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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 85
Chapter 4, Problem 85

Complete and balance each acid–base equation.
a. H2SO4(aq) + Ca(OH)2(aq) →
b. HClO4(aq) + KOH(aq) →
c. H2SO4(aq) + NaOH(aq) →

Verified step by step guidance
1
Identify the type of reaction: This is an acid-base neutralization reaction where sulfuric acid (H2SO4) reacts with sodium hydroxide (NaOH).
Write the unbalanced chemical equation: H2SO4(aq) + NaOH(aq) → Na2SO4(aq) + H2O(l).
Balance the equation by ensuring the number of atoms of each element is the same on both sides. Start by balancing the sodium (Na) atoms.
Since H2SO4 has two acidic hydrogens, it will react with two NaOH molecules. Adjust the coefficients: H2SO4(aq) + 2 NaOH(aq) → Na2SO4(aq) + 2 H2O(l).
Verify the balance: Check that the number of each type of atom (H, S, O, Na) is equal on both sides of the equation.

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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 context, sulfuric acid (H2SO4) acts as an acid, donating protons, while sodium hydroxide (NaOH) serves as a base, accepting protons. The result is the formation of water and a salt, showcasing the neutralization process typical of acid-base reactions.
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Balancing Chemical Equations

Balancing chemical equations is essential to ensure that the number of atoms for each element is the same on both sides of the equation. This reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. In the given equation, coefficients are adjusted to achieve balance, particularly for the products formed.
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Strong Acids and Bases

Strong acids and bases completely dissociate in aqueous solutions. H2SO4 is a strong acid that dissociates into H+ and HSO4- ions, while NaOH is a strong base that dissociates into Na+ and OH- ions. Understanding their complete dissociation is crucial for predicting the products of the reaction and for balancing the equation accurately.
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