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Calculate how much of a concentrated acetic acid solution (w 36%, p 1.0449 g %3D / ml) is required to prepare 1100 ml of a diluted solution with a molar concentration of 0.4 mol / L.

Calculate how much of a concentrated acetic acid solution (w 36%, p 1.0449 g %3D / ml) is required to prepare 1100 ml of a diluted solution with a molar concentration of 0.4 mol / L.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
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**Problem Description:** Calculate how much of a concentrated acetic acid solution (w = 36%, ρ = 1.0449 g/ml) is required to prepare 1100 ml of a diluted solution with a molar concentration of 0.4 mol/L. **Solution Explanation:** To solve this problem, it's essential to understand how to use the concepts of concentration and density to prepare a diluted solution from a concentrated one. 1. **Determine the Molar Mass of Acetic Acid (CH₃COOH):** - Carbon (C): 12.01 g/mol - Hydrogen (H): 1.01 g/mol - Oxygen (O): 16.00 g/mol - Molar mass of CH₃COOH = 2(12.01) + 4(1.01) + 2(16.00) = 60.05 g/mol 2. **Calculate the Amount of Acetic Acid Required:** - Desired molarity of diluted solution: 0.4 mol/L - Volume of diluted solution: 1100 ml = 1.1 L - Amount in moles of acetic acid needed = Molarity × Volume = 0.4 mol/L × 1.1 L = 0.44 mol 3. **Convert Moles to Grams:** - Mass of acetic acid = Moles × Molar Mass = 0.44 mol × 60.05 g/mol = 26.42 g 4. **Determine the Volume of Concentrated Acetic Acid Solution Required:** - Weight/volume percentage (w/v) = 36% - This means 36 g of acetic acid is present in 100 ml of solution. - Use density (ρ = 1.0449 g/ml) to convert volume to mass: - Required volume in ml = (Required mass / (w% × density)) × 100 - Calculation: (26.42 g / (36 / 100) × 1.0449 g/ml) = approximately 70 ml Thus, approximately 70 ml of the concentrated acetic acid solution is needed to prepare the desired diluted solution. Remember, these calculations can be affected by rounding, so exact measurements in practice might vary slightly. Always follow lab safety guidelines when handling concentrated acids.
Transcribed Image Text:**Problem Description:** Calculate how much of a concentrated acetic acid solution (w = 36%, ρ = 1.0449 g/ml) is required to prepare 1100 ml of a diluted solution with a molar concentration of 0.4 mol/L. **Solution Explanation:** To solve this problem, it's essential to understand how to use the concepts of concentration and density to prepare a diluted solution from a concentrated one. 1. **Determine the Molar Mass of Acetic Acid (CH₃COOH):** - Carbon (C): 12.01 g/mol - Hydrogen (H): 1.01 g/mol - Oxygen (O): 16.00 g/mol - Molar mass of CH₃COOH = 2(12.01) + 4(1.01) + 2(16.00) = 60.05 g/mol 2. **Calculate the Amount of Acetic Acid Required:** - Desired molarity of diluted solution: 0.4 mol/L - Volume of diluted solution: 1100 ml = 1.1 L - Amount in moles of acetic acid needed = Molarity × Volume = 0.4 mol/L × 1.1 L = 0.44 mol 3. **Convert Moles to Grams:** - Mass of acetic acid = Moles × Molar Mass = 0.44 mol × 60.05 g/mol = 26.42 g 4. **Determine the Volume of Concentrated Acetic Acid Solution Required:** - Weight/volume percentage (w/v) = 36% - This means 36 g of acetic acid is present in 100 ml of solution. - Use density (ρ = 1.0449 g/ml) to convert volume to mass: - Required volume in ml = (Required mass / (w% × density)) × 100 - Calculation: (26.42 g / (36 / 100) × 1.0449 g/ml) = approximately 70 ml Thus, approximately 70 ml of the concentrated acetic acid solution is needed to prepare the desired diluted solution. Remember, these calculations can be affected by rounding, so exact measurements in practice might vary slightly. Always follow lab safety guidelines when handling concentrated acids.
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