Domanda del libro di testo
Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. b. 0.085 M CaI2; K2SO4
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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 111
What is the minimum concentration of KOH required for precipitation to begin for each of the following cation solutions? a. 0.015 M CaCl2 b. 0.0025 M Fe(NO3)2 c. 0.0018 M MgBr2
Guida verificata passo dopo passo1
Identify the relevant solubility product constant (K_sp) for each cation's hydroxide compound: Ca(OH)_2, Fe(OH)_2, and Mg(OH)_2.
Write the balanced chemical equation for the precipitation reaction of each cation with OH^- ions: Ca^{2+} + 2OH^- \(\rightarrow\) Ca(OH)_2, Fe^{2+} + 2OH^- \(\rightarrow\) Fe(OH)_2, Mg^{2+} + 2OH^- \(\rightarrow\) Mg(OH)_2.
Express the K_sp expression for each hydroxide: K_{sp} = [Ca^{2+}][OH^-]^2, K_{sp} = [Fe^{2+}][OH^-]^2, K_{sp} = [Mg^{2+}][OH^-]^2.
Substitute the given concentration of each cation into the K_sp expression to solve for the minimum [OH^-] required for precipitation: [OH^-] = \(\sqrt{\frac{K_{sp}\)}{[Ca^{2+}]}}, [OH^-] = \(\sqrt{\frac{K_{sp}\)}{[Fe^{2+}]}}, [OH^-] = \(\sqrt{\frac{K_{sp}\)}{[Mg^{2+}]}}, where [Ca^{2+}], [Fe^{2+}], and [Mg^{2+}] are the given concentrations.
Calculate the minimum concentration of KOH required, which is equal to the [OH^-] concentration found in the previous step, since KOH dissociates completely in solution.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
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 in a saturated solution at a given temperature. For precipitation to occur, the product of the ion concentrations must exceed the Ksp value of the compound being formed, indicating that the solution is supersaturated.
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Percorso guidato
01:47
Solubility Product Constant
Precipitation Reaction
A precipitation reaction occurs when two soluble salts react in solution to form an insoluble compound, or precipitate. This process is driven by the formation of a solid that separates from the liquid phase. In the context of the question, KOH reacts with cations from the given solutions to form insoluble hydroxides, leading to precipitation.
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Percorso guidato
01:53Selective Precipitation
Ion Concentration and Stoichiometry
Ion concentration refers to the amount of a specific ion present in a solution, typically expressed in molarity (M). Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. To determine the minimum concentration of KOH needed for precipitation, one must consider the stoichiometric ratios of KOH to the cations in the solutions and their respective solubility limits.
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Percorso guidato
01:16Stoichiometry Concept
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