Final answer:
The boiling point of a glycerin solution is higher than that of pure water. To calculate it, the molality of the solution and the ebullioscopic constant of water are needed; however, not enough information was provided to determine the exact boiling point for the student's specific solution.
Step-by-step explanation:
The student is asking about the boiling point of a solution of glycerin in water. To find the boiling point of the solution, we would typically use colligative properties which include the calculation of boiling point elevation. However, the student has provided the mass of water (200 ml) but not the mass of glycerin; therefore, without the amount of glycerin, the precise boiling point cannot be calculated. For the example given with 1.0 g of glycerin in 47.8 g of water, one would assume ideal solution behavior to calculate the boiling point elevation using the formula:
ΔT = i × Kb × m
Where ΔT is the boiling point elevation, i is the van't Hoff factor (which is 1 for non-electrolytes like glycerin), Kb is the ebullioscopic constant of water, and m is the molality of the glycerin solution. Since we do not have the specific data for the example the student has described (200 ml water), we cannot calculate the exact boiling point elevation. However, we can assert that the boiling point of glycerin in water would be higher than that of pure water, considering that glycerin is essentially nonvolatile at typical temperatures, and thus would not contribute to the vapor pressure of the solution.