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.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
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 17, Problema 74f
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: 40 mL.
Guida verificata passo dopo passo1
Identify the reaction: Pyridine (C5H5N) is a weak base and reacts with HCl, a strong acid, to form pyridinium ion (C5H5NH+).
Calculate the initial moles of pyridine using its concentration and volume: \( \text{moles of pyridine} = 0.125 \text{ M} \times 0.025 \text{ L} \).
Calculate the moles of HCl added using its concentration and volume: \( \text{moles of HCl} = 0.100 \text{ M} \times 0.040 \text{ L} \).
Determine the limiting reactant and calculate the moles of pyridinium ion formed and any excess reactant remaining after the reaction.
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 \( K_b \) 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 monitoring these changes allows for the calculation of the unknown concentration.
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03:04
Acid-Base Titration
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. In the context of the titration of pyridine (a weak base) with HCl (a strong acid), the buffer capacity is crucial for understanding how the pH will change before and after the equivalence point.
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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, as it allows for the determination of pH at various points during the titration, especially when the solution is still in the buffer region.
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02:40Henderson-Hasselbalch Equation
Pratica correlata
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: 0 mL, 10 mL, 20 mL, equivalence point, one-half equivalence point, 40 mL, 50 mL. Sketch the titration curve.
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Domanda del libro di testo
Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.
(i) Which acid solution is more concentrated?
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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: equivalence point.
1863
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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: 50 mL.
332
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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: 20 mL.
356
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