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 74g
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.
Guida verificata passo dopo passo1
Identify the initial moles of pyridine (C5H5N) 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 limiting reactant by comparing the initial moles of pyridine and the moles of HCl added.
Calculate the moles of pyridine and pyridinium ion (C5H5NH^+) after the reaction, considering the stoichiometry of the reaction: \( \text{C5H5N} + \text{HCl} \rightarrow \text{C5H5NH}^+ + \text{Cl}^- \).
Use the Henderson-Hasselbalch equation to find the pH: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{C5H5N}]}{[\text{C5H5NH}^+]} \right) \), 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 various points.
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Percorso guidato
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 the case of pyridine, a weak base, when titrated with HCl, it forms a buffer system that can maintain a relatively stable pH until a significant amount of acid is added. Understanding how buffers work is essential for predicting the pH at different stages of the titration.
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Percorso guidato
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 acid and the ratio of the concentrations of the conjugate base and the 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.
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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?
1496
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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: 40 mL.
1123
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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
Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.
(ii) Which acid has the larger Ka?
895
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