You have aqueous solutions of Ag* and PO43 that have equal concentrations. You mix them according to the following table: Test Tube # Number of drops Ag Number of drops PO4³- 0 5 4 1 3 3 9 2 8 3 6 6 4 8 Assuming the product of the reaction is insoluble, which test tube will contain the most precipitate? 5 9 3
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![You have aqueous solutions of Ag⁺ and PO₄³⁻ that have equal concentrations. You mix them according to the following table:
| Test Tube # | 1 | 2 | 3 | 4 | 5 |
|-------------|---|---|---|---|---|
| Number of drops Ag⁺ | 3 | 4 | 6 | 8 | 9 |
| Number of drops PO₄³⁻ | 9 | 8 | 6 | 4 | 3 |
**Question:** Assuming the product of the reaction is insoluble, which test tube will contain the most precipitate?
- [ ] 5
- [ ] 1
- [ ] 4
- [ ] 2
- [ ] 3
Explanation: The table shows the number of drops of Ag⁺ and PO₄³⁻ added to each test tube. To determine which test tube contains the most precipitate, consider the stoichiometry of the reaction and the limiting reagents.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff753bfa8-1ffa-4ebf-8e17-943d9e514202%2Fd4cdee0b-cb33-4e2b-bde7-946592b46059%2F57suxcl_processed.jpeg&w=3840&q=75)
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