Textbook Question
Classify each of the following reactions as a precipitation, acid–base neutralization, or oxidation–reduction. (a) (b) (c)
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Ch.4 - Reactions in Aqueous Solution
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- 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
Chapter 4, Problem 75
Write net ionic equations for the reactions listed in Problem 4.73.
Verified step by step guidance1
Identify the reactants and products in the given chemical reaction.
Write the balanced molecular equation for the reaction.
Dissociate all strong electrolytes (soluble salts, strong acids, and strong bases) into their constituent ions.
Identify and cancel out the spectator ions that appear on both sides of the equation.
Write the net ionic equation with the remaining species, ensuring it is balanced in terms of both mass and charge.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Net Ionic Equations
Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions that do not change during the reaction. They are derived from complete ionic equations by removing ions that appear on both sides of the equation. This simplification helps to focus on the essential chemical changes occurring in the reaction.
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Net Ionic Equations
Spectator Ions
Spectator ions are ions that exist in the same form on both the reactant and product sides of a chemical equation. They do not participate in the actual chemical reaction and can be omitted when writing net ionic equations. Identifying spectator ions is crucial for accurately simplifying the reaction to its net ionic form.
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Balancing Chemical Equations
Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both the reactant and product sides of the equation. This is essential for obeying the law of conservation of mass. A balanced equation provides a clear representation of the stoichiometry of the reaction, which is necessary for deriving the net ionic equation.
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Related Practice
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Ethylene glycol, C2H6O2, is the principal constituent of auto-mobile antifreeze. If the density of a 40.0 mass % solution of ethylene glycol in water is 1.0514 g/mL at 20 °C, what is the molarity?
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Textbook Question
Write net ionic equations for the reactions listed in Problem 4.72.
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Textbook Question
Which of the following substances are likely to be soluble in water?(a) PbSO4(b) Ba(NO3)2 (c) SnCO3(d) (NH4)3PO4
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Which of the following substances are likely to be soluble in water?(a) ZnS (b) AU2(CO3)3 (c) PbCl2(d) Na2S
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Textbook Question
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. (a)
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