π = CRT
where, π = osmotic pressure
R = 0.0821, constant to give pressure in atm
T = Temperature in K
C = concentration of the solution
so,
π = 0.204*0.0821*310
π = 5.19
atm
Calculate the osmotic pressure of a 0.204 M aqueous solution of sucrose, C12H22O11, at 37
The nonvolatile, nonelectrolyte sucrose, C12H22O11 (342.30 g/mol), is soluble in water H2O. Calculate the osmotic pressure generated when 11.6 grams of sucrose are dissolved in 156 ml of a water solution at 298 K. The molarity of the solution is _____ M. The osmotic pressure of the solution is ______ atmospheres.
an Iso osmotic sucrose (C12H22O11)solution has a concentration of 0.30 M calculate its concentration in percent mass to volume.
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28) 28) What is the osmotic pressure of a 0.25 M solution of sucrose at 37°C? (R = 0.0821 L-atm/K mol) A) 100 atm B) 6.4 atm 6.6 x 10-5 atm D) 940 atm E) 0.76 atm
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Calculate the molarity of 147 grams of sucrose, C12H22O11, in 4.50 liters of solution. M sucrose
An aqueous sucrose (C12H22O11) solution of unknown concentration is found to have a freezing point of –0.912°C. What is the normal boiling point and the partial pressure (in torr) of water at 25°C of this solution? Kb (H2O) = 0.51°C/m; P°(H2O) = 23.800 torr at 25°C.
An aqueous solution was made up by dissolving 34.5 g of sucrose, C12H22O11, in enough water to make 250 cm^3 of solution. The mass density of the resulting solution was 1040 kg/m^3. Calculate the molar concentration and molarity of sucrose in the solution. Answer: 0,388 mol/kg
The nonvolatile, nonelectrolyte sucrose, C12H22011 (342.30 g/mol), is soluble in water H20. Calculate the osmotic pressure generated when 12.4 grams of sucrose are dissolved in 201 ml of a water solution at 298 K. The molarity of the solution is M. The osmotic pressure of the solution is atmospheres.
What will the solution vapor pressure be for a solution of 53.09 mol of sucrose (C12H22O11) dissolved in 1.000L of water at 20.0 °C? The vapor pressure of pure water at 20.0 °C is 17.5 torr