1. Solubility

2. Dissolving Particles of the solute move into the solvent

3. Crystallization After a while, solute particles which are already dissolved begin to collide with un- dissolved particles, returning them to solid

4. As more particles dissolve, more particles crystallize until EQUILIBRIUM is reached

5. Equilibrium The rate where particles dissolve equals the rate where particles crystallize. When equilibrium is reached un-dissolved solute remains visible no matter what

6. Saturated Solution no more solute will dissolve max amount of solute at a particular temperature particles dissolve and crystallize but the concentration remains the same

7. Supersaturated Solution a substance that has been heated to dissolve additional solute and then carefully cooled (more than saturated)

8. Qualitative Solubility relative solubility in terms of soluble, low solubility or insoluble

9. Quantitative Solubility The concentration of a solute in a saturated solution at a given temperature # of moles of solute needed to form 1 litre of saturated solution at a specified temp.

10. Solubility of a saturated solution - aka molarity - aka concentration

11. Example A saturated solution produced by dissolveing hydrogen chloride gas in water is called concentrated hydrochloric acid. If 46.5g of hydrogen chloride gas is required to prepare 100mL of concentrated hydrochloric acid at 25C, what is the solubility of hydrogen chloride at 25C?

12. mol/L = HCl

13. Factors that Affect Solubility Temperature temperature (energy) increases the solubility temp decreases the solubility of gases

14. Pressure Increasing the pressure of gases increases the solubility no effect on liquids or solids

15. Nature of Solute and Solvent Depends on the nature of the bonds (polar and non polar) i.e. grease will dissolve in gas but not in water

16. Precipitates 2 aqueous solutions combine & the positive ion (cation) of one combines with the negative ion (anion) of the other to form an insoluble compound (a solid precipitate)

17. Write the net ionic equation and use a solubility table to determine whether a solid will form

18. Example Write the net ionic equation for the formation of a precipitate when aqueous solution of potassium hydroxide and magnesium chloride are mixed 2KOH(aq) + MgCl2(aq)  2KCl(?) + Mg(OH)2(?)

19. Total ionic equation Net ionic equation