Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1. Use 100 °C as the boiling point of water. A) 108 °C B) 92 °C C) 130 °C D) 70 °C E) 8.3 °C

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Quizplus · Accepted Answer

The boiling point elevation is calculated using ΔT_b = i * K_b * m, where i = 1 for ethylene glycol (non-electrolyte), K_b = 0.512 °C m^-1, and m is the molality. Molality (m) = moles of solute/kg of solvent. Moles of ethylene glycol = 500 g / 62.07 g/mol = 8.06 mol. Molality = 8.06 mol / 0.5 kg = 16.12 m. ΔT_b = 1 * 0.512 °C m^-1 * 16.12 m = 8.25 °C. Boiling point = 100 °C + 8.25 °C ≈ 108 °C.

Calculate the Boiling Point of a Solution of 500