Domanda del libro di testo
A buffer contains significant amounts of acetic acid and sodium acetate. Write equations showing how this buffer neutralizes added acid and added base.
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Ch.18 - Aqueous Ionic Equilibrium
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 18, Problema 33c
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. c. a mixture that is 0.15 M in HF and 0.15 M in NaF
Guida verificata passo dopo passo1
Identify the components of the solution: HF is a weak acid and NaF is its conjugate base, making this a buffer solution.
Write the equilibrium expression for the dissociation of HF: \( \text{HF} \rightleftharpoons \text{H}^+ + \text{F}^- \).
Set up an ICE table (Initial, Change, Equilibrium) to determine the concentrations of each species at equilibrium. Initially, [HF] = 0.15 M and [F^-] = 0.15 M, with [H^+] = 0.
Use the expression for the acid dissociation constant \( K_a \) of HF: \( K_a = \frac{[\text{H}^+][\text{F}^-]}{[\text{HF}]} \). Substitute the equilibrium concentrations from the ICE table into this expression.
Solve for \([\text{H}^+]\) using the \( K_a \) value for HF, and then calculate the pH using the formula \( \text{pH} = -\log[\text{H}^+] \).
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Weak Acids and Conjugate Bases
HF (hydrofluoric acid) is a weak acid that partially dissociates in solution, while NaF (sodium fluoride) provides the conjugate base F-. The presence of both a weak acid and its conjugate base in a solution creates a buffer system, which helps maintain a relatively stable pH when small amounts of acid or base are added.
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01:46
Conjugate Acid-Base Relationships
ICE Table (Initial, Change, Equilibrium)
An ICE table is a tool used to organize the initial concentrations, the changes in concentrations as the reaction reaches equilibrium, and the final equilibrium concentrations. For the equilibrium problem involving HF and F-, the ICE table will help calculate the concentrations of H+ ions, which are necessary for determining the pH of the solution.
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01:14ICE Charts and Equilibrium Amount
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the concentration of the weak acid and its conjugate base. It is expressed as pH = pKa + log([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant. This equation simplifies the calculation of pH in buffer solutions like the one formed by HF and NaF.
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02:40Henderson-Hasselbalch Equation
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Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. 0.15 M HF
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