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

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Identify the reactants and their chemical formulas: nitric acid is HNO₃ and magnesium hydroxide is Mg(OH)₂.

Write the unbalanced molecular equation by combining the reactants: HNO₃ + Mg(OH)₂ → products (which will be a salt and water).

Determine the products: nitric acid (an acid) reacts with magnesium hydroxide (a base) to form magnesium nitrate (Mg(NO₃)₂) and water (H₂O).

Balance the molecular equation by ensuring the number of atoms of each element is equal on both sides. Pay attention to the nitrate ion (NO₃^-) and hydroxide ion (OH^-) stoichiometry.

Write the net ionic equation by dissociating all strong electrolytes into ions, then canceling out the spectator ions to show only the species that participate directly in the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations ensures the law of conservation of mass is obeyed by having equal numbers of each type of atom on both sides of the reaction. This involves adjusting coefficients to balance atoms without changing the chemical formulas of reactants or products.

Molecular vs. Net Ionic Equations

Molecular equations show all reactants and products as intact compounds, while net ionic equations display only the species that undergo chemical change, omitting spectator ions. This highlights the actual chemical process occurring in solution.

Acid-Base Neutralization Reactions

An acid-base neutralization involves an acid reacting with a base to produce water and a salt. In this case, nitric acid (HNO3) reacts with magnesium hydroxide (Mg(OH)2) to form magnesium nitrate and water, demonstrating proton transfer and ionic compound formation.

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