<img src="https://d5nxst8fruw4z.cloudfront.net/atrk.gif?account=iA1Pi1a8Dy00ym" style="display:none" height="1" width="1" alt="" />
Skip Navigation
You are viewing an older version of this Concept. Go to the latest version.

Saturated and Unsaturated Solutions

Types of solutions defined

Atoms Practice
Estimated4 minsto complete
Practice Saturated and Unsaturated Solutions
Estimated4 minsto complete
Practice Now
Saturated and Unsaturated Solutions

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.

\text{NaCl}(s) \rightleftarrows \text{NaCl}(aq)

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.

\text{NaCl}(s) \rightleftarrows \text{Na}^+ (aq)+\text{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 below illustrates the above process and shows the distinction between unsaturated and saturated.

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.


  • Saturated and unsaturated solutions are defined.
  • Solution equilibrium exists when the rate of dissolving equals the rate of recrystallization.


Watch the video at the link below and answer the following questions:


  1. What is the initial solution used?
  2. What is the heat source for evaporation?
  3. Why does the salt precipitate out of solution?


  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?

Image Attributions

Explore More

Sign in to explore more, including practice questions and solutions for Saturated and Unsaturated Solutions.


Please wait...
Please wait...

Original text