1. Notes:Color Guide Gold : Important concept. Write this down. Orange : Definition. Write this down. Blue : Important information, but you do not need to copy. Red : Example. Copy if needed. White : General Discussion (Don’t Copy)

2. Solutions Part 1: Mixtures Sodium Chloride: Liquid Solution Air : Gaseous Solution

3. Mixtures of different substances exist all around us. Many of these mixtures are invisible, and we never notice them. Definition: mixture – a combination of different substances that is NOT formed by chemical reactions.  Mixtures can be separated!

4. Mixtures can be categorized into two groups: Heterogeneous is a mixture that does not look the same all over.  Definition: heterogeneous mixture (HT) – a mixture that is not evenly dispersed.  Dispersed means “spread out”.  The particles in a HT mixture can be seen. Orange juice with pulp is an example of a heterogeneous mixture.

5. Heterogeneous Mixtures Different fragments make up this rock. This rock is a heterogeneous mixture.

6. There are a two different types of heterogeneous mixtures:  Definition: suspension – HT mixture in which particles are floating (suspended) in a fluid.  Many suspensions do not transmit light and will “settle” over time.  Examples: Muddy Water Dusty Air Orange Juice with Pulp Salad Dressing

7. –Definition: colloid – a suspension made of particles too small to settle out.  Many colloids do transmit light and will not “settle” over time. –Examples: Mayonnaise Milk Whipped Cream Butter

8. Homogeneous mixtures look the same all over. Definition: homogeneous mixture (HM) – a mixture in which the particles are spread evenly.  The particles that make up a HM mixture cannot be seen.  Sweet tea is an example of a homogenous mixture.  There are several different substances (tea, water, and sugar) but you cannot see them.  The tea looks uniform (the same) throughout.

9. We can call homogeneous mixtures by another name: solutions.  Definition: solution - a HM mixture of 2 or more substances that are evenly dispersed.

10. Part 2: Solutions

11. Solutions are formed by the process of dissolving.  Definition: dissolving – the process by which substances mix to form a solution. These tablets are dissolving in the water to form a solution.

12. When substances dissolve, there are two parts to the solution it creates…  The Solute and the solvent. Definition: solute - a substance that gets dissolved and is generally presented in the lesser amount. Definition: solvent - a substance that does the dissolving and is generally presented in the greater amount.

13. For example:  When you stir sugar into water, the sugar dissolves.  The water is the solvent.  The sugar is the solute. Solute SolventSolution + =

14. Definition: Solvation- occurs when and where the solute and the solvent particles come in contact with each other. And we all *probably* know some ways to speed up the process.

15. There are three common ways to increase the collisions between the solute and solvent particles and thus increase the rate at which the solute dissolves. Increasing the surface area: Making a solute smaller makes it dissolve faster.  By crushing up a solute, you increase the surface area.  The solvent can pull the solute apart faster when it is smaller. Rock Salt Crushed Salt

16. Agitating the mixture: Stirring or shaking will make a SOLID solute dissolve faster.

17. Increasing the temperature: Heating the solvent will make a SOLID solute dissolve faster. Faster moving atoms means faster dissolving! Which one will dissolve sugar Fastest?

18. Did you know? Liquids dissolve gases best when:  The liquid is cold.  The liquid is under lots of pressure. Gases dissolve gases best when:  The gas is cold.  The gas is under lots of pressure CO 2 Gas is also dissolved into your soda!

19. Part 3: Like Dissolves Like

20. Water is very good at dissolving things.  Water is known as “The Universal Solvent”  Water can dissolve any ionic compound, and many covalent compounds.

21. The water molecule has a positive end and a negative end.  This is called being “polar”. H H O Because water is polar, it can attract molecules and ions like a magnet. Na Cl

22. Because water’s + and – charges are not spread out evenly, it is “polar”.  Definition: polar compound – a molecule that has a positive side and a negative side.  Because water is a polar compound, it is a good solvent. The Earth is Polar! It has two separate sides.

23. Water can only dissolve other polar compounds.  If water cannot dissolve a substance, then that substance is “nonpolar”. Water and Vinegar? No Problem! Water and Oil? NO WAY.

24.  Definition: nonpolar compound – has an even charge on its molecules.  The charges are spread out evenly.  Nonpolar substances can only dissolve other nonpolar substances.  Example – oil-based paint will not dissolve in water. A nonpolar solvent must be used.

25.  General rule: “Like Dissolves Like”.  Polar substances can only dissolve other polar substances.  Nonpolar substances can only dissolve other nonpolar substances.

26. Other definitions to know:  Definition: Soluble – when a substance dissolves in a solvent.  Definition: Insoluble- When a substance does not dissolve in a solvent.  Definition: Miscible- When two liquids are soluble in each other.  Definition: Immiscible- When two liquids are not soluble in each other.

27. Part 4: Solubility & Concentration

28. Some substances dissolve easier than others. This property is called “solubility” Definition: solubility – the max amount of a solute that will dissolve in a certain amount of solvent.  Substances have different solubility.  Some will dissolve completely in water, while others will dissolve only a small amount.

29. The amount of solute dissolved in a solvent affects its concentration.  Definition: concentration – a description of the amount of a solute in a certain amount of solution.  Think of concentration as being how “strong” a solution is. Not Very Concentrated Very Concentrated

30. “Concentrated” substances have lots of solute. “Diluted” substances only have a little solute. Add water to OJ concentrate to dilute it.

31. When a solvent can no longer hold any more solute, we called it “saturated”.  Definition: saturated solution – a solution that CANNOT dissolve any more of a solute.  Definition: unsaturated – a solution that CAN hold more solute.

32. Sometimes, a solvent can be made to hold more solute than normal. The solution is called “supersaturated”.  Definition: supersaturated – a solution that has more solute than normal.  A HOT solution can hold lots of solute.  When it COOLS, it becomes supersaturated.

33. Supersaturated solutions are unstable.  The extra solute can “fall out” if the solution is shaken! The crystals in the supersaturated solution were “shaken out”!

34. Part 5: Conductivity

35. Some solutions have the ability to conduct electricity… Definition: electrolyte – a solution that can conduct electricity.  Most electrolytes contain ionic compounds.

36.  All ionic compounds form electrolytes.  Covalent compounds cannot conduct electricity when dissolved in a solution.  They are called nonelectrolytes. Definition: nonelectrolyte – a solution that does not conduct electricity.