# Section 18.1-2

```Solubility and Complexation
Equilibria
Chapter 18
Is AgCl soluble or insoluble?
Dissolution Reactions and Ksp Expressions
AgCl(s)
Mg(OH)2(s)
Ca3(PO4)2(s)
Standard Reaction Types:
Determining Ksp Experimentally
The solubility of PbF2 is found to be 0.525 g/L. What is Ksp?
Predicting Solubility
+


AgCl(s) 
Ag
(aq)
+
Cl
(aq)

Ksp = [Ag + ][Cl- ] = 1.8  10-10

 3 Zn 2+ (aq) + 2 PO 43- (aq)
Zn 3 (PO 4 ) 2 (s) 

K sp = [Zn 2+ ]3[PO 43- ]2 = 9.1  10-33

 Fe3+ (aq) + 3 OH - (aq)
FeCl3 (s) 

Ksp = [Fe3+ ][OH- ]3 = 2.0  10-39
Can you eyeball rank solubilities?
AgCl
AgBr
AgCl
CaF2
Standard Types
Determining if a precipitation will occur:
Determining if a precipitation will occur:
If 5.0 mL of 1.0 x 10-3 M NaCl is added to 1.0 mL of 1.0 x 10-3 M Pb(NO3)2,
will solid PbCl2 (Ksp = 1.7 x 10-5) precipitate?
If a precipitate will not form, what chloride ion concentration
will cause a precipitate of lead chloride to form?
Determining if a precipitation will occur:
If 5.0 mL of 1.0 x 10-3 M NaCl is added to 1.0 mL of 1.0 x 10-3 M Pb(NO3)2,
will solid PbCl2 (Ksp = 1.7 x 10-5) precipitate?
If a precipitate will not form, what chloride ion concentration
will cause a precipitate of lead chloride to form?
Common Ion Effect: The presence of an ion common to a
solubility equilibrium will decrease solubility of the salt.
Will PbCl2 be more soluble in pure water or
in a 0.200 M NaCl solution?
Common Ion Effect: The presence of an ion common to a
solubility equilibrium will decrease solubility of the salt.
What is the solubility of PbCl2 in pure water and
in a 0.200 M NaCl solution? (Ksp = 1.7 x 10-5)
Common Ion Effect: The presence of an ion common to a
solubility equilibrium will decrease solubility of the salt.
What is the solubility of PbCl2 in pure water and
in a 0.200 M NaCl solution?
```
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