewis base, it primarily participates in reactions by donating its electron pairs to other substances that can accept them.
This ability to donate electron pairs makes \( \text{CaO} \) an active participant in acid-base reactions, such as the one occurring in power plant scrubbers.
Sulfur Dioxide
Sulfur dioxide, known chemically as \( \text{SO}_2 \), is a pungent, toxic gas commonly associated with volcanic activity and industrial emissions. It plays an integral role in atmospheric chemistry and environmental science, where it can influence air quality and health.

From a chemical perspective, sulfur dioxide acts as a Lewis acid. This is due to the presence of electron-deficient sites on the sulfur atom, allowing it to accept electron pairs from other molecules.
  • Environmental Impact: Sulfur dioxide is a significant air pollutant and can lead to the formation of acid rain.
  • Reactivity: As a Lewis acid, \( \text{SO}_2 \) readily accepts electron pairs from bases, making it reactive in industrial processes.
In a reaction with calcium oxide, \( \text{SO}_2 \) accepts electrons, demonstrating its role as a Lewis acid in acid-base chemistry.
Electron Pair Donation
Electron pair donation is a fundamental concept in chemistry and plays a critical role in Lewis acid-base reactions. It involves one molecule or ion providing a pair of electrons to another, creating or strengthening bonds between them.

The entity donating the electron pair is the Lewis base, while the one accepting it is the Lewis acid.
  • Mechanism: During the reaction, the Lewis base uses its lone pairs to form a new bond with the electron-deficient species, the Lewis acid.
  • Outcome: This interaction leads to the formation of compounds, as seen with calcium oxide donating an electron pair to \( \text{SO}_2 \) in a power plant scrubber.
Understanding this concept aids in comprehending various chemical reactions and how new compounds, like calcium sulfite, are formed through such interactions.

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Most popular questions from this chapter

Write a balanced net ionic equation and the corresponding equilibrium equation for the reaction of the following weak bases with water: (a) Dimethylamine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\) (b) Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) (c) Cyanide ion, CN

You may have been told not to mix bleach and ammonia. The reason is that bleach (sodium hypochlorite) reacts with ammonia to produce toxic chloramines, such as \(\mathrm{NH}_{2} \mathrm{Cl}\). For example, in basic solution: \(\mathrm{OCl}^{-}(a q)+\mathrm{NH}_{3}(a q) \longrightarrow \mathrm{OH}^{-}(a q)+\mathrm{NH}_{2} \mathrm{Cl}(a q)\) (a) The following initial rate data for this reaction were obtained in basic solution at \(25^{\circ} \mathrm{C}:\) $$ \begin{array}{lccc} \hline \mathrm{pH} & \text { Initial }\left[\mathrm{OCl}^{-}\right] & \text {Initial }\left[\mathrm{NH}_{3}\right] & \text { Initial Rate }(\mathrm{M} / \mathrm{s}) \\ \hline 12 & 0.001 & 0.01 & 0.017 \\ 12 & 0.002 & 0.01 & 0.033 \\ 12 & 0.002 & 0.03 & 0.100 \\ 13 & 0.002 & 0.03 & 0.010 \\ \hline \end{array} $$ What is the rate law for the reaction? What is the numerical value of the rate constant \(k\), including the correct units? (b) The following mechanism has been proposed for this reaction in basic solution: \(\mathrm{H}_{2} \mathrm{O}+\mathrm{OCl} \rightleftharpoons \mathrm{HOCl}+\mathrm{OH}^{-} \quad\) Fast, equilibrium constant \(K_{1}\) \(\mathrm{HOCl}+\mathrm{NH}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{NH}_{2} \mathrm{Cl}\) Slow, rate constant \(\mathrm{k}_{2}\) Assuming that the first step is in equilibrium and the second step is rate- determining, calculate the value of the rate constant \(k_{2}\) for the second step. \(K_{a}\) for \(\mathrm{HOCl}\) is \(3.5 \times 10^{-8} .\)

Aqueous solutions of hydrogen sulfide contain \(\mathrm{H}_{2} \mathrm{~S}, \mathrm{HS}^{-}, \mathrm{S}^{2-}\). \(\mathrm{H}_{3} \mathrm{O}^{+}, \mathrm{OH}^{-}\), and \(\mathrm{H}_{2} \mathrm{O}\) in varying concentrations. Which of these species can act only as an acid? Which can act only as a base? Which can act both as an acid and as a base?

Calculate the concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+}\) and \(\mathrm{SO}_{4}^{2-}\) in a solution prepared by mixing equal volumes of \(0.2 \mathrm{M} \mathrm{HCl}\) and \(0.6 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\left(K_{a 2}\right.\) for \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is \(\left.1.2 \times 10^{-2}\right)\)

Lactated Ringer's solution is given intravenously to replenish fluids in patients who have experienced significant blood loss. The solution contains several different ions including sodium, potassium, chloride, calcium, and lactate \(\left(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}_{3}^{-}\right) .\) Lactate is the only species that affects the \(\mathrm{pH}\). The solution has a lactate concentration of \(0.028 \mathrm{M}\) and \(\mathrm{pH}\) of 8.15. What is the value of \(K_{\mathrm{b}}\) for lactate?
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