Textbook Question
Predict the products of the following acid–base reactions.
(a) H2SO4 + CH3COO– ⇌
(b) CH3COOH + (CH3)3N: ⇌
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3. Acids and Bases
Acids and Bases
5:25 minutesProblem 9b
Textbook Question
Ammonia appears in [TABLE 2-2 ] as both an acid and a conjugate base. a. Explain how ammonia can act as both an acid and a base. Which of these roles does it commonly fill in aqueous solutions?
b. Show how water can serve as both an acid and a base.
Verified step by step guidance1
Ammonia (NH₃) can act as both an acid and a base due to its ability to donate and accept protons. As a base, ammonia accepts a proton from water, forming ammonium ion (NH₄⁺) and hydroxide ion (OH⁻). As an acid, ammonia can donate a proton to form the amide ion (NH₂⁻). In aqueous solutions, ammonia commonly acts as a base, accepting protons from water.
Water (H₂O) can serve as both an acid and a base due to its amphoteric nature. As an acid, water can donate a proton to form hydroxide ion (OH⁻). As a base, water can accept a proton to form hydronium ion (H₃O⁺). This dual ability allows water to participate in acid-base reactions in both roles.
In the table, ammonia is shown as a conjugate base of the ammonium ion (NH₄⁺), indicating its role as a base when it accepts a proton. The equilibrium reaction is: NH₄⁺ + H₂O ⇌ H₃O⁺ + NH₃.
The table also shows water as both an acid and a conjugate base. As an acid, water donates a proton to form hydroxide ion (OH⁻), and as a base, it accepts a proton to form hydronium ion (H₃O⁺). The equilibrium reactions are: H₂O + H₂O ⇌ H₃O⁺ + OH⁻.
The concept of conjugate acid-base pairs is crucial in understanding these roles. A conjugate acid is formed when a base gains a proton, and a conjugate base is formed when an acid loses a proton. This concept helps explain the dual roles of ammonia and water in acid-base chemistry.
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Video duration:
5mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Amphoteric Nature of Substances
Ammonia (NH3) is amphoteric, meaning it can act as both an acid and a base. As a base, it can accept a proton (H+) to form the ammonium ion (NH4+). Conversely, it can donate a proton in the presence of a stronger base, thus acting as an acid. This dual behavior is crucial for understanding its role in various chemical reactions, especially in aqueous solutions.
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Conjugate Acid-Base Pairs
In acid-base chemistry, every acid has a conjugate base and vice versa. When ammonia acts as a base, it forms its conjugate acid, the ammonium ion (NH4+). Conversely, when it acts as an acid, it donates a proton to form its conjugate base, which is the amide ion (NH2-). Understanding these pairs helps clarify the equilibrium between acids and bases in solution.
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Water as an Acid and Base
Water (H2O) is also amphoteric and can act as both an acid and a base. It can donate a proton to form the hydroxide ion (OH-) when acting as an acid, or accept a proton to form the hydronium ion (H3O+) when acting as a base. This property is fundamental in many chemical reactions, particularly in aqueous environments, where water is often the solvent.
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