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Conjugate Bases of Brønsted Acids: Formulas and Descriptions
Chapter 9, Problem 12(choose chapter or problem)
Write a formula for the conjugate base formed when each of the following behaves as a Brønsted acid:
a. \(\mathrm{HSO}_{4}^{-}\)
b. \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\)
c. \(\mathrm{HClO}_{4}\)
d. \(\mathrm{NH}_{4}{ }^{+}\)
e. \(\mathrm{HCl}\)
Questions & Answers
QUESTION:
Write a formula for the conjugate base formed when each of the following behaves as a Brønsted acid:
a. \(\mathrm{HSO}_{4}^{-}\)
b. \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\)
c. \(\mathrm{HClO}_{4}\)
d. \(\mathrm{NH}_{4}{ }^{+}\)
e. \(\mathrm{HCl}\)
ANSWER:Step 1 of 6
The single proton transfer between acidic and basic species causes the generation of conjugate acid and base. Conjugate acids are compounds formed by the acceptance of protons by a basic species. Conjugate bases are compounds formed by the donation of protons by an acidic species.
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Conjugate Bases of Brønsted Acids: Formulas and Descriptions
Want To Learn More? To watch the entire video and ALL of the videos in the series:
This video delves into the fundamental concept of conjugate bases in the context of the Brønsted-Lowry theory of acids and bases, explaining how when acids donate protons, they transform into their respective conjugate bases. This understanding is exemplified through the specific reactions of various compounds, illustrating how each Brønsted acid, upon proton donation, gives rise to its corresponding conjugate base.