Domanda del libro di testo
Use the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: SO42-, CO32-, SO32-, and PO43-.
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Ch.16 - Acid-Base 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
Capitolo 16, Problema 73b
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.
Guida verificata passo dopo passo1
Step 1: Understand the problem. We are given a weak base, ephedrine, with a concentration of 0.035 M and a pH of 11.33. We need to calculate the base dissociation constant, K_b.
Step 2: Calculate the concentration of OH^- ions. Use the pH to find the pOH: \( \text{pOH} = 14 - \text{pH} \). Then, calculate the concentration of OH^- using \( [\text{OH}^-] = 10^{-\text{pOH}} \).
Step 3: Set up the equilibrium expression for the dissociation of ephedrine. The reaction is: \( \text{C}_{10}\text{H}_{15}\text{ON} + \text{H}_2\text{O} \rightleftharpoons \text{C}_{10}\text{H}_{15}\text{ONH}^+ + \text{OH}^- \).
Step 4: Write the expression for K_b. The base dissociation constant is given by \( K_b = \frac{[\text{C}_{10}\text{H}_{15}\text{ONH}^+][\text{OH}^-]}{[\text{C}_{10}\text{H}_{15}\text{ON}]} \).
Step 5: Substitute the known values into the K_b expression. Use the initial concentration of ephedrine and the calculated concentration of OH^- to find K_b.
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Weak Bases and Kb
Weak bases are substances that partially ionize in solution, establishing an equilibrium between the un-ionized base and its ions. The base dissociation constant (Kb) quantifies the strength of a weak base, indicating the extent to which it can accept protons from water. A higher Kb value signifies a stronger base, while a lower value indicates a weaker base.
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Percorso guidato
00:51
ICE Charts of Weak Bases
pH and pOH Relationship
pH is a measure of the hydrogen ion concentration in a solution, while pOH measures the hydroxide ion concentration. The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. In the context of weak bases, knowing the pH allows for the calculation of pOH, which is essential for determining the concentration of hydroxide ions in the solution.
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Percorso guidato
02:09pH and pOH Calculations
Equilibrium Expressions
Equilibrium expressions describe the ratio of the concentrations of products to reactants at equilibrium for a given reaction. For the dissociation of a weak base, the Kb expression is formulated as Kb = [BH+][OH-] / [B], where [B] is the concentration of the un-ionized base, [BH+] is the concentration of the conjugate acid, and [OH-] is the concentration of hydroxide ions. This expression is crucial for calculating Kb from the concentrations at equilibrium.
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03:20Equilibrium Constant Expressions
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-?
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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?
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