A 0.517 âg sample of a nonvolatile solid solute dissolved in 15.0 gof t-butanol. The freezing point of the solution is 22.7 ?.
-What is the molality of the solute in the solution?

-Calculate the molar mass of the solute.

-The mass of solute is dissolved in 15.0 g of cyclohexane insteadof t-butanol. What is the expected freezing point change of thissolution?

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Nestor RutherfordLv2

24 Jun 2019

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A 0.194 g sample of a nonvolatile solid solute dissolves in 9.82 gof cyclohexane.?
the change in the freezing point is 2.94 C.

Kf= 20

a)- What is the molality of the solute in the solution?

b) Calculate the molar mass (sig figs)

c) The same mass of solute is disolved in 9.82 g of t-butanolinstead of cyclohexane. WHat is the freezing point? (Kf=9.1)(Freezing Point= 25.5 C)

Calculate the molar mass for ∆T_f, molality of t butanol, and experimental molar mass of the solute given the following experimental data:

Freezing point of t-butanol = 23.3 °C

Freezing point of the solution = 20.3 °C

Weight of butanol = 3.701 g

Weight of solute (ethyl paraben) = 0.195 g

(K_f for t butanol is 8.3°C/m)