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Ch.16 - Acids and Bases
All textbooksTro 4th EditionCh.16 - Acids and BasesProblem 95
Chapter 16, Problem 95

Determine if each anion acts as a weak base in solution. For those anions that are basic, write an equation that shows how the anion acts as a base. a. Br– b. ClO– c. CN– d. Cl–

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Identify the anion in question: ClO^- (hypochlorite ion).
Determine if the anion can act as a base by considering its ability to accept a proton (H^+).
Recall that anions derived from weak acids tend to be basic. Hypochlorous acid (HClO) is a weak acid, so ClO^- is likely to be a weak base.
Write the chemical equation showing ClO^- acting as a base by accepting a proton from water: ClO^- + H_2O \rightarrow HClO + OH^-.
Conclude that ClO^- acts as a weak base in solution, as it increases the concentration of OH^- ions.

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Key Concepts

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

Weak Bases

Weak bases are substances that partially ionize in solution to accept protons (H+) from acids. Unlike strong bases, which completely dissociate, weak bases establish an equilibrium between the undissociated base and its ions. Understanding the behavior of weak bases is crucial for predicting their interactions in solution, particularly in acid-base reactions.
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Anions and Basicity

Anions can act as bases if they can accept protons. The basicity of an anion depends on its conjugate acid's strength; if the conjugate acid is weak, the anion is likely to be a stronger base. For example, the hypochlorite ion (ClO-) can accept a proton to form hypochlorous acid (HClO), indicating its basic nature.
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Equilibrium in Acid-Base Reactions

In acid-base reactions, equilibrium plays a vital role in determining the extent of the reaction. When an anion acts as a base, it establishes an equilibrium between the anion, the proton it accepts, and the resulting conjugate acid. This equilibrium can be represented by a chemical equation, illustrating how the anion interacts with protons in solution.
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Related Practice
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