Textbook Question
Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:
(a) NH4+(aq) + OH-(aq) ⇌
(b) CH3COO-(aq) + H3O+(aq) ⇌
(c) HCO3-(aq) + F-(aq) ⇌
Ch.16 - Acid-Base Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 16, Problem 29
Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:
(a) O2-(aq) + H2O(l) ⇌
(b) CH3COOH(aq) + HS-(aq) ⇌
(c) NO2-(aq) + H2O(l) ⇌
Verified step by step guidance1
Identify the acid and base in the reaction. Here, \( \text{NO}_2^- \) acts as a base and \( \text{H}_2\text{O} \) acts as an acid.
Determine the conjugate acid and conjugate base. \( \text{NO}_2^- \) will accept a proton to form \( \text{HNO}_2 \), and \( \text{H}_2\text{O} \) will donate a proton to form \( \text{OH}^- \).
Write the balanced chemical equation for the reaction: \( \text{NO}_2^- + \text{H}_2\text{O} \rightleftharpoons \text{HNO}_2 + \text{OH}^- \).
Consider the strength of the acids and bases involved. \( \text{HNO}_2 \) is a weak acid, and \( \text{OH}^- \) is a strong base.
Predict the direction of the equilibrium. Since \( \text{OH}^- \) is a strong base, the equilibrium will lie to the left, favoring the reactants.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, an acid donates a proton, while a base accepts it. Understanding the roles of acids and bases is crucial for predicting the products of the reaction and determining the direction of equilibrium.
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Acid-Base Reaction
Equilibrium Position
The position of equilibrium in a chemical reaction indicates the relative concentrations of reactants and products at equilibrium. If the equilibrium lies to the right, products are favored; if to the left, reactants are favored. Factors such as concentration, temperature, and the nature of the reactants influence this position.
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Water as a Solvent
Water is often referred to as the 'universal solvent' due to its ability to dissolve many substances, including acids and bases. In acid-base reactions, water can act as a medium for proton transfer, and its role in the reaction can affect the strength of the acids and bases involved, influencing the overall reaction dynamics.
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Related Practice
Textbook Question
Which of the following is the stronger Brønsted–Lowry acid, HBrO or HBr?
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Textbook Question
Write a chemical equation that illustrates the autoionization of water.
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: (e) NH3.