Solubility Product KSP

Please Write Solubility: Is the maximum amount of a substance that can dissolve in a given volume of solvent. Dependent on temperature. mol/L or g/L Unsaturated solution: More solute can be dissolved. Saturated solution: Any solute added will precipitate out. An equilibrium is formed: Solute (s) ⇆ + ion (aq) + - ion (aq) Dissolved Ions Solid Solute

Ksp - solubility product Please Write AgCl(s)⇆ Ag+(aq) + Cl-(aq) Ksp = [Ag+][Cl-] If the ion concentration is high: Ksp >1 High solubility Substance is “soluble” If the ion concentration is low: Ksp <1 Low solubility Substance is “insoluble”

Ex. 1 If the solubility of BaSO3 is 0.0025g/L, find the Ksp. Please Write BaSO3(s)⇆ Ba2+(aq) + SO32-(aq) Ksp = [Ba2+][SO32-] Ex. 1 If the solubility of BaSO3 is 0.0025g/L, find the Ksp. Since it dissociates with 1:1, the [Ba2+] & [SO32-] = #moles of BaSO3 dissolved (0.0025 g/L). We have to convert g/L into mol/L 1 𝑚𝑜𝑙 𝐵𝑎𝑆𝑂3 𝑥 = 217.4𝑔 0.0025𝑔 x = 1.15x10-5 mol/L So [Ba2+] = [SO32-] = 1.15x10-5 mol/L Ksp = [Ba2+][SO32-] =(1.15x10-5)(1.15x10-5) = 1.32x10-10

Ex.2 What is the solubility Al(OH)3? Ksp = 2.6 x 10-39 Please Write Ex.2 What is the solubility Al(OH)3? Ksp = 2.6 x 10-39 Al(OH)3 (s)  Al+3 (aq) + 3OH- (aq) 1 : 1 : 3 Ksp = [Al+3][OH-]3 2.6 x 10-39 = [x][3x]3 Al(OH)3 = 9.9 x 10-11 M 2.6 x 10-39 = 27x4

Ksp practice questions If the dissociation of Calcium chloride produces a solution containing a concentration of 0.0300 mol/L of Calcium ions and 0.0600 mol/L of Chloride ions, what is the Ksp of the reaction? If the solubility of MgF2 is 1.30×10-4 g/100 mL, find the Ksp of this reaction. If the Ksp of barium cyanide, Ba(CN)2, is 0.00260 at 25°C, find the concentration of deadly cyanide ions (CN-) at equilibrium.