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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) \(\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}_{3}(a q)\)

Short Answer

Expert verified
In the given reactions: (a) Lewis base: OH⁻; Lewis acid: HNO₂ (b) Lewis base: Br⁻; Lewis acid: FeBr₃ (c) Lewis base: NH₃; Lewis acid: Zn²⁺ (d) Lewis base: H₂O; Lewis acid: SO₂

Step by step solution

01

Reaction (a)

In this reaction, the OH⁻ ion donates a pair of electrons to the hydrogen in HNO₂, forming a bond and creating H₂O. The HNO₂ molecule accepts the electron pair. Thus, OH⁻ is the Lewis base, and HNO₂ is the Lewis acid: Lewis base: OH⁻ Lewis acid: HNO₂
02

Reaction (b)

In this reaction, the Br⁻ ion donates a pair of electrons to the FeBr₃ molecule, creating a bond and forming FeBr₄⁻. The FeBr₃ molecule accepts the electron pair. Thus, Br⁻ is the Lewis base, and FeBr₃ is the Lewis acid: Lewis base: Br⁻ Lewis acid: FeBr₃
03

Reaction (c)

In this reaction, the NH₃ molecules each donate a pair of electrons to the Zn²⁺ ion, creating bonds and forming Zn(NH₃)₄²⁺. The Zn²⁺ ion accepts the electron pairs. Thus, NH₃ is the Lewis base, and Zn²⁺ is the Lewis acid: Lewis base: NH₃ Lewis acid: Zn²⁺
04

Reaction (d)

In this reaction, the H₂O molecule donates a pair of electrons to the sulfur atom in the SO₂ molecule, creating a bond and forming H₂O₃. The SO₂ molecule accepts the electron pair. Thus, H₂O is the Lewis base, and SO₂ is the Lewis acid: Lewis base: H₂O Lewis acid: SO₂

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Most popular questions from this chapter

If a solution of \(\mathrm{HF}\left(K_{a}=6.8 \times 10^{-4}\right)\) has a pH of \(3.65,\) calculate the concentration of hydrofluoric acid.

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: \((\mathbf{a})\mathrm{CH}_{3} \mathrm{COO}^{-},(\mathbf{b}) \mathrm{HCO}_{3}^{-},(\mathbf{c}) \mathrm{O}^{2-},(\mathbf{d}) \mathrm{Cl}^{-},(\mathbf{e}) \mathrm{NH}_{3}\)

Butyric acid is responsible for the foul smell of rancid butter. The \(\mathrm{pK}_{a}\) of butyric acid is 4.84 (a) Calculate the pK \(_{b}\) for the butyrate ion. (b) Calculate the pH of a 0.050 \(M\) solution of butyric acid. (c) Calculate the pH of a 0.050\(M\) solution of sodium butyrate.

How many milliliters of concentrated hydrochloric acid solution \((36.0 \%\) HCl by mass, density \(=1.18 \mathrm{g} / \mathrm{mL})\) are required to produce 10.0 \(\mathrm{L}\) of a solution that has a pH of 2.05\(?\)

Calculate the \(\mathrm{pH}\) of each of the following solutions \((K_{a}\) and \(K_{b}\) values are given in Appendix \(\mathrm{D} ) :\) (a) 0.095\(M\) propionicacid \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOH}\right),(\mathbf{b}) 0.100 M\) hydrogen chromate ion \(\left(\mathrm{HCrO}_{4}^{-}\right),(\mathbf{c}) 0.120 M\) pyridine \(\left(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\right) .\)
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