Textbook Question
Complete and balance each acid–base equation.
a. H2SO4(aq) + Ca(OH)2(aq) →
b. HClO4(aq) + KOH(aq) →
c. H2SO4(aq) + NaOH(aq) →
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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Chapter 4, Problem 84
Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.
Verified step by step guidance1
Identify the reactants and products: Nitric acid (HNO₃) reacts with calcium hydroxide (Ca(OH)₂) to form calcium nitrate (Ca(NO₃)₂) and water (H₂O).
Write the balanced molecular equation: Combine the reactants to form the products, ensuring that the number of atoms of each element is the same on both sides of the equation.
Dissociate all strong electrolytes into their ions for the complete ionic equation: Break down HNO₃, Ca(OH)₂, and Ca(NO₃)₂ into their respective ions.
Cancel out the spectator ions to write the net ionic equation: Identify ions that appear on both sides of the complete ionic equation and remove them.
Write the final net ionic equation: Include only the ions and molecules directly involved in the chemical reaction.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balanced Molecular Equation
A balanced molecular equation represents the reactants and products of a chemical reaction with their correct stoichiometric coefficients. It ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. For the reaction between nitric acid and calcium hydroxide, the balanced molecular equation illustrates the complete ionic compounds involved before any dissociation occurs.
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Balancing Chemical Equations
Net Ionic Equation
A net ionic equation focuses on the species that actually participate in the chemical reaction, omitting spectator ions that do not change during the reaction. This equation highlights the essential chemical change occurring, providing a clearer understanding of the reaction dynamics. In the case of nitric acid reacting with calcium hydroxide, the net ionic equation will show the formation of water and calcium nitrate, emphasizing the acid-base neutralization process.
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Acid-Base Reaction
An acid-base reaction involves the transfer of protons (H⁺ ions) from the acid to the base, resulting in the formation of water and a salt. In this specific reaction, nitric acid (HNO₃) acts as the acid, while calcium hydroxide (Ca(OH)₂) serves as the base. Understanding this concept is crucial for predicting the products of the reaction and for writing both the balanced molecular and net ionic equations accurately.
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Related Practice
Textbook Question
Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
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Textbook Question
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl- Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations for the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
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Textbook Question
Write balanced complete ionic and net ionic equations for each acid–base reaction. a. HBr(aq) + NaOH(aq) → b. HF(aq) + NaOH(aq) → c. HC2H3O2(aq) + RbOH(aq) →
Textbook Question
Complete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq) →
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Textbook Question
Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.
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