Transcript Precipitation Equillibria

Expression for Ksp :

write the equation for the ionization of AgCl.
Remember (s) or pure (l), do not appear in
equilibrium expressions.
Also the concentration of each ion is raised to a
power equal to its coefficient
Calculation or [ ] of one ion
knowing that of the other.
2. Determination of whether a
precipitate will form.
3. Water solubility
4. Common ion effect.
1.
Solubilasaurus
What is the [Pb2+] in a solution with lead (II) chloride if
the [Cl-] = 0.0200M?
PbCl2
Ksp= 1.7x10-5
Write the ionization equation
Write the Ksp expression
Plug in known values, solve for [Pb2+]
Q>Ksp the solution contains a higher
[ion] than it can hold at equilibrium.
A PRECIPITATE FORMS.
Q<Ksp the solution contains a lower
[ion] of ions than is required for
equilibrium.
NO PRECIPITATE
Q=Ksp saturated w/ions to the point of
precipitation. (…just 1 more ion)
Cadmium (II) hydroxide has a Ksp = 2.5x10-14
if the [Cd2+] = 1.5 x 10-6, what is the [OH-]?
Calculate the concentration of each of the
following ions in equilibrium with 0.0034M Ba2+
F-
SO42-
BaSO4  Ba2+ + SO42-
Ksp = 1.1 x 10-10
Ions of different charges:
BaF2  Ba2+ + 2 F-
Ksp = 1.8 x 10-7
A solution already containing one of the ions.
BaSO4   Ba2+ + SO42Ksp = 1.1 x 10-10
Find the solubility (s) mol/L of 0.10M Na2SO4
Using insoluble compounds to remove an ion from
solution.
How could you separate Na+ ions and Mg2+ ions?
Which of the following anions would remove Mg2+ ?
ClC2H3O2OHCO3-
A flask contains 0.10M Cl- and 0.010 M CrO42Which ion precipitates first when AgNO3 is added?
Ksp AgCl = 1.8 x 10-10
Ag2CrO4 = 1.0 x 10-12
Calculate the [Ag+] needed to ppt the ions.