2. is the maximum amount of solute in a solvent at a given temperature saturated solution, [ ]max equilibrium between: solid crystals  dissolved ions eg. AgNO 3(s)  Ag 1+ (aq) + NO 3 1- (aq)

3. 1 st - H 2 O needs to separate - H-bonding needs to be overcome - dissolving - NRG input 1 st

4. 3 rd 2 nd 2 nd - H 2 O removes ions from the lattice - dissociation - NRG input 3 rd - hydration of ions - Ion – dipole force -  with  H 2 O - NRG output

5. solubility is a contest between: lattice energies vs hydration energies ionic bond strengths vs ion-dipole forces usually exothermic with increased disorder if undissolved solid is present, then it is a mixture with a saturated sol’n phase

6. equilibrium expression for slightly soluble salts If:A x B y(s)  xA m+ (aq) + yB n- (aq) Then:

7. Saturation can be tested by Q: If:Q = Ksp thenit is a saturated solution Q > Ksp there is noticeable precipitate Q < Ksp unsaturated refers to the amount of solid that can dissolve not how much is in solution solubility units are g/100g or g/100 mL or g/L

8. To find Concentration from Solubility: [ ]max = solubility  M solute and V adjustment eg. Solubility of Mg(OH) 2 is 3.45 g/100 mL. = molar solubility To find Solubility from Concentration: Solubility = molar solubility x M solute and V change

10. 1) Ksp from solubility eg.Calculate the K sp of Ag 2 CO 3 given its solubility of 0.0014 g/100g. 1 st - calculate the [ ] from solubility: 2 nd - create ICE table. - Since dealing with a solid, the equilibrium is simplified

11. Q – not necessary 100 Rule – not necessary

12. 2) Solubility from Ksp types:solubility, molar solubility, [ion] eq, amount of solid that will dissolve - all from calculating “x” eg.How much PbI 2 at SATP will dissolve in 1.00 L of water? Give the solute ion concentration, [Pb 2+ ] eq, solubility (g/100mL) and molar solubility. Ksp of PbI 2 from textbook is 8.5 x 10 -9 -when not given the Ksp and not asked to calculate it, find it in the reference table or the textbook

13. -as the solid is not included and the [ion] i = 0, we can write ICE horizontally instead of vertically ICE +x +2x = the molar solubility

14. Predicting Precipitation: Used to determine precipitation when mixing 2 sol’ns just like in double displacement rxns Don’t  by 100 - it is a unit 100 mL

15. eg.Will precipitation occur when 5.0 ml of 0.030 M AgNO 3 is mixed with 1.0 ml of 0.0050 M Na 2 CrO 4 ? (K sp = 1.1 x 10 -12 for Ag 2 CrO 4 )? 1 st – write down each reaction and calculate the V and C values

16. 2 nd – write down the equilibrium equation, calculate the new [ ] in the combined sol’n 3 rd – calculate Q and compare with K sp