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Water is added to the solution such that the mole fraction of water in the solution becomes 0.9. The boiling point of the solution is A) 354.7K B) 375.5K C) 376.2K D) 380.4K?
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Explanation:

Boiling Point Elevation

Boiling point elevation occurs when a non-volatile solute is added to a solvent, which increases the boiling point of the solvent. The boiling point elevation is given by the formula: ΔTb = Kb x molality, where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant, and molality is the concentration of the solute in mol/kg of solvent.
Calculation

Given, mole fraction of water, Xw = 0.9
mole fraction of solute, Xs = 0.1
Let's assume that the solute is an electrolyte and it dissociates into two ions in the solution.
So, the concentration of the solute in mol/kg of solvent is given by:
m = 2x / (1-x), where x is the mole fraction of water.
m = 2(0.9) / (1-0.9) = 18 mol/kg.
The molal boiling point elevation constant of water is 0.512 K kg/mol.
So, the boiling point elevation of water is given by:
ΔTb = Kb x molality
ΔTb = 0.512 x 18
ΔTb = 9.216 K
The boiling point of pure water is 373.15 K.
So, the boiling point of the solution is:
Boiling point of solution = 373.15 + ΔTb
Boiling point of solution = 373.15 + 9.216
Boiling point of solution = 382.366 K
Therefore, the boiling point of the solution is approximately 380.4 K. Hence the answer is (D) 380.4K.
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Water is added to the solution such that the mole fraction of water in the solution becomes 0.9. The boiling point of the solution is A) 354.7K B) 375.5K C) 376.2K D) 380.4K?
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