Domanda del libro di testo
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (b) chlorous acid (HClO2).
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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
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Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 47a
Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 47aCapitolo 17, Problema 47a
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).
Guida verificata passo dopo passo1
Identify the type of titration: This is a strong base (NaOH) being titrated with a strong acid (HBr). At the equivalence point, the moles of NaOH will equal the moles of HBr added.
Write the balanced chemical equation for the reaction: NaOH + HBr → NaBr + H₂O. This shows that NaOH reacts with HBr to form NaBr and water.
Determine the concentration of the resulting solution at the equivalence point: Since both solutions are 0.200 M and mixed in equal volumes, the resulting solution will be neutral, as NaBr is a neutral salt.
Understand the pH of a neutral solution: For a strong acid-strong base titration, the pH at the equivalence point is determined by the nature of the salt formed. NaBr does not hydrolyze in water, so the solution remains neutral.
Conclude the pH at the equivalence point: Since the solution is neutral and neither the cation (Na⁺) nor the anion (Br⁻) affects the pH, the pH at the equivalence point is 7.
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Titration and Equivalence Point
Titration is a quantitative analytical method used to determine the concentration of a solute in a solution. The equivalence point occurs when the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample. At this point, the reaction between the acid and base is complete, and the pH of the solution is determined by the properties of the resulting salt and any remaining species.
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Percorso guidato
03:06
Equivalence Point in Titration
pH and its Calculation
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. At the equivalence point of a strong base like sodium hydroxide (NaOH) titrated with a strong acid like HBr, the resulting solution contains the salt (NaBr) and water. The pH can be calculated based on the hydrolysis of the salt, which may affect the concentration of hydrogen ions in the solution.
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02:15pH Calculation Example
Hydrolysis of Salts
When a salt dissolves in water, it can undergo hydrolysis, where the ions react with water to form either acidic or basic solutions. In the case of NaBr, the sodium ion does not hydrolyze, while the bromide ion is the conjugate base of a strong acid (HBr) and does not affect the pH significantly. Therefore, the pH at the equivalence point for the titration of NaOH with HBr will be neutral, around 7, since neither ion contributes to acidity or basicity.
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00:50Ionic Salts
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