Domanda del libro di testo
Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (a) 0.095 M propionic acid (C2H5COOH) (b) 0.100 M hydrogen chromate ion (HCrO4-)
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Ch.16 - Acid-Base 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
Capitolo 16, Problema 64c
Determine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (c) 0.165 M hydroxylamine.
Guida verificata passo dopo passo1
Identify that hydroxylamine (NH2OH) is a weak base and will partially dissociate in water.
Write the equilibrium expression for the dissociation of hydroxylamine: NH2OH + H2O \(\rightleftharpoons\) NH3OH^+ + OH^-.
Use the given concentration of hydroxylamine (0.165 M) as the initial concentration in the ICE table.
Set up the expression for the base dissociation constant (Kb) using the equilibrium concentrations from the ICE table: Kb = \(\frac{[NH3OH^+][OH^-]}{[NH2OH]}\).
Solve for the hydroxide ion concentration [OH^-] using the Kb value, then calculate the pOH and finally the pH using the relation pH + pOH = 14.
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Acid-Base Theory
Acid-base theory explains the behavior of acids and bases in solution. According to the Brønsted-Lowry theory, acids are proton donors and bases are proton acceptors. Hydroxylamine (NH2OH) can act as a weak base, accepting protons from water to form hydroxylammonium ions (NH3OH+), which is essential for calculating the pH of the solution.
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Percorso guidato
02:08
Bronsted-Lowry Acid-Base Theory
Dissociation Constants (Ka and Kb)
Dissociation constants, Ka for acids and Kb for bases, quantify the strength of an acid or base in solution. For hydroxylamine, the Kb value is used to determine how much it dissociates in water. The relationship between Kb and pH is crucial for calculating the concentration of hydroxylammonium ions and the resulting pH of the solution.
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Percorso guidato
03:01Ka and Kb Relationship
pH Calculation
pH is a measure of the hydrogen ion concentration in a solution, calculated using the formula pH = -log[H+]. For weak bases like hydroxylamine, the pH can be determined by first calculating the concentration of hydroxide ions (OH-) produced, then using the relationship between pH, pOH, and the ion product of water (Kw) to find the final pH value.
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Percorso guidato
02:15pH Calculation Example