Suppose you had an unknown solution that contained either dissolved NaCL, or NaNO3. You added AgNO3 to the unknown solution and observed that no solid forms. What can be concluded about the unknown solution? (use the solubility rules
There is no chloride in the sample; hence the solution must have NaNO3 if it must be either NaCl or NaNO3.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
To determine what can be concluded about the unknown solution, we need to consult the solubility rules for common salts.
The first step is to understand the solubility rules for various ions. In general, salts containing alkali metal cations (such as Na+) and most nitrate (NO3-) salts are soluble in water.
Based on these solubility rules:
1. Salts containing alkali metals (Group 1 elements) are usually soluble in water.
2. Nitrates (NO3-) are generally soluble in water.
Now, let's analyze the situation. When AgNO3 is added to the unknown solution, it will react with any chloride ions (Cl-) or nitrate ions (NO3-) present to form an insoluble silver salt. The possible reactions are:
AgNO3 + NaCl → AgCl + NaNO3
AgNO3 + NaNO3 → No reaction
If a solid forms when AgNO3 is added, it means that an insoluble silver salt (AgCl) has formed, indicating the presence of chloride ions (Cl-) in the solution. However, if no solid forms, it means that no insoluble silver salt is produced, suggesting the absence of chloride ions (Cl-) in the solution.
Therefore, in this case, since no solid forms, we can conclude that the unknown solution does not contain dissolved NaCl (sodium chloride), but it may still contain NaNO3 (sodium nitrate) or any other soluble salts that do not react with AgNO3 to form an insoluble silver salt.