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.
2830
views
Ch.18 - Aqueous Ionic Equilibrium
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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 33a
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. 0.15 M HF
Guida verificata passo dopo passo1
Write the balanced chemical equation for the dissociation of HF in water: \( \text{HF} \rightleftharpoons \text{H}^+ + \text{F}^- \).
Set up the ICE table (Initial, Change, Equilibrium) for the concentrations of HF, H⁺, and F⁻. Initially, [HF] = 0.15 M, [H⁺] = 0, and [F⁻] = 0.
Define the change in concentration for the reaction: let \( x \) be the amount of HF that dissociates. At equilibrium, [HF] = 0.15 - x, [H⁺] = x, and [F⁻] = x.
Write the expression for the acid dissociation constant \( K_a \) for HF: \( K_a = \frac{[\text{H}^+][\text{F}^-]}{[\text{HF}]} \). Substitute the equilibrium concentrations into this expression.
Solve the equation for \( x \) to find the concentration of \( \text{H}^+ \), then calculate the pH using the formula \( \text{pH} = -\log[\text{H}^+] \).
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
3mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Equilibrium and ICE Tables
Equilibrium in chemistry refers to the state where the concentrations of reactants and products remain constant over time. An ICE table (Initial, Change, Equilibrium) is a tool used to organize the concentrations of species involved in a reaction at different stages. It helps in calculating the changes in concentration as the system reaches equilibrium, which is essential for solving equilibrium problems.
Video consigliato:
Percorso guidato
01:14
ICE Charts and Equilibrium Amount
Weak Acids and pH Calculation
Weak acids, like hydrofluoric acid (HF), do not completely dissociate in solution, leading to an equilibrium between the undissociated acid and its ions. The pH of a weak acid solution can be calculated using the acid dissociation constant (Ka) and the initial concentration of the acid. The formula pH = -log[H⁺] is used, where [H⁺] can be derived from the equilibrium concentrations established in the ICE table.
Video consigliato:
Percorso guidato
07:51Calculating pH of Weak Acids Example
Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of a weak acid in solution, representing the equilibrium constant for its dissociation into ions. A higher Ka value indicates a stronger weak acid, while a lower Ka suggests a weaker acid. For HF, knowing its Ka value allows for the calculation of the concentration of hydrogen ions at equilibrium, which is crucial for determining the pH of the solution.
Video consigliato:
Percorso guidato
03:50Characteristics of Ka and Kb
Pratica correlata
Domanda del libro di testo
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
1766
views
Domanda del libro di testo
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. 0.15 M NaF
508
views
Domanda del libro di testo
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b solution that is 0.15 M in HCHO2 and 0.25 M in NaCHO2
Domanda del libro di testo
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. a solution that is 0.25 M in NH3 and 0.18 M in NH4Cl
Domanda del libro di testo
Calculate the percent ionization of a 0.20 M benzoic acid solution in pure water and in a solution containing 0.25 M sodium benzoate. Why does the percent ionization differ significantly in the two solutions?