# Chapter 13, Problem 13.80QP

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### CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

#### Solutions

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FindFindarrow_forward

### CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933
Interpretation Introduction

Interpretation:

Freezing point depression and osmotic pressure measurement used to determine the molar mass of a compound but boiling point elevation and vapor pressure lowering not used to be described.

Concept introduction

• Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is 100°C That is water changes from liquid phase to gas phase.

ΔTb= Tb- Tb°

Where,

ΔTb change in boiling point

Tb Boiling point of the solution

Tb° -  Boiling point of pure solvent

• Boiling point elevation (ΔTb)   is distinction between boiling point of the pure solvent (Tb°) and the boiling point of the solution (Tb) .

ΔTb= Kbm

Where,

ΔTb Change in boiling point

Kb Molal boiling point constant

m - molality of the solution

• Freezing point is the temperature at which liquid turns into solid.
• Freezing point depression (ΔTf) is distinction between freezing point of the pure solvent (Tf°) and the freezing point of the solution (Tf) .

ΔTf= Kfm

Where,

ΔTf Change in freezing point

Kf Molal freezing point constant

m- Molality of the solution

• Osmotic pressure is the pressure that is needed to stop osmosis. Osmotic pressure of the solution is directly proportional to the concentration of the solution.

Osmotic pressure (π) = MRT

Where,

M – Molarity of the solution (mole/L)

R- Ideal gas constant (0.08206 L atm mol-1K-1 )

T-Temperature in Kelvin

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