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Solubility Product Constant

Solubility Product Constant. What is Ksp ? Relationship . Go here to visualize salt dissolving in water. . Solubility Product Constant ( Ksp ). Solubility Product Constant, K sp is the equilibrium constant for a solid substance dissolving in an aqueous solution.

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Solubility Product Constant

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  1. Solubility Product Constant What is Ksp? Relationship

  2. Go here to visualize salt dissolving in water.

  3. Solubility Product Constant (Ksp) • Solubility Product Constant, Ksp is the equilibrium constant for a solid substance dissolving in an aqueous solution. • It represents the level at which a solute dissolves in solution. • The more a substance dissolves, the higher the Kspvalue it has.

  4. BaSO4(s) Ba2+(aq) + SO42−(aq) Solubility Products Consider the equilibrium that exists in a saturated solution of BaSO4 in water: The equilibrium constant expression for this equilibrium is Ksp= [Ba2+] [SO42−] where the equilibrium constant, Ksp, is called the solubility product.

  5. Oh – you mean like solubility? • Ksp is not the same as solubility. • Solubility is generally expressed as: - mass of solute dissolved in volume (g/mL) - mol/L (M).

  6. Example 1 • Calculate the solubility product constant for lead(II) chloride, if 50.0 mL of a saturated solution was found to contain 0.2207 g of lead (II) chloride dissolved in it. Write reaction and Ksp expression. PbCl2(s)  Pb2+(aq) + 2Cl-(aq) Ksp = [Pb2+][Cl-]2

  7. Example 1 • Calculate the solubility product constant for lead(II) chloride, if 50.0 mL of a saturated solution was found to contain 0.2207 g of lead (II) chloride dissolved in it. Convert to Molarity! 0.0159 M PbCl2 ICE TABLE! Ksp = [0.0159][0.0318]2 = 1.61 x 10-5

  8. Example 2 (Other Direction) • Estimate the solubility of Ag2CrO4 in pure water if the solubility product constant for silver chromate is 1.1 x 10-12 Write reaction and Ksp expression. Ag2CrO4(s) 2 Ag+(aq) + CrO42-(aq) Ksp = [Ag+]2[CrO42-]

  9. Example 2 (Other Direction) • Estimate the solubility of Ag2CrO4 in pure water if the solubility product constant for silver chromate is 1.1 x 10-12 Let "x" be the number of moles of silver chromate that dissolves in every liter of solution (molassuming 1 L) ICE TABLE! 1.1 x 10-12 = [2x]2[x] x = 6.50 x 10-5 M

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