We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 23.76 Hg to 22.5 Hg at 25°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the boiling point of this solution? (Hint: find the molality first, and for water, kb = .510 m/°C; boiling point of water: 100.0°C.)

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We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 23.76 Hg to 22.5 Hg at 25°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the boiling point of this solution? (Hint: find the molality first, and for water, kb = .510 m/°C; boiling point of water: 100.0°C.)

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Step 1

According to the question,

The vapor pressure of the pure solvent is given by = Po = 23.76 Hg = 0.794 atm

The vapor pressure of the solution is given by = P = 22.5 Hg = 0.752 atm

The mass of water is given by = m =346 g

The molar mass of water = 18.02 g/mol

The molar mass of ethylene glycol =62.07 g/mol

Kb for water is given by  = 0.510 m/°C

 

Find- Boiling point of the solution.

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