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Ch.16 - Acid-Base Equilibria
All textbooksBrown 14th EditionCh.16 - Acid-Base EquilibriaProblem 19b
Chapter 16, Problem 19b

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

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Identify the concept of conjugate acid-base pairs: A conjugate acid is formed when a base gains a proton (H+), and a conjugate base is formed when an acid loses a proton.
Determine the conjugate acid of HSO_3^-: Add a proton (H+) to HSO_3^- to form its conjugate acid.
Write the chemical equation for the formation of the conjugate acid: HSO_3^- + H^+ \rightarrow H_2SO_3.
Determine the conjugate base of HSO_3^-: Remove a proton (H+) from HSO_3^- to form its conjugate base.
Write the chemical equation for the formation of the conjugate base: HSO_3^- \rightarrow SO_3^{2-} + H^+.

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Key Concepts

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

Conjugate Acid-Base Pairs

In acid-base chemistry, a conjugate acid is formed when a base gains a proton (H+), while a conjugate base is formed when an acid loses a proton. This relationship is essential for understanding how substances interact in chemical reactions, particularly in the context of the Brønsted-Lowry theory of acids and bases.
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Conjugate Acid-Base Pairs

HSO3- as a Base

HSO3- (bisulfite ion) acts as a base because it can accept a proton to form its conjugate acid, H2SO3 (sulfurous acid). Recognizing the role of HSO3- in acid-base reactions is crucial for determining its conjugate acid and base, as it highlights the dynamic nature of proton transfer in these processes.
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Base Example

Identifying Conjugates

To identify the conjugate acid and base of a given species, one must consider the addition or removal of protons. For HSO3-, the conjugate acid is H2SO3, formed by adding a proton, while its conjugate base is SO3^2- (sulfite ion), formed by removing a proton. This systematic approach aids in understanding the behavior of acids and bases in various chemical contexts.
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Related Practice
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)

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Textbook Question

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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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.

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Textbook Question

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

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Textbook Question

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

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Textbook Question

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (a) CH3COO-

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