5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0...
5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0 mL of solution. The osmotic pressure at 25C is 278.0 torr. What is the molar mass of the solid? 6a. Calculate the van't Hoff factor of a 0.085M potassium sulfate solution that has an osmotic pressure of 5.4atm at 25C 5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0 ml. of solution. The osmotic pressure at 25...
A 4.75-g sample of an unknown compound is dissolved in enough water to make 100.0 mL of solution. This solution has an osmotic pressure of 25.0 torr at 25oC. Find the molar mass of the unknown.
1 A solution is prepared by dissolved 65.0 grams of a molecular unknown in 200.0 grams of water. The observed freezing point is at -4.2 °C. a) Calculate the value of the unknown molar mass. b Calculate the value of osmotic pressure for this solution at 25.0 °C.
. 8.00 g of a nonvolatile solute was dissolved in 200.0 g of water at 30.0 oC. The vapor pressure of the solution was measured and found to be 31.20 torr. The vapor pressure of pure water at 30.0 oC is 31.82 torr. Calculate the molar mass of the unknown solute.
A compound is found to have a molar mass of 598 g/mol. If 35.8 mg of the compound dissolved in enough water to make 175 ml of solution at 25 degrees C what is the osmotic pressure of the resulting solution ?
What mass of insulin must be dissolved in 36.0 ml of water to produce a solution with an osmotic pressure of 15.9 mmhg at 25 C? the molar mass of insulin is 5808 g/mol
When 4.57 g of a nonelectrolyte solute is dissolved in water to make 835 mL of solution at 23 °C, the solution exerts an osmotic pressure of 869 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? moles of solute: mol What is the molar mass of the solute? molar mass: g/mol
When 2.34 g of a nonelectrolyte solute is dissolved in water to make 405 mL of solution at 27 °C, the solution exerts an osmotic pressure of 905 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? moles of solute: mol What is the molar mass of the solute? molar mass: g/mol
When 3.42 g of a nonelectrolyte solute is dissolved in water to make 885 mL of solution at 22 °C, the solution exerts an osmotic pressure of 873 torr. What is the molar concentration of the solution? concentration: concentration: How many moles of solute are in the solution? moles of solute mol What is the molar mass of the solute? g/mol molar mass
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures. 3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the...