The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute...
The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant R. Suppose the osmotic pressure of a certain solution is measured to be 6.0 atm at an absolute temperature of 359. K. Write an equation that will let you calculate the molarity c of this solution. Your equation should contain only symbols. Be sure you define each symbol other than R.
What is the molarity of the protein solution if the osmotic pressure is 5.80 torr and the temperature is 23.1℃? Assume that the van't Hoff factor is 1.00
Determine the molarity of each of the following solutions from its osmotic pressure at 25°C. Include the van't Hoff factor for the solution when the factor is given. Part 1 II = 0.0211 atm for a solution of urea (CH4N2O): Part 2 II = 0.664 atm for a solution of KI, i=1.90:What molality of a nonvolatile, nonelectrolyte solute is needed to raise the boiling point of water by 7.35°C (K- 0.520°C/m)?
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.
Determine the molarity of each of the following solutions from its osmotic pressure at 25°C. Include the van't Hoff factor for the solution when the factor is given. 0.0237 atm for a solution of urea (CH4N2O): 0.675 atm for a solution of KI, i = 1.90:
Determine the molarity of each of the following solutions from its osmotic pressure at 25 degree C. Include the van't Hoff factor for the solution when the factor is given. pi = 0.0270 atm for a solution of urea (CH_4 N_2 O) pi = 0.623 atm for a solution of KI, i = 1.90
Determine the molarity of each of the following solutions from its osmotic pressure at 25°C. Include the van't Hoff factor for the solution when the factor is given. Π = 0.520 atm for a solution of ethanol (C2H5OH): Π = 0.0265 atm for a solution of aspirin (C9H8O4): Π = 0.693 atm for a solution of CaCl2, i = 2.47:
Determine the osmotic pressure at 25 °C of an aqueous solution that is 0.028 M NaNO3. p = i M R T (R = 0.08206 atm L/mol K) For some reason the answer is 1.37 atm, but I am getting .685 atm.
Question 20 0/5 pts The osmotic pressure of blood is 7.65 atm at 37°C. If blood were considered a solution of NaCl, what is the molar concentration of NaCl in blood? Assume an ideal van't Hoff factor Where: n = iMRT R is the ideal gas law constant (0.08205 bar mol K and T is the absolute temperature 23.2
18. What osmotic pressure in atmospheres would you expect for each of the following solutions? a) 5.00 g of NaCl in 350.0 mL of aqueous solution at 50 °C b) 6.33 g of sodium acetate, CH3CO2Na, in 55.0 mL of aqueous solution at 10 °C. 19. Human blood gives rise to an osmotic pressure of approximately 7.7 atm at body temperature, 37.0 °C. What must the molarity of an intravenous glucose solution be to give rise to the same osmotic...