Question

When 19.1g of a nonvolatile and nonelectrolyte solute of unknown identity are dissolved in 150ml of water at room temperature of 25 degrees Celsius, with an osmotic pressure of 23 atm and a density of the solution at 1.06g/ml, which statement is correct?

a) The molar mass of the solute is 51.3 g/mol
b) The molar concentration of the solution is 0.2 mol/L
c) The van't Hoff factor of the solute is 2
d) The freezing point depression of the solution is 6.68°C

Answer 1

To ascertain the validity of the provided statements regarding the solute in a solution, one must perform calculations involving osmotic pressure (Π = MRT) to derive the molarity, and then use it to find the molar mass of the solute.

Step-by-step explanation:

To determine which statement is correct about the nonvolatile and nonelectrolyte solute dissolved in water with the given osmotic pressure, we first need to calculate the molarity of the solution using the formula for osmotic pressure (i.e., Π = MRT). Given that the osmotic pressure (Π) is 23 atm, the temperature (T) is 298 K (25°C + 273), and R is the ideal gas constant, we can find the molarity (M). Once we have M, we can calculate the molar mass of the solute by dividing the mass of the solute by the moles of solute as determined by the molarity and the volume of the solution.

Without the exact calculations presented here, we cannot confidently state which option is correct. However, with the provided data, a student or a practitioner of chemistry can perform these calculations to find out the accurate molar mass, molar concentration, van't Hoff factor, or freezing point depression for the given solution.