When 4.30 g4.30 g of a nonelectrolyte solute is dissolved in water to make 935 mL935 mL of solution at 24 °C,24 °C, the solution exerts an osmotic pressure of 885 torr.885 torr. 1.What is the molar concentration of the solution? 2.How many moles of solute are in the solution? 3.What is the molar mass of the solute?

A solution is prepared by dissolving 1.494 g of potassium permanganate, KMnO4 (molecular weight = 158.034 g/mol), with enough water to make 406.59 mL of solution. What would the osmotic pressure be at 25.0�? Assume the solute is completely ionic.  115.2774 torr    57.6387 torr  1.1377 atm  0.5689 atm

When 2.60 g of a nonelectrolyte solute is dissolved in water to make 275 mL of solution at 29 °C, the solution exerts an osmotic pressure of 915 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? mol moles of solute: What is the molar mass of the solute? molar mass: g/mol

149. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.107 atm at 25.0 °C. Calculate the molar mass of the protein. Round your answer to 3 significant digits. Ox10 mol ?

453. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.132 atm at 25.0 °C. Calculate the molar mass of the protein. Be sure your answer has the correct number of significant digits. x10 mol

114. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.0231 atm at 25.0 °C. Calculate the molar mass of the protein. Be sure your answer has the correct number of significant digits. mol

An aqueous solution of a compound used in antifreeze has an osmotic pressure of 0.589 atm at 20.0°C. It is prepared by dissolving 1.14 g of the compound in enough water to make 0.750 L of solution. What is the molar mass of the antifreeze compound? O 62.1 g/mol O 124 g/mol O 82.8 g/mol O 54.4 g/mol O 4.23 g/mol

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245. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.180 atm at 25.0 °C. Calculate the molar mass of the protein. Be sure your answer has the correct number of significant digits. g x10 mol

5. If a solution has 0.20 moles of NaCl dissolved in 100.0g of water, what is it's molality? 6. If the density of the solution in problem 5 is 1.05 g/mL, what is the molarity of the solution?