Domanda del libro di testo
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
1101
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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 79d
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)
Guida verificata passo dopo passo1
Identify the ions present in each of the aqueous solutions. For example, if the solutions are of NaCl and AgNO3, the ions would be Na^+, Cl^-, Ag^+, and NO3^-.
Determine the possible combinations of cations and anions that can form new compounds. In our example, the possible combinations are NaNO3 and AgCl.
Use the solubility rules to determine if any of the new combinations form an insoluble compound (precipitate). According to solubility rules, AgCl is insoluble in water.
If a precipitate forms, write the balanced molecular equation for the reaction. For example, AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq).
Write the net ionic equation by removing the spectator ions (ions that do not participate in the formation of the precipitate) from the balanced molecular equation. For the example, the net ionic equation is Ag^+(aq) + Cl^-(aq) -> AgCl(s).
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Precipitation Reactions
Precipitation reactions occur when two aqueous solutions are mixed, resulting in the formation of an insoluble solid, known as a precipitate. This happens when the product of the reaction has a solubility product (Ksp) that is exceeded in the solution, leading to the aggregation of ions into a solid form. Understanding the solubility rules helps predict whether a precipitate will form.
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Percorso guidato
01:53
Selective Precipitation
Solubility Rules
Solubility rules are guidelines that help predict the solubility of various ionic compounds in water. These rules indicate which compounds are generally soluble or insoluble in aqueous solutions, based on the ions present. For example, most nitrates are soluble, while many carbonates are not. Familiarity with these rules is essential for determining the outcome of mixing different ionic solutions.
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Percorso guidato
00:28Solubility Rules
Net Ionic Equations
Net ionic equations represent the actual chemical species involved in a precipitation reaction, excluding spectator ions that do not participate in the reaction. To write a net ionic equation, one must first identify the ions in solution, determine which form a precipitate, and then write the equation showing only the ions and compounds that undergo a change. This simplifies the reaction and highlights the key components involved.
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Percorso guidato
00:51Net Ionic Equations
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