Domanda del libro di testo
What is the pH of a solution in which 121 mL of HCl(g), measured at and 0.855 atm, is dissolved in 1.5 L of aqueous solution?
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
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Capitolo 17, Problema 68
Determine the [H3O+] and pH of a 0.100 M solution of formic acid.
Guida verificata passo dopo passo1
Identify the chemical formula for formic acid, which is HCOOH, and recognize that it is a weak acid.
Write the dissociation equation for formic acid in water: \( \text{HCOOH} + \text{H}_2\text{O} \rightleftharpoons \text{H}_3\text{O}^+ + \text{HCOO}^- \).
Use the acid dissociation constant \( K_a \) for formic acid to set up an expression: \( K_a = \frac{[\text{H}_3\text{O}^+][\text{HCOO}^-]}{[\text{HCOOH}]} \).
Assume that the initial concentration of \( \text{H}_3\text{O}^+ \) and \( \text{HCOO}^- \) is 0, and let \( x \) be the change in concentration at equilibrium, leading to \( [\text{H}_3\text{O}^+] = x \), \( [\text{HCOO}^-] = x \), and \( [\text{HCOOH}] = 0.100 - x \).
Substitute these expressions into the \( K_a \) expression and solve for \( x \), which represents \( [\text{H}_3\text{O}^+] \), then calculate the pH using \( \text{pH} = -\log[\text{H}_3\text{O}^+] \).
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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 formic 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 formic acid, knowing its Ka value allows us to set up an equilibrium expression to calculate the concentration of H3O+ ions in a 0.100 M solution, which is essential for determining pH.
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03:50Characteristics of Ka and Kb
pH Scale
The pH scale is a logarithmic scale used to specify the acidity or basicity of a solution. It is 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. Understanding how to calculate pH from the concentration of H3O+ is vital for interpreting the acidity of the formic acid solution.
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02:33The pH Scale
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