Domanda del libro di testo
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 10 mL.
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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 72b
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 5 mL.
Guida verificata passo dopo passo1
Determine the initial moles of propanoic acid (C2H5COOH) using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Calculate the moles of KOH added using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Determine the moles of propanoic acid that react with KOH, considering the stoichiometry of the reaction: \( \text{C2H5COOH} + \text{KOH} \rightarrow \text{C2H5COOK} + \text{H2O} \).
Calculate the moles of propanoic acid and its conjugate base (propanoate ion, C2H5COO-) remaining after the reaction.
Use the Henderson-Hasselbalch equation to find the pH: \( \text{pH} = \text{pKa} + \log \left( \frac{[\text{C2H5COO-}]}{[\text{C2H5COOH}]} \right) \), where \( \text{pKa} \) is the acid dissociation constant of propanoic acid.
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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 can be monitored to determine the endpoint.
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Percorso guidato
03:04
Acid-Base Titration
Weak Acid and Strong Base Reaction
In this titration, propanoic acid (a weak acid) reacts with potassium hydroxide (a strong base). The weak acid does not fully dissociate in solution, which affects the pH at various points during the titration. The resulting solution will have a pH that is influenced by the remaining weak acid and the produced salt, as well as the strong base added.
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01:09Strong Acid-Strong Base Titration
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation is a formula used to calculate the pH of a buffer solution. It relates the pH to the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the weak acid. This equation is particularly useful in titration scenarios to determine the pH at points before, at, and after the equivalence point, especially when dealing with weak acids and their conjugate bases.
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02:40Henderson-Hasselbalch Equation
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Domanda del libro di testo
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: equivalence point.
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Domanda del libro di testo
Consider the titration of a 20.0-mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each quantity. b. the volume of added base required to reach the equivalence point
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Domanda del libro di testo
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: one-half equivalence point.
948
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Domanda del libro di testo
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 0 mL, 5 mL, 10 mL, equivalence point, one-half equivalence point, 20 mL, 25 mL. Sketch the titration curve.
236
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Domanda del libro di testo
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 0 mL.
322
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