Cathy Notes
Sample Analysis. Precipitates and Complexes of Silver Ion
Data for Determining Formulas
Solutions containing NH3, CO32–, Cl–, I–, PO43–, and S2O32– ions were added to equal proportions of a silver nitrate solution, which contained the complex ion Ag(H2O)2+. All of the added solutions were also clear and colorless.
|AgNO3 (aq) by itself |Colorless solution |
|AgNO3 (aq) with NH3 (aq) |Colorless solution |
|AgNO3 (aq) with Na2CO3 (aq) |Pale yellow precipitate |
|AgNO3 (aq) with NaCl (aq) |White precipitate |
|AgNO3 (aq) with NaI (aq) |Yellow precipitate |
|AgNO3 (aq) with Na3PO4 (aq) |Yellow precipitate |
|AgNO3 (aq) with Na2S2O3 (aq) |Colorless solution |
Formulas of Silver Complexes and Precipitates
Ag+ ions formed precipitates with CO32–, Cl–, I–, and PO43– ions. Solids are electrically neutral; the charges of all their ions add up to zero. Therefore, the formulas of these precipitates are: Ag2CO3, AgCl, AgI, and Ag3PO4. It is not obvious from these observations that Ag+ ions formed soluble complex ions with NH3 and S2O32– ions. However, data on the next page shows that solutions containing NH3 and S2O32– ions were able to convert the pale yellow precipitate Ag2CO3 into colorless solutions. Thus, complex ions more stable than Ag2CO3 must have formed. Ag+ has a coordination number of 2, so it binds to two ligands when it forms complex ions. The formulas of the
Data for Determining Formulas
Solutions containing NH3, CO32–, Cl–, I–, PO43–, and S2O32– ions were added to equal proportions of a silver nitrate solution, which contained the complex ion Ag(H2O)2+. All of the added solutions were also clear and colorless.
|AgNO3 (aq) by itself |Colorless solution |
|AgNO3 (aq) with NH3 (aq) |Colorless solution |
|AgNO3 (aq) with Na2CO3 (aq) |Pale yellow precipitate |
|AgNO3 (aq) with NaCl (aq) |White precipitate |
|AgNO3 (aq) with NaI (aq) |Yellow precipitate |
|AgNO3 (aq) with Na3PO4 (aq) |Yellow precipitate |
|AgNO3 (aq) with Na2S2O3 (aq) |Colorless solution |
Formulas of Silver Complexes and Precipitates
Ag+ ions formed precipitates with CO32–, Cl–, I–, and PO43– ions. Solids are electrically neutral; the charges of all their ions add up to zero. Therefore, the formulas of these precipitates are: Ag2CO3, AgCl, AgI, and Ag3PO4. It is not obvious from these observations that Ag+ ions formed soluble complex ions with NH3 and S2O32– ions. However, data on the next page shows that solutions containing NH3 and S2O32– ions were able to convert the pale yellow precipitate Ag2CO3 into colorless solutions. Thus, complex ions more stable than Ag2CO3 must have formed. Ag+ has a coordination number of 2, so it binds to two ligands when it forms complex ions. The formulas of the