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Chapter 16: Problem 96

Identify the Lewis acid and Lewis base in each of the following reactions: (a) $\mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ (b) $\mathrm{FeBr}_{3}(s)+\mathrm{Br}^{-}(a q) \rightleftharpoons \mathrm{FeBr}_{4}^{-}(a q)$ (c) $\mathrm{Zn}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q)$ (d) $\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)$

Short Answer

Expert verified
In the given reactions: (a) Lewis acid: \(\mathrm{HNO}_{2}\), Lewis base: \(\mathrm{OH}^{-}\) (b) Lewis acid: \(\mathrm{FeBr}_{3}\), Lewis base: \(\mathrm{Br}^{-}\) (c) Lewis acid: \(\mathrm{Zn}^{2+}\), Lewis base: \(\mathrm{NH}_{3}\) (d) Lewis acid: \(\mathrm{SO}_2\), Lewis base: \(\mathrm{H}_{2}\mathrm{O}\)

Step by step solution

01

Identify Lewis Acid in Reaction (a)

In this reaction, the \(\mathrm{HNO}_{2}\) molecule, when acting as an electron-pair acceptor, can form the bond with the \(\mathrm{OH}^{-}\) ion. Therefore, \(\mathrm{HNO}_{2}\) is the Lewis acid.
02

Identify Lewis Base in Reaction (a)

The hydroxide ion (\(\mathrm{OH}^{-}\)) has a lone pair of electrons which it can donate to form a bond with \(\mathrm{HNO}_{2}\). Thus, \(\mathrm{OH}^{-}\) is the Lewis base. (b) $\mathrm{FeBr}_{3}(s)+\mathrm{Br}^{-}(a q) \rightleftharpoons \mathrm{FeBr}_{4}^{-}(a q)$
03

Identify Lewis Acid in Reaction (b)

In this reaction, the \(\mathrm{FeBr}_{3}\) molecule can accept an electron pair from the \(\mathrm{Br}^{-}\) ion. Therefore, \(\mathrm{FeBr}_{3}\) is the Lewis acid.
04

Identify Lewis Base in Reaction (b)

The bromide ion (\(\mathrm{Br}^{-}\)) has a lone pair of electrons which it can donate to form a bond with \(\mathrm{FeBr}_{3}\). Thus, \(\mathrm{Br}^{-}\) is the Lewis base. (c) $\mathrm{Zn}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q)$
05

Identify Lewis Acid in Reaction (c)

In this reaction, the \(\mathrm{Zn}^{2+}\) ion can accept electron pairs from the four ammonia (\(\mathrm{NH}_{3}\)) molecules. Therefore, \(\mathrm{Zn}^{2+}\) is the Lewis acid.
06

Identify Lewis Base in Reaction (c)

Ammonia (\(\mathrm{NH}_{3}\)) has a lone pair of electrons it can donate to form bonds with the \(\mathrm{Zn}^{2+}\) ion. Thus, \(\mathrm{NH}_{3}\) is the Lewis base. (d) $\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)$
07

Identify Lewis Acid in Reaction (d)

In this reaction, the \(\mathrm{SO}_{2}\) molecule can accept a lone pair of electrons from the water (\(\mathrm{H}_{2}\mathrm{O}\)) molecule to form \(\mathrm{H}_{2}\mathrm{SO}_{3}\). Therefore, \(\mathrm{SO}_{2}\) is the Lewis acid.
08

Identify Lewis Base in Reaction (d)

Water (\(\mathrm{H}_{2}\mathrm{O}\)) can donate a lone pair of electrons to form a bond with the \(\mathrm{SO}_{2}\) molecule. Thus, \(\mathrm{H}_{2}\mathrm{O}\) is the Lewis base.

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Most popular questions from this chapter

Codeine \(\left(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{NO}_{3}\right)\) is a weak organic base. A \(5.0 \times 10^{-3} \mathrm{M}\) solution of codeine has a pH of 9.95. Calculate the value of \(K_{b}\) for this substance. What is the \(\mathrm{p} K_{b}\) for this base?

(a) Give the conjugate base of the following Brønsted Lowry acids: (i) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-},\) (ii) HBr. (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) \(\mathrm{CN}^{-},\) (ii) \(\mathrm{HSO}_{4}^{-}\).

Label each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each case write the formula of its conjugate base, and indicate whether the conjugate base is a strong base, a weak base, or a species with negligible basicity: $(\mathbf{a}) \mathrm{HCOOH},(\mathbf{b}) \mathrm{H}_{2},(\mathbf{c}) \mathrm{CH}_{4},$ (d) \(\mathrm{HF}\) (e) \(\mathrm{NH}_{4}^{+}\).

Saccharin, a sugar substitute, is a weak acid with \(\mathrm{p} K_{a}=2.32\) at \(25^{\circ} \mathrm{C}\). It ionizes in aqueous solution as follows: $$ \mathrm{HNC}_{7} \mathrm{H}_{4} \mathrm{SO}_{3}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{NC}_{7} \mathrm{H}_{4} \mathrm{SO}_{3}^{-}(a q) $$ What is the pH of a \(0.25 \mathrm{M}\) solution of this substance?

Calculate the molar concentration of \(\mathrm{OH}^{-}\) in a \(0.724 \mathrm{M}\) solution of hypobromite ion $\left(\mathrm{BrO}^{-} ; K_{b}=4.0 \times 10^{-6}\right) .\( What is the \)\mathrm{pH}$ of this solution?
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