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Ch.22 - Chemistry of the Nonmetals
All textbooksBrown 15th EditionCh.22 - Chemistry of the NonmetalsProblem 66
Chapter 22, Problem 66

Complete the exercises below. Complete and balance the following equations: b. NaHCO₃ (g) + H⁺ (aq) →

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1
Identify the reactants and products in the chemical equation. Here, the reactants are sodium bicarbonate (NaHCO₃) and a hydrogen ion (H⁺).
Determine the products of the reaction. When NaHCO₃ reacts with H⁺, it typically forms carbon dioxide (CO₂), water (H₂O), and sodium ion (Na⁺).
Write the unbalanced chemical equation: NaHCO₃ (g) + H⁺ (aq) → Na⁺ (aq) + CO₂ (g) + H₂O (l).
Balance the chemical equation by ensuring that the number of atoms of each element is the same on both sides of the equation. Start by balancing the elements that appear in only one reactant and one product.
Check the charges on both sides of the equation to ensure they are balanced. Adjust coefficients as necessary to achieve charge balance, ensuring the equation is both mass and charge balanced.

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⁺ ions) between reactants. In this case, NaHCO₃, or sodium bicarbonate, acts as a base that can accept a proton from an acid, represented by H⁺. Understanding this concept is crucial for predicting the products of the reaction and balancing the equation.
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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 to achieve balance. For the given reaction, identifying the products and ensuring the equation is balanced is essential.
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Products of Sodium Bicarbonate Reaction

When sodium bicarbonate reacts with an acid, it typically produces carbon dioxide (CO₂), water (H₂O), and a salt. In this case, the reaction with H⁺ will yield carbonic acid (H₂CO₃), which can decompose into CO₂ and H₂O. Recognizing these products is vital for completing and balancing the equation correctly.
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Related Practice