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A certain ideal dilute solution has an osmotic pressure of 0.50 atm at 300. K. Calculate...
At 298 K, the osmotic pressure of a glucose solution (C6H12O6 (aq)) is 21.7 atm. Calculate the freezing point of the solution. The density of the solution is 1.060 g/mL. FP=____________________C
At 298 K, the osmotic pressure of a glucose solution (C6H12O6 (aq)) is 18.9 atm. Calculate the freezing point of the solution. The density of the solution is 1.052 g/mL FP = oC
Calculate the osmotic pressure of the following case at 298 K; (a) the left compartment contains 200 g of hemoglobin in 1L of solution, the right compartment contains pure water (b) the left contains the same hemoglobin solution as in part A, the left compartment initially contains 6g of NaCl in 1L of solution. Assume that the pH of the solution is such that the hemoglobin molecules are in the Na+ Hb- form. The molar mass of Hemoglobin is 65,000...
1.) A 0.046 M aqueous solution of FeCl, has an osmotic pressure of 4.09 atm at 28°C. a. Calculate the percentage difference of the van't Hoff factor from the ideal value. b. What should be the concentration of this aqueous solution if this is in ideal condition?
A dilute aqueous CaCl2 solution at 25 degrees celsius has an osmotic pressure pi = 10bar. What is the vapor pressure(in bar units) above the solution? The density of water at 25 degrees Celsius is water (25 degrees Celsius) = 0.997gmL.
1.a)The average osmotic pressure of sea water is 30 atm (atmospheres). Calculate the concentration of urea (CH4ON2) at 25 ° C that exerts the same pressure as seawater. R = 0.082 atm L/ mol K 1.b) There is a 1M solution of CH3COOH (acetic acid) in a total volume of 450 mL. What is the molality (m) of the solution? (ρ solution = 1.15 g / mL).
The osmotic pressure of an aqueous solution at 300 K is 120 kPa. Calculate the freezing point of the solution.
1) calculate the osmotic pressure,in atm, of a solution containing 3.00mg of sugar (342g/mol) in 15.0 mL of water at 25C. 2) if a substance has a vapor pressure of 120.0 torr at 20C and vapor pressure of 143.7 torr at 30C , calculate it's enthalpy of vaporization in appropriate units.
The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein’s molar mass. The solution contained 3.50-g of protein dissolved in sufficient water to form 5.00-L of solution. The osmotic pressure of the solution at 25oC was found to be 1.54-mmHg. (Hint: Remember to convert mmHg to atm) Calculate the molar mass of the protein.
calculate the vapour pressure
of this solution at 29.8 degree celsius/ you may assume that the
solution is so dilute that its density is 1.00 gm cm^-3 Pa
M Correct! A protein has a molar mass of 169000 g mol-1. An aqueous solution of this protein has an osmotic pressure of 0.294 kPa at 29.8 °C. Calculate the concentration of the protein (in g L1) in this solution. 19.72 g L. the tolerance is +/-2% SHOW ANSWER SHOW HINT LINK...