3.) An aqueous solution of Alz(S04), has a freezing point temperature of -7.8585 °C and an...

Question

Question

3.) An aqueous solution of Alz(S04), has a freezing point temperature of -7.8585 °C and an osmotic pressure of 46.71 atm. Cal

engineering Chemical-Engineering

Answer 1

Answer #1

Hope this will be helpful

Page 1

Osmotic Pressure (71) = ; C RT C= concentration in mol/L R= universal gas constant 0.0821 (L.afm) KK.mol) T = Temperature = 2

Please Give your feedback

Answer 2

Similar Homework Help Questions

An aqueous solution is 23% glucose by mass (d = 1.090 g/mL at 20.°C). Calculate its...

An aqueous solution is 23% glucose by mass (d = 1.090 g/mL at 20.°C). Calculate its freezing point, boiling point at 1 atm, and osmotic pressure.
ch.13 answer each of these please What is the boiling point of an aqueous solution that...

ch.13 answer each of these please What is the boiling point of an aqueous solution that has a vapor pressure of 22.5 torr at 25°C? (Puo 23.78 torn; Kb = 0,512 °C/m). Express your answer using four significant figures. VO AXO ? c A solution contains 10.55 g of unknown compound (non-electrolyte) dissolved in 50,0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -4,35 °C. The mass percent composition of...
1. 1200 mL aqueous solution of 45 g of ethylene glycol and 80 g of sucrose...

1. 1200 mL aqueous solution of 45 g of ethylene glycol and 80 g of sucrose were prepared with a density of 1.37 g/mL. Assume that the solution behaves ideally. Notes: The vapor pressures of water and ethylene glycol at 20 °C are 17.54 torr and 0.06 torr, respectively, and Kb and Kf of water are 0.51 K/m and 1.86 K/m, at 25 °C respectively. a. What is the freezing point of this solution? b. What is the vapor pressure,...

4. An aqueous solution is 20.% glucose by mass (d = 1.078 g/mL at 20 °C)....

4. An aqueous solution is 20.% glucose by mass (d = 1.078 g/mL at 20 °C). Calculate the following: (Some useful constants for water: Kr = 1.86 °C/m and Ko = 0.512 °C/m) [-2.6°C] a) freezing point [100.71 °C] b) boiling point at 1 atm c) osmotic pressure (29 atm]
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor...

An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...
2. What is the freezing point of an aqueous solution containing 69.5g NaNO3 (MM=85.00g/mol) dissolved in...

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?

1.) A 0.046 M aqueous solution of FeCl, has an osmotic pressure of 4.09 atm at...

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?
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypotheti...

An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...
2.) An aqueous solution of KI has a boiling point temperature of 100.512°C. Calculate the molarity...

2.) An aqueous solution of KI has a boiling point temperature of 100.512°C. Calculate the molarity concentration of the solution if it has a density of 1.30 g/ml.

A solution is prepared by dissolving 25.0g of CaCl2 in 275 mL of water. Water has...

A solution is prepared by dissolving 25.0g of CaCl2 in 275 mL of water. Water has a density of 1.0g/mL.The solution has a final volume of 279 mL. (A) What is the total solute molality? (B) What is the freezing point of the solution? Assume ideal behavior. (C) What is the osmotic pressure of the solution at 25 C?