1. Kc
Ksp!!!!! Kp Kw Ka Kb

2. Recall:
Strong acids and bases dissociate fully,
HBr + H2O  H3O Br Ka = large
whereas weak acids and bases don’t.
HF + H2O ↔ H3O F Ka = 7.2x10-4
Ionic compounds (salts) work the same way!!!

3. Strong salts = soluble salts Weak salts = insoluble salts
(salts containing alkali metals, NO3-1 and NH4+1)
Connect:
“Strong” salts dissociate fully,
NaBr(s)  Na Br Ksp = large
whereas “weak” salts don’t.
PbBr2(s) ↔ Pb Br Ksp = 5x10-4
Weak salts = insoluble salts
(insoluble salts dissolve, just in extremely small amounts)
Ionic compounds (salts) work the same way!!!

4. MX(s) ↔ Ionic Equilibrium:
All you need to know about slightly soluble salts …
MX(s) ↔

5. 3.00 grams of AgBr is added to 50 mL of water.
Ionic Equilibrium:
Silver bromide, AgBr
3.00 grams of AgBr is added to 50 mL of water.

6. Ionic Equilibrium: Silver bromide, AgBr
- Write the equation for AgBr dissolving in water.
- Write the equilibrium constant expression.
- The molarity of Ag+ in 50 mL of saturated solution is 7.35x10-7 M. What is the Ksp value for AgBr ?
- An additional 50 mL of water is added to the previous solution, more AgBr dissolves, and equilibrium is achieved again. What is the [Ag+]?

7. e. Does the concentration of solution at equilibrium (saturated solution) change with volume???
If a solution is saturated (or at equilibrium), the ion conc.’s will be the same

8. Ionic Equilibrium: Lead(II) iodide, PbI2
Lead nitrate and sodium iodide solutions are mixed to produce a precipitate.
- Write the solubility product constant expression for the precipitate produced
- What is molar concentration of PbI2 if the Ksp = 8.8x10-9?
- The [Pb+2]? The [I-1]?
- What volume of water would be required to completely dissolve 10 grams of lead(II) iodide? (PbI2 is 461 g/mol)

9. Practice:
Try 1, 3 and 6 right now!

10. Practice:
Try 1, 3 and 6 right now!

11. Practice:

12. Old stuff

13. Remember some old stuff:
Ionic compounds are made of cations and anions, usually metals and non-metals
Ionic compounds are called salts
A given volume of solvent can only hold so much dissolved solute …
When a solution contains this maximum amount it is saturated

14. Ionic Equilibrium:
Key points about saturated solutions …
1. A saturated solution is one in which an equilibrium has been established between the solid salt and the dissolved ions.

15. Key points about saturated solutions …
Ionic Equilibrium:
Key points about saturated solutions …
1. A saturated solution is one in which an equilibrium has been established between the solid salt and the dissolved ions.
2. The concentration of ions in solution at equilibrium (saturated) does NOT depend on volume.

16. The max solubility at this temp is 5g/L
g of diss. salt sat’d? conc.
-Fill to 500 mL 
-Fill to 1 L 
-Fill to 1.5 L 
-Add another 5 g of salt 
Key points about saturated and unsaturated solutions . . .
1. A saturated solution is one in which an equilibrium has been established between the solid salt and the dissolved ions.
2. The concentration of ions in solution at equilibrium (saturated) does NOT depend on volume.
5 grams

17. Key points about saturated solutions …
Ionic Equilibrium:
Key points about saturated solutions …
1. A saturated solution is one in which an equilibrium has been established between the solid salt and the dissolved ions.
2. The concentration of ions in solution at equilibrium (saturated) does NOT depend on volume.
3. All salts ionize to some extent: the “insoluble” salts from the sol. rules are those with extremely low solubilities