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dolphi86 [110]
3 years ago
7

The cells of a tomato contain mostly an aqueous solution of sugar and other substances. If a typical tomato freezes at -2.5 °C,

what is the molality of the sugar in solution? (Hint: sugar is a covalent compound, it does not dissociate in water)
Chemistry
1 answer:
DIA [1.3K]3 years ago
6 0

Answer:

1.35 m

Explanation:

We can solve this problem by using the <em>freezing point depression formula</em>:

  • ΔT = Kf * m * i

Where:

  • ΔT is the temperature difference between the freezing point of the pure solvent (water) and the solution. In this case it is (<em>0 °C - -2.5 °C = 2.5 °C</em>).
  • Kf is the cryoscopic constant, <em>for water it is 1.853  °C*kg/mol.</em>
  • m is the molality.
  • i is the van't Hoff factor, <em>as sugar does not dissociate in water, it has a value of 1</em>.

We <u>input the data</u>:

  • 2.5 °C = 1.853 °C*kg/mol * m * 1

And <u>solve for m</u>:

  • m = 1.35 m
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