What is the minimum mass of glycerol
(C3H8O3) that must be dissolved in
895 mg of water to prevent the solution from freezing at −15.0°C?
(Assume ideal behavior.) |
What is the minimum mass of glycerol (C3H8O3) that must be dissolved in 895 mg of...
What is the minimum mass of ethylene glycol (C2H6O2) that must be dissolved in 14.5 kg of water to prevent the solution from freezing at −18.6°F? (Assume ideal behavior.) g?
What is the minimum mass of ethylene glycol (C2H6O2) that must be dissolved in 14.5 kg of water to prevent the solution from freezing at −16.6°F?
A 2.350×10−2 M solution of glycerol (C3H8O3) in water is at 20.0∘C. The sample was created by dissolving a sample of C3H8O3 in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.0 mL . The density of water at 20.0∘C is 0.9982 g/mL. Include units. Part A: Calculate the molality of the glycerol solution. Part B: Calculate the mole fraction of glycerol in this solution....
Pt 1 - Glycerol (C3H8O3), also called glycerine, is widely used in the food and pharmaceutical industries. Glycerol is polar and dissolves readily in water and polar organic solvents like ethanol. Calculate the mole fraction of the solvent in a solution that contains 2.21 g glycerol dissolved in 22.00 mL ethanol (CH3CH2OH; density = 0.7893 g/mL). Round to four significant digits. Pt 2 - Use your answer to Part 2 to calculate the vapor pressure of the solution at 20°C...
Calculate the vapor pressure of a solution containing 36.5 g of glycerol (C3H8O3) and 125 mL of water at 30.0 °C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerol is not volatile and dissolves molecularly (i.e., it is not ionic) and use a density of 1.00 g/mL for the water.
21. What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 °C? The freezing point depression constant, Kfp, of water is -1.86 °C/m. Assume the van't Hoff factor for Na2SO4 is 2.95.
6. A 1.07 mg sample of a compound was dissolved in 78.1 mg of camphor. The resulting solution melted at 176.0 C. What is the molecular mass of the compound? The melting point of pure camphor is 179.5 C. The freezing-point-depression constant for camphor Kf is 40.0 C/m. 7. A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at...
2. What is the freezing point of an aqueous solution containing 69.5g NaNO3 (MM=85.00g/mol) dissolved in 175g water? Kf=1.86°C/m for water and assume "ideal" behavior. 10. An RV antifreeze is an aqueous solution containing 5.68 M proplyene glycol (MM=76.09 g/mol). If the density of the antifreeze is 1.080 g/mL, what is the molality of the solution?
What mass of naphthalene must be dissolved in 1.60 x 102 g of benzene to give a solution with a freezing point 1.70°C below that of pure benzene?
What mass of NaClO must be dissolved in 450 g of deionized water to make a 100 ppm solution? Assume the density of the resulting solution is 1.00 g·mL-1.