An aqueous solution of a certain organic compound has a density of 1.063 g/mL, an osmotic pressure of 12.16 atm at 25.0 °C, and a freezing point of -1.03 °C. The compound is known not to dissociate in water. What is the molar mass of the compound?

Osmotic pressure is the pressure required to prevent the flow of solvent into a solution through a semipermeable membrane. It is directly proportional to the molarity of the solute and can be calculated using the formula π = iCRT, where π is the osmotic pressure, i is the van 't Hoff factor (which is 1 for non-dissociating compounds), C is the molarity, R is the ideal gas constant, and T is the temperature in Kelvin.

Freezing point depression is a colligative property that describes the lowering of the freezing point of a solvent when a solute is added. The extent of freezing point depression can be calculated using the formula ΔTf = iKf m, where ΔTf is the change in freezing point, Kf is the freezing point depression constant of the solvent, and m is the molality of the solution. This concept is essential for determining the molar mass of the solute.

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the molar mass of a solute from colligative properties, one can rearrange the formulas for osmotic pressure or freezing point depression to solve for molar mass, using the measured values of osmotic pressure, freezing point change, and the properties of the solvent. This calculation is crucial for identifying the molecular weight of the organic compound in the question.