Textbook Question
Consider the decomposition of barium carbonate: BaCO3(s) ⇌ BaO(s) + CO2(g) Using data from Appendix C, calculate the equilibrium pressure of CO2 at (b) 1100 K.
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Ch.19 - Chemical Thermodynamics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 19, Problem 83a
The value of Ka for nitrous acid (HNO2) at 25 °C is given in Appendix D. (a) Write the chemical equation for the equilibrium that corresponds to Ka.
Verified step by step guidance1
Identify the chemical formula for nitrous acid, which is HNO2.
Recognize that the dissociation of an acid in water typically results in the formation of hydrogen ions (H+) and the conjugate base of the acid.
Write the chemical equation for the dissociation of nitrous acid in water: HNO2(aq) ⇌ H+(aq) + NO2-(aq).
Understand that Ka, the acid dissociation constant, quantifies the strength of the acid in solution, indicating how completely the acid dissociates in water.
The equilibrium expression corresponding to this reaction is Ka = [H+][NO2-] / [HNO2], where the concentrations are those at equilibrium.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Equilibrium
Acid-base equilibrium refers to the state in which the concentrations of the reactants and products in an acid-base reaction remain constant over time. For weak acids like nitrous acid (HNO2), this equilibrium involves the dissociation of the acid into its ions, which is characterized by the acid dissociation constant (Ka). Understanding this concept is crucial for writing the correct equilibrium expression.
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Triprotic Acid Equilibrium
Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of an acid in solution. It is defined as the ratio of the concentration of the products (the dissociated ions) to the concentration of the undissociated acid at equilibrium. A higher Ka value indicates a stronger acid that dissociates more completely in solution, which is essential for determining the behavior of HNO2 in aqueous solutions.
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Chemical Equations and Equilibrium Expressions
Chemical equations represent the reactants and products involved in a chemical reaction, while equilibrium expressions mathematically describe the relationship between the concentrations of these species at equilibrium. For HNO2, the equilibrium equation would show the dissociation into H+ and NO2-, allowing for the calculation of Ka. Writing these equations correctly is fundamental for analyzing acid-base reactions.
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Related Practice
Textbook Question
The value of Ka for nitrous acid (HNO2) at 25 °C is given in Appendix D. (b) By using the value of Ka, calculate ΔG° for the dissociation of nitrous acid in aqueous solution.
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Textbook Question
Consider the decomposition of barium carbonate: BaCO3(s) ⇌ BaO(s) + CO2(g) Using data from Appendix C, calculate the equilibrium pressure of CO2 at (a) 298 K.
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Textbook Question
The value of Ka for nitrous acid (HNO2) at 25 °C is given in Appendix D. (c) What is the value of ΔG at equilibrium?
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Textbook Question
The value of Ka for nitrous acid (HNO2) at 25 °C is given in Appendix D. (d) What is the value of ΔG when [H+] = 5.0⨉10-2 M, [NO2-] = 6.0⨉10-4 M, and [HNO2] = 0.20 M?
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