Question

If 4.270g of sucrose (C₁₂​H₂₂​O₁₁​) are dissolved in 15.20g of water, what will be the boiling point of the resulting solution? (K_b​ for water = 0.5120∘C/m)

Answer 1

To determine the boiling point of the resulting solution, use the formula ΔT = Kb * m * i. Calculate the molality of the solution using the formula m = moles of solute / mass of solvent (in kg). Use the calculated molality to find the change in boiling point, and then add this change to the boiling point of pure water to find the new boiling point.

Step-by-step explanation:

To determine the boiling point of the resulting solution, we need to use the formula: ΔT = Kb * m * i, where ΔT is the change in boiling point, Kb is the molal boiling point elevation constant for water, m is the molality of the solution, and i is the van't Hoff factor.

First, we calculate the molality (m) of the solution using the formula: m = moles of solute / mass of solvent (in kg). The molar mass of sucrose is calculated by adding the atomic masses of its constituent elements: 12.01 g/mol (carbon) + 1.01 g/mol (hydrogen) + 16.00 g/mol (oxygen) = 342.34 g/mol.

Using the molality of the solution, we can now calculate the change in boiling point (ΔT) using the formula above. Plugging in the values, we get: ΔT = (0.5120 ℃/m) * (0.0125 mol/kg) * (1). Solving this equation gives us a change in boiling point of 0.0064 ℃.

To find the new boiling point, we add the change in boiling point to the boiling point of pure water (100.00 ℃). Thus, the boiling point of the resulting solution would be 100.0064 ℃.