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## PowerPoint Slideshow about ' Solubility Equilibria' - acton

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### Solubility Equilibria

Ksp and Qsp

The dissociation equation is written as a reversible reaction. You need to use the table of ions and always remember to balance.

example: silver chloride

AgCl (s) Ag+(aq) + Cl-(aq)

Ksp = [Ag+] [Cl-]

Since the equilibrium constant of such a dissolving reaction is written as the product of the ion concentrations, it is usually called the “solubility product” & written as Ksp instead of Keq.

Meaning of the reaction. You need to use the table of ions and always remember to balance.Ksp

Ksp for AgCl is 1.56 x 10-10. This really means that in a saturated solution containing Ag+ and Cl- ions, the product of the concentrations of Ag+ and Cl-must always equal 1.56 x 10-10 .

Thus if [Ag+] [Cl-] > Ksp, the solution is “supersaturated” and some of the Ag+ & Cl- ions will recombine & precipitate out. If [Ag+] [Cl-] < Ksp, the solution is not saturated and more AgCl will dissolve.

Example: Show the Ksp expression for the dissolving of copper (II) iodate.

Iron (III) hydroxide Ksp values p.578 in text

Ksp reaction. You need to use the table of ions and always remember to balance. Problem Types

Type 1: Finding an equilibrium concentration given the Ksp & other conditions

Example: What will be the [I-] in a saturated solution of AgI where [Ag+] is 0.010 M. Ksp for AgI is 1.5 x 10-16

Type 2: reaction. You need to use the table of ions and always remember to balance. Finding Ksp, given solubility in moles/L (M).

Example 1: The solubility of BaSO4 is 3.9 x 10-5 moles/L. Determine Ksp.

Example 2: Solubility of Al(OH)3 is 0.004 moles/L. Determine Ksp.

Type 3: reaction. You need to use the table of ions and always remember to balance. Find Ksp given solubility in g/L.

Example: the solubility of CaF2 is 0.0180 g/L. Find the Ksp of CaF2.

Type 4: reaction. You need to use the table of ions and always remember to balance.Given Ksp, find the solubility in moles/L or g/L.

Example: The Ksp for Ag2S is 1.6 x 10-49. Find its solubility in a) moles/L b) g/L

Type 5: reaction. You need to use the table of ions and always remember to balance. Predicting if precipitation will occur (Qsp).

Example: Will there be a precipitate of AgCl formed when these are mixed: 250 mL of 0.01 M Ag2SO4 & 250 mL of 0.02 M FeCl3. Ksp of AgCl = 1.8 x 10-10

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