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Chapter 16: Problem 13

(a) What is the difference between the Arrhenius and the Bronsted-Lowry definitions of an acid? (b) \(\mathrm{NH}_{3}(g)\) and \(\mathrm{HCl}(g)\) react to form the ionic solid \(\mathrm{NH}_{4} \mathrm{Cl}(s) .\) Which substance is the Bronsted-Lowry acid in this reaction? Which is the Bronsted-Lowry base?

Short Answer

Expert verified
(a) The Arrhenius definition states that an acid is a substance that dissociates in water to produce hydrogen ions (H+), while a base produces hydroxide ions (OH-). The Bronsted-Lowry definition states that an acid is a proton (H+) donor and a base is a proton (H+) acceptor. (b) In the reaction \(\mathrm{NH}_{3}(g) + \mathrm{HCl}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\), HCl is the Bronsted-Lowry acid as it donates a proton to NH3. NH3 is the Bronsted-Lowry base since it accepts the proton from HCl.

Step by step solution

01

Define the Arrhenius and Bronsted-Lowry acids

According to the Arrhenius theory, an acid is a substance that dissociates in water to produce hydrogen ions (H+) while a base is a substance that dissociates in water to produce hydroxide ions (OH-). Meanwhile, the Bronsted-Lowry theory states that an acid is a proton (H+) donor, and a base is a proton (H+) acceptor.
02

Identify the Bronsted-Lowry acid and base in the given reaction

We have the reaction: \(\mathrm{NH}_{3}(g) + \mathrm{HCl}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl} (s)\) In this reaction, the NH3 molecule accepts a proton (H+) from the HCl molecule to form the NH4+ ion, while the Cl- ion is left behind. According to the Bronsted-Lowry definition, the proton donor is the acid and the proton acceptor is the base.
03

Determine the Bronsted-Lowry acid and base

In the reaction: \(\mathrm{NH}_{3}(g) + \mathrm{HCl}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) The HCl molecule donates a proton (H+) to the NH3 molecule, making it the Bronsted-Lowry acid. The NH3 molecule accepts the proton from HCl, making it the Bronsted-Lowry base.

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Most popular questions from this chapter

(a) Why is \(\mathrm{NH}_{3}\) a stronger base than \(\mathrm{H}_{2} \mathrm{O} ?\) (b) Why is \(\mathrm{NH}_{3}\) a stronger base than \(\mathrm{CH}_{4} ?\)

Indicate whether each of the following statements is correct or incorrect. For those that are incorrect, explain why they are wrong. (a) Every Bronsted-Lowry acid is also a Lewis acid. (b) Every Lewis acid is also a Bronsted-Lowry acid. (c) Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases. (d) \(\mathrm{K}^{+}\) ion is acidic in water because it causes hydrating water molecules to become more acidic. (e) The percent ionization of a weak acid in water increases as the concentration of acid decreases.

Write the chemical equation and the \(K_{b}\) expression for the reaction of each of the following bases with water: (a) propylamine,\(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{NH}_{2} ;\) (b) monohydrogen phosphate ion, \(\mathrm{HPO}_{4}^{2-}\); (c) benzoate ion, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2}^{-}\).

Deuterium oxide \(\left(\mathrm{D}_{2} \mathrm{O},\right.\) where \(\mathrm{D}\) is deuterium, the hydrogen- 2 isotope) has an ion-product constant, \(K_{w^{+}}\) of \(8.9 \times 10^{-16}\) at \(20^{\circ} \mathrm{C}\). Calculate \(\left[\mathrm{D}^{+}\right]\) and \(\left[\mathrm{OD}^{-}\right]\) for pure (neutral) \(\mathrm{D}_{2} \mathrm{O}\) at this temperature.

Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (a) \(\mathrm{NH}_{4} \mathrm{Br}\), (b) \(\mathrm{FeCl}_{3},(\mathrm{c})\) \(\mathrm{Na}_{2} \mathrm{CO}_{3},\) (d) \(\mathrm{KClO}_{4},\) (e) \(\mathrm{NaHC}_{2} \mathrm{O}_{4}\)
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