Textbook Question
(b) Write the expression for the solubility-product constant for each of the following ionic compounds: MnCO3, Hg(OH)2, and Cu3(PO4)3.
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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 52a
(a) True or false: 'solubility' and 'solubility-product constant' are the same number for a given compound.
Verified step by step guidance1
Understand the definition of 'solubility': Solubility refers to the maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature, usually expressed in grams per liter (g/L) or moles per liter (M).
Understand the definition of 'solubility-product constant' (Ksp): The solubility-product constant is an equilibrium constant that applies to the dissolution of a sparingly soluble ionic compound. It is expressed in terms of the concentrations of the ions produced, raised to the power of their stoichiometric coefficients in the dissolution equation.
Recognize the difference in units: Solubility is typically expressed in units of concentration (g/L or M), while the solubility-product constant is unitless, as it is a product of the concentrations of the ions, each raised to the power of their coefficients in the balanced chemical equation.
Consider the relationship between solubility and Ksp: While both solubility and Ksp describe aspects of a compound's ability to dissolve, they are not the same numerical value. Solubility is a direct measure of how much of a compound can dissolve, whereas Ksp describes the extent to which a compound can dissolve into its constituent ions at equilibrium.
Conclude the truth value: Given the differences in definition, units, and what they measure, 'solubility' and 'solubility-product constant' are not the same number for a given compound, making the statement false.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Solubility
Solubility refers to the maximum amount of a solute that can dissolve in a solvent at a given temperature and pressure. It is typically expressed in terms of concentration, such as moles per liter (M). Solubility can vary with temperature and the nature of the solute and solvent, making it a crucial factor in understanding how substances interact in solution.
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00:28
Solubility Rules
Solubility-Product Constant (Ksp)
The solubility-product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. Ksp provides a quantitative measure of a compound's solubility and is temperature-dependent.
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01:47Solubility Product Constant
Relationship Between Solubility and Ksp
While solubility and Ksp are related, they are not the same. Solubility is a measure of how much of a compound can dissolve, while Ksp is a constant that reflects the equilibrium condition of the dissolved ions. For a given compound, the solubility can be calculated from Ksp, but the two values differ, especially for compounds that dissociate into multiple ions.
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01:12Ksp and Solubility Example
Related Practice
Textbook Question
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (b) chlorous acid (HClO2).
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Textbook Question
(a) I f t he molar solubility of CaF2 at 35°C i s 1.24 × 10–3 mol/L, what is Ksp at this temperature?
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Textbook Question
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (c) benzoic acid (C6H5COOH).
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Textbook Question
(b) It is found that 1.1 × 10-2 g SrF2 dissolves per 100 mL of aqueous solution at 25°C. Calculate the solubility product for SrF2.
Textbook Question
The solubility of two slightly soluble salts of M2 + , MA and MZ2, is the same, 4 * 10-4 mol/L. (c) If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+?
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