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. (a) HCl
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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 109
Use Le Châtelier’s principle to explain the following changes in the solubility of Ag2CO3 in water. (a) Decrease on addition of AgNO3 (b) Increase on addition of HNO3 (c) Decrease on addition of Na2CO3 (d) Increase on addition of NH3
Guida verificata passo dopo passo1
Step 1: Identify the equilibrium reaction for the dissolution of Ag2CO3 in water: Ag2CO3(s) \(\rightleftharpoons\) 2Ag^+(aq) + CO3^{2-}(aq).
Step 2: (a) Addition of AgNO3 increases the concentration of Ag^+ ions. According to Le Châtelier’s principle, the equilibrium will shift to the left to reduce the stress of increased Ag^+ concentration, decreasing the solubility of Ag2CO3.
Step 3: (b) Addition of HNO3 introduces H^+ ions, which react with CO3^{2-} ions to form H2CO3, reducing CO3^{2-} concentration. The equilibrium shifts to the right to replace the CO3^{2-} ions, increasing the solubility of Ag2CO3.
Step 4: (c) Addition of Na2CO3 increases the concentration of CO3^{2-} ions. The equilibrium shifts to the left to reduce the stress of increased CO3^{2-} concentration, decreasing the solubility of Ag2CO3.
Step 5: (d) Addition of NH3 forms a complex with Ag^+ ions (Ag(NH3)2^+), reducing the free Ag^+ ion concentration. The equilibrium shifts to the right to replace the Ag^+ ions, increasing the solubility of Ag2CO3.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Le Châtelier’s Principle
Le Châtelier’s principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle is crucial for predicting how the solubility of a compound, like Ag2CO3, will respond to various external changes, such as concentration or pressure.
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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. For Ag2CO3, the Ksp value helps determine how changes in concentration of ions in solution affect its solubility, guiding predictions about the effects of adding different substances.
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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 Ag2CO3, adding AgNO3 introduces Ag+ ions, which shifts the equilibrium to the left, reducing the solubility of Ag2CO3 due to the increased concentration of the common ion.
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Percorso guidato
02:53Common Ion Effect
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