Solutions & Mixtures

1. Solutions & Mixtures

2. Mixture • Something that consists of different parts. • Example: • Trail Mix • Chex Mix • Kool-Aid • Salt Water

3. Heterogeneous Homogeneous The parts are evenly mixed You can’t see the difference between the parts of the mixture. Examples: Kool-Aid, salt water, lemonade, etc. • The parts are not evenly mixed throughout. • You can see the differences between parts. • Examples: Chex Mix, Trail mix, Salad, etc. Heterogeneous vs. Homogeneous Mixtures

4. Suspension • Have larger particles • Are heterogeneous • The majority of mixtures fall into this category.

5. Colloids • Mixture in between a suspension and a solution. • Parts are smaller. • Almost appears cloudy. • Usually homogenous. • Example: Homogenized milk is a mixture of cream and butterfat particles in skim milk.

6. Solution • An example of a homogenous mixture. • Parts are evenly mixed. • Consists of two parts: • Solute • Solvent

7. Solvent Solute The substance that is being dissolved by the solvent. Example: The salt in salt water would be the solute. • The substance that dissolves the solute. • Example: The water in salt water would be the solvent. Solvent vs. Solute

8. What is the Universal Solvent??? Water

9. Dissolve • When something seems to disappear into another substance. • Examples: Kool-aid into water, salt into water, etc.

10. Soluble Solubility The amount of solute that can be dissolved in a given solvent. Usually expressed as a percent. • The ability to be dissolved. Soluble and Solubility

11. Insoluble • Not able to dissolve in a solvent • Example: chalk is insoluble in water.

12. Concentration • The strength of a solution that is determined by the amount of solute dissolved in the solvent. • Concentrated- • Is a solution which is made by dissolving a large amount of solute in a small amount of solvent.

13. Saturated • The point at which a solution can not dissolve any more solute. • It contains all the solute that it can hold under existing conditions. • This is called the Saturation Point. • Can this be altered? • Yes

14. Altering Saturation Point • Add more solvent. • Change the temperature • Increasing temperature, increases the kinetic energy, which increases the amount of solute that can be dissolved. • Stir (increases kinetic energy)

15. Boiling Point Elevation and Freezing Point Depression • Adding a substance to another substance can alter the boiling and freezing point of that substance. • Boiling Point Elevation • The amount by which the boiling point of the solvent is raised when the solvent is dissolved in it. • Freezing Point Depression • The amount by which the freezing point of the solvent is lowered when the solvent is dissolved in it.

16. Desalination • The process of removing excess salt or minerals from a solution. • Involves boiling the water and catching the evaporated water using a special setup. • Why is this important? • Purifies water so that it can be consumed.

17. Chromatography • Process to separate a solution based on the solute’s different properties. • Example: You can use chromatography to separate different liquid components in a solution.

18. Other Methods of Separation… • Distillation • A solution is heated until it evaporates, leaving behind dissolved materials. • Evaporation is the process by which a liquid gradually changes into a gas • Using a Filter • Separates different sized particles through a different filters.