1. Solubility Do Now: p.4

2. Remember…likes dissolve like Things that dissolve in water – Soluble ionic – Acids (ex HCl) – Bases (ex. NaOH) – Polar covalent molecules

3. Factors that affect the rate at which something dissolves Temperature Stirring or agitation Surface area (crushing/grinding)

4. Solubility = the max amount of solute that can be dissolved in a solvent Many solids can dissolve in water As you increase the temperature, you can dissolve more solid Where can you go to find if an ionic compound is soluble or insoluble in water? Table F

5. When Ionic Compound (which are solids) dissolved in water they dissociate (or ionize) Cl - Water will arrange itself around the ions according to their charge

6. Many gases also dissolve in water As you increase the temperature, you can dissolve more solid, do you think this works the same for gases? As you increase the temperature, gases have more KE, so they do not stay dissolved in In order to dissolve some gases, you must increase pressure.

7. Summary: Factors Affecting Solubility Nature of the solvent and the solute: Nature of the solvent and the solute: LIKE DISSOLVES LIKE Temperature Temperature Pressure (for systems with gases) Pressure (for systems with gases)

8. Solubility curves show the relationship between solubility and temperature. Can you guess which of these compounds are gases?! How do you know?!

9. Reading a solubility curve?! Table G tells you the max amount of solute you can dissolve in 100 g of H 2 O at a given temperature

10. How much KCl will dissolve in 100g of water at 50  C? Problem: X = 42g KCl

11. How much KCl will dissolve in 300g of water at 50  C? Hint: Use the graph to set up a proportion Problem: 42 g KCl = X g KCl 100 g H 2 O 300 g H 2 O X = 126g KCl

12. How much H 2 O is required to just dissolve 200 g NaNO 3 at 20  C? 88 g NaNO 3 = 100 g H 2 O 200 g NaNO 3 X g of H 2 O X = 227.3 g H 2 O

13. On the line – saturated (full, cannot hold any more solute Below the line – unsaturated (can hold more solute) Above the line – supersaturated (holding more solute then it should – very unstable)

14. Unsaturated solution

15. Saturated Solution Is in equilibrium between solid particles dissociating into ions and ions forming crystals Cl - (aq)

16. Supersaturated Solution very unstable ( this picture is showing the addition of 100 g of glucose to 100ml of water at 25 0 C) Note: at 25 0 C, only 91g of glucose will dissolve in 100 ml of water Let’s see what happens Let’s see what happens

17. Precipitation problems A saturated solution of KNO 3 is prepared in 100 g of water at 50  C and then cooled down to 10  C. How much KNO 3 will precipitate? A saturated solution of KNO 3 is prepared in 100 g of water at 50  C and then cooled down to 10  C. How much KNO 3 will precipitate?

18. 88 g KNO 3 in 100 g H 2 O at 50  C 20 g KNO 3 in 100 g H 2 O at 10  C 88 g – 20 g = 68 g KNO 3 precipitates