Domanda del libro di testo
Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37 °C), Kw = 2.4×10–14. What are the [H3O+] and pH of pure water at body temperature?
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Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 17, Problema 58
The value of Kw increases with increasing temperature. Is the autoionization of water endothermic or exothermic?
Guida verificata passo dopo passo1
Understand that the autoionization of water is represented by the equation: \( \text{H}_2\text{O} (l) \rightleftharpoons \text{H}^+ (aq) + \text{OH}^- (aq) \).
Recall that \( K_w \) is the equilibrium constant for the autoionization of water, and it is given by \( K_w = [\text{H}^+][\text{OH}^-] \).
Recognize that an increase in \( K_w \) with temperature suggests that the equilibrium shifts to the right, favoring the formation of \( \text{H}^+ \) and \( \text{OH}^- \).
Apply Le Chatelier's principle, which states that if a system at equilibrium is subjected to a change in temperature, the system will adjust to counteract that change. An increase in temperature favors the endothermic direction.
Conclude that since the equilibrium shifts to the right with increasing temperature, the autoionization of water is endothermic.
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Autoionization of Water
The autoionization of water refers to the process where two water molecules react to form a hydronium ion (H3O+) and a hydroxide ion (OH-). This reaction is represented by the equilibrium expression: 2 H2O ⇌ H3O+ + OH-. At 25°C, the ion product constant of water (Kw) is 1.0 x 10^-14, but this value changes with temperature, indicating the dynamic nature of this equilibrium.
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Percorso guidato
01:23
Reaction with Water
Endothermic vs. Exothermic Reactions
Endothermic reactions absorb heat from their surroundings, resulting in a decrease in temperature of the environment, while exothermic reactions release heat, increasing the temperature. The classification of a reaction as endothermic or exothermic is determined by the change in enthalpy (ΔH). If ΔH is positive, the reaction is endothermic; if negative, it is exothermic.
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02:30Endothermic & Exothermic Reactions
Temperature Dependence of Kw
The value of Kw, the ion product of water, is temperature-dependent. As temperature increases, Kw also increases, indicating that the equilibrium shifts to favor the formation of H3O+ and OH- ions. This shift suggests that the autoionization of water absorbs heat, thus classifying it as an endothermic process, as higher temperatures promote the reaction.
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01:24Kw Temperature Dependence
Pratica correlata
Domanda del libro di testo
Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H3O+] = 0.044 M [H3O+] = 0.045 M [H3O+] = 0.046 M
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Domanda del libro di testo
Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52
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Domanda del libro di testo
Complete the table. (All solutions are at 25 °C.)
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Domanda del libro di testo
For each strong acid solution, determine [H3O+], [OH–], and pH. a. 0.25 M HCl
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Domanda del libro di testo
Complete the table. (All solutions are at 25 °C.)
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