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Chapter 15: Problem 135

Describe the hydration of \(\mathrm{SO}_{2}\) as a Lewis acid-base reaction. (Hint: Refer to the discussion of the hydration of \(\mathrm{CO}_{2}\) in Section \(\left.15.12 .\right)\)

Short Answer

Expert verified
In the hydration of \(\mathrm{SO}_{2}\), \(\mathrm{SO}_{2}\) acts as a Lewis acid and water (\(H_{2}O\)) as a Lewis base. The oxygen atom of \(H_{2}O\) donates an electron pair to \(\mathrm{SO}_{2}\), forming sulphurous acid (\(H_{2}SO_{3}\)). This process is a representation of a Lewis acid-base reaction.

Step by step solution

01

Identifying Lewis Acids and Bases

In a Lewis acid-base reaction, a Lewis acid is a species that accepts an electron pair, while a Lewis base is a species that donates an electron pair. In the case of the hydration of \(\mathrm{SO}_{2}\), water (\(H_{2}O\)) acts as the Lewis base and \(\mathrm{SO}_{2}\) as the Lewis acid since the latter accepts the electron pair from the water molecule.
02

Writing Down the Reaction

Now that the Lewis acid and base have been identified, the hydration reaction can be written as follows: \[\mathrm{SO}_{2} + H_{2}O \rightarrow H_{2}SO_{3}\]where \(\mathrm{SO}_{2}\) (Lewis acid) accepts an electron pair from \(H_{2}O\) (Lewis base) to form \(H_{2}SO_{3}\) (sulphurous acid).
03

Detailing the Bond Formation

In detail, the oxygen atom of water molecule donates its electron pair to form a bond with the sulfur atom of \(\mathrm{SO}_{2}\). Thus, the sulfur of \(\mathrm{SO}_{2}\) shares its vacant orbital with water's electron pair, leading to the formation of sulphurous acid (\(H_{2}SO_{3}\)).

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Most popular questions from this chapter

Hydrocyanic acid (HCN) is a weak acid and a deadly poisonous compound -in the gaseous form (hydrogen cyanide) it is used in gas chambers. Why is it dangerous to treat sodium cyanide with acids (such as HCl) without proper ventilation?

A typical reaction between an antacid and the hydrochloric acid in gastric juice is \(\mathrm{NaHCO}_{3}(s)+\mathrm{HCl}(a q) \rightleftharpoons\) $$ \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g) $$ Calculate the volume (in L) of \(\mathrm{CO}_{2}\) generated from \(0.350 \mathrm{~g}\) of \(\mathrm{NaHCO}_{3}\) and excess gastric juice at 1.00 atm and \(37.0^{\circ} \mathrm{C}\).

A 1.294-g sample of a metal carbonate \(\left(\mathrm{MCO}_{3}\right)\) is reacted with \(500 \mathrm{~mL}\) of a \(0.100 \mathrm{M} \mathrm{HCl}\) solution. The excess HCl acid is then neutralized by \(32.80 \mathrm{~mL}\) of \(0.588 M \mathrm{NaOH} .\) Identify \(\mathrm{M}\).

Prove the statement that when the concentration of a weak acid HA decreases by a factor of \(10,\) its percent ionization increases by a factor of \(\sqrt{10}\). State any assumptions.

Classify each of the following species as a Lewis acid or a Lewis base: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{H}_{2} \mathrm{O},\) (c) \(\mathrm{I}^{-}\), (f) \(\mathrm{OH}^{-},(\mathrm{g}) \mathrm{H}^{+},\) (d) \(\mathrm{SO}_{2}\), (e) \(\mathrm{NH}_{3}\), (h) \(\mathrm{BCl}_{3}\).
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