Consider the unbalanced equation for the neutralization of acetic acid: HC 2 H 3 O 2 (aq) + Ba(OH) 2 (aq) → H 2 O(l) + Ba(C 2 H 3 O 2 ) 2 (aq) Balance the equation and determine how many moles of Ba(OH) 2 are required to completely neutralize 0.461 mole of HC 2 H 3 O 2 .

Hey everyone. Our question here is asking us to determine the mass in g of calcium hydroxide required to completely neutralize 3.41 g of acetic acid. Now looking at our equation, we can see that it's unbalanced. Since we have two acetate ions connected to our calcium and only one acetate ion in our react inside. In order to bounce this out, we're going to have to add a coefficient of two prior to our acetic acid. And since we added this coefficient of two, we're going to need to recheck our hydrogen as well In order to balance out our hydrogen is we're going to need to add a coefficient of two before our H20, which is our water. So rechecking if everything is balanced, we have our complete balanced chemical equation. So let's go ahead and move on with our problem. So starting off with 3.41 g of acetic acid. We're going to need to get the molar mass of acetic acid. And when we look that up, we end up with a molar mass of 60.052 g per mole of acetic acid. So, plugging that into our dimensional analysis, We have 52 g per one mole of acetic acid. Now we want to relate this to moles of calcium hydroxide. So looking at our balanced chemical equation, we see that per two moles of acetic acid, we have one mall of calcium hydroxide. Now in order to figure out the grams, we're going to need to calculate the molar mass of calcium hydroxide. And when we do that, we find that our molar mass is going to be 74.09 g per mole of calcium hydroxide. And plugging this into our dimensional analysis, We know that we have 74.09 g of calcium hydroxide per one mole. So calculating this out, We end up with a value of 2.10 g of calcium hydroxide, and this is going to be our final answer. So I hope this made sense and let us know if you have any questions.

Ch.4 - Chemical Reactions and Chemical Quantities

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Tro 5th Edition

Ch.4 - Chemical Reactions and Chemical Quantities

Problem 26

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Chapter 4, Problem 26

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 0.461 mole of HC₂H₃O₂.

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Identify the reactants and products in the chemical equation: HC_2H_3O_2 (acetic acid) and Ba(OH)_2 (barium hydroxide) react to form H_2O (water) and Ba(C_2H_3O_2)_2 (barium acetate).

Write the unbalanced chemical equation: HC_2H_3O_2(aq) + Ba(OH)_2(aq) → H_2O(l) + Ba(C_2H_3O_2)_2(aq).

Balance the equation by ensuring the number of atoms of each element is the same on both sides. Start by balancing the acetate ions (C_2H_3O_2^-).

Determine the stoichiometric coefficients that balance the equation. You will find that 2 moles of HC_2H_3O_2 react with 1 mole of Ba(OH)_2 to produce 2 moles of H_2O and 1 mole of Ba(C_2H_3O_2)_2.

Use the balanced equation to calculate the moles of Ba(OH)_2 needed: Since 2 moles of HC_2H_3O_2 react with 1 mole of Ba(OH)_2, divide the moles of HC_2H_3O_2 (0.461 moles) by 2 to find the moles of Ba(OH)_2 required.

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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 the nature of neutralization is essential for balancing the chemical equation and determining the stoichiometric relationships between reactants and products.

Balancing Chemical Equations

Balancing a chemical equation involves ensuring that the number of atoms of 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 crucial to accurately reflect the stoichiometry of the neutralization process, which will help in calculating the moles of Ba(OH)2 needed.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows us to calculate the amount of reactants required or products formed based on the balanced equation. In this scenario, knowing the stoichiometric coefficients from the balanced equation will enable us to determine how many moles of Ba(OH)2 are necessary to neutralize 0.461 moles of acetic acid.

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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 0.461 mole of HC2H3O2.

Verified Solution

Key Concepts

Neutralization Reaction

Balancing Chemical Equations

Stoichiometry

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 0.461 mole of HC₂H₃O₂.