Question

Write a formula for the conjugate base formed when each of the following behaves as a Bronsted acid: a. $\mathrm{HSO}_3{ }^{-}$ b. $\mathrm{HPO}_4^{2-}$ c. $\mathrm{HClO}_3$ d. $\mathrm{CH}_3 \mathrm{NH}_3{ }^{+}$ e. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$

Name: Problem 11, Chapter 9: Chemistry for Today: General, Organic, and Biochemistry
Uploaded: 2022-02-23T23:43:35-08:00
Duration: 2 min 12 s
Channel: Mystique Till
Description: Write a formula for the conjugate base formed when each of the following behaves as a Bronsted acid: a. HSO3 ^- b. HPO4^2- c. HClO3 d. CH3 NH3 ^+ e. H2 C2 O4

   Write a formula for the conjugate base formed when each of the following behaves as a Bronsted acid:
a. $\mathrm{HSO}_3{ }^{-}$
b. $\mathrm{HPO}_4^{2-}$
c. $\mathrm{HClO}_3$
d. $\mathrm{CH}_3 \mathrm{NH}_3{ }^{+}$
e. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$

Chemistry for Today: General, Organic, and Biochemistry

Spencer L. Seager,… 10th Edition

Chapter 9, Problem 11

Instant Answer

Solved by Expert Mystique Till

02/23/2022

Step 1

A Brønsted acid is a substance that donates a proton (H⁺) to another substance. The conjugate base is what remains after the acid has donated a proton. Show more…

Show all steps

Thanks for your feedback!

Write a formula for the conjugate base formed when each of the following behaves as a Bronsted acid: a. $\mathrm{HSO}_3{ }^{-}$ b. $\mathrm{HPO}_4^{2-}$ c. $\mathrm{HClO}_3$ d. $\mathrm{CH}_3 \mathrm{NH}_3{ }^{+}$ e. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$

Play audio

Feedback

Mystique Till and 62 other educators are ready to help you.

Ask a new question

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Conjugate Base

The conjugate base is the species that results when a Bronsted acid donates a proton. It is essentially the original molecule after it has lost a hydrogen ion, usually carrying a negative charge or a reduced positive charge compared to the acid. Understanding the formation and properties of conjugate bases is crucial in analyzing acid-base equilibrium and predicting further chemical reactions.

Bronsted Acid

A Bronsted acid is defined as any species that is capable of donating a proton (H+) in a chemical reaction. This concept is fundamental in acid-base chemistry, where the acid loses a proton to form its corresponding conjugate base. Recognizing a compound as a Bronsted acid helps in predicting its behavior when it reacts with a base.

Please give Ace some feedback