reactant
B: (NH4)2C2O4 (aq) → 2 NH4+ (aq) + C2O42- (aq)
D: CaCl2 (aq) → Ca2+ (aq) + 2 Cl- (aq)
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 |
Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.
Write a net ionic equation for the reaction that occurs in the experiment 5.
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Based on our data, we think this problem is relevant for Professor Ngo's class at URI.