Textbook Question
Calculate the molar solubility of PbCrO4 in: (a) Pure Water(d) 1.0 x 10^-3 M K2CrO4
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Ch.17 - Applications of Aqueous Equilibria
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 17, Problem 110a
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. (a) HCl
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Identify the dissolution reaction of BaF2 in water: BaF2(s) ⇌ Ba^{2+}(aq) + 2F^{-}(aq).
Recognize that HCl is a strong acid and will dissociate completely in water to form H^{+}(aq) and Cl^{-}(aq).
Understand that the addition of HCl increases the concentration of H^{+}(aq) in the solution.
Consider the common ion effect and Le Châtelier's principle. The increase in H^{+}(aq) can react with F^{-}(aq) to form HF(aq), which decreases the concentration of F^{-}(aq).
Predict the shift in equilibrium: With the decrease in F^{-}(aq) concentration, the equilibrium will shift to the right to produce more F^{-}(aq), thus increasing the solubility of BaF2.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Le Châtelier's Principle
Le Châtelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle is crucial for predicting how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction.
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Le Chatelier's Principle
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, and changes in concentration of the ions can shift the equilibrium, affecting the solubility of the compound.
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Common Ion Effect
The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. In the case of BaF2, adding HCl introduces Cl- ions, which can shift the equilibrium and reduce the solubility of BaF2 due to the increased concentration of one of its constituent ions.
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Related Practice
Textbook Question
If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?(a) 50.0 mL of 0.100 M HBr and 30.0 mL of 0.200 M KOH
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Textbook Question
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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Textbook Question
Use the values of Ksp in Appendix C to calculate the solubility of the following compounds (in g/L): (c) Cu3(PO4)2
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Textbook Question
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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Textbook Question
Use the values of Ksp in Appendix C to calculate the molar solubility of the following compounds: (b) Mg(OH)2
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