Domanda del libro di testo
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) calcium hydroxide titrated with perchloric acid.
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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 38c
Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 38cCapitolo 17, Problema 38c
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (c) pyridine titrated with nitric acid.
Guida verificata passo dopo passo1
Identify the nature of the substances involved in the titration: Pyridine is a weak base, and nitric acid is a strong acid.
Understand the reaction: When a weak base is titrated with a strong acid, the resulting solution at the equivalence point will contain the conjugate acid of the weak base.
Consider the properties of the conjugate acid: The conjugate acid of pyridine is pyridinium ion, which can donate a proton to water, making the solution acidic.
Predict the pH at the equivalence point: Since the solution contains an acidic species (pyridinium ion), the pH at the equivalence point will be below 7.
Conclude: The equivalence point of the titration of pyridine with nitric acid is below pH 7.
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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. During the titration, a solution of known concentration (the titrant) is added to a solution of unknown concentration until the reaction reaches the equivalence point, where the amount of acid equals the amount of base. The pH at this point can vary depending on the strength of the acid and base involved.
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03:04
Acid-Base Titration
Strength of Acids and Bases
Acids and bases are classified as strong or weak based on their ability to dissociate in water. Strong acids, like nitric acid, completely dissociate into ions, while weak bases, such as pyridine, only partially dissociate. This difference in dissociation affects the pH at the equivalence point of a titration, with strong acids and weak bases typically resulting in a pH below 7 at the equivalence point due to the presence of excess hydrogen ions.
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00:50Strength of Conjugate Acids and Bases
Equivalence Point and pH
The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample. The pH at this point is influenced by the nature of the acid and base involved. In the case of titrating a weak base with a strong acid, the resulting solution will have a pH less than 7 due to the formation of a conjugate acid, which contributes to the acidity of the solution.
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07:28pH at the Equivalence Point Example
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Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (a) How many moles of HA have been added at the equivalence point?
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Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (b) What is the predominant form of B at the equivalence point?
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