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Ch.4 - Chemical Reactions and Chemical Quantities
All textbooksTro 6th EditionCh.4 - Chemical Reactions and Chemical QuantitiesProblem 30
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Chapter 4, Problem 30

Consider the unbalanced equation for the neutralization of acetic acid: HC2H3O2(aq) + Ba(OH)2(aq) → H2O(l) + Ba(C2H3O2)2(aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 1.22 mol of HC2H3O2.

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Key Concepts

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

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, acetic acid (HC2H3O2) reacts with barium hydroxide (Ba(OH)2) to form water (H2O) and barium acetate (Ba(C2H3O2)2). Understanding this concept is crucial for balancing the chemical equation and determining the stoichiometric relationships between the reactants and products.
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Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is achieved by adjusting the coefficients of the reactants and products. For the given reaction, balancing is essential to accurately reflect the conservation of mass and to determine the correct mole ratios needed for calculations.
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Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows us to calculate the amount of one substance needed to react with a given amount of another. In this question, stoichiometry will help determine how many moles of Ba(OH)2 are required to neutralize 1.22 moles of acetic acid based on the balanced equation.
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