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Chapter 1: Problem 11

What is the Lowry-Bensted acid in (a) HCl dissolved in water; (b) HC1 (unionized) dissolved in benzene? (c) Which solution is the more strongly acidic?

Short Answer

Expert verified
The Lowry-Bensted acid is HCl in both (a) HCl dissolved in water and (b) HCl (unionized) dissolved in benzene. However, HCl dissolved in water is more strongly acidic due to its nearly 100% ionization and formation of hydronium ions (H3O+), while HCl remains mostly unionized in benzene and doesn't have a strong acidic nature. Therefore, the more strongly acidic solution is HCl dissolved in water (solution a).

Step by step solution

01

Identify the Lowry-Bensted acids in each solution.

(a) In a solution of HCl dissolved in water, the Lowry-Bensted acid is HCl. (b) In an HCl (unionized) dissolved in benzene solution, the Lowry-Bensted acid is also HCl.
02

Compare the acidic properties of the two solutions.

To determine which solution is more strongly acidic, we need to consider the extent of proton (H+) ionization in each solution. (a) In the case of HCl dissolved in water, it ionizes nearly 100% to produce H+ (as hydronium ions, H3O+) and Cl- ions: \[ HCl_{(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)} + Cl^-_{(aq)} \] This means the HCl in this solution acts as a strong acid. (b) In the case of HCl dissolved in benzene (a nonpolar solvent), the HCl remains unionized, meaning it doesn't dissociate into its constituent ions: \[ HCl_{(benzene)} \rightleftharpoons H^+_{(benzene)} + Cl^-_{(benzene)} \] Since HCl remains largely unionized in benzene, it doesn't act as a strong acid in this solution.
03

Determine the more strongly acidic solution.

Comparing the two solutions, HCl dissolved in water exhibits a more strongly acidic character due to its nearly 100% ionization and formation of hydronium ions (H3O+). On the other hand, HCl remains mostly unionized in benzene and doesn't have a strong acidic nature. So, the more strongly acidic solution is HCl dissolved in water (solution a).

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Most popular questions from this chapter

(a) Although HC1 (1.27 A) is a longer molecule than HF (0.92 A), it has a smaller dipole moment (1.03 D compared to 1.75 D). How do you account for this fact? (b) The dipole moment of \(\mathrm{CH}_{3} \mathrm{~F}\) is \(1.847 \mathrm{D}\), and of \(\mathrm{CD}_{3} \mathrm{~F}, 1.858 \mathrm{D}\). (D is \({ }^{2} \mathrm{H}\), deuterium.) Compared with the \(\mathrm{C}-\mathrm{H}\) bond, what is the direction of the \(C-D\) dipole?

What are the characteristics which ionic, ion-dipole, and dipole-dipole bonds have in common? How do they differ?

When hydrogen chloride dissolves in water, the product is "hydrochloric acid." Such a solution contains water, \(\mathrm{H}_{3} \mathrm{O} \oplus\), and \(\mathrm{Cl}^{(-)}\). Which of these species are Lewis acids? Lewis bases? If you have more than one compound per category, arrange them in order of decreasing strength.

Why does hydrogen fluoride undergo intermolecular self association while the other hydrogen halides do not?

A gas of molecular weight 58 was found to contain \(82.8 \%\) \(\mathrm{C}\) and \(17.2 \% \mathrm{H}\). What is the molecular formula of this compound?
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