Domanda del libro di testo
A formic acid solution has a pH of 3.25. Which of these substances will raise the pH of the solution upon addition? Explain your answer. a. HCl b. NaBr c. NaCHO2 d. KCl
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Ch.17 - Aqueous Ionic Equilibrium
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
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Capitolo 17, Problema 30
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. a solution that is 0.195 M in HC2H3O2 and 0.125 M in KC2H3O2 b. a solution that is 0.255 M in CH3NH2 and 0.135 M in CH3NH3Br
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Identify the type of solution: Both solutions are buffer solutions. Solution (a) is an acetic acid (HC2H3O2) and acetate ion (C2H3O2-) buffer, while solution (b) is a methylamine (CH3NH2) and methylammonium ion (CH3NH3+) buffer.
Use the Henderson-Hasselbalch equation for buffer solutions: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \) for acidic buffers and \( \text{pOH} = \text{pK}_b + \log \left( \frac{[\text{B}]}{[\text{BH}^+]} \right) \) for basic buffers.
For solution (a), find the \( \text{pK}_a \) of acetic acid (HC2H3O2) using a reference table. Then, substitute \([\text{A}^-] = 0.125 \text{ M}\) and \([\text{HA}] = 0.195 \text{ M}\) into the Henderson-Hasselbalch equation to find the pH.
For solution (b), find the \( \text{pK}_b \) of methylamine (CH3NH2) using a reference table. Then, substitute \([\text{B}] = 0.255 \text{ M}\) and \([\text{BH}^+] = 0.135 \text{ M}\) into the Henderson-Hasselbalch equation to find the pOH.
Convert the pOH to pH for solution (b) using the relation \( \text{pH} = 14 - \text{pOH} \).
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Equilibrium and ICE Tables
An ICE table (Initial, Change, Equilibrium) is a tool used to organize the concentrations of reactants and products in a chemical equilibrium problem. It helps in calculating the changes in concentration that occur as the system reaches equilibrium. Understanding how to set up and interpret an ICE table is crucial for solving equilibrium problems, including those involving weak acids and bases.
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Percorso guidato
01:14
ICE Charts and Equilibrium Amount
pH and Acid-Base Chemistry
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. In the context of weak acids and their conjugate bases, the pH can be calculated using the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the concentration of the acid and its conjugate base. This concept is essential for determining the pH of solutions containing weak acids and their salts.
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Percorso guidato
02:39pH of Strong Acids and Bases
Buffer Solutions
A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base or a weak base and its conjugate acid. Understanding how buffers work is important for calculating the pH of solutions that contain both a weak acid and its salt, as seen in the given problem.
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Percorso guidato
03:02Buffer Solutions
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