You choose to investigate some of the solubility guidelines for two ions not listed in Table the chromate ion (CrO4 2-) and the oxalate ion (C2O42 - ). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts:
Solution | Solute | Color of Solution |
A | Na2CrO4 | Yellow |
B | (NH4)2C2O4 | Colorless |
C | AgNO3 | Colorless |
D | CaCl2 | Colorless |
When these solutions are mixed, the following observations are made:
Experiment Number | Solutions Mixed | Result |
1 | A + B | No precipitate, yellow solution |
2 | A + C | Red precipitate forms |
3 | A + D | Yellow precipitate forms |
4 | B + C | White precipitate forms |
5 | B + D | White precipitate forms |
6 | C + D | White precipitate forms |
(a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments.
Table Solubility Guidelines for Common Ionic Compounds in Water
Soluble Ionic Compounds |
| Important Exceptions |
Compounds containing | NO3– | None |
| CH3COO– | None |
| Cl– | Compounds of Ag+, Hg22+, and Pb2+ |
| Br– | Compounds of Ag+, Hg22+, and Pb2+ |
| I– | Compounds of Ag+, Hg22+and P2++ |
| SO42- | Compounds of Sr2+, Ba2+, Hg22+, and Pb2+ |
Insoluble Ionic Compounds |
| Important Exceptions |
Compounds containing | S2- | Compounds of NH4+, the alkali metal cations, Ca2+, Sr2+, and Ba2+ |
| CO32– | Compounds of NH4+ and the alkali metal cations |
| PO43– | Compounds of NH4+ and the alkali metal cations |
| OH– | Compounds of NH4+, the alkali metal cations, Ca2+, Sr2+, and Ba2+ |
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