Domanda del libro di testo
Write the chemical equation and the Kb expression for the reaction of each of the following bases with water: (a) propylamine, C3H7NH2
752
views
Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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
Capitolo 16, Problema 72
Calculate the molar concentration of OH- in a 0.724 M solution of hypobromite ion BrO-; Kb = 4.0 * 10^-6. What is the pH of this solution?
Guida verificata passo dopo passo1
Step 1: Write the equilibrium expression for the base dissociation of hypobromite ion (BrO^-). The reaction is: \[ \text{BrO}^- + \text{H}_2\text{O} \rightleftharpoons \text{OH}^- + \text{HBrO} \]
Step 2: Set up the expression for the base dissociation constant (K_b) using the concentrations of the products and reactants at equilibrium: \[ K_b = \frac{[\text{OH}^-][\text{HBrO}]}{[\text{BrO}^-]} \]
Step 3: Assume that the change in concentration of BrO^- due to dissociation is small compared to the initial concentration. Let x be the concentration of OH^- at equilibrium. Then, \[ [\text{OH}^-] = x, [\text{HBrO}] = x, [\text{BrO}^-] = 0.724 - x \approx 0.724 \]
Step 4: Substitute the equilibrium concentrations into the K_b expression and solve for x: \[ 4.0 \times 10^{-6} = \frac{x^2}{0.724} \]
Step 5: Calculate the pH of the solution using the concentration of OH^- found in the previous step. First, find the pOH: \[ \text{pOH} = -\log[\text{OH}^-] \], then use the relation \[ \text{pH} = 14 - \text{pOH} \] to find the pH.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Equilibrium Constant (Kb)
The base dissociation constant (Kb) quantifies the strength of a base in solution. It is defined as the equilibrium constant for the reaction where a base accepts a proton from water, producing hydroxide ions (OH-) and the conjugate acid. A higher Kb value indicates a stronger base, which in this case helps determine the concentration of OH- ions produced from the hypobromite ion (BrO-).
Video consigliato:
Percorso guidato
01:14
Equilibrium Constant K
Hydrolysis of Hypobromite Ion
Hypobromite ion (BrO-) can undergo hydrolysis in water, reacting with water to form hydroxide ions (OH-) and hypobromous acid (HBrO). This reaction is essential for calculating the concentration of OH- in the solution. The extent of this reaction is governed by the Kb value, allowing us to set up an equilibrium expression to find the concentration of OH- ions.
Video consigliato:
Percorso guidato
06:17Ion Formation
pH and pOH Relationship
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. Conversely, pOH measures the concentration of hydroxide ions. The relationship between pH and pOH is given by the equation pH + pOH = 14 at 25°C. Once the concentration of OH- is determined, pOH can be calculated, and subsequently, pH can be derived from this relationship.
Video consigliato:
Percorso guidato
02:09pH and pOH Calculations
Pratica correlata
Domanda del libro di testo
Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (a) What are the equilibrium concentrations of C10H15ON, C10H15ONH+, and OH-?
1229
views
Domanda del libro di testo
Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (b) Calculate Kb for ephedrine.
462
views
Domanda del libro di testo
Codeine 1C18H21NO32 is a weak organic base. A 5.0 * 10-3M solution of codeine has a pH of 9.95. Calculate the value of Kb for this substance. What is the pKb for this base?
2159
views
3
rank
Domanda del libro di testo
Write the chemical equation and the Kb expression for the reaction of each of the following bases with water: (c) benzoate ion, C6H5CO2-
512
views