Final answer:
One mole of a molecular solute like glucose or sucrose dissolved in 1000 g of water raises the boiling point by 0.51°C, due to the molal boiling point elevation constant of water. For ionic substances like NaCl, the elevation is about 1.02°C, while for CaCl₂ it is 1.53°C.
Step-by-step explanation:
One mole of any molecule or ion dissolved in 1000 g of water raises the boiling point of the water by the extent defined by the molal boiling point elevation constant, which for water is 0.51°C/m. For substances that do not dissociate into ions, such as glucose or sucrose, this would result in a boiling point elevation of 0.51°C.
However, for electrolytes like NaCl which dissociate into ions, the boiling point elevation will be approximately twice as large because 1 mole of NaCl yields 2 moles of ions, resulting in a boiling point elevation of 1.02°C for a 1.00 m NaCl solution. Similarly, for CaCl₂, which dissociates into three ions, the elevation would be 3 × 0.51°C = 1.53°C for a 1.00 m solution.