Textbook Question
The solubility product for Zn1OH22 is 3.0 * 10-16. The formation constant for the hydroxo complex, Zn1OH242 - , is 4.6 * 1017. What concentration of OH- is required to dissolve 0.015 mol of Zn1OH22 in a liter of solution?
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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 105
The solubility product constants of PbSO4 and SrSO4 are 6.3 * 10-7 and 3.2 * 10-7, respectively. What are the values of 3SO4 2 - 4, 3Pb2 + 4, and 3Sr2 + 4 in a solution at equilibrium with both substances?
Verified step by step guidance1
Identify the dissolution reactions for PbSO_4 and SrSO_4: PbSO_4 (s) \(\rightleftharpoons\) Pb^{2+} (aq) + SO_4^{2-} (aq) and SrSO_4 (s) \(\rightleftharpoons\) Sr^{2+} (aq) + SO_4^{2-} (aq).
Write the expressions for the solubility product constants (K_{sp}) for each salt: K_{sp, PbSO_4} = [Pb^{2+}][SO_4^{2-}] and K_{sp, SrSO_4} = [Sr^{2+}][SO_4^{2-}].
Let the solubility of PbSO_4 be 's_1' and that of SrSO_4 be 's_2'. At equilibrium, [Pb^{2+}] = s_1 and [Sr^{2+}] = s_2, while [SO_4^{2-}] = s_1 + s_2.
Substitute the expressions for [Pb^{2+}], [Sr^{2+}], and [SO_4^{2-}] into the K_{sp} expressions: K_{sp, PbSO_4} = s_1(s_1 + s_2) and K_{sp, SrSO_4} = s_2(s_1 + s_2).
Solve the system of equations formed by the K_{sp} expressions to find the values of s_1, s_2, and [SO_4^{2-}] at equilibrium.
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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 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 equation. For example, for PbSO4, Ksp = [Pb2+][SO4^2-]. Understanding Ksp is crucial for predicting the solubility of salts in solution.
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Solubility Product Constant
Equilibrium in Chemical Reactions
Equilibrium in chemical reactions occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the context of solubility, this means that the dissolution of a solid and the precipitation of its ions occur at the same rate. Analyzing equilibrium conditions helps determine the concentrations of ions in a saturated solution of salts like PbSO4 and SrSO4.
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Common Ion Effect
The common ion effect refers to the decrease in solubility of a salt when a common ion is added to the solution. This phenomenon occurs because the presence of a common ion shifts the equilibrium position according to Le Chatelier's principle, favoring the formation of the solid phase. In this question, the presence of either Pb2+ or Sr2+ ions will influence the solubility of PbSO4 and SrSO4, respectively, affecting the equilibrium concentrations of the ions.
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Related Practice
Textbook Question
The solubility-product constant for barium permanganate, Ba1MnO422, is 2.5 * 10-10. Assume that solid Ba1MnO422 is in equilibrium with a solution of KMnO4. What concentration of KMnO4 is required to establish a concentration of 2.0 * 10-8 M for the Ba2 + ion in solution?
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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?
Textbook Question
A solid sample of Fe1OH23 is added to 0.500 L of 0.250 Maqueous H2SO4. The solution that remains is still acidic. Itis then titrated with 0.500 M NaOH solution, and it takes12.5 mL of the NaOH solution to reach the equivalencepoint. What mass of Fe1OH23 was added to the H2SO4solution?
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