Respuesta :
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 = [tex]\frac{42.5 g}{184.2 g/mol}=0.2307 mol[/tex]
Mass of the solvent that acetic acid = 825 g = 0.825 kg
[tex]molality=\frac{\text{Moles of solute}}{\text{Mass of solvent}}[/tex]
Molality of the solution (m):
[tex]m=\frac{0.2307 mol}{0.825 kg}=0.2796 m[/tex]
Elevation in boiling point is given as:
[tex]\Delta T_b=i\times K_b\times m[/tex]
i = 1 (organic compound)
[tex]=1\times 3.07^oC/m\times 0.2796 m=0.8585^oC[/tex]
[tex]\Delta T_b=T_b-T[/tex]
[tex]T_b[/tex] = Boiling temperature of solution.
T = boiling temperature of solvent that is acetic acid=117.9°C
[tex]0.8585^oC=T_b-117.9^oC[/tex]
[tex]T_b=118.75 ^oC[/tex]
118.75°C is the boiling point of a solution.
