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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
All textbooksBrown 15th EditionCh.16 - Acid-Base EquilibriaProblem 22
Chapter 16, Problem 22

Identify the Brønsted–Lowry acid and the Brønsted– Lowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side.
(a) HBrO(aq) + H2O(l) ⇌ H3O+(aq) + BrO-(aq)
(b) HSO4-(aq) + HCO3-(aq) ⇌ SO42-(aq) + H2CO3(aq)
(c) HSO3-(aq) + H3O+(aq) ⇌ H2SO3(aq) + H2O(l)

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1
Identify the species that donates a proton (H⁺) on the left side of the equation. This species is the Brønsted–Lowry acid.
Identify the species that accepts a proton (H⁺) on the left side of the equation. This species is the Brønsted–Lowry base.
On the right side of the equation, identify the species that results from the Brønsted–Lowry acid after it donates a proton. This is the conjugate base.
On the right side of the equation, identify the species that results from the Brønsted–Lowry base after it accepts a proton. This is the conjugate acid.
Summarize the identifications: Brønsted–Lowry acid and base on the left, and conjugate acid and base on the right.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Brønsted–Lowry Acid-Base Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework emphasizes the transfer of protons (H⁺ ions) during chemical reactions, allowing for a broader understanding of acid-base behavior beyond just the presence of hydroxide or hydronium ions.
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Bronsted-Lowry Acid-Base Theory

Conjugate Acid-Base Pairs

In the Brønsted–Lowry theory, a conjugate acid is formed when a base gains a proton, while a conjugate base is what remains after an acid donates a proton. This relationship highlights the reversible nature of acid-base reactions, where the products can act as acids or bases in subsequent reactions.
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Conjugate Acid-Base Pairs

Identifying Species in Reactions

To analyze acid-base reactions, it is essential to identify the reactants and products correctly. In the given equation, recognizing which species donate or accept protons allows for the determination of the Brønsted–Lowry acid and base, as well as their corresponding conjugate pairs, facilitating a deeper understanding of the reaction dynamics.
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Related Practice
Textbook Question

The hydrogen sulfite ion 1HSO3-2 is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water.

Textbook Question

Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.

Textbook Question

Identify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equations, and also identify the conjugate acid and conjugate base of each on the right side:

(a) NH4+(aq) + CN-(aq) ⇌ HCN(aq) + NH3(aq)

(b) (CH3)3N(aq) + H2O(l) ⇌ (CH3)3NH+(aq) + OH-(aq)

(c) HCOOH(aq) + PO43-(aq) ⇌ HCOO-(aq)+ HPO42-(aq)

Textbook Question

Give the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.

Textbook Question

What is the conjugate acid of HSO3-? What is its conjugate base?

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Textbook Question

Write an equation for the reaction in which H2C6H7O5-1aq2 acts as a base in H2O1l2.