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Why does the freezing point of a pure solvent remain as a constant value but the freezing point of a solution decreases with steady cooling?

Why does the freezing point of a pure solvent remain as a constant value but the freezing point of a solution decreases with steady cooling?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section13.7: Colligative Properties Of Solutions
Problem 13.17CE
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Why does the freezing point of a pure solvent remain as a constant value but the freezing point of a solution decreases with steady cooling? 

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What do you mean by how the solution is more concentrated? So does the solution decrease because it contain more substance (and is more concentrated). The solvent is constant because it is made up of one thing?

 

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