| 1010 - Ksp |
| 1010 - Know that the solubility product constant, Ksp, defines the equilibrium constant for the dissolution of an ionic compound into its constituent ions. |
| 1020 - Calculate the molar solubility of an ionic compound in pure water using the Ksp expression and an ICE table. |
| 1030 - Know that the solubility of an ionic compound is lower in a solution containing a common ion than in pure water. |
| 1040 - Calculate the molar solubility of an ionic compound in the presence of a common ion using the Ksp expression and an ICE table. |
| 1050 - Know that the solubility of an ionic compound containing a basic anion increases with decreasing pH. |
| 1020 - Qualitative Analysis |
| 1010 - Know that the precipitation of an ionic compound upon mixing aqueous solutions can be predicted using the Q expression and comparing Q to Ksp. |
| 1020 - Define selective precipitation, and know and understand how cations can be selectively precipitated based on their differential solubility with various anions. |
| 1030 - Know and understand that differential precipitation is the basis of the qualitative analysis of cations in solution. |
| 1040 - Apply the qualitative analysis scheme based on sequentially insoluble chlorides, acidinsoluble sulfides, base-insoluble sulfides and hydroxides, insoluble phosphates, and alkali metals and ammonium. |
| 1050 - Know that alkali metals give a characteristic color upon heating in an open flame. |
| 1030 - Complex Ions |
| 1010 - Define complex ion and ligand. |
| 1020 - Know that metal cations form complex ions with a series of anionic and neutral ligands. |
| 1030 - Calculate complex ion equilibria using formation constants, Kf, and cation and ligand concentrations. |
| 1040 - Know that amphoteric metal hydroxides, like Al(OH)3, are more soluble in acidic and in basic solution than in pure water. |