Domanda del libro di testo
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (b) 20.0 mL (c) 59.0 mL.
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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
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Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 45b
Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 45bCapitolo 17, Problema 45b
A 35.0-mL sample of 0.150 M acetic acid 1CH3COOH2 is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (b) 17.5 mL.
Guida verificata passo dopo passo1
Step 1: Identify the type of reaction. In this case, it's an acid-base titration. Acetic acid (CH3COOH) is a weak acid and sodium hydroxide (NaOH) is a strong base. When they react, they form water and the acetate ion (CH3COO-).
Step 2: Calculate the initial moles of acetic acid. This can be done by multiplying the initial volume of the acetic acid solution (in liters) by its molarity. Remember that molarity is defined as moles per liter.
Step 3: Calculate the moles of NaOH added. This can be done by multiplying the volume of the NaOH solution added (in liters) by its molarity.
Step 4: Determine the limiting reactant. In this case, since the molarity of the acetic acid and NaOH are the same, and the volume of NaOH added is half the volume of the acetic acid, the NaOH will be the limiting reactant. This means that all of the NaOH will react with an equal amount of acetic acid, and there will be some acetic acid left over.
Step 5: Calculate the pH of the resulting solution. Since there is still some acetic acid left over, the solution will be a buffer. The pH of a buffer can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the acetate ion and [HA] is the concentration of the remaining acetic acid. The pKa of acetic acid is 4.76.
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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 of the solution changes during the titration, and this change can be monitored to find the endpoint.
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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. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. In the case of acetic acid and sodium hydroxide, the acetic acid acts as a weak acid, and as NaOH is added, it forms its conjugate base, acetate, which helps maintain the pH within a certain range until the equivalence point is reached.
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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 to 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 before and after the equivalence point.
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02:40Henderson-Hasselbalch Equation
Pratica correlata
Domanda del libro di testo
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (d) 25.0 mL. (e) 30.0 mL.
Domanda del libro di testo
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (e) 61.0 mL (f) 65.0 mL.
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Domanda del libro di testo
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (c) 24.0 mL.
2003
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Domanda del libro di testo
Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) sodium hydroxide (NaOH).