Textbook Question
Write balanced complete ionic and net ionic equations for each reaction. d. HC2H3O2(aq) + K2CO3(aq) → H2O(l ) + CO2(g) + KC2H3O2(aq)
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Ch.5 - Introduction to Solutions and Aqueous Solutions
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 5, Problem 59
Write balanced molecular and net ionic equations for the reaction between hydrochloric acid and rubidium hydroxide.
Verified step by step guidance1
Identify the reactants and products: Hydrochloric acid (HCl) and rubidium hydroxide (RbOH) react to form water (H2O) and rubidium chloride (RbCl).
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: HCl and RbOH are strong electrolytes, so they dissociate completely in water.
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: The net ionic equation should only include 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.
Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, hydrochloric acid (HCl) acts as an acid, donating a proton, while rubidium hydroxide (RbOH) acts as a base, accepting the proton. The result is the formation of water and a salt, which is a typical outcome of neutralization reactions.
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Acid-Base Reaction
Balanced Chemical Equations
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This ensures the law of conservation of mass is upheld. For the reaction between HCl and RbOH, the balanced molecular equation must reflect the stoichiometry of the reactants and products accurately.
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01:32Balancing Chemical Equations
Net Ionic Equations
Net ionic equations simplify chemical reactions by removing spectator ions—ions that do not participate in the reaction—from the full ionic equation. This focuses on the actual chemical species that undergo change. In the case of HCl and RbOH, the net ionic equation highlights the formation of water from H+ and OH- ions.
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
A 15.00-mL sample of an unknown HClO4 solution requires titration with 17.03 mL of 0.1000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO4(aq) + NaOH(aq) → H2O(l ) + NaClO4(aq)
Textbook Question
Write balanced complete ionic and net ionic equations for each acid–base reaction.
b. HCHO2(aq) + NaOH(aq) →
c. HC2H3O2(aq) + LiOH(aq) →
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Textbook Question
Complete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq) →
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