Domanda del libro di testo
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (d) Ba1NO322
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Ch.17 - Applications of Aqueous Equilibria
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 17, Problema 111
Calculate the molar solubility of PbCrO4 in: (a) Pure Water (d) 1.0 x 10^-3 M K2CrO4
Guida verificata passo dopo passo1
Step 1: Write the dissolution equation for PbCrO4.
Step 2: Write the expression for the solubility product constant (Ksp) of PbCrO4.
Step 3: For part (a), set up an expression for the molar solubility in pure water using the Ksp expression.
Step 4: For part (b), consider the common ion effect due to the presence of CrO4^2- from K2CrO4 and modify the Ksp expression accordingly.
Step 5: Solve the modified Ksp expression for the molar solubility in the presence of 1.0 x 10^-3 M K2CrO4.
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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 solubility changes with different conditions, such as the presence of common ions or changes in temperature.
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Percorso guidato
04:13
Molar Solubility Example
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, adding K2CrO4 introduces CrO4^2- ions, which shifts the equilibrium of the dissolution of PbCrO4, reducing its molar solubility due to Le Chatelier's principle.
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Percorso guidato
02:53Common Ion Effect
Equilibrium Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. For PbCrO4, Ksp can be used to calculate its molar solubility in pure water and in the presence of other ions, as it relates the concentrations of the ions in solution at equilibrium.
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01:14Equilibrium Constant K
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Domanda del libro di testo
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (c) NaNO3
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Domanda del libro di testo
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (b) KF
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