A salt was completely soluble in water. When this solution was treated with AgNO3 no precipitate was formed. What anions could be present?
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
To determine the possible anions present in the solution, we need to consider the solubility rules for common salts. Let's go through the process step by step:
1. Start by identifying the salt that was completely soluble in water. Since it was completely soluble, it means that the cation of the salt is not the determining factor for the lack of precipitation when AgNO3 is added. Therefore, we can focus on the anions.
2. Consider the solubility rules for common anions:
- Most nitrate (NO3-) salts are soluble and do not form precipitates with AgNO3.
- Most chloride (Cl-), bromide (Br-), and iodide (I-) salts are soluble. However, they do form precipitates with AgNO3.
- Most sulfate (SO42-) salts are soluble, but there are exceptions. Certain sulfates, such as barium sulfate (BaSO4) and lead(II) sulfate (PbSO4), are insoluble and do form precipitates with AgNO3.
- Carbonate (CO32-), phosphate (PO43-), and sulfide (S2-) ions generally form insoluble salts that will precipitate with AgNO3.
3. Based on the given information that there was no precipitate when AgNO3 was added, we can eliminate the possibility of chloride, bromide, iodide, carbonate, phosphate, and sulfide anions being present.
4. This leaves us with nitrate (NO3-) and sulfate (SO42-) as possible anions. Since nitrate salts are generally soluble and do not form precipitates with AgNO3, the most likely anions present in the solution are nitrate (NO3-).
So, in conclusion, the anion that could be present in the solution is nitrate (NO3-).