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Chapter 16: Problem 72

In the following reactions indicate which is the Lewis acid and which is the Lewis base: (a) \(\mathrm{SOI}_{2}+\mathrm{BaSO}_{3} \longrightarrow \mathrm{Ba}^{2+}+2 \mathrm{I}^{-}+2 \mathrm{SO}_{2}\) (b) \(\mathrm{HgCl}_{3}^{-}+\mathrm{Cl}^{-} \longrightarrow \mathrm{HgCl}_{4}^{2}\)

Short Answer

Expert verified
In reaction (a) the Lewis acid is BaSO3 and the Lewis base is SOI2. In reaction (b) the Lewis acid is HgCl3- and the Lewis base is Cl-.

Step by step solution

01

Identifying the Lewis Acid and Base in Reaction (a)

In reaction (a), SOI2 is interacting with BaSO3 to produce Ba2+, I-, and SO2. The Lewis base, SOI2, donates an iodine ion which accepts an electron pair from BaSO3, the Lewis acid. Thus, BaSO3 is the Lewis acid, because it receives the electron pair, and SOI2 is the Lewis base, because it donates the electron pair to BaSO3.
02

Identifying the Lewis Acid and Base in Reaction (b)

In reaction (b), HgCl3- is interacting with Cl- to produce HgCl42-. In this reaction, Cl- (the Lewis base) donates its electron pair to HgCl3- (the Lewis acid) which accepts the electron pair. Thus, the Lewis base in this reaction is Cl-, while the Lewis acid is HgCl3-. The Cl- donates an electron pair and the HgCl3- accepts it.

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Most popular questions from this chapter

Which is the stronger acid of each of the following pairs of acids? Explain your reasoning. (a)\( HBr or HI;\) (b\() HOClO or HOBr; (c) I_SCCH_CH_COOH\) or \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CCl}_{2} \mathrm{COOH}\).

\(\mathrm{CO}_{2}(\mathrm{g})\) can be removed from confined quarters (such as a spacecraft) by allowing it to react with an alkali metal hydroxide. Show that this is a Lewis acid-base reaction. For example, $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{LiOH}(\mathrm{s}) \longrightarrow \mathrm{LiHCO}_{3}(\mathrm{s})$$

Complete the following equations in those instances in which a reaction (hydrolysis) will occur. If no reaction occurs, so state. (a) \(\mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (b) \(\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{NO}_{2}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (c) \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (d) \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq})+\) (e) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{O} \longrightarrow\)

Calculate \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) and \(\mathrm{pH}\) in saturated \(\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})\) which contains \(3.9 \mathrm{g} \mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\) per \(100 \mathrm{mL}\) of solution.

The following four equilibria lie to the right: \(\mathrm{N}_{2} \mathrm{H}_{5}^{+}+\) \(\mathrm{CH}_{3} \mathrm{NH}_{2} \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}+\mathrm{CH}_{3} \mathrm{NH}_{3}^{+} ; \mathrm{H}_{2} \mathrm{SO}_{3}+\mathrm{F}^{-} \longrightarrow\) \(\mathrm{HSO}_{3}^{-}+\mathrm{HF} ; \mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \longrightarrow \mathrm{CH}_{3} \mathrm{NH}_{2}+\) \(\mathrm{H}_{2} \mathrm{O} ;\) and \(\mathrm{HF}+\mathrm{N}_{2} \mathrm{H}_{4} \longrightarrow \mathrm{F}^{-}+\mathrm{N}_{2} \mathrm{H}_{5}^{+}\) (a) Rank all the acids involved in order of decreasing acid strength. (b) Rank all the bases involved in order of decreasing base strength. (c) State whether each of the following two equilibria lies primarily to the right or to the left: (i) \(\mathrm{HF}+\mathrm{OH}^{-} \longrightarrow \mathrm{F}^{-}+\mathrm{H}_{2} \mathrm{O} ;\) (ii) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\) \(\mathrm{HSO}_{3}^{-} \longrightarrow \mathrm{CH}_{3} \mathrm{NH}_{2}+\mathrm{H}_{2} \mathrm{SO}_{3}\).
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