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Ch.5 - Introduction to Solutions and Aqueous Solutions
All textbooksTro 6th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 60-
Chapter 5, Problem 60-

Write balanced molecular and net ionic equations for the reaction between nitric acid and magnesium hydroxide.

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Identify the reactants and products: Nitric acid (HNO_3) reacts with magnesium hydroxide (Mg(OH)_2) to form magnesium nitrate (Mg(NO_3)_2) and water (H_2O).
Write the balanced molecular equation: Combine the reactants and products, ensuring the number of atoms for each element is equal on both sides of the equation.
Dissociate all strong electrolytes into their ions for the complete ionic equation: Break down HNO_3, Mg(OH)_2, and Mg(NO_3)_2 into their respective ions.
Identify and cancel the spectator ions: These are ions that appear on both sides of the complete ionic equation and do not participate in the reaction.
Write the net ionic equation: Include only the ions and molecules directly involved in the chemical change.

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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 a chemical reaction with all reactants and products in their molecular forms, ensuring that the number of atoms for each element is the same on both sides of the equation. This equation provides a clear picture of the substances involved and their stoichiometric relationships, which is essential for understanding the reaction's dynamics.
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Net Ionic Equation

A net ionic equation focuses on the species that actually participate in the reaction, omitting spectator ions that do not change during the reaction. This equation highlights the essential chemical changes and is particularly useful in reactions occurring in aqueous solutions, where ions are present in a dissociated form.
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Acid-Base Neutralization Reaction

An acid-base neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, nitric acid (a strong acid) reacts with magnesium hydroxide (a strong base), resulting in the formation of magnesium nitrate and water. Understanding this concept is crucial for predicting the products and writing the corresponding equations.
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Related Practice
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

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

Write balanced molecular and net ionic equations for the reaction between hydrochloric acid and rubidium hydroxide.

Textbook Question

Complete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq) →

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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

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)