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 33b
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. 0.15 M NaF
Guida verificata passo dopo passo1
Step 1: Identify the major species in the solution. In this case, we have NaF which will dissociate into Na+ and F-. Since Na+ is a spectator ion, we can ignore it. So, the major species are F- and H2O.
Step 2: Write the chemical equation for the reaction that occurs. F- will act as a base and react with water to form HF and OH-. The equation is: F- + H2O ⇌ HF + OH-.
Step 3: Set up an ICE (Initial, Change, Equilibrium) table. The initial concentration of F- is 0.15 M, and we can assume the initial concentrations of HF and OH- are 0. The change in F- is -x, the change in HF is +x, and the change in OH- is also +x. At equilibrium, we have 0.15 - x M F-, x M HF, and x M OH-.
Step 4: Write the expression for the equilibrium constant. For this reaction, we use the Kb (base ionization constant) because F- is acting as a base. The Kb expression is: Kb = [HF][OH-] / [F-].
Step 5: Substitute the equilibrium concentrations from the ICE table into the Kb expression and solve for x. This will give you the concentration of OH-. Then, use the formula pOH = -log[OH-] to find the pOH. Finally, use the formula pH = 14 - pOH to find the pH of the solution.
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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.
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Percorso guidato
01:14
ICE Charts and Equilibrium Amount
Acid-Base Chemistry
Acid-base chemistry involves the study of acids, bases, and their reactions. In this context, NaF (sodium fluoride) acts as a salt that can affect the pH of a solution. When dissolved, NaF dissociates into Na+ and F- ions, where F- can react with water to form HF and OH-, influencing the pH of the solution and demonstrating the concept of hydrolysis.
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02:00Arrhenius Acids and Bases
pH Calculation
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. To calculate pH, one must first determine the concentration of H+ ions in the solution, which can be derived from the equilibrium concentrations obtained from the ICE table. Understanding how to relate the equilibrium concentrations to pH is crucial for solving the problem presented.
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Percorso guidato
02:15pH Calculation Example
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