If a chemist mixed 100.00 mL of dichloromethane (CH2Cl2) which has a density of 1.33 g/mL and formula weight of 84.93 g/mole with 100.00 mL of acetic anhydride (C4H6O3) which has a density of 1.08 g/mL and a formula weight of 102.09 g/mole then determine which chemical is the solute and which one is the solvent. Next determine the mass percentage of each chemical. Next determine the mole percentage of each chemical. Next determine the Molarity (M) of the solution. Finally determine the molality (m) of the solution.
If a chemist mixed 100.00 mL of dichloromethane (CH2Cl2) which has a density of 1.33 g/mL and formula weight of 84.93 g/mole with 100.00 mL of acetic anhydride (C4H6O3) which has a density of 1.08 g/mL and a formula weight of 102.09 g/mole then determine which chemical is the solute and which one is the solvent. Next determine the mass percentage of each chemical. Next determine the mole percentage of each chemical. Next determine the Molarity (M) of the solution. Finally determine the molality (m) of the solution.
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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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If a chemist mixed 100.00 mL of dichloromethane (CH2Cl2) which has a density of 1.33 g/mL and formula weight of 84.93 g/mole with 100.00 mL of acetic anhydride (C4H6O3) which has a density of 1.08 g/mL and a formula weight of 102.09 g/mole then determine which chemical is the solute and which one is the solvent. Next determine the mass percentage of each chemical. Next determine the mole percentage of each chemical. Next determine the Molarity (M) of the solution. Finally determine the molality (m) of the solution.
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