31:25Molarity, Molality, Volume & Mass Percent, Mole Fraction & Density - Solution Concentration ProblemsThe Organic Chemistry Tutor873views1rank
Multiple ChoiceCalculate mole fraction of a 2.4 m aqueous solution of citric acid (C6H8O7).912views1comments
Multiple ChoiceIf mole fraction of urea is 4.55 x 10-1, what is the mass of urea needed to dissolve in 38.0 g of water? The molar mass of urea is 60.062 g/mol.668views2rank2comments
Multiple ChoiceCalculate the mole fraction of sucrose (molar mass = 342.3 g/mol) in an aqueous solution that is 1.80 M sucrose? The density of solution is 1.08 g/mL.494views
Textbook QuestionThe density of acetonitrile 1CH3CN2 is 0.786 g>mL and the density of methanol 1CH3OH2 is 0.791 g>mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (a) What is the mole fraction of methanol in the solution?999views
Textbook QuestionThe density of toluene 1C7H82 is 0.867 g>mL, and the density of thiophene 1C4H4S2 is 1.065 g>mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (a) Calculate the mole fraction of thiophene in the solution.588views
Textbook QuestionCaffeine 1C8H10N4O22 is a stimulant found in coffee and tea. If a solution of caffeine in the solvent chloroform 1CHCl32 has a concentration of 0.0500 m, calculate (b) the mole fraction of caffeine in the solution. 825views
Textbook QuestionHow would you prepare each of the following solutions? (c) A solution of methyl alcohol (methanol) and water in which Xmethanol = 0.15 and Xwater = 0.85389views
Textbook QuestionA solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g>mL and 1.00 g>mL, respectively. For this solution, calculate the concentration in each unit. e. mole percent331views
Textbook QuestionA solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g>mL and 1.00 g>mL, respectively. For this solution, calculate the concentration in each unit. d. mole fraction2022views
Textbook QuestionAn aqueous solution contains 36% HCl by mass. Calculate the molality and mole fraction of the solution.1594views
Textbook QuestionWhat is the concentration of each of the following solutions? (b) The mole fraction of each component of a solution pre- pared by dissolving 2.25 g of nicotine, C10H14N2, in 80.0 g of CH2Cl2610views
Textbook QuestionHousehold bleach is a 5.0 mass % aqueous solution of sodium hypochlorite, NaOCl. What is the molality of the bleach? What is the mole fraction of NaOCl in the bleach?828views
Textbook QuestionA 0.944 M solution of glucose, C6H12O6, in water has a density of 1.0624 g/mL at 20 °C. What is the concentration of this solution in the following units?(a) Mole fraction1157views
Textbook QuestionThe estimated average concentration of NO2 in air in the United States in 2006 was 0.016 ppm. (a) Calculate the partial pressure of the NO2 in a sample of this air when the atmospheric pressure is 755 torr (99.1 kPa).500views
Textbook QuestionLactose, C12H22O11, is a naturally occurring sugar found in mammalian milk. A 0.335 M solution of lactose in water has a density of 1.0432 g/L at 20 °C. What is the concentra- tion of this solution in the following units? (b) Mass percent1047views
Textbook QuestionAcetonitrile 1CH3CN2 is a polar organic solvent that dissolves a wide range of solutes, including many salts. The density of a 1.80 M LiBr solution in acetonitrile is 0.826 g>cm3. Calculate the concentration of the solution (b) mole fraction of LiBr,814views
Textbook QuestionFind the mass of urea (CH4N2O) needed to prepare 50.0 g of a solution in water in which the mole fraction of urea is 0.0770.2324views1comments
Open QuestionA solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.265views
Open QuestionA solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 ml.250views