MgCl₂ has a van't Hoff factor of 2.70. What would be the boiling point (in °C) of an aqueous solution containing 4.30 mol of MgCl₂ in 1.00 kg of water? (Kb for water is 0.512 °C/m. The boiling point for water is 100.0˚C.)
MgCl₂ has a van't Hoff factor of 2.70. What would be the boiling point (in °C) of an aqueous solution containing 4.30 mol of MgCl₂ in 1.00 kg of water? (Kb for water is 0.512 °C/m. The boiling point for water is 100.0˚C.)
When a non volatile solute is added to a pure solvent it's point is increased . The increase in boiling point is called elevation of boiling point ( ∆Tb ).
If To is boiling point of pure solvent and T is it's boiling point in solution , then the difference (T-To ) is called elevation in boiling point
∆Tb = T - To
Experimentally it was found that , ∆Tb is proportional to molality of solution and also depends on van't Hoff factor " i "
∆Tb = i×Kb×molality
molality = n/W
n = moles of solute
W = nass of solvent in kg
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