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Solubilities

Solubilities. Relative solubility. Comparing how soluble one salt is to another can only be predicted by comparing K sp values only for salts that produce the same total number of ions . MX  M + + X - K sp = [ M + ] [ X - ] [M + ] = [ X - ] K sp = x 2

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Solubilities

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  1. Solubilities

  2. Relative solubility Comparing how soluble one salt is to another can only be predicted by comparing Ksp values onlyfor salts that produce the same total number of ions. MX M+ + X- Ksp= [M+] [X-] [M+] = [X-] Ksp = x2 MX2  M2++ 2 X- Ksp = [M2+] [X-]2 [M+] =2 [X-] Ksp = 4x3

  3. The Common Ion Effect This is dissolving a salt in a solution that contains one the ions. You will need an ICE chart. Calculate the solubility of solid CaF2 (Ksp = 4.0 x 10-11) in a 0.025 MNaF solution.

  4. pH and Solubility This is primarily LeChâtelier’s principle If a compound contains the conjugate base of a weak acid, addition of H3O+from a strong acid will increase the compound’s solubility. Predict the Effect on Solubility Write balanced equations to show how addition of HNO3 will affect the solubility of a) calcium fluoride b) zinc acetate c)silver iodide.

  5. Predicting the Formation of a Precipitate: Kspvs. Qsp Dissociation equations Solid (precipitate) ⇌ Dissolved If Ksp=Qsp, then the solution is saturated and no change occurs. If Ksp < Qsp, then a precipitate forms until the solution is saturated. If Ksp> Qsp, then the solution is unsaturated and no precipitate forms.

  6. Predicting Whether a Precipitate Will Form Phosphate in natural waters often precipitates as insoluble salts,such as Ca3(PO4)2. In a certain river, [Ca2+]init2.0 x 10-8M. and [PO43-]init=1.0 x 10-9 M. Will Ca3(PO4)2 precipitate? Kspof Ca3(PO4)2= 1.2 x 10-29.

  7. Selective Precipiation Selective precipitation is a technique to separate metal ions from a solution with multiple ions present. A reagent whose anion forms a precipitate with either one or a few metal ions in the mixture will precipitate certain metals out of solution and leave the others. So a solution of Ca2+ K+, can be separated by adding a CO32- ion because this will form a precipitate with calcium

  8. Problem A solution contains 1.0 x10-4 M Cu+ and 2.0 x10-3 M Pb2+. If a source of I- is added gradually to this solution, will PbI2 (Ksp = 1.4 x10-8) or CuI (Ksp = 5.3 x10-12) precipitate first? Specify the concentration of I- necessary to begin precipitation of each salt.

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