1. SOLUTIONS

2. Do you remember???? What is a mixture???  2 or more pure substances that can be separated based on physical properties What is a homogeneous mixture??  A mixture that is the same throughout What is another name for homogeneous mixture?  solution

3. What a solution is not!!! Heterogenous Mixture  Suspension  Particles will settle out over time  Does not show a positive Tyndall Effect  Examples Pizza Salad Dressing  Colloid  Particles will not settle out over time  Displays a positive Tyndall effect  Examples Fog

4. What are the parts of a solution? A solution is composed of 2 parts  Solute: the part of the solution that gets dissolved  Can be either a solid, liquid or gas  Solvent: the part of the solution that does the dissolving  Typically liquids or gases  Water is known as the universal solvent as it dissolves more solutes than any other substance on earth

5. Why doesn’t oil and water mixture? From a chemical perspective, in order to make a solution the two substances must be similar in make up  Ionic compounds will dissolve Ionic compounds and polar covalent compounds  Polar covalent compounds will dissolve polar covalent compounds  Nonpolar compounds will dissolve nonpolar compounds  We remember “LIKE DISSOLVES LIKE”

6. How do we make solutions? Take a solid and dissolve it into a liquid The question really is….how much solute and how much solvent?  The ratio of the amount of solute to the amount of solvent is known as the concentration of the solution  More solute = more concentration (less dilute)  Less solute = less concentration (more dilute)

7. How do you measure concentration of a solution? The amount of concentration in a solution is measured by a unit called MOLARITY.  Molarity is a measure of the moles of a solute per liters of solution  The unit for molarity is M.  The mathematical formula used to calculate molarity is M= moles of solute liters of solution

8. How do you use the formula? Lets take a few minutes and do the practice problems on our worksheet.

9. What are the types of solutions? The type of solution is based on concentration  Unsaturated Solution  Contains less than the maximum amount of solute  If you add more solute to the solution, the solute will dissolve  Saturated Solution  Contains the maximum amount of solute at a given temperature  If you add more solute to the solution, the solute will not dissolve and will settle to the bottom  Supersaturated Solution  Contains more than the maximum amount of solute at a given temperature  The solution has been heated and then cooled  If you add more solute, all of the solute will crystalize out

10. Type:JPG What axis is the solute on? What axis is the temperature on? What is the relationship between temperature and solubility on NaNO 3 ? What is the relationship for Ce 2 (SO 4 ) 3 ? Solubility Curve Website for this image Solubility Curve saskschools.ca Full-size image 650 × 831 (1.7x larger), 206KB More sizes Search by image Similar images Related searches: solubility chart Images may be subject to copyright.

11. Solubility Curve…more Which substance is most affected by temperature? Which substance is least affected by temperature? If 70g of NH 3 was dissolved at 10 0 C, what type of solution would you have? 50g of KCLO 3 at 20 0 C? 10g of NaCL at 100 0 C?

12. GATEWAY ALERT!!!!!!!!!!! What will happen to fish when the temperature of water is increased because a manufacturing plant begins dumping hot water into the stream  As the temperature of water increases, the solubility of a gas decreases  Fish breath dissolved oxygen in the water  The fish will suffocate and die

13. Why do you put salt out when there is ice on the stairs? Colligative properties are properties of solutions that depend on the number of molecules in a given volume of solvent and not on the properties/identity (e.g. size or mass) of the molecules More particles of solute means more colligative properties

14. Boiling Point Elevation Boiling-point elevation describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solventboiling pointliquid solventsolution

15. Freezing point depression Freezing-point depression describes the phenomenon in which the freezing point of a liquid (a solvent) is depressed when another compound is added, meaning that a solution has a lower freezing point than a pure solvent.freezing pointliquidsolventsolutionsolvent