Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 33

Would the \(\mathrm{pH}\) at the equivalence point of a titration of a weak acid with a strong base be less than, equal to, or greater than 7.0\(?\)

Short Answer

Expert verified
The pH at the equivalence point of a titration of a weak acid with a strong base would be greater than 7.

Step by step solution

01

Understand the Solution at Equivalence Point during Titrations

During a titration, the equivalence point is the point at which the quantity of titrant added is enough to react completely with the substance being titrated. When titrating a weak acid with a strong base, the strong base ionizes completely while the weak acid only partially ionizes. At the equivalence point, all of the weak acid has reacted with the strong base to produce a salt and water.
02

Determine the Basicity at Equivalence Point

The salt formed in the reaction of a weak acid and a strong base undergoes hydrolysis (a reaction with water), where the anion of the salt reacts with water to form a weak base and a hydronium ion. This leads to an increase in the concentration of hydroxide ions (\( OH^- \)). The excess of \( OH^- \) ions makes the solution basic.
03

Infer the pH at Equivalence Point

A basic solution has a pH greater than 7. Since the solution at the equivalence point is basic due to the reaction of a weak acid with a strong base, the pH at the equivalence point is therefore greater than 7.

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

Describe how you would prepare one or more buffer solutions, including which compounds to use. Predict the pH of each solution. If your teacher provides the needed materials, measure the pH to test your prediction.

How much \(\mathrm{HCl}\) would you need to dissolve in 1.0 \(\mathrm{L}\) of water so that \(\left[\mathrm{OH}^{-}\right]=\) \(6.0 \times 10^{-12} \mathrm{M} ?\)

Describe two precautions that should be taken to ensure an accurate titration.

Can you neutralize a strong acid solution by adding an equal volume of a weak base having the same molarity as the acid? Support your position.

Explain the difference between end point and equivalence point. Why is it important that both occur at approximately the same pH in a titration?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

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