   Chapter 12.8, Problem 12.17E General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

Estimate the boiling point of a 0.050 m aqueous MgCl2 solution. Assume a value of i based on the formula.

Interpretation Introduction

Interpretation:

The boiling point of 0.050 m aqueous Magnesium chloride solution has to be determined.

Concept Introduction:

Elevation in boiling point is a colligative property which refers to increase in boiling point of the solution due to the addition of non-volatile solute.  It is expressed as,

ΔTb = Kb.cm

Where,

ΔTb = elevation in boiling pointKb = boiling point elevation constantcm = molal concentration

For ionic solutions, the above expression becomes

ΔTb = i×Kb.cm

Where,

i = van't Hoff factor

van’t Hoff factor refers to the number of moles of ions furnished by per unit formula of the ionic substance when it is dissolved.

Molality or molal concentration is a parameter used to express concentration of a solution.  It is expressed as,

Molality = number of moles of solutemass of solvent in kg

Explanation

Given that molality of the aqueous Magnesium chloride solution is 0.050 m.

From the data given in the table 12.3 in text book, for water, Kb= 0.512°C/m

Therefore, elevation in boiling point is,

ΔTb  = i×Kb.cm

For Magnesium chloride, ‘i’ value is 3. Substitute the values –

ΔTb  = 3×0.512°C/m × 0.050  m = 0.077°C

The elevation in boiling point is equivalent to the difference between boiling temperature of solution and that of pure solvent

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