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Chapter 16: Problem 12

For each of these reactions, identify the acid and base among the reactants, and state if the acids and bases are Lewis, Arrhenius, and/or Bronsted-Lowry: (a) \(\mathrm{PCl}_{4}^{+}+\mathrm{Cl}^{-} \longrightarrow \mathrm{PCl}_{5}\) (b) \(\mathrm{NH}_{3}+\mathrm{BF}_{3} \longrightarrow \mathrm{H}_{3} \mathrm{NBF}_{3}\) (c) \(\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}\right]^{2+}+\mathrm{H}_{3} \mathrm{O}^{+}\)

Short Answer

Expert verified
(a) Acid: \(\mathrm{PCl}_{4}^{+}\) (Lewis acid); Base: \(\mathrm{Cl}^{-}\) (Lewis base) (b) Acid: \(\mathrm{BF}_{3}\) (Lewis acid); Base: \(\mathrm{NH}_{3}\) (Lewis base) (c) Acid: \(\left[\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{6}\right]^{3+}\) (Bronsted-Lowry acid); Base: \(\mathrm{H}_{2}\mathrm{O}\) (Bronsted-Lowry base)

Step by step solution

01

Identify the acid and base among the reactants

For this reaction, \(\mathrm{PCl}_{4}^{+}\) is donating a \(\mathrm{Cl}^{-}\) to the reactant, which means it is acting as an acid, and \(\mathrm{Cl}^{-}\) is accepting it, so it is acting as the base.
02

Determine the type of acids and bases

Since \(\mathrm{PCl}_{4}^{+}\) is donating a \(\mathrm{Cl}^{-}\), it is a Lewis acid. Since \(\mathrm{Cl}^{-}\) is accepting a \(\mathrm{Cl}^{-}\), it is a Lewis base. The reaction does not involve donating or accepting protons (H\(^+\)), so this reaction does not involve Arrhenius or Bronsted-Lowry acids and bases. (b) \(\mathrm{NH}_{3}+\mathrm{BF}_{3} \longrightarrow \mathrm{H}_{3}\mathrm{NBF}_{3}\)
03

Identify the acid and base among the reactants

In this reaction, \(\mathrm{NH}_{3}\) donates a lone pair of electrons to \(\mathrm{BF}_{3}\). Therefore, \(\mathrm{NH}_{3}\) is acting as the base and \(\mathrm{BF}_{3}\) is acting as the acid.
04

Determine the type of acids and bases

Since this reaction involves the transfer of a lone pair of electrons, both the acid and base in this reaction are Lewis acids and bases. There is no proton (H\(^+\)) transfer, so there are no Arrhenius or Bronsted-Lowry acids and bases in this reaction. (c) \(\left[\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{6}\right]^{3+}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}\mathrm{OH}\right]^{2+}+\mathrm{H}_{3} \mathrm{O}^{+}\)
05

Identify the acid and base among the reactants

In this reaction, \(\left[\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{6}\right]^{3+}\) is donating a proton (H\(^+\)) to the water molecule (H\(_{2}\)O). Hence, \(\left[\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{6}\right]^{3+}\) acts as the acid and water acts as the base (H\(_{2}\)O).
06

Determine the type of acids and bases

Since the reaction involves the transfer of a proton (H\(^+\)), both the acid and base in this reaction are Bronsted-Lowry acids and bases. As there are no lone pairs of electrons being transferred, there are no Lewis acids or bases in this reaction. The reaction involves water, but the dissociation of ions is not evident, so there are no Arrhenius acids and bases in this reaction.

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Most popular questions from this chapter

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 pH of this solution?

Calculate the \(\mathrm{pH}\) of a solution made by adding 2.50 \(\mathrm{g}\) of lithium oxide \(\left(\mathrm{Li}_{2} \mathrm{O}\right)\) to enough water to make 1.500 \(\mathrm{L}\) of solution.

The acid-dissociation constant for chlorous acid \(\left(\mathrm{HClO}_{2}\right)\) is \(1.1 \times 10^{-2} .\) Calculate the concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+}, \mathrm{ClO}_{2}^{-}\) and \(\mathrm{HClO}_{2}\) at equilibrium if the initial concentration of \(\mathrm{HClO}_{2}\) is 0.0125 \(\mathrm{M} .\)

A particular sample of vinegar has a pH of \(2.90 .\) If acetic acid is the only acid that vinegar contains \(\left(K_{a}=1.8 \times 10^{-5}\right)\) calculate the concentration of acetic acid in the vinegar.

(a) Given that \(K_{a}\) for acetic acid is \(1.8 \times 10^{-5}\) and that for hypochlorous acid is \(3.0 \times 10^{-8}\) , which is the stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) Calculate \(K_{b}\) values for \(C H_{3} C O O^{-}\) and \(C 1 O^{-}.\)
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