Textbook Question
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide
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Ch.4 - Reactions in Aqueous Solution
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 4, Problem 40b
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (b) Solid chromium(III) hydroxide reacts with nitrous acid.
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Write the formulas for the reactants: Solid chromium(III) hydroxide is Cr(OH)₃ and nitrous acid is HNO₂.
Combine the reactants in a balanced chemical equation. Since Cr(OH)₃ is a base and HNO₂ is an acid, they will react in a typical acid-base neutralization to form water and a salt. The salt in this case would be chromium(III) nitrite, Cr(NO₂)₃.
Balance the equation by ensuring that the number of atoms for each element is the same on both sides of the equation. This involves adjusting the coefficients of the reactants and products.
Write the total ionic equation by breaking all soluble compounds into their ions. Chromium(III) hydroxide is slightly soluble, so it will mostly remain as Cr(OH)₃(s). Nitrous acid is a weak acid but can be ionized as H⁺ and NO₂⁻.
Identify and remove the spectator ions (ions that appear on both sides of the equation in the same form) to write the net ionic equation. In this case, the net ionic equation will involve the reaction of H⁺ ions with OH⁻ ions from Cr(OH)₃ to form water, and the formation of the chromium(III) nitrite precipitate.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Neutralization Reactions
Neutralization reactions occur when an acid reacts with a base to produce water and a salt. In this context, chromium(III) hydroxide acts as a base, while nitrous acid serves as the acid. The general form of a neutralization reaction can be represented as: acid + base → salt + water.
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Balancing Chemical Equations
Balancing chemical equations is essential to ensure that the number of atoms of each element is conserved in a reaction. This involves adjusting the coefficients of the reactants and products so that they match. For the given reaction, one must account for the chromium, oxygen, hydrogen, and nitrogen atoms to achieve a balanced equation.
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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. To derive the net ionic equation, one must first write the complete ionic equation and then eliminate the ions that appear unchanged on both sides. This focuses on the essential components of the reaction.
Related Practice
Textbook Question
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.
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Textbook Question
Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (d) Ba1OH22.
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Textbook Question
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (c) Aqueous nitric acid and aqueous ammonia react.
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Textbook Question
Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO(s) + 2 HClO4(aq) → Fe(ClO4)2(aq) + H2O(l) (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueous solution of nitric acid.
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