To calculate the increase in boiling point of a solution containing 240 grams of non-electrolyte sucrose dissolved in 850 grams of water, we first need to calculate the molality of the solution. Molality is the number of moles of solute per kilogram of solvent. In this case, the mass of solvent is 850 grams, which is equal to 0.85 kilograms. The number of moles of sucrose can be calculated by dividing the mass of sucrose by its molar mass, which is 342 grams per mole. The calculated number of moles of sucrose is 0.7029 moles. Dividing the number of moles of sucrose by the mass of the solvent gives the molality, which is 0.8259 mol/kg.
Using the equation for boiling point elevation, we can calculate the increase in boiling point. The equation is ΔTb = Kb * m * i, where ΔTb is the increase in boiling point, Kb is the molal boiling point elevation constant for water, m is the molality of the solute, and i is the van't Hoff factor, which is 1 for a non-electrolyte like sucrose. Substituting the known values into the equation gives ΔTb = (0.512 °C/m) * (0.8259 m) * 1 = 0.4238 °C.
Thus, the boiling point of the solution would increase by approximately 0.424 °C (to three significant figures) when 240 grams of sucrose is dissolved in 850 grams of water.
