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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

An aqueous solution contains 0.180 g of an unknown, nonionic solute in 50.0 g of water. The solution freezes at −0.040 °C. What is the molar mass of the solute?

Interpretation Introduction

Interpretation: The molar mass of unknown nonionic solute has to be determined.

Concept introduction:

Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are,

  • Decrease in the vapor pressure
  • Increase in the boiling point
  • Decline in the freezing point
  • Osmotic pressure

Change in freezing point is calculated by using the equation,

  ΔTfp=Kfpmsolute

  where,

  Kfp is the molal freezing point depression constant.

The number of moles of any substance can be determined using the equation

  Numberofmole=GivenmassofthesubstanceMolarmass

Explanation

The molar mass of unknown nonionic solute is calculated.

Given,

  ΔT=0.0400C

  Mass of unknown nonionic solute is 0.180g

  Mass of water is 50g=0.050kg

  Molal freezing point depression constant of water is 1.860C/m

Change in freezing point is calculated by using the equation,

  ΔTfp=Kfpmsolute

Hence,

The concentration is calculated by,

  Concentration,msolute=ΔTfpKfp=(0.0400C)(1.860C/m)=0.0215m

The amount of unknown nonionic solute is,

  (0

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