Write balanced ionic equations for the following reactions. (b) Aqueous barium hydroxide is neutralized by aqueous nitric acid.

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Identify the reactants and products in the reaction: Barium hydroxide (Ba(OH)_2) and nitric acid (HNO_3) react to form barium nitrate (Ba(NO_3)_2) and water (H_2O).

Write the balanced molecular equation for the reaction: Ba(OH)_2(aq) + 2HNO_3(aq) → Ba(NO_3)_2(aq) + 2H_2O(l).

Break down the soluble ionic compounds into their constituent ions to write the complete ionic equation: Ba^{2+}(aq) + 2OH^-(aq) + 2H^+(aq) + 2NO_3^-(aq) → Ba^{2+}(aq) + 2NO_3^-(aq) + 2H_2O(l).

Identify and cancel out the spectator ions that appear on both sides of the complete ionic equation: Ba^{2+}(aq) and NO_3^-(aq) are spectator ions.

Write the net ionic equation by removing the spectator ions: 2OH^-(aq) + 2H^+(aq) → 2H_2O(l).

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Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, barium hydroxide (a base) reacts with nitric acid (an acid) to form barium nitrate and water. Understanding this concept is crucial for predicting the products of the reaction and writing the balanced equation.

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05:56

Lewis Dot Structures: Neutral Compounds

Ionic Equations

Ionic equations represent the species involved in a chemical reaction in their ionic forms. In aqueous solutions, strong electrolytes dissociate into their constituent ions. Writing balanced ionic equations requires identifying the ions present in the reactants and products, which helps in visualizing the actual chemical changes occurring during the reaction.

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Net Ionic Equations

Balancing Chemical Equations

Balancing chemical equations 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. This involves adjusting coefficients in front of compounds rather than changing subscripts. Mastery of this concept is essential for accurately representing the stoichiometry of the reaction.

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