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29 You have a solution which is 43.4% by mass isopropyl alcohol (MM = 60.11 g/mol)...
29 You have a solution which is 43.4% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The density of this solution is 0.905 g/mL. b What is the molarity of the isopropyl alcohol in the solution? > 1 point с What is the mole fraction of the isopropyl alcohol in the solution? 1 point d What intermolecular forces are shared between isopropyl alcohol and water? 1 point
You have a solution which is 43.4% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The density of this solution is 0.905 g/mL. What is the molality of the isopropyl alcohol in the solution?
You have a solution which is 43.9% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The density of this solution is 0.905 g/mL. What is the molality of the isopropyl alcohol in the solution? What is the molarity of the isopropyl alcohol in the solution? What is the mole fraction of the isopropyl alcohol in the solution? What intermolecular forces are shared between isopropyl alcohol and water?
A solution of NaCl (MW = 58.5 g/mol) in water (MW = 18.0 g/mol) has the molality of 3.01 molal and the density of 1.112 g/mL. Consider mass of solvent 1 Kg A) What is the mass percent of the solute? (B) What is the molarity of the solution? (C)What is the mole fraction of H2O?
We have an aqueous solution with a mass percent of 44.2 % for C2H5OH (C2H5OH is the only solute). The density of this solution is 0.947 g/mL. Calculate the molarity, molality, and mole fraction of C2H5OH in this aqueous solution. We have an aqueous solution with a mass percent of 44.2% for C2H5OH (C2H5OH is the only solute). The density of this solution is 0.947 g/ml. Calculate the molarity, molality, and mole fraction of C2H5OH in this aqueous solution.
We have an aqueous solution with a mass percentage of 43.9% for C2H5OH (C2H5OH is the only solute). The density of this solution is 0.956 g / mL. Calculate the molarity, molality, and mole fraction of C2H5OH in this aqueous solution Thank you
a.) Salt solution is 12.0% NaCl by mass, with a density of 1.023 g/mL. What are the molarity, molality, and mole fraction of this solution? b.) How many grams of salt would you need to add to 500 mL of this solution to raise its mole % to 5.00?
help on questions 26-30 26. Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality. 27. Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. The density of water is 0.997 g/mL. A) 1.51 % B) 7.57 % C) 13.3 % D) 15.2 % E) None of these 28. What is the molarity of a solution that is 5.50% by...
You have a 1.8M sodium phosphate solution , whose density is 1.13 g/ml. Calculate its: a) mol fraction. b) mass %. c) Molality. d) Normal freezing point. e) Normal boiling point.
Calculate the mole fraction of phosphoric acid (H3PO4) in a 25.4% (by mass) aqueous solution. (Assume 750 mL of solution.) What is the molarity of the solution? What is the molality? (At 20 ° C, the density of phosphoric acid is 1.1462 g/mL and the density of water is 0.99823 g/mL.)