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 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
Guida verificata passo dopo passo1
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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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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Percorso guidato
07:32
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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Percorso guidato
01:47Solubility Product Constant
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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Percorso guidato
02:53Common Ion Effect
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