Domanda del libro di testo
A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: one-half equivalence.
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Ch.18 - Aqueous Ionic Equilibrium
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 18, Problema 74b
A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 10 mL.
Guida verificata passo dopo passo1
Identify the initial moles of pyridine (C5H5N) in the solution using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Calculate the moles of HCl added using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Determine the reaction between pyridine (a weak base) and HCl (a strong acid), which forms pyridinium ion (C5H5NH^+). The reaction is: \( \text{C5H5N} + \text{HCl} \rightarrow \text{C5H5NH}^+ + \text{Cl}^- \).
Calculate the moles of pyridine and pyridinium ion after the reaction to find the remaining moles of pyridine and the moles of pyridinium ion formed.
Use the Henderson-Hasselbalch equation to calculate the pH: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{base}]}{[\text{acid}]} \right) \), where \( \text{pK}_a \) is derived from the \( \text{K}_b \) of pyridine.
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Acid-Base Titration
An acid-base titration is a quantitative analytical method used to determine the concentration of an acid or base in a solution. In this process, a solution of known concentration (the titrant) is added to a solution of unknown concentration until the reaction reaches its equivalence point, where the amount of acid equals the amount of base. The pH changes during the titration, and understanding this change is crucial for calculating the pH at specific volumes of titrant added.
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03:04
Acid-Base Titration
Buffer Solutions
Buffer solutions are mixtures that can resist changes in pH upon the addition of small amounts of acid or base. In this case, pyridine acts as a weak base and can form a buffer with its conjugate acid, pyridinium ion, when titrated with HCl. The presence of a buffer system is essential for understanding the pH changes during the titration, especially before reaching the equivalence point, where the solution can maintain a relatively stable pH.
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03:02Buffer Solutions
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution. It relates the pH of the solution to the pKa of the weak acid and the ratio of the concentrations of the conjugate base and the weak acid. This equation is particularly useful in titration problems involving weak acids and bases, as it allows for the determination of pH at various points in the titration process, including before and after the addition of titrant.
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02:40Henderson-Hasselbalch Equation
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