Domanda del libro di testo
What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?
a. pH = 1.25 b. pH = 1.75 c. pH = 2.85
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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 67
Determine the [H3O+] and pH of a 0.200 M solution of benzoic acid.
Guida verificata passo dopo passo1
Identify the chemical formula for benzoic acid, which is C6H5COOH, and recognize that it is a weak acid.
Write the equilibrium expression for the dissociation of benzoic acid in water: C6H5COOH + H2O \(\rightleftharpoons\) C6H5COO^- + H3O^+.
Use the acid dissociation constant (Ka) for benzoic acid, which is typically provided in a table, to set up the expression: Ka = \(\frac{[C6H5COO^-][H3O^+]}{[C6H5COOH]}\).
Assume that the initial concentration of benzoic acid is 0.200 M and that the change in concentration of H3O^+ and C6H5COO^- is x, leading to the expression: Ka = \(\frac{x^2}{0.200 - x}\).
Solve for x, which represents [H3O^+], and then calculate the pH using the formula: pH = -\(\log\)[H3O^+].
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Acid-Base Equilibrium
Acid-base equilibrium refers to the balance between the concentrations of acids and their conjugate bases in a solution. In the case of weak acids like benzoic acid, this equilibrium is established when the acid partially dissociates in water, producing hydronium ions (H3O+) and its conjugate base. Understanding this concept is crucial for calculating the concentration of H3O+ in the solution.
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Percorso guidato
6:47
Triprotic Acid Equilibrium
Dissociation Constant (Ka)
The dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution. It represents the equilibrium constant for the dissociation of the acid into its ions. For benzoic acid, knowing its Ka value allows us to set up an equilibrium expression to find the concentration of H3O+ ions, which is essential for determining the pH of the solution.
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03:50Characteristics of Ka and Kb
pH Scale
The pH scale is a logarithmic scale used to measure the acidity or basicity of a solution, defined as the negative logarithm of the hydronium ion concentration: pH = -log[H3O+]. A lower pH indicates a more acidic solution, while a higher pH indicates a more basic one. Calculating the pH from the concentration of H3O+ is a fundamental step in understanding the properties of the solution.
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02:33The pH Scale
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