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 1.22 mol 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 6th Edition

Ch.4 - Chemical Reactions and Chemical Quantities

Problem 30

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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Step 1: Write the unbalanced chemical equation: \[ \text{HC}_2\text{H}_3\text{O}_2(\text{aq}) + \text{Ba(OH)}_2(\text{aq}) \rightarrow \text{H}_2\text{O}(\text{l}) + \text{Ba(C}_2\text{H}_3\text{O}_2)_2(\text{aq}) \]

Step 2: Balance the equation by ensuring the number of atoms of each element is the same on both sides. Start by balancing the acetate ions (C₂H₃O₂⁻) and then balance the water molecules.

Step 3: The balanced equation should look like this: \[ 2\text{HC}_2\text{H}_3\text{O}_2(\text{aq}) + \text{Ba(OH)}_2(\text{aq}) \rightarrow 2\text{H}_2\text{O}(\text{l}) + \text{Ba(C}_2\text{H}_3\text{O}_2)_2(\text{aq}) \]

Step 4: Use the stoichiometry of the balanced equation to determine the mole ratio between HC₂H₃O₂ and Ba(OH)₂. From the balanced equation, 2 moles of HC₂H₃O₂ react with 1 mole of Ba(OH)₂.

Step 5: Calculate the moles of Ba(OH)₂ needed to neutralize 1.22 moles of HC₂H₃O₂ using the mole ratio: \[ \text{Moles of Ba(OH)}_2 = \frac{1.22 \text{ moles HC}_2\text{H}_3\text{O}_2}{2} \]

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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.

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.

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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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.

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 1.22 mol of HC₂H₃O₂.