1. Ksp Values that indicate how soluble a solute is.
Leads us to calculate the molarity of ions in solution.

2. Solubility Equilibrium
All compounds ionize to some extent:
PbCl2(s) ↔ Pb+2(aq) + 2Cl-1(aq)
NaCl(s) ↔Na+(aq) + Cl-(aq)
Solubility constants are known values for the relative solubility in room temp
Ksp for PbCl2 = 1.6 x 10-5
Ksp for NaCl = 36
smaller number = less soluble

3. Which substance is more soluble?
CaCO3
Ksp = 4.7 x10-9
Mg(OH)2
Ksp = 8.8 x 10-12
The larger the
number the
more soluble the
substance is

4. Solubility Product Expression
Is written from the ionization of the compound
PbCl2(s) ↔ Pb+2(aq) + 2Cl-1(aq)
Ksp = [Pb+2][Cl-1]2
multiply

5. Practice problem
The solubility product constant of lead II chloride is 1.6 x 10-5 at 25oC. Calculate concentrations of the lead & chloride ions in solution.
Step 1: write ionization reaction
Step 2: assign Xs
Step 3: solubility product expression
Step 4: substitute using Xs & solve
[Pb+2] = 1.6x10-2
[Cl-] = 3.2x10-2

6. How did you get those answers??????

7. The [Ni2+] in a saturated solution of nickel II hydroxide is 2
The [Ni2+] in a saturated solution of nickel II hydroxide is 2.2x10-12 M. What is the Ksp?
4.26x10-35

8. How did
you get THAT??????

9. The Ksp of aluminum sulfate is 1. 42 x 10-12 at 25oC
The Ksp of aluminum sulfate is 1.42 x at 25oC. Calculate the concentrations of the aluminum ions and sulfate ions in a saturated solution.
[Al+3] = 3.3x10-3 M or mol/L
[SO4 -2] = 5.0x10-3 M or mol/L

10. How did
you get THAT??????

11. The ENd