Textbook Question
The value of Ksp for Cd(OH)2 is 2.5 × 10-14. (a) What is the molar solubility of Cd(OH)2?
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 17, Problem 111b
(b) As the acid is titrated, the pH of the solution after the addition of 11.05 mL of the base is 4.89. What is the Ka for the acid?
Verified step by step guidance1
Identify the type of titration: Since the pH is given after adding a base to an acid, this is an acid-base titration.
Use the Henderson-Hasselbalch equation: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \), where \([\text{A}^-]\) is the concentration of the conjugate base and \([\text{HA}]\) is the concentration of the acid.
Rearrange the equation to solve for \( \text{pK}_a \): \( \text{pK}_a = \text{pH} - \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \).
Convert \( \text{pK}_a \) to \( K_a \) using the relationship \( K_a = 10^{-\text{pK}_a} \).
Determine the concentrations of \([\text{A}^-]\) and \([\text{HA}]\) using the initial concentrations and volumes of the acid and base to find \( K_a \).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Titration
An acid-base titration is a quantitative analytical method used to determine the concentration of an acid or base in a solution. During the titration, a base is gradually added to an acid (or vice versa) until the reaction reaches the equivalence point, where the amount of acid equals the amount of base. The pH of the solution changes throughout the process, and specific pH values can indicate the strength of the acid or base involved.
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Acid-Base Titration
pH and pKa Relationship
The pH of a solution is a measure of its acidity or basicity, defined as the negative logarithm of the hydrogen ion concentration. The pKa is the negative logarithm of the acid dissociation constant (Ka) and indicates the strength of an acid; lower pKa values correspond to stronger acids. The Henderson-Hasselbalch equation relates pH, pKa, and the concentrations of the acid and its conjugate base, allowing for the calculation of Ka when pH and concentrations are known.
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Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of an acid in solution, representing the equilibrium constant for the dissociation of the acid into its ions. A higher Ka value indicates a stronger acid that dissociates more completely in solution. The Ka can be calculated using the concentrations of the products and reactants at equilibrium, which is essential for determining the strength of the acid in the titration scenario presented.
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Related Practice
Textbook Question
A concentration of 10–100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Using Ksp values from Appendix D, calculate the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium with (b) AgBr (c) AgI.
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Textbook Question
(a) Write the net ionic equation for the reaction that occurs when a solution of hydrochloric acid (HCl) is mixed with a solution of sodium formate 1NaCHO22.
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Textbook Question
(a) A 0.1044-g sample of an unknown monoprotic acid requires 22.10 mL of 0.0500 M NaOH to reach the end point. What is the molar mass of the unknown?
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