Briefly explain the difference between molarity, osmolarity and osmotic pressure?

A nonelectrolyte compound is found to have a molar mass of 598 g/mol. If 33.7 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C, what is the osmotic pressure of the resulting solution? 5.98 torr 5.01 torr 3.42 torr 8.36 torr 6.36 torr

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

Convert the following concentrations into the desired units. A solution of diethylether (C4H10O) in acetone (C3H6O) that has a mole fraction of 0.25 to molality.