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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
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Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 47b
Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 47bCapitolo 17, Problema 47b
Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (b) hydroxylamine 1NH2OH2.
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Identify the chemical reaction: Hydroxylamine (NH2OH) reacts with hydrobromic acid (HBr) to form NH3OH+ and Br-. The balanced equation is: NH2OH + HBr -> NH3OH+ + Br-.
Determine the nature of the species at the equivalence point: At the equivalence point, all NH2OH has reacted to form NH3OH+. This is a weak acid, and its concentration will be the same as the initial concentration of NH2OH, which is 0.200 M.
Calculate the pH using the weak acid equilibrium: The pH at the equivalence point is determined by the hydrolysis of NH3OH+. Use the expression for the acid dissociation constant (Ka) of NH3OH+ to find the concentration of H+ ions.
Use the relationship between Ka and Kb: Since NH2OH is a weak base, you can find the Ka of NH3OH+ using the relation Ka * Kb = Kw, where Kw is the ion-product constant of water (1.0 x 10^-14 at 25°C).
Calculate the pH: Once you have the concentration of H+ ions from the hydrolysis of NH3OH+, use the formula pH = -log[H+] to find the pH at the equivalence point.
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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 solution being titrated. 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 titration involving a weak base and a strong acid, the resulting solution may contain the conjugate acid of the weak base, which can affect the pH. The pH can be calculated using the concentration of the conjugate acid and its dissociation constant (Ka).
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Percorso guidato
02:15pH Calculation Example
Hydroxylamine as a Weak Base
Hydroxylamine (NH2OH) is a weak base that can accept protons, forming its conjugate acid, hydroxylammonium (NH3OH+). When titrated with a strong acid like HBr, the hydroxylamine will be converted to its conjugate acid at the equivalence point. The pH at this point will depend on the concentration of the conjugate acid and its ability to donate protons back to the solution, which can be analyzed using its dissociation constant.
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00:51ICE Charts of Weak Bases
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