Domanda del libro di testo
Predict whether a precipitation reaction will occur when aqueous solutions of the following substances are mixed. For those that form a precipitate, write the net ionic reaction. (d)
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Ch.4 - Reactions in Aqueous Solution
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 4, Problema 81
Which of the following solutions will not form a precipitate when added to 0.10 M NaOH? (a) 0.10 M MgBr2 (b) 0.10 M NH4Br (c) 0.10 M FeCl2
Guida verificata passo dopo passo1
Identify the ions present in each solution when dissolved in water: (a) MgBr2 dissociates into Mg^{2+} and 2 Br^{-}, (b) NH4Br dissociates into NH4^{+} and Br^{-}, (c) FeCl2 dissociates into Fe^{2+} and 2 Cl^{-}.
Consider the ions present in the NaOH solution: NaOH dissociates into Na^{+} and OH^{-}.
Determine the possible precipitates by considering the solubility rules: Mg(OH)2 is insoluble, NH4OH is soluble, and Fe(OH)2 is insoluble.
Predict the formation of precipitates: (a) Mg^{2+} + 2 OH^{-} \(\rightarrow\) Mg(OH)2 (precipitate), (b) NH4^{+} + OH^{-} \(\rightarrow\) NH4OH (no precipitate), (c) Fe^{2+} + 2 OH^{-} \(\rightarrow\) Fe(OH)2 (precipitate).
Conclude that the solution that will not form a precipitate when added to 0.10 M NaOH is (b) 0.10 M NH4Br.
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Solubility Rules
Solubility rules are guidelines that help predict whether a compound will dissolve in water or form a precipitate. For example, most alkali metal salts and ammonium salts are soluble, while many transition metal hydroxides are not. Understanding these rules is essential for determining the outcome of mixing solutions, particularly in the context of precipitation reactions.
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00:28
Solubility Rules
Precipitation Reactions
A precipitation reaction occurs when two soluble salts react in solution to form an insoluble compound, known as a precipitate. This process is driven by the formation of a product that is less soluble than the reactants. Identifying the ions present in the solutions and their potential interactions is crucial for predicting whether a precipitate will form.
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01:53Selective Precipitation
Ion Concentration and Reaction Quotient
The reaction quotient (Q) compares the concentrations of the products and reactants in a solution. If Q exceeds the solubility product constant (Ksp) for a given compound, a precipitate will form. In this context, understanding the concentrations of ions in the solutions being mixed helps determine if a precipitate will form when NaOH is added.
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00:49Reaction Quotient Q
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