An aquous solution freezes at -0.186 then elevation of boiling point is
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Both freezing point depression and boiling point elevation are colligative properties, so they follow essentially the same equations which are of the form
ΔT = kf m i
where
kf is the freezing point depression constant (or boiling point elevation constant)
m is the molality of the solute
i is the van't Hoff factor (the number of particles per mole of the solute)
Since this is one solution, the values for m and i are the same. So the b.p. elevation will be
(-5.5°C)×(b.p. elevation constant)/(f.p. depression constant)
Add that to the normal b.p. of water, and there you go.
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