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.
NANO3 = 2 ions, Na+ and NP3-
then
P = i*M*RT
P = 2*0.028*0.08206*(25+273) = 1.36941728 atm
You are CORRECT
we must account for NaNO3 dissociation Na+ and NO3-
which is i = 2
the answer you are providing (0.685 atm) does not accounts for that
Determine the osmotic pressure at 25 °C of an aqueous solution that is 0.028 M NaNO3....
What is the osmotic pressure of 0.250 M aqueous urea (CON2H4) at 25 °C. R = 0.08206 L atm/mol K and R = 8.3145 J/K mol)
A 36.5% by mass of C6H12O6, aqueous solution is prepared in the lab. the density of the solution is 2.97 g/ml. what is the osmotic pressure of the solution at 42 OC ( R=0.08206 L*atm/mol*K)
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
Determine the osmotic pressure of a 0.0125 M solution of CrCl3 at 25°C. Assume 100% dissociation of CrCl3. 0.280 atm 0.560 atm 0.840atm 1.22atm 1.40atm
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.
What is the osmotic pressure (atm) of an aqueous solution with a volume of 0.750 L that contains 5.0 g of methanol, CH3OH, at 37∘C? Round the answer to two significant figures.
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)?
I’m just missing these two questions ? Help please P24. What is the osmotic pressure π), in atm, at 25 °C of an aqueous solution containing 2.75 grams of beryllium fluoride, BeF2, dissolved in 500 mL of water? BeF2 is an electrolyte compound. [Hint: van't Hoff Factor] & (R 0.0821 L atm/mol K) 2.61 atm b) 3.05 atm 7.15 atm 8.59 atm
8. Estimate the melting point and osmotic pressure of a 2.0-L aqueous solution that contains 0.18 mol of NaCl and 0.30 mol of MgCl2 at 25°C. (solution density=1.02 g/cm').
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?