Textbook Question
Determine if each compound is more soluble in acidic solution than it is in pure water. Explain. a. BaCO3 b. CuS c. AgCl d. PbI2
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Ch.18 - Aqueous Ionic Equilibrium
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 18, Problem 102b
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. b. 0.25 M MCl2
Verified step by step guidance1
Step 1: Understand the dissolution process of MX in water. The dissolution of MX can be represented as: \[ \text{MX} \rightleftharpoons \text{M}^{2+} + \text{X}^{-} \]
Step 2: Write the expression for the solubility product constant (Ksp) for MX. The expression is: \[ K_{sp} = [\text{M}^{2+}][\text{X}^{-}] \]
Step 3: Consider the common ion effect due to the presence of 0.25 M MCl2. Since MCl2 dissociates completely, it contributes 0.25 M of \( \text{M}^{2+} \) ions to the solution.
Step 4: Let the molar solubility of MX be \( s \). The concentration of \( \text{M}^{2+} \) ions from MX will be \( s \), but due to the common ion effect, the total concentration of \( \text{M}^{2+} \) ions will be \( 0.25 + s \). The concentration of \( \text{X}^{-} \) ions will be \( s \).
Step 5: Substitute these concentrations into the Ksp expression: \[ K_{sp} = (0.25 + s)(s) \]. Since \( K_{sp} \) is very small, assume \( s \) is much smaller than 0.25, simplifying the expression to \[ K_{sp} \approx 0.25s \]. Solve for \( s \) to find the molar solubility.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Solubility
Molar solubility refers to the maximum amount of a solute that can dissolve in a given volume of solvent at equilibrium, expressed in moles per liter (M). It is a crucial concept in understanding how substances dissolve and is often determined using the solubility product constant (Ksp) for sparingly soluble salts.
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Molar Solubility Example
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that quantifies the solubility of a sparingly soluble ionic compound. 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. A lower Ksp value indicates lower solubility.
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Common Ion Effect
The common ion effect describes the decrease in solubility of a salt when a common ion is added to the solution. In this case, the presence of MCl2 introduces the ion M+, which shifts the equilibrium of the dissolution reaction of MX, reducing its molar solubility due to Le Chatelier's principle.
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Related Practice
Textbook Question
Consider the compounds with the generic formulas listed and their corresponding molar solubilities in pure water. Which compound has the smallest value of Ksp? a. AX; molar solubility = 1.35⨉10-4 M b. AX2; molar solubility = 2.25⨉10-4 M c. A2X; molar solubility = 1.75⨉10-4 M
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Textbook Question
Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water
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Textbook Question
A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO3)2. Does a precipitate form in the mixed solution? If so, identify the precipitate.
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Textbook Question
The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.
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Textbook Question
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4
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