Domanda del libro di testo
A solution is made 1.1⨉10-3 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains?
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Ch.18 - Aqueous Ionic Equilibrium
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- 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
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 18, Problema 117
Use the appropriate values of Ksp and Kf to find the equilibrium constant for the reaction. FeS(s) + 6 CN-(aq) ⇌ Fe(CN)64-(aq) + S2-(aq)
Guida verificata passo dopo passo1
Identify the relevant equilibrium reactions and their constants: The dissolution of FeS and the formation of the complex ion Fe(CN)_6^{4-}.
Write the dissolution reaction for FeS: FeS(s) \(\rightleftharpoons\) Fe^{2+}(aq) + S^{2-}(aq) with its solubility product constant K_{sp}.
Write the formation reaction for the complex ion: Fe^{2+}(aq) + 6 CN^-(aq) \(\rightleftharpoons\) Fe(CN)_6^{4-}(aq) with its formation constant K_f.
Combine the two reactions to obtain the overall reaction: FeS(s) + 6 CN^-(aq) \(\rightleftharpoons\) Fe(CN)_6^{4-}(aq) + S^{2-}(aq).
Calculate the equilibrium constant for the overall reaction by multiplying the K_{sp} of FeS and the K_f of Fe(CN)_6^{4-}.
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Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It quantifies the extent to which a compound can dissolve in water, represented by the concentrations of its ions at equilibrium. For the reaction involving FeS, Ksp helps determine the solubility of FeS in the presence of complexing agents like CN-.
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01:47
Solubility Product Constant
Formation Constant (Kf)
The formation constant (Kf) is a measure of the stability of a complex ion in solution. It quantifies the equilibrium between the free ions and the complex formed when they react. In the given reaction, Kf is crucial for understanding how effectively CN- ions bind with Fe2+ to form the complex ion Fe(CN)64-, influencing the overall equilibrium of the reaction.
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02:20Complex Ions and Formation Constant
Equilibrium Constant (K)
The equilibrium constant (K) for a reaction is derived from the concentrations of the products and reactants at equilibrium. It provides insight into the extent of the reaction and can be calculated using Ksp and Kf values. In this case, the equilibrium constant for the reaction involving FeS and CN- can be determined by combining the Ksp of FeS and the Kf for the formation of the complex ion, reflecting the relationship between solubility and complexation.
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01:14Equilibrium Constant K