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Chapter 16: Problem 95

Identify the Lewis acid and Lewis base among the reactants in each of the following reactions: (a) $\mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{3}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons$ $$ \left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}(a q)+3 \mathrm{ClO}_{4}^{-}(a q) $$ (b) $\mathrm{CN}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)$ (c) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}(g)+\mathrm{BF}_{3}(g) \rightleftharpoons\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NBF}_{3}(s)$ (d) $\mathrm{HIO}(l q)+\mathrm{NH}_{2}^{-}(l q) \rightleftharpoons \mathrm{NH}_{3}(l q)+\mathrm{IO}^{-}(l q)$ (lg denotes liquid ammonia as solvent)

Short Answer

Expert verified
In the given reactions: (a) \(\mathrm{Fe}^{3+}\) is the Lewis acid and \(\mathrm{H}_{2}\mathrm{O}\) is the Lewis base. (b) \(\mathrm{H}_{2} \mathrm{O}\) is the Lewis acid and \(\mathrm{CN^{-}}\) is the Lewis base. (c) \(\mathrm{BF}_{3}\) is the Lewis acid and \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\) is the Lewis base. (d) \(\mathrm{HIO}(l q)\) is the Lewis acid and \(\mathrm{NH}_{2}^{-}(l q)\) is the Lewis base.

Step by step solution

01

Reaction (a)

In this reaction \(\mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{3}(s)+6 \mathrm{H}_{2}\mathrm{O}(l) \rightleftharpoons\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}(a q)+3\mathrm{ClO}_{4}^{-}(a q)\), we need to identify the Lewis acid and Lewis base. The six water molecules \((\mathrm{H}_{2} \mathrm{O})\) each donate an electron pair to \(\mathrm{Fe}^{3+}\). Thus, the water is the Lewis base, and \(\mathrm{Fe^{3+}}\) is the Lewis acid.
02

Reaction (b)

In this reaction \(\mathrm{CN}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)\), we need to identify the Lewis acid and Lewis base. In this case, the \(\mathrm{CN^{-}}\) ion donates an electron pair to the \(\mathrm{H}\) atom in water. So, the \(\mathrm{CN^{-}}\) ion is the Lewis base, and \(\mathrm{H}_{2} \mathrm{O}\) is the Lewis acid.
03

Reaction (c)

In this reaction \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}(g)+\mathrm{BF}_{3}(g) \rightleftharpoons\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NBF}_{3}(s)\), we need to identify the Lewis acid and Lewis base. Trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}(g)\), donates an electron pair to the boron atom in \(\mathrm{BF}_{3}(g)\). Therefore, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\) is the Lewis base, and \(\mathrm{BF}_{3}\) is the Lewis acid.
04

Reaction (d)

In this reaction \(\mathrm{HIO}(l q)+\mathrm{NH}_{2}^{-}(l q) \rightleftharpoons \mathrm{NH}_{3}(l q)+\mathrm{IO}^{-}(l q)\), we need to identify the Lewis acid and Lewis base. In this case, \(\mathrm{NH}_{2}^{-}(l q)\) donates an electron pair to the \(\mathrm{H}\) atom in \(\mathrm{HIO}(l q)\). Thus, \(\mathrm{NH}_{2}^{-}(l q)\) is the Lewis base, and \(\mathrm{HIO}(l q)\) is the Lewis acid.

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Most popular questions from this chapter

Arrange the following \(0.10 \mathrm{M}\) solutions in order of increasing acidity: (i) \(\mathrm{HCOONH}_{4}\), (ii) \(\mathrm{NH}_{4} \mathrm{Br}\), (iii) \(\mathrm{NaNO}_{3}\), (iv) \(\mathrm{HCOOK},(\mathrm{v}) \mathrm{KF} .\)

In many reactions, the addition of \(\mathrm{AlCl}_{3}\) produces the same effect as the addition of \(\mathrm{H}^{+}\). (a) Draw a Lewis structure for \(\mathrm{AlCl}_{3}\) in which no atoms carry formal charges, and determine its structure using the VSEPR method. (b) What characteristic is notable about the structure in part (a) that helps us understand the acidic character of \(\mathrm{AlCl}_{3}\) ? (c) Predict the result of the reaction between \(\mathrm{AlCl}_{3}\) and \(\mathrm{NH}_{3}\) in a solvent that does not participate as a reactant. (d) Which acid-base theory is most suitable for discussing the similarities between \(\mathrm{AlCl}_{3}\) and \(\mathrm{H}^{+}\) ?

Succinic acid $\left(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{4}\right),\( which we will denote \)\mathrm{H}_{2} \mathrm{Suc}$ is a biologically relevant diprotic acid with the structure shown below. At \(25^{\circ} \mathrm{C}\), the acid-dissociation constants for succinic acid are \(K_{a 1}=6.9 \times 10^{-5}\) and \(K_{a 2}=2.5 \times 10^{-6} .\) (a) Determine the pH of a \(0.32 \mathrm{M}\) solution of $\mathrm{H}_{2} \mathrm{Suc}\( at \)25^{\circ} \mathrm{C}$, assuming that only the first dissociation is relevant. (b) Determine the molar concentration of \(\mathrm{Suc}^{2-}\) in the solution in part (a). (c) Is the assumption you made in part (a) justified by the result from part (b)? (d) Will a solution of the salt NaHSuc be acidic, neutral, or basic?

Which member of each pair produces the more acidic aqueous solution: \((\mathbf{a}) \mathrm{Zn} \mathrm{Br}_{2}\) or \(\mathrm{CdCl}_{2},\) (b) \(\mathrm{CuCl}\) or \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\), (c) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) or \(\mathrm{NiBr}_{2} ?\)

Calculate \(\left[\mathrm{OH}^{-}\right]\) for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) $\left[\mathrm{H}^{+}\right]=0.00010 \mathrm{M} ;(\mathbf{b})\left[\mathrm{H}^{+}\right]=7.3 \times 10^{-14} \mathrm{M} ;(\mathbf{c})\( a solution in which \)\left[\mathrm{OH}^{-}\right]$ is 100 times greater than \(\left[\mathrm{H}^{+}\right]\).
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