Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 75

\(\mathrm{Al}^{3+}\) is not a Brønsted acid but \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) is. Explain.

Short Answer

Expert verified
The Al3+ ion cannot act as a Bronsted acid because it has no proton to donate, while Al(H2O)6 3+ can due to the ability of its water molecules to donate a proton, resulting in the formation of a hydronium ion (H3O+).

Step by step solution

01

Description of the ions

Al3+ refers to the aluminum ion, which is a positively charged ion formed by loss of 3 electrons from an neutral aluminum atom. On the other hand, Al(H2O)6 3+ is an complex ion formed when aluminum ion interacts with six water molecules.
02

Identifying Proton Donors

In Al3+, there are no substance which can act as a source of proton (H+). Therefore, Al3+ cannot act as a Bronsted acid because it has no proton to donate.
03

Recognizing the capacity of Al(H2O)6 3+ as a Bronsted acid

In the Al(H2O)6 3+ complex ion, there are 6 water molecules. A water molecule (H2O) has two hydrogen atoms which are potential sources for proton (H+) donation. Thus, when one of these water molecules loses a proton it results in the formation of a hydroxide ion (OH-) and a hydronium ion (H3O+). The generation of the H3O+ ion indicates that the complex ion Al(H2O)6 3+ can indeed act as a Bronsted acid because it shows the ability to donate a proton.

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

Compare the strengths of the following pairs of acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SeO}_{4}\), (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{3} \mathrm{AsO}_{4}\).

Explain why small, highly charged metal ions are able to undergo hydrolysis.

From the relationship \(K_{\mathrm{a}} K_{\mathrm{b}}=K_{\mathrm{w}},\) what can you deduce about the relative strengths of a weak acid and its conjugate base?

Use Le Châtelier's principle to predict the effect of the following changes on the extent of hydrolysis of sodium nitrite \(\left(\mathrm{NaNO}_{2}\right)\) solution: (a) \(\mathrm{HCl}\) is added, (b) \(\mathrm{NaOH}\) is added, (c) \(\mathrm{NaCl}\) is added, (d) the solution is diluted.

You are given two beakers, one containing an aqueous solution of strong acid (HA) and the other an aqueous solution of weak acid (HB) of the same concentration. Describe how you would compare the strengths of these two acids by (a) measuring the \(\underline{p H},\) (b) measuring electrical conductance, (c) studying the rate of hydrogen gas evolution when these solutions are reacted with an active metal such as \(\mathrm{Mg}\) or \(\mathrm{Zn}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

Organic 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.

Sign-up for free