Ch.9 - Thermochemistry: Chemical Energy

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.9 - Thermochemistry: Chemical Energy

Problem 153d

Chapter 9, Problem 153d

(d) What is the molarity of the KOH solution prepared in part (c), and how many milliliters of 0.554 M H2SO4 are required to neutralize it?

Verified step by step guidance

insert step 1: Determine the moles of KOH in the solution prepared in part (c). Use the formula: moles = mass (g) / molar mass (g/mol).

insert step 2: Calculate the molarity of the KOH solution. Molarity (M) is defined as moles of solute per liter of solution. Use the formula: M = moles of KOH / volume of solution in liters.

insert step 3: Write the balanced chemical equation for the neutralization reaction between KOH and H2SO4: 2 KOH + H2SO4 -> K2SO4 + 2 H2O.

insert step 4: Use stoichiometry to determine the moles of H2SO4 required to neutralize the moles of KOH. From the balanced equation, 1 mole of H2SO4 reacts with 2 moles of KOH.

insert step 5: Calculate the volume of 0.554 M H2SO4 needed to provide the required moles of H2SO4. Use the formula: volume (L) = moles of H2SO4 / molarity of H2SO4, and convert the volume from liters to milliliters.

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Key Concepts

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

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (M). Understanding molarity is essential for calculating how much of a substance is present in a solution, which is crucial for stoichiometric calculations in chemical reactions.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, sulfuric acid (H2SO4) will react with potassium hydroxide (KOH). The stoichiometry of the reaction, which involves the balanced equation, is important for determining the volumes and concentrations needed for complete neutralization.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to predict how much of each substance is needed or produced in a reaction. In this case, stoichiometry will help determine the volume of H2SO4 required to neutralize the KOH solution by using the molarity and the mole ratio from the balanced equation.

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Textbook Question

Acid spills are often neutralized with sodium carbonate or sodium hydrogen carbonate. For neutralization of acetic acid, the unbalanced equations are

(1) CH₃CO₂H(l) + Na₂CO₃(s) → CH₃CO₂Na(aq) + CO₂(g) + H₂O(l)

(2) CH₃CO₂H(l) + NaHCO₃(s) → CH₃CO₂Na(aq) + CO₂(g) + H₂O(l)

(b) How many kilograms of each substance is needed to neutralize a 1.000-gallon spill of pure acetic acid (density = 1.049 g/mL)?

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Textbook Question

Reaction of gaseous fluorine with compound X yields a single product Y, whose mass percent composition is 61.7% F and 38.3% Cl. (a) What is a probable molecular formula for product Y, and what is a probable formula for X?

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Textbook Question

(b) Use the data in Appendix B to calculate ΔH° for the reaction of potassium metal with water.

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Textbook Question

(c) Assume that a chunk of potassium weighing 7.55 g is dropped into 400.0 g of water at 25.0 °C. What is the final temperature of the water if all the heat released is used to warm the water?

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