Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 7

Write a balanced equation showing how the \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) ion can be either a Bronsted-Lowry acid or a Bronsted-Lowry base.

Short Answer

Expert verified
Question: Write two balanced equations showing \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) acting as a Bronsted-Lowry acid and a Bronsted-Lowry base. Answer: As an acid: \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-} \longleftrightarrow \mathrm{H}^+ + \mathrm{H}\mathrm{PO}_{4}^{2-}\); As a base: \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-} + \mathrm{H}^+ \longleftrightarrow \mathrm{H}_{3}\mathrm{PO}_{4}\).

Step by step solution

01

Acting as an Acid

When \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) acts as an acid, it donates a proton, releasing \(\mathrm{H}^+\) and forming \(\mathrm{H}\mathrm{PO}_{4}^{2-}\). The reaction can be represented as: \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-} \longleftrightarrow \mathrm{H}^+ + \mathrm{H}\mathrm{PO}_{4}^{2-}\)
02

Acting as a Base

When \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) acts as a base, it accepts a proton, forming \(\mathrm{H}_{3}\mathrm{PO}_{4}\). The reaction can be represented as: \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-} + \mathrm{H}^+ \longleftrightarrow \mathrm{H}_{3}\mathrm{PO}_{4}\)

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

The \(\mathrm{pH}\) of a \(0.129 \mathrm{M}\) solution of a weak acid, \(\mathrm{HB}\), is \(2.34\). What is \(K_{\mathrm{a}}\) for the weak acid?

Butyric acid, \(\mathrm{HC}_{4} \mathrm{H}_{7} \mathrm{O}_{2}\), is responsible for the odor of rancid butter and cheese. Its \(K_{\mathrm{a}}\) is \(1.51 \times 10^{-5} .\) Calculate \(\left[\mathrm{H}^{+}\right]\) in solutions prepared by adding enough water to the following to make \(1.30 \mathrm{~L}\). (a) \(0.279 \mathrm{~mol}\) (b) \(13.5 \mathrm{~g}\)

Solution \(\mathrm{X}\) has \(\mathrm{pH}\) 11.7. Solution \(\mathrm{Y}\) has \(\left[\mathrm{OH}^{-}\right]=4.5 \times 10^{-2}\). Which solution is more basic? Which has the higher \(\mathrm{pOH}\) ?

Barbituric acid \(\left(K_{\mathrm{a}}=1.1 \times 10^{-4}\right)\) is used in the manufacture of some sedatives. For a \(0.673 \mathrm{M}\) solution of barbituric acid, calculate (a) \(\left[\mathrm{H}^{+}\right]\) (b) \(\left[\mathrm{OH}^{-}\right]\) (c) \(\mathrm{pH}\) (d) \% ionization

Calculate \(K_{a}\) for the weak acids that have the following \(\mathrm{pK}_{\mathrm{a}}\) values. (a) \(3.9\) (b) \(10.12\) (c) \(13.07\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

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