Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074



Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Some ethylene glycol, HOCH2CH2OH, is added to your car’s cooling system along with 5.0 kg of water. If the freezing point of the water-glycol solution is −15.0 °C, what mass of HOCH2CH2OH must have been added?

Interpretation Introduction

Interpretation: The mass of ethylene glycol has to be identified.

Concept introduction:

Freezing point elevation: The freezing point of the solution varies with the solute concentration.

Depression in Freezing point = ΔTfp= Kfp. msolute,where,Kfpismolal boiling point elevation constant,msoluteis molality of solute

  • Calculate the molality of ethylene glycol:

Given data:

ΔTfp =Thefreezingpointofthesolution-freezingpointofwaterΔTfp= -15.0oC-0.0oC=-15.0oCFreezing point of water = 0oCKfp ofWater=-1.86oC/mAmountofsolvent=5kg

Calculate the molality of solute in solution(m):_Freezing point Depression, ΔTfp= Kfp. msolute,-15.0oC=(-1.86oC/m)(msolute)msolute=-15

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