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Dmitry_Shevchenko [17]
3 years ago
7

Barbiturates are synthetic drugs used as sedatives and hypnotics. Barbital ( = 184.2 g/mol) is one of the simplest of these drug

s. What is the boiling point of a solution prepared by dissolving 42.5 g of barbital in 825 g of acetic acid? Kb = 3.07°C/m; boiling point of pure acetic acid = 117.9°C
Chemistry
1 answer:
DanielleElmas [232]3 years ago
6 0

Answer:

118.75°C is the boiling point of a solution.

Explanation:

Mass of the solute that is barbiturates = 42.5 g

Molar mass of a solute = 184.2 g/mol

Moles of solute = \frac{42.5 g}{184.2 g/mol}=0.2307 mol

Mass of the solvent that acetic acid = 825 g = 0.825 kg

molality=\frac{\text{Moles of solute}}{\text{Mass of solvent}}

Molality of the solution (m):

m=\frac{0.2307 mol}{0.825 kg}=0.2796 m

Elevation in boiling point is given as:

\Delta T_b=i\times K_b\times m

i = 1 (organic compound)

=1\times 3.07^oC/m\times 0.2796 m=0.8585^oC

\Delta T_b=T_b-T

T_b = Boiling temperature of solution.

T = boiling temperature of solvent that is acetic acid=117.9°C

0.8585^oC=T_b-117.9^oC

T_b=118.75 ^oC

118.75°C is the boiling point of a solution.

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