Domanda del libro di testo
Write a chemical equation that illustrates the autoionization of water.
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 28b
Write the expression for the ion product constant for water, Kw.
Guida verificata passo dopo passo1
Understand that the ion product constant for water, denoted as \( K_w \), is a special equilibrium constant for the self-ionization of water.
Recognize the self-ionization reaction of water: \( 2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq) \).
Simplify the reaction to: \( H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq) \), where \( H^+ \) is often used interchangeably with \( H_3O^+ \).
Write the expression for the equilibrium constant \( K_w \) as the product of the concentrations of the ions: \( K_w = [H^+][OH^-] \).
Note that \( K_w \) is temperature-dependent and at 25°C, \( K_w \) is typically \( 1.0 \times 10^{-14} \).
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Ion Product Constant for Water (Kw)
The ion product constant for water, denoted as Kw, is the equilibrium constant for the self-ionization of water. It is defined as the product of the concentrations of hydrogen ions [H+] and hydroxide ions [OH-] in pure water at a given temperature. At 25°C, Kw is equal to 1.0 x 10^-14, indicating that the concentrations of H+ and OH- are both 1.0 x 10^-7 M in neutral water.
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Percorso guidato
01:47
Solubility Product Constant
Self-Ionization of Water
Self-ionization of water refers to the process where two water molecules react to form one hydronium ion (H3O+) and one hydroxide ion (OH-). This reaction is represented by the equation: 2 H2O ⇌ H3O+ + OH-. This equilibrium is crucial for understanding acid-base chemistry, as it establishes the basis for the pH scale and the behavior of acids and bases in aqueous solutions.
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02:22Auto-Ionization and Kw
Acid-Base Equilibrium
Acid-base equilibrium involves the balance between acids and bases in a solution, which is influenced by the concentrations of H+ and OH- ions. The pH scale, which ranges from 0 to 14, is a logarithmic scale that measures the acidity or basicity of a solution based on the concentration of H+. Understanding this equilibrium is essential for predicting how substances will behave in solution and for calculating pH and pOH.
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6:47Triprotic Acid Equilibrium
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