Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 16: Problem 5

With which of the following bases will the ionization of acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) proceed furthest toward completion (to the right): (a) \(\mathrm{H}_{2} \mathrm{O} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{Cl}^{-}\) (d) \(\mathrm{NO}_{3}^{-} ?\) Explain your answer.

Short Answer

Expert verified
The ionization of acetic acid proceeds furthest toward completion with \(NO_3^-\) as the base.

Step by step solution

01

Identifying the Bases

Here, the substances \(H_2O\), \(NH_3\), \(Cl^-\), and \(NO_3^-\) are given. In the context of the Bronsted-Lowry theory, these could act as bases, as they have the potential to accept protons.
02

Analyzing the Proton Affinity of the Bases

Given that acetic acid is a weak acid, it will ionize most readily with the base that has the greatest proton affinity. Water and ammonia are both neutral molecules which can act as bases, but their proton affinity is less than that of the negatively charged ions \(Cl^-\) and \(NO_3^-\). Consequently, we can eliminate \(H_2O\) and \(NH_3\).
03

Final Comparison Between \(Cl^-\) and \(NO_3^-\)

Comparing \(Cl^-\) and \(NO_3^-\), the chloride ion is less likely to accept a proton because it is a conjugate base of hydrochloric acid \(HCl\), which is a strong acid. The nitrate ion \(NO_3^-\) is the conjugate base of the weak acid \(HNO_3\). A strong acid has a weak conjugate base and vice versa. Therefore, \(NO_3^-\) has a greater proton affinity than \(Cl^-\).

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Explain why trichloroacetic acid, \(\mathrm{CCl}_{3} \mathrm{COOH},\) is a stronger acid than acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\).

What is the (a) degree of ionization and (b) percent ionization of propionic acid in a solution that is \(0.45 \mathrm{M}\) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H} ?\) $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}\\\ &&\mathrm{p} K_{\mathrm{a}}=4.89 \end{aligned}$$

The conjugate acid of \(\mathrm{HPO}_{4}^{2-}\) is (a) \(\mathrm{PO}_{4}^{3-}\) (b) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-} ;(\mathrm{c}) \mathrm{H}_{3} \mathrm{PO}_{4} ;(\mathrm{d}) \mathrm{H}_{3} \mathrm{O}^{+} ;\) (e) none of these.

Of the following, the amphiprotic ion is (a) \(\mathrm{HCO}_{3}^{-}\) (b) \(\mathrm{CO}_{3}^{2-} ;\) (c) \(\mathrm{NH}_{4}^{+} ;\) (d) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+} ;\) (e) \(\mathrm{ClO}_{4}^{-}\).The \(\mathrm{pH}\) in \(0.10 \mathrm{M} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}(\mathrm{aq})\) must be (a) equal to \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in \(0.10 \mathrm{M} \mathrm{HNO}_{2}(\mathrm{aq}) ;\) (b) less than the \(\mathrm{pH}\) in \(0.10 \mathrm{M} \mathrm{HI}(\mathrm{aq}) ;\) (c) greater than the \(\mathrm{pH}\) in \(0.10 \mathrm{M} \mathrm{HBr}(\mathrm{aq}) ;\) (d) equal to \(1.0.\)

Write the formula of the conjugate base in the reaction of each acid with water. (a) \(\mathrm{HIO}_{3} ;\) (b) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\) (c) \(\mathrm{HPO}_{4}^{2-} ;\) (d) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

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.

Sign-up for free