A salt was completely solbuble in water when this solution was treated with AgNO3 no precipitate was formed. What anions could be present?
To determine the possible anions present in the solution, we need to consider the solubility rules of commonly encountered salts.
1. Start by referencing a solubility table or chart, which provides information on the solubility of different salts in water. This table outlines which salts are soluble and which are insoluble in water.
2. Look specifically for salts that are soluble in water. If the original salt in question was completely soluble, this means that the anion from the original salt is compatible with water and forms a stable, soluble compound.
3. Identify the anions that do not form precipitates when treated with silver nitrate (AgNO3). The common anions that form soluble compounds with silver ion (Ag+) are chloride (Cl-), nitrate (NO3-), sulfate (SO4^2-), and acetate (C2H3O2-).
4. However, the absence of a precipitate when AgNO3 is added suggests that none of these anions are present in the solution. This could indicate that the anion present is none of the above or is present in a very low concentration.
5. It is important to note that this conclusion is solely based on the absence of a precipitate when AgNO3 is added. Further tests or analysis methods would be needed to confirm the presence or absence of specific anions.
In summary, based on the information provided, the anion in the solution could be any anion that does not form a precipitate with AgNO3, except for chloride (Cl-), nitrate (NO3-), sulfate (SO4^2-), and acetate (C2H3O2-). Additional tests or information would be required for further identification.