Textbook Question
Refer to the Ksp values in Table 18.2 to calculate the molar solubility of each compound in pure water. a. AgBr
Ch.18 - Aqueous Ionic Equilibrium
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 18, Problem 91c
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. c. Ag2CrO4
Verified step by step guidance1
Identify the dissolution process of the ionic compound Ag_2CrO_4 in water.
Write the balanced chemical equation for the dissolution: Ag_2CrO_4(s) \(\rightleftharpoons\) 2Ag^+(aq) + CrO_4^{2-}(aq).
Understand that the solubility product constant (K_{sp}) is an equilibrium constant for the dissolution of a sparingly soluble compound.
Write the expression for the solubility product constant (K_{sp}) based on the balanced equation: K_{sp} = [Ag^+]^2[CrO_4^{2-}].
Note that the concentrations of the ions are raised to the power of their coefficients in the balanced equation.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of ionic compounds. It represents the maximum concentration of ions that can exist in a saturated solution at a given temperature. Ksp is calculated from the concentrations of the ions in solution, raised to the power of their coefficients in the balanced dissolution equation.
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Solubility Product Constant
Dissolution of Ionic Compounds
The dissolution of ionic compounds involves the separation of the compound into its constituent ions when it is added to water. For example, when silver chromate (Ag2CrO4) dissolves, it dissociates into two silver ions (Ag+) and one chromate ion (CrO4^2-). This process is represented by a balanced chemical equation that shows the stoichiometry of the ions produced.
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Balancing Chemical Equations
Balancing chemical equations is essential to ensure that the number of atoms of each element is conserved during a chemical reaction. In the context of dissolution, this means that the total number of each type of ion produced must match the number of ions in the original compound. This is crucial for accurately writing the Ksp expression, which is derived from the balanced equation.
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Related Practice
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