At –11.5 °C (a common temperature for household freezers), what is the maximum mass of sucralose (C12H19Cl3O8) you can add to 1.00 kg of pure water and still have the solution freeze? Assume that sucralose is a molecular solid and does not ionize when it dissolves in water. Kf = 1.86 °C/m.
Please explain how you got to the answer.
Please explain how you got to the answer.
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Δt = i · Kf · m
Δt = 11.5 °C (since the since water becomes liquid after 0 °C)
i = 1 (does not ionize)
Kf = 1.86 °C/m
m = x / (1kg of water), x in this case is going to be the moles of sucralose
Plug everything in the formula, solve for x and you get it to be 6.1828 moles of Sucralose.
Molar mass of Sucralose is 397.64 g/mol.
Thus, maximum mass of sucralose is 6.1828 moles · 397.64 g/mol = 2458.53 g ≈ 2460 g
Δt = 11.5 °C (since the since water becomes liquid after 0 °C)
i = 1 (does not ionize)
Kf = 1.86 °C/m
m = x / (1kg of water), x in this case is going to be the moles of sucralose
Plug everything in the formula, solve for x and you get it to be 6.1828 moles of Sucralose.
Molar mass of Sucralose is 397.64 g/mol.
Thus, maximum mass of sucralose is 6.1828 moles · 397.64 g/mol = 2458.53 g ≈ 2460 g