A solid mixture contains MgCl2 (molar mass = 95.218 g/mol) and NaCl (molar mass = 58.443 g/mol). When 0.5000 g of this solid is dissolved in enough water to form 1.000 L of solution, the osmotic pressure at 25.0 oC is observed to be 0.3950 atm. What is the mass percent of MgCl2 in the solid? (Assume ideal behavior for the solution.)

What is the osmotic pressure, in atm, of a 0.199 M solution of MgCl₂ at 37.0 °C? (assume complete dissociation).

[Item #3] *refer to the photo below*

At 25.0°C, 100.0 mL of aqueous sol containing 45.2 mg of a molecular solute has an osmotic pressure of 18.4 Torr. The molar mass of the solute is ___ g/mol

An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2g of the compound in sufficient water to form 250ml of solution. The solution has an osmotic pressure of 1.2 atm at 25 degree celcius. What is the molar mass (g/mole) of the compound?

When 10.1 g of an organic compound known to be 54.53% C, 9.2% H, and 36.32% O by mass is dissolved in 677.6 g of cyclohexane, the freezing point is 3.07 °C. The normal freezing point of cyclohexane is 6.59 °C. What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. Kf values for various solvents are given in the colligative constants table. molecular formula: CHO

A chemist wants to determine the molar mass of a naturally occurring substance isolated from spearmint. She adds 5.131 g of this substance to 25.00 g of acetone (C3H6O; molar mass 58.08 g/mol). The vapor pressure of the solution is determined to be 0.2444 atm at 25°C. If the vapor pressure of pure acetone at this temperature is 0.2630 atm, what is the mole fraction of the solvent in this solution? Give your answer to four significant digits.

Suppose you dissolve 0.210 g of a newly isolated protein in 25.o ml of water. The solution has an osmotic pressure of 0.00353 atm at 275 K. What is the molar mass of this protein?

At 25.0 °C, 100.0 mL of an aqueous solution containing 45.2 mg of a molecular solute has an osmotic pressure of 18.4 Torr. The molar mass of the solute is ___ g/mol.

A solution is made from 540.0 g sucrose (C₁₂H₂₂O₁₁, MM = 342.3 g/mol) dissolved in water to a total volume of 551 mL of solution at a temperature of 52.0 °C. Calculate the osmotic pressure of solution. R = 0.08206 L･atm/K･mol