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Chapter 16: Problem 26

(a) Which of the following is the stronger Br酶nstedLowry acid, \(\mathrm{HBrO}\) or \(\mathrm{HBr}\) ? (b) Which is the stronger Br酶nsted-Lowry base, \(\mathrm{F}^{-}\) or \(\mathrm{Cl}^{-} ?\) Briefly explain your choices.

Short Answer

Expert verified
(a) The stronger Br酶nsted-Lowry acid is HBr as its conjugate base (Br鈦�) is more stable than that of HBrO (BrO鈦�). (b) The stronger Br酶nsted-Lowry base is Cl鈦� as its conjugate acid (HCl) is less stable than that of F鈦� (HF).

Step by step solution

01

Compare the Br酶nsted-Lowry acidity of HBrO and HBr

To compare the acidity of HBrO and HBr, we must compare the stability of their conjugate bases, which are BrO鈦� and Br鈦� respectively.
02

Determine the stability of BrO鈦� and Br鈦�

BrO鈦� is a conjugate base formed by the removal of a proton from the O-H bond in HBrO, while Br鈦� is formed by the removal of a proton from the H-Br bond in HBr. The stability of a conjugate base depends on the strength of the bond between the proton and the atom to which it is attached. In HBrO, the proton is attached to an oxygen atom, while in HBr, the proton is attached to a bromine atom. The bond strength of O-H is generally stronger than that of H-Br.
03

Compare their acidity

As the O-H bond in HBrO is stronger than the H-Br bond in HBr, it is expected that the conjugate base BrO鈦� will be less stable than Br鈦�. The less stable the conjugate base, the weaker the acid. Therefore, HBrO is a weaker acid than HBr. So, the stronger Br酶nsted-Lowry acid is HBr.
04

Compare the Br酶nsted-Lowry basicity of F鈦� and Cl鈦�

To compare the basicity of F鈦� and Cl鈦�, we must compare the stability of their conjugate acids, which are HF and HCl respectively.
05

Determine the stability of HF and HCl

The stability of a conjugate acid is related to the strength of the bond between the proton (H) and the atom to which it is attached. In HF, the H-F bond is stronger than the H-Cl bond in HCl, which means that HF is more stable than HCl.
06

Compare their basicity

As HF is more stable than HCl, F鈦� is a weaker base than Cl鈦�. The less stable the conjugate acid, the stronger the base. Therefore, the stronger Br酶nsted-Lowry base is Cl鈦�.
07

Summary

(a) The stronger Br酶nsted-Lowry acid is HBr. (b) The stronger Br酶nsted-Lowry base is Cl鈦�.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid-Base Theory
The Br酶nsted-Lowry acid-base theory defines an acid as a substance that can donate a proton (H+), and a base as a substance that can accept a proton. According to this theory, acids and bases always come in pairs known as conjugate acid-base pairs. When an acid donates a proton, it forms a conjugate base; conversely, when a base accepts a proton, it forms a conjugate acid.

In the context of the given exercise, when comparing HBrO and HBr, we consider the concept of bond strength and the stability of the resulting conjugate bases. A stronger bond in the acid means it's less likely to donate its proton, rendering it a weaker acid. Therefore, by scrutinizing the stability of the conjugate bases (BrO鈦� and Br鈦�), we can infer the relative strengths of the acids (HBrO and HBr).
Conjugate Acid-Base Pairs
Understanding conjugate acid-base pairs is critical for interpreting reactions in acid-base chemistry. When an acid like HBrO loses a proton, it becomes its conjugate base, BrO鈦�. Similarly, HBr, upon losing a proton, forms Br鈦�. These pairs are of great importance because they help explain the reversibility of acid-base reactions and provide insight into the strength of acids and bases.

For example, the stronger an acid, the weaker its conjugate base. This principle can be applied to the exercise problem where we compare the acid strength of HBrO and HBr by examining their conjugate bases. Since Br鈦� (conjugate base of HBr) is more stable than BrO鈦� (conjugate base of HBrO), HBr emerges as the stronger acid.
Bond Strength and Acidity
The strength of a bond between a hydrogen atom and its attached atom significantly influences the acidity of a molecule. Stronger bonds generally mean that the molecule is less likely to release a hydrogen ion, making it a weaker acid. The stability of the conjugate base formed after the acid donates a proton is also an important factor influencing acidity.

In the textbook exercise, we compare the stability of the conjugate bases BrO鈦� and Br鈦�. Since the bond strength in HBr, which involves a hydrogen-bromine bond, is weaker than that in HBrO, which has a hydrogen-oxygen bond, HBr is more willing to donate its hydrogen ion, categorizing it as a stronger acid. Thus, the trend in bond strength directly impacts the acidity in this scenario, helping us understand why HBr is the stronger acid compared to HBrO.

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Most popular questions from this chapter

Indicate whether each of the following statements is correct or incorrect. For those that are incorrect, explain why they are wrong. (a) Every Br酶nsted-Lowry acid is also a Lewis acid. (b) Every Lewis acid is also a Br酶nsted-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.

Although \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) have very different properties as pure substances, their aqueous solutions possess many common properties. List some general properties of these solutions, and explain their common behavior in terms of the species present.

(a) What does the term autoionization mean? (b) Explain why pure water is a poor conductor of electricity. (c) You are told that an aqueous solution is acidic. What does this statement mean?

(a) Which of the following is the stronger Br酶nstedLowry acid, \(\mathrm{HBrO}\) or \(\mathrm{HBr}\) ? (b) Which is the stronger Br酶nsted-Lowry base, \(\mathrm{F}^{-}\) or \(\mathrm{Cl}^{-} ?\) Briefly explain your choices.

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 \(\mathrm{H}^{+}\) ?
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