Saturated and Unsaturated
Solutions
Ck12 Science
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Printed: January 4, 2016
AUTHOR
Ck12 Science
www.ck12.org
C HAPTER
Chapter 1. Saturated and Unsaturated Solutions
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Saturated and Unsaturated
Solutions
• Define saturated solution.
• Define unsaturated solution.
• Define solution equilibrium.
How do you make sure a compound is pure?
When compounds are synthesized, they often have contaminating materials mixed in with them. The process of
recrystallization can be used to remove these impurities. The crystals are dissolved in a hot solvent, forming a
solution. When the solvent is cooled the compound is no longer as soluble and will precipitate out of solution,
leaving other materials still dissolved.
Saturated and Unsaturated Solutions
Table salt (NaCl) readily dissolves in water. Suppose that you have a beaker of water to which you add some salt,
stirring until it dissolves. So you add more and that dissolves. You keep adding more and more salt, eventually
reaching a point that no more of the salt will dissolve no matter how long or how vigorously you stir it. Why? On
the molecular level, we know that action of the water causes the individual ions to break apart from the salt crystal
and enter the solution, where they remain hydrated by water molecules. What also happens is that some of the
dissolved ions collide back again with the crystal and remain there. Recrystallization is the process of dissolved
solute returning to the solid state. At some point the rate at which the solid salt is dissolving becomes equal to the
rate at which the dissolved solute is recrystallizing. When that point is reached, the total amount of dissolved salt
remains unchanged. Solution equilibrium is the physical state described by the opposing processes of dissolution
and recrystallization occurring at the same rate. The solution equilibrium for the dissolving of sodium chloride can
be represented by one of two equations.
NaCl(s) NaCl(aq)
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While this shows the change of state back and forth between solid and aqueous solution, the preferred equation also
shows the dissociation that occurs as an ionic solid dissolves.
NaCl(s) Na+ (aq) + Cl− (aq)
When the solution equilibrium point is reached and no more solute will dissolve, the solution is said to be saturated.
A saturated solution is a solution that contains the maximum amount of solute that is capable of being dissolved. At
20°C, the maximum amount of NaCl that will dissolve in 100. g of water is 36.0 g. If any more NaCl is added past
that point, it will not dissolve because the solution is saturated. What if more water is added to the solution instead?
Now more NaCl would be capable of dissolving in the additional solvent. An unsaturated solution is a solution
that contains less than the maximum amount of solute that is capable of being dissolved. Figure 1.1 illustrates the
above process and shows the distinction between unsaturated and saturated.
FIGURE 1.1
When 30.0 g of NaCl is added to 100 ml
of water, it all dissolves, forming an unsaturated solution. When 40.0 g is added,
36.0 g dissolves and 4.0 g remains undissolved, forming a saturated solution.
How can you tell if a solution is saturated or unsaturated? If more solute is added and it does not dissolve, then the
original solution was saturated. If the added solute dissolves, then the original solution was unsaturated. A solution
that has been allowed to reach equilibrium but which has extra undissolved solute at the bottom of the container
must be saturated.
Summary
• Saturated and unsaturated solutions are defined.
• Solution equilibrium exists when the rate of dissolving equals the rate of recrystallization.
Practice
Questions
Watch the video at the link below and answer the following questions:
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Chapter 1. Saturated and Unsaturated Solutions
MEDIA
Click image to the left or use the URL below.
URL: http://www.ck12.org/flx/render/embeddedobject/63353
http://www.youtube.com/watch?v=gawS3sBHMQw
1. What is the initial solution used?
2. What is the heat source for evaporation?
3. Why does the salt precipitate out of solution?
Review
Questions
1. Why is the preferred equation for solution equilibrium of NaCl an equilibrium between solid NaCl and the
ions.
2. If I add water to a saturated sucrose solution, what will happen?
3. If I heat a solution and remove water, I see crystals at the bottom of the container. What happened?
• recrystallization: The process of dissolved solute returning to the solid state.
• saturated solution: A solution that contains the maximum amount of solute that is capable of being dissolved.
• solution equilibrium: The physical state described by the opposing processes of dissolution and recrystallization occurring at the same rate.
• unsaturated solution: A solution that contains less than the maximum amount of solute that is capable of
being dissolved.
References
1. User:Ragesoss/Wikimedia Commons. http://commons.wikimedia.org/wiki/File:MSG_crystals.JPG .
2. CK-12 Foundation - Christopher Auyeung. .
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