/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 26 (a) Which of the following is th... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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�.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

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.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

In which of the following cases is the approximation that the equilibrium concentration of \(\mathrm{H}^{+}(a q)\) is small relative to the initial concentration of HA likely to be most valid: (a) initial \([\mathrm{HA}]=0.100 \mathrm{M}\) and \(K_{a}=1.0 \times 10^{-6}\), (b) initial \([\mathrm{HA}]=0.100 \mathrm{M}\) and \(K_{a}=1.0 \times 10^{-4}\), (c) initial \([\mathrm{HA}]=0.100 \mathrm{M}\) and \(K_{a}=1.0 \times 10^{-3} ?[\) Section \(16.6]\)

If a substance is a Lewis acid, is it necessarily a Br酶nsted-Lowry acid? Is it necessarily an Arrhenius acid? Explain.

(a) How does the strength of an acid vary with the polarity and strength of the \(\mathrm{H}-\mathrm{X}\) bond? (b) How does the acidity of the binary acid of an element vary as a function of the electronegativity of the element? How does this relate to the position of the element in the periodic table?

The odor of fish is due primarily to amines, especially methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right) .\) Fish is often served with a wedge of lemon, which contains citric acid. The amine and the acid react forming a product with no odor, thereby making the less-than-fresh fish more appetizing. Using data from Appendix \(D\), calculate the equilibrium constant for the reaction of citric acid with methylamine, if only the first proton of the citric acid \(\left(K_{a 1}\right)\) is important in the neutralization reaction.

Explain the following observations: (a) \(\mathrm{HNO}_{3}\) is a stronger acid than \(\mathrm{HNO}_{2} ;\) (b) \(\mathrm{H}_{2} \mathrm{~S}\) is a stronger acid than \(\mathrm{H}_{2} \mathrm{O} ;\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a stronger acid than \(\mathrm{HSO}_{4}^{-} ;\) (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a stronger acid than \(\mathrm{H}_{2} \mathrm{SeO}_{4} ;\) (e) \(\mathrm{CCl}_{3} \mathrm{COOH}\) is a stronger acid than \(\mathrm{CH}_{3} \mathrm{COOH}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.